Chemistry for Changing Times, 13E Hill, McCreary, Kolb Solution Manual

Chemistry for Changing Times, 13E By Hill,McCreary, Kolb

Email: Richard@qwconsultancy.com

Chapter 1: Chemistry Overview Chapter 1 introduces the student to the concepts of science—its ability to solve problems as well as its limitations. The student is then introduced to the concept of matter and energy and the physical means by which they are measured.

Lecture Outline 1.1

1.2 1.3

1.4 1.5 1.6 1.7

1.8

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Science and Technology: The Roots of Knowledge Many students are confused about the differences between science and technology. Technology is the direct application of knowledge to solve problems. Science seeks an understanding of underlying principles.

Changing Perceptions and Changing Practices Science: Reproducible, Testable, Tentative, Predictive, and Explanatory The scientific method, from hypothesis to law, theory, or model. is best explained by example.

Science and Technology: Risks and Benefits Chemistry: Its Central Role Solving Society’s Problems: Scientific Research Research can be basic or applied.

Chemistry: A Study of Matter and Its Changes Matter is anything that has mass.

Mass is a measure of the amount of matter present.

Weight is mass times gravitational attraction.

Matter exhibits chemical and physical properties.

Chemical properties tell us how matter will combine to form new and different substances (a chemical change).

Physical properties are directly observable: Color, state (solid, liquid, or gas), and texture are examples.

An excellent demonstration is to burn a candle (chemical change) and boil water (physical change).

Classification of Matter (a) States of Matter • Solids, liquids, and gases (b) Substances and Mixtures • Substances have constant composition.

• The composition of a mixture is variable.

▪ Homogeneous mixtures appear the same throughout (milk, paint, and saltwater are examples).

▪ Heterogeneous mixtures appear different throughout (pizza, raisin bread, and chocolate chip cookies are examples.) (c) Elements and Compounds • Substances are either elements or compounds.

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1.9

1.10 1.11

1.12

Elements are fundamental building blocks of all matter.

Lead, silver, gold, carbon, and oxygen are examples.

▪ Compounds are two or more elements chemically combined in fixed ratios. Water, ammonia. and propane are examples. (d) Atoms and Molecules The Measurement of Matter Most students have been introduced to the metric system during their K–12 education; the SI system used in science is based on the metric system. The difference lies in the base units.

• Base units: kilograms (kg) for mass, meter (m) for length, and seconds (s) for time. The four other base units are shown in Table 1.4.

Density Density is the mass-to-volume ratio of matter.

Energy: Heat and Temperature The SI unit of temperature is the kelvin (K); however, the temperature scale used in the chemistry laboratory is usually the Celsius scale. The Celsius scale was developed with the freezing and boiling points of pure water at a pressure of 1 atmosphere as the reference frames. (Students find the history of the development of the Fahrenheit scale much more interesting!)

Critical Thinking

Demonstrations 1. Place samples of various elements (e.g., copper, sulfur, zinc, mercury, aluminum, carbon, etc.) in small stoppered bottles or flasks that can be passed around.

2. Ask students: "Which is heavier: lead or aluminum?" They will say "lead".

Then bring out two flasks, a 50-mL flask with about 10 mL of lead shot and a 500-mL flask about 3/4 full of aluminum pellets. Point out that the aluminum is heavier. But we need to compare samples of the same size (volume).

Weight per unit volume is density. Lead has the greater density.

3. Compare a yardstick and a meter stick. A meter is slightly bigger than a yard.

A sugar cube is approximately 1 mL. An ordinary paper clip weighs about 1 gram.

A liter is a little bit (6%) larger than a quart.

4. Use Crispix® and Raisin Bran® to illustrate the difference between a compound and a mixture. Raisins and bran flakes are easily separated, and the ratio of raisins to flakes can vary. Crispix® has a 1:1 ratio of corn and rice flakes, and they cannot be easily separated.

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5. Ice floats on water because the density of ice is less than that of water.

Alcohol has a much lower density. If you use alcohol instead of water, the ice will sink. Place a glass of water and a glass of alcohol side by side and add an ice cube to each one.

6. The Cartesian diver is a popular demonstration about density. Completely fill a 2-liter plastic bottle with water and put just enough water into a medicine dropper so that it can barely float. Put the dropper into the bottle, and cap the bottle. Squeeze and release the bottle to make the "diver" go up and down.

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Chapter 2: Atoms Overview Chapter 2 begins with the Greek concept of matter and moves chronologically forward through the development of the atomistic model of matter.

Lecture Outline 2.1

2.2

2.3

2.4

2.5

Atoms: Ideas from the Ancient Greeks The Greek philosophers had two main ideas regarding matter: (a) The atomistic view (Leucippus and Democritus) (b) The continuous view (Aristotle) Scientific Laws: Conservation of Mass and Definite Proportions Lavoisier was the first great experimentalist. More than anything, he introduced experimental chemistry to Western civilization. Through his experiments, he formulated the Law of Conservation of Mass, which states that matter is neither created nor destroyed during a chemical reaction.

John Dalton and the Atomic Theory of Matter John Dalton summarized the work of Lavoisier and Proust to form the famous Atomic theory.

Mendeleev and the Periodic Table John Dalton established relative atomic masses using hydrogen as a base.

Mendeleev arranged a table of elements according to increasing atomic weights placing elements with similar properties in the same column. This was the beginning of the modern periodic table.

Atoms and Molecules: Real and Relevant

Demonstrations 1. Electrolysis of water.

2. Fill three flasks with zinc (gray powder), sulfur (yellow powder), and zinc sulfide (white powder), and show to the class to illustrate how the properties of a compound differ from those of the component elements. (Or use mercury [silver liquid], oxygen [colorless gas], and mercuric oxide [red powder].)

3. Use samples of metals and nonmetals to demonstrate the difference in their properties. (Aluminum foil, copper wire, nickel coin, zinc strip; capped bottle of liquid bromine, balloon filled with hydrogen, bottles of carbon, sulfur, etc.)

4. Using the largest nuts and bolts you can find, start with unequal numbers of nuts and bolts (e.g., 5 and 7). Connect the pairs of nuts and bolts, with some remaining unpaired, to illustrate the Law of Definite Proportions.

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5. Heat a sample of HgO in a large test tube with a burner. Mercury droplets form on the inside of the tube. Test for oxygen with a glowing splint, which bursts into flame when inserted into the test tube.

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Chapter 3: Atomic Structure Overview Chapter 3 examines the experimental evidence leading to Modern Atomic theory. The chapter opens with the earliest experiments that indicated the electrical nature of matter and concludes with Modern Quantum theory.

Lecture Outline 3.1

3.2

3.3

3.4

3.5

3.6

3.7

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Electricity and the Atom Humphry Davy’s experiments with the voltaic pile led to the electrolysis of molten salts. Michael Faraday refined Davy’s procedures and became the father of electrochemistry. Cathode-ray tube experiments conducted by J. J. Thomson allowed him to calculate the mass-to-charge ratio of the electron. Conducting similar experiments, Eugen Goldstein discovered the proton. Millikan’s oil-drop experiment enabled him to calculate the charge of the electron, and thus its mass.

Serendipity in Science: X-Rays and Radioactivity Roentgen, in 1895, stumbled upon X-rays while conducting cathode-ray experiments.

Three Types of Radiation The alpha particle () is a helium nucleus.

The beta particle () is an electron.

The gamma ray () is a high-energy photon.

Rutherford’s Experiment: The Nuclear Model of the Atom The gold-foil experiment was strong and convincing evidence that led to the Theory of the Nuclear Atom.

The Atomic Nucleus The nucleus contains protons (+1 charge), neutrons (neutral), and nearly all the mass of the atom. Electrons are outside the nucleus, have a -1 charge, and only a fraction of the mass of the proton and neutron. It is the number of protons that defines an element. Isotopes are atoms of the same element having different numbers of neutrons, and thus varying in mass.

Electron Arrangement: The Bohr Model Spectroscopic evidence led Bohr to conclude that only certain energy levels, or orbits, were allowed for electrons.

Electron Arrangement: The Quantum Model Louis de Broglie showed that the electron had wave properties.

Schrodinger used the de Broglie Wave theory and the Bohr Quantum theory to derive the Quantum Mechanical theory of the atom. The Quantum Mechanical theory describes the positioning of electrons about the nucleus and electron energies.

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Electron Configurations and the Periodic Table Figure 3.23 is an excellent tool for teaching students about electronic configurations, using shorthand spectroscopic notation based on element locations in the periodic table.

Demonstrations 1. Demonstrate the use of a cathode-ray tube, using a magnet to deflect the beam of electrons.

2. Models that can be used to demonstrate the Rutherford gold-foil experiment are described in Tested Demonstrations, Vol. II, by George Gilbert, et al., on pages L-2,3,4.

3. An overhead projector version of the Rutherford experiment is described by Hau in J. Chem. Educ., 1982, p. 973.

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Chapter 4: Chemical Bonds Overview Chemical bonds determine the properties of matter. Chapter 4 examines ionic and covalent bonds, the symbolism used to represent bonds, and the resulting shape and properties of molecules and compounds that result from different types of bonding.

Lecture Outline 4.1

4.2

4.3

4.4

4.5

4.6

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The Art of Deduction: Stable Electron Configurations The most stable electron configurations are those of the noble gases.

Other elements that can alter their electron structures to become like those of noble gases would become less reactive by doing so.

Formation of isoelectronic ions Lewis (Electron-Dot) Symbols Use the periodic table to determine the number of valence electrons.

Lewis dot symbols use “dots” to represent valence electrons.

The Reaction of Sodium and Chlorine Facts: Sodium reacts with chlorine to form sodium chloride (salt) according to the chemical equation: 2 Na + Cl2 → 2 NaCl (Na+ and Cl- ions) Theory: Chlorine takes an electron from sodium, forming the chloride and sodium ions.

The sodium and chloride ions are pulled together by coulombic forces (attraction of positive and negative, the electromagnetic force), forming what is called an ionic bond.

Although the names of atoms and ions are similar, the atom and the ion are quite different chemically, so it is important that we make distinctions and use precise terminology.

Using Lewis Symbols for Ionic Compounds Active metal—active nonmetal compounds form ionic bonds.

Generally speaking, metallic elements in Groups 1A and 2A react with nonmetallic elements in Groups 6A and 7A to form ionic compounds.

These are stable crystalline solids.

Atoms gain or loose electrons to have an octet of electrons, similar to the noble gas configurations.

Formulas and Names of Binary Ionic Compounds Learn to write the names and formulas for binary ionic compounds.

Generally, the crossover method can be used to get the correct formula for a binary compound. Write each ion with its charge (positive ion to the left), then transpose the charge numbers (but not the plus and minus signs), and write them as subscripts.

Covalent Bonds: Shared Electron Pairs Generally nonmetal–nonmetal compounds form covalent bonds.

4.7

4.8

4.9 4.10

4.11

4.12

The bond formed by a shared pair of electrons is called a covalent bond.

Formation of double and triple bonds maintain octets.

The systematic names of compounds are discussed.

Unequal Sharing: Polar Covalent Bonds Difference of covalent and polar covalent In H—Cl, the chlorine atoms have a greater attraction for a shared pair of electrons than do hydrogen atoms; chlorine is said to be more electronegative than hydrogen.

Electronegativity increases as you move toward fluorine.

Polyatomic Molecules: Water, Ammonia, and Methane In general, many nonmetals often form a number of covalent bonds equal to eight minus the group number.

Hydrogen forms one bond, oxygen forms two bonds (with two lone pairs), nitrogen forms three bonds (with one lone pair), carbon forms four bonds (with no lone pairs).

Polyatomic Ions Table 4.4 lists the common polyatomic ions to be discussed Rules for Writing Lewis Formulas The five steps for writing electron dot formulas appear in this section.

An atom or molecule with unpaired electrons is called a free radical.

Examples are ClO2, NO, NO2.

Molecular Shapes: The VSEPR Theory The common bonding and shapes of molecules appear in this section.

Table 4.6 lists bonding and the shapes of molecules Shapes and Properties: Polar and Nonpolar Molecules H—Cl, water, ammonia, and methane are revisited Green chemistry and chemical bonds Learning the chemical vocabulary

Demonstrations 1. Use a conductivity apparatus (with light bulb or bell) to test various ionic and covalent compounds.

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Chapter 5: Chemical Accounting Overview Chapter 5 explains chemical nomenclature, mass relationships, molar masses, and the gas laws. Nomenclature of metal–nonmetal compounds, nonmetal–nonmetal compounds, polyatomic ions, and binary ionic compounds are discussed. The chapter concludes with balancing chemical equations and mole–mass relationships.

Lecture Outline 5.1

5.2 5.3 5.4 5.5

Chemical Sentences: Equations Remember that, matter is neither created nor destroyed in chemical reactions, and chemical equations and the balancing of chemical equations make sense.

Volume Relationships in Chemical Equations Avogadro's Number and the Mole Molar Mass: Mole-to-Mass and Mass-to-Mole Conversions Solutions

Demonstrations 1. Display 1 mole samples of some common elements and compounds. Stoppered flasks make suitable containers for both display and storage. Use 50-mL flasks for 12 g of carbon, 32 g of sulfur, 207 g of lead, 27 g of aluminum, 18 g of water, 58.5 g of salt (sodium chloride), etc. Use a 250-mL flask for 180 g of glucose and a 500-mL flask for 342 g of sucrose.

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Chapter 6: Gases, Liquids, Solids . . . and Intermolecular Forces Overview Chapter 6 discusses the states of matter and intermolecular forces, and introduces the empirical gas laws.

Lecture Outline 6.1 6.2 6.3 6.4 6.5 6.6

6.7

Solids, Liquids, and Gases Comparing Ionic and Molecular Compounds Forces between Molecules Forces in Solutions Gases: The Kinetic–Molecular Theory The Simple Gas Laws Pressure is inversely proportional to volume.

Volume is directly proportional to temperature.

Volume is directly proportional to number of moles.

The Ideal Gas Law pV = nRT is the Ideal Gas law.

Demonstrations

1. Put a little water in an empty soda can and heat it to boiling. Lift the can with tongs, and quickly invert it in a beaker of cold water. Air pressure causes the can to collapse.

2. Fill a gallon-sized milk jug (or a 2-liter soda bottle) with very hot water. Then pour out the water and quickly stopper the bottle. The bottle collapses on cooling.

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Chapter 7: Acids and Bases Overview Acids and bases are important to us in many ways. We consume products that are acids or bases on a daily basis. The balance of acids and bases is crucial for the life processes.

Chapter 7 defines acids and bases, distinguishes between strong and weak acids and bases, introduces the pH scale, and discusses some acid–base consumer issues.

Lecture Outline 7.1 7.2 7.3 7.4

7.5 7.6 7.7 7.8

Acids and Bases: Experimental Definitions Acids, Bases, and Salts Acidic and Basic Anhydrides Strong and Weak Acids and Bases Strong acids and bases undergo 100% dissociation. There are six strong acids: H2SO4, HClO4, HNO3 , HCl, HBr, and HI Neutralization The pH Scale pH of 7 is neutral; pH < 7 is acidic; pH > 7 is basic.

Buffers and Conjugate Acid–Base Pairs Acids and Bases in Industry and in Us

Demonstrations 1. Place 6 or 8 small beakers on the overhead projector. Put a little (10 mL) dilute acid in half of the beakers and a little dilute base in the other half. Into each acid–base pair, add several drops of some selected indicator (e.g., methyl orange, bromocresol green, methyl violet, phenol red, etc.), showing the variety of color changes exhibited by acid– base indicators.

2. Some indicators exhibit more than one color change. In three small beakers on the overhead projector, place small amounts of dilute acid, water, and dilute base. Then add a drop of thymol blue indicator to each sample. The colors will be red, yellow, and blue.

3. On the overhead projector, place four beakers containing small amounts of water, 0.01 M HCl, 1 M HCl, and 6 M HCl. To each sample, add a few drops of methyl violet indicator solution. The colors will be violet, blue, green, and yellow.

4. On the overhead projector, place six small beakers containing 5–10 mL of the following: 6 M NaOH, 1 M NaOH, tap water, distilled water, 1 M HCl, and 6 M HCl. To each sample, add a few drops of bromothymol blue indicator. The colors will be violet, blue, green, yellow, orange, and red. (If the tap water turns blue, add a little more indicator solution.)

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5. Place some flower petals in a beaker with about 1/4 cup of rubbing alcohol. (Almost any kind of flower petals can be used.) Use a stirring rod to mash up the petals in the alcohol. (Sometimes it helps to heat the mixture for a few minutes.) Pour off the clear, colored extract, filtering it if necessary, and pour into several small beakers. Add vinegar to one, ammonia to another, and other acids or bases to the rest.

6. Take several red cabbage leaves and place them in a blender along with about a cup of water. Blend the mixture until the cabbage has been chopped into fine pieces.

Pour off the liquid, using a tea strainer to get rid of the very small bits of solid material.

Pour some of the deep-colored liquid into each of five glasses or beakers. Into each container, pour one of the following: vinegar, bottled soda water, tap water, baking soda dissolved in water, or clear ammonia. The colors will be red, pink, violet, blue, or green.

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Chapter 8: Oxidation and Reduction Overview The process of oxidation and reduction occurs in and around us every second of every day. Chapter 8 begins by defining oxidation-reduction reactions, and then discusses some important types of oxidation-reduction reactions. The chapter concludes with a brief overview of the importance of oxidation-reduction reactions to living organisms.

Lecture Outline 8.1

8.2

8.3

8.4

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8.6 8.7

Oxidation and Reduction: Three Views Oxidation is the gaining of oxygen atoms. Reduction is the loss of oxygen atoms.

Oxidation is the loss of hydrogen atoms. Reduction is the gaining of hydrogen atoms.

Oxidation is the loss of electrons. Reduction is the gaining of electrons.

Oxidizing and Reducing Agents The substance oxidized is the reducing agent.

The substance reduced is the oxidizing agent.

Electrochemistry: Cells and Batteries The passage of the electrons of an oxidation–reduction reaction through a circuit yields energy.

Corrosion and Explosion Loss of useful metals through the process of oxidation is a costly but unavoidable process. An explosion is a very rapid oxidation–reduction reaction.

Oxygen: An Abundant and Essential Oxidizing Agent Oxygen is the most important oxidizing agent. Oxygen exists as O2 and constitutes 21% of Earth’s atmosphere.

Some Common Reducing Agents Oxidation, Reduction, and Living Things Plants use solar energy and reduce carbon dioxide to form complex carbohydrates. Animals oxidize complex carbohydrates for energy.

Demonstrations 1. Using tongs, hold a strip of magnesium metal in a flame. The oxidation reaction gives off an intense white light.

2. Place a small pile of iodine crystals mixed with zinc dust in the middle of a Pyrex watch glass. The elements do not react. Then add a little water with a medicine dropper.

The reaction to produce zinc iodide proceeds with the evolution of heat and purple vapor from the sublimation of iodine.

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3. Mix a little shampoo into some fresh 3% hydrogen peroxide and then add a little MnO2. The oxygen gas given off from the oxidation of the hydrogen peroxide produces foam.

4. To a small pile of fine crystals of potassium permanganate in a Pyrex watch glass, add a little glycerol. The reaction starts slowly but produces a lot of white smoke and a violet flame.

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Chapter 9: Organic Chemistry Overview Chapter 9 discusses the chemistry of the carbon atom, the only element that has a major field of chemistry devoted to the study of its compounds. Of the tens of millions of known chemical compounds, more than 95% are compounds of carbon. The types of hydrocarbons are discussed, and various functional groups are introduced.

Lecture Outline 9.1

9.2

9.3 9.4

9.5

9.6

Aliphatic Hydrocarbons Carbon can form an almost infinite number of molecules of various shapes, sizes, and compositions.

Hydrocarbons: Compounds only containing H and C, often called saturated hydrocarbons.

Alkanes are hydrocarbons with only single carbon-to-carbon bonds.

Formulas and names for the first 10 hydrocarbons and their isomers are discussed.

Cyclic hydrocarbons are ring or loop structures.

Unsaturated Hydrocarbons: Alkenes and Alkynes Alkenes are hydrocarbons with at least one double carbon-to-carbon bond.

Alkynes are hydrocarbons with at least one triple carbon-to-carbon bond.

Aromatic Compounds: Benzene and Its Relatives The structure of aromatic compounds and their structural features Aromatic hydrocarbons have delocalized electrons.

Halogenated Hydrocarbons: Many Uses, Some Hazards Chlorofluorocarbons (CFCs) are one type of chlorinated hydrocarbon.

The Functional Group Functional groups determine the chemistry of the organic molecule.

Table 9.4 shows functional groups and Table 9.5 shows some common alkyl groups Alcohols, Phenols, and Ethers The general structure and names of alcohols, phenols and ethers OH R—OH, such as ethanol CH3CH2OH Phenols: An aromatic hydrocarbon and alcohol Ethers: R—O—R’ Aldehydes and Ketones Some simple aldehydes and ketones, and their important properties are discussed.

O

Aldehyde R—CHO R

C

H

O

Ketone: A carbon chain with a carbon–oxygen double bond R 9.7 .

Carboxylic Acids and Esters

C

R

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Some simple acids and esters, and their important properties are discussed.

General formula of an acid R—COOH Esters: The sweet smell of RCOOR’ The art of organic synthesis: Green chemists find a better way.

Nitrogen-Containing Compounds: Amines, Amides, and Heterocyclic Compounds Amine: NH2 Amide: Oxygen double bonded to a carbon with a nitrogen next to the carbon.

Heterocyclic compounds: Alkaloids and others Compounds with atoms other than carbon in the ring are heterocyclic.

Demonstrations 1. On the overhead projector, place small beakers containing about 5–10 mL samples of an alkane and an alkene (e.g., cyclohexane and cyclohexene). Add one dropperful of dilute KMnO4 solution to each sample. The purple permanganate will remain unreacted in the alkane, but the alkene will be oxidized by the permanganate, and the purple color will disappear.

2. Place a small beaker containing a little ethyl alcohol on the stage of an overhead projector. Add some acidic dichromate solution and note the darkening of the mixture.

This is the reaction on which the "breathalyzer" test is based.

3. Place a little alcohol in a gallon-sized milk jug, cap the bottle, and shake vigorously.

Uncap the bottle, pour out the alcohol, and then replace the cap on the "empty" bottle until it is ready for demonstration. Hold a flame close to the mouth of the opened bottle and note the violent combustion.

4. Demonstrate a "carbide cannon," in which calcium carbide powder is reacted with water to form acetylene, which is then ignited by a spark.

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Chapter 10: Polymers Overview Chapter 10 introduces the student to the marvelous variety of materials made from polymers. The chapter starts by discussing the history of polymers, then discusses the various types of polymers and their uses. The chapter concludes with a look into the future developments and uses of polymers.

Lecture Outline 10.1

10.2

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Polymerization: Making Big Ones Out of Little Ones Polymers are huge molecules made from many small molecules, monomers.

Natural polymers: Wood, wool, and proteins are all natural polymers.

Celluloid: Billiard balls and collars The synthetic material celluloid is derived from natural cellulose.

Celluloid is used to make billiard balls and historically, movie film. It is also used to make collars stiff.

Polyethylene: From the Battle of Britain to Bread Bags Polyethylene is the simplest and cheapest polymer made from the monomer ethylene (CH2=CH2).

Three main types of polyethylene: LDPE, HDPE, and LLDPE Thermoplastics and thermosetting polymers and their properties Addition Polymers: One + One + One + . . . Gives One! Polypropylene, polystyrene, vinyl polymers, and teflon are examples of addition polymers, which are made by adding monomers together to form a macromolecule. Table 10.1 shows some addition polymers.

Rubber and Other Elastomers Natural rubber is isoprene, a naturally occurring polymer.

The importance of crosslinking is discussed, especially vulcanization (the addition of sulfur to isoprene to make the substance harder).

Synthetic rubber, neoprene, and SBR are discussed.

Condensation Polymers: Monomers Minus Water Water is eliminated, and the monomers are added together to form polyamides and polyesters.

Nylon, polyester, and Bakelite are examples of condensation polymers.

Other polymers: polycarbonates, composite materials, and silicones Properties of Polymers The glass transition temperature is an important property of polymers.

In crystalline polymers, the monomers are in line, giving high tensile strength.

In amorphous polymers, the monomers are randomly ordered.

Plastics and the Environment Problems with plastics; plastics last almost forever. Landfills, incineration, biodegradation, and recycling are ways of disposing of plastics.

Sustainable plastics are discussed as well as greener polymers.

Plastics and fire hazards: Fumes given off during house fires are very dangerous, owing in large part to the polymers in the modern home.

Plasticizers and pollution: Plasticizers make some plastics, such as vinyl polymers, more flexible, but resist decomposition and bioaccumulate.

Plastics and the future: From medical uses to pipes and airplanes Demonstrations 1. On a Petri dish about half-full of acetone, place a cup made of polystyrene foam.

The cup will appear to melt away as the polystyrene dissolves in the acetone.

2. Beads of polystyrene can be mixed with beads of polyethylene and then separated by pouring the mixture into a beaker filled with water. The polyethylene will float, while the polystyrene will sink.

3. A sample of high-density polyethylene (HDPE) can be separated from a sample of low -density polyethylene (LDPE) using a 1:1 mixture of methanol and water. The LDPE will float, while the HDPE will sink. (The HDPE sample can be cut from a gallonsized milk jug. The LDPE sample can be cut from a waxy squeeze bottle. The samples might be cut in the shapes of an H and an L, respectively.)

4. Insert a copper wire into a cork, and holding the cork, heat the copper wire in a flame.

Touch the hot wire to a piece of plastic and return the wire to the flame. If the flame turns green, the plastic contains a halogen. It is likely to be polyvinyl chloride (PVC).

(This is the Beilstein test.)

5. If you hold a foamed plastic egg carton in a flame, the flame becomes very sooty because the foamed plastic is polystyrene, which has a very high carbon to hydrogen ratio.

6. If you hold a piece of polyethylene in a flame, the odor will be like that of a burning candle.

7. Make “slime” by adding about 5 mL of saturated Borax solution to 30 mL of 4% polyvinyl alcohol solution in a paper cup. Stir vigorously with a wooden stick until the mixture forms a gel. Remove the gel from the cup and knead it into a ball.

When laid on a flat surface, the ball flattens. When pulled apart very slowly, it stretches. When pulled apart rapidly, it breaks. The “slime” can usually be stored in an air-tight plastic bag for at least a week. After a while, it will start to mold and should be thrown away.

8. Another polymer gel, similar to “slime,” can be made from a white glue, such as Elmer's. Mix about 30 mL of the glue with 30 mL of water and mix well. (A few drops of food color can be added, if desired.) Then add about 20 mL of 4%, or saturated, borax solution and stir well until the mixture forms a semi-solid mass on the .

end of the stirrer. Remove the gel and form it into a ball. Try bouncing the ball. The polymer can be treated and stored like “slime”. (Adding a few drops of Lysol® to the Borax solution will slow down the mold growth .)

9. Polystyrene is a glassy polymer, whereas polyethylene is crystalline. When you step on a transparent polystyrene cup, it shatters. When you step on a cup or bottle made of polyethylene, it bends but does not break.

10. Have six or more students stand before the class, an arm's length apart from each other, with their hands clasped about 6 inches in front of their chests. They represent ethylene molecules. “Initiate the reaction” by unclasping the hands of the student on the far left, placing an object such as an eraser, in her right hand. Her left hand then “attacks” the next “molecule,” grabbing her right hand and leaving her left hand free to “attack” the next one, in a “chain reaction”. At the end of the line, the last student has a free left hand, which you can grab as a “chain stopper”.

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Chapter 11: Nuclear Chemistry Overview Chapter 11 discusses the structure of the nucleus, radioactivity, half-life, artificial transmutation, and induced radioactivity. These concepts are then applied to nuclear medicine, radioisotopic dating, the nuclear bomb, and nuclear power.

Lecture Outline 11.1

11.2

11.3

11.4

11.5

11.6 11.7

11.8

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Natural Radioactivity Background radiation: Natural sources of radiation The two particles of the nucleus are the proton (+) and the neutron (neutral). Two atoms with the same number of protons but different number of neutrons are isotopes, some of which are radioactive Nuclear Equations The equations are simple if you follow the rule that both mass and charge are conserved. That is, the sums of the nucleons and nuclear charges must be the same before and after a reaction. Another way to think about the problem is that the sum of the superscripts on the left side of the reaction arrow must equal the sum of the superscripts on the right side of the arrow. The same rule holds for the subscripts.

Half-Life and Radioisotopic Dating Half life: The time it takes for half of a radioactive substance to disintegrate.

Use of the half-lives of radioactive isotopes, and assumption of constant decay rates over time, makes it is possible to determine the age of items.

Artificial Transmutation Bombardment of various nuclei with protons, neutrons, alpha particles, or other fundamental particles brings about transmutation, each element being changed into another.

Uses of Radioisotopes The main use of radioisotopes is as tracers. Because radioisotopes are radioactive, their locations can be traced.

Radioactive isotopes are used for diagnostic tests as well as for therapy.

More people have had their lives improved by the use of radioactive materials than have been killed or injured.

Table 11.6: Radioisotopes and Their Medical Applications Penetrating Power of Radiation Gamma > Beta > Alpha Energy from the Nucleus Einstein, E = mc2, and binding energy Chain reactions—fission and fusion Nuclear Bombs The building of the bomb and how uranium and plutonium bombs are used.

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The highly secret Manhattan Project was set up to do this.

Radioactive fallout and its implications Uses of Nuclear Energy From bombs to nuclear power plants Figure 11.16 lists some constructive uses of nuclear energy.

Green remediation of nuclear waste

Demonstrations 1. Demonstrate the use of a Geiger counter. Using a compound of thorium or uranium, show the large amount of radioactivity in such a compound. (If you can find an old piece of orange dinnerware, it can be compared with a piece of some other color. The old orange pieces were glazed with uranium oxide and are quite radioactive.)

2. Using the alpha, beta, and gamma emitters that came with the Geiger counter (or can be purchased separately), show that a sheet of paper will stop alpha rays, and a sheet of aluminum will stop alpha or beta rays, but neither of these will stop gamma radiation. A thin piece of lead foil will readily block out alpha or beta radiation, but it takes several cm of lead to block out gamma radiation.

3. Show (qualitatively) that as you move the detector away from the source of radiation, the count goes down significantly. (If you move just 3 feet away from a radioactive source, you get only 1/9 as much radiation.)

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Chapter 12: Chemistry of Earth Overview Chapter 12 discusses the components of Earth and the use that modern civilization makes of Earth’s constituents. The chapter begins by describing the substances in Earth’s crust and how they formed. Next, the chapter discusses the uses and abuses that modern civilization makes of Earth’s resources.

Lecture Outline 12.1 Spaceship Earth: The Materials Manifest Earth is mostly oxygen, silicon, and hydrogen.

Organic: coal, petroleum, and natural gas Inorganic: silicates, carbonates, oxides, and sulfides 12.2 Silicates and the Shapes of Things The silicates are quartz, mica, and asbestos.

Modified silicates: ceramics, glass, and cement 12.3 Metals and Ores The most important metals are copper, iron, and aluminum.

12.4 Earth’s Dwindling Resources Land pollution: solid wastes The three R’s of garbage: reduce, reuse, and recycle How crowded is our spaceship?

Demonstrations 1. Make a “super ball” by adding 6–8 mL of ethyl alcohol to 25 mL of sodium silicate in a paper cup. Stir with a wooden stick until the mixture forms a solid material. Wearing disposable plastic gloves, press the solid between the palms of the hands, and roll it into a ball.

2. Using a plain or a quartered Petri dish, place four pieces of rock (e.g., limestone, marble, sandstone, and granite) in the dish. With a dropper, add a little 3 M HCl to each rock. If bubbles form, the rock is probably calcium carbonate. Limestone and marble are two of the many forms of calcium carbonate.

.

Chapter 13: Air Overview Chapter 13 begins by defining the layers and composition of Earth’s atmosphere. The chapter then moves in cycles. The chapter concludes with detailed discussions about various air pollution and the dynamic nature of the atmosphere as seen through the nitrogen and oxygen.

Lecture Outline 13.1 Earth’s Atmosphere: Divisions and Composition Composition and layers of the atmosphere. Air is composed of 78% nitrogen.

13.2 Chemistry of the Atmosphere Nitrogen and oxygen cycles Temperature inversions The majority of nitrogen fixation is performed by bacteria.

13.3 Pollution through the Ages Natural and industrial sources of pollution Methods of pollution control and cleanup Air pollution in China Coal + fire → industrial smog 13.4 Automobile Emissions In urban areas, automobile contribution to smog can exceed 90%.

The main gases in automobile emissions The study of carbon monoxide and catalytic converters 13.5 Photochemical Smog: Making Haze while the Sun Shines Photochemical smog is produced when it is sunny and warm.

The origin of photochemical smog Solutions to photochemical smog 13.6 Acid Rain: Air Pollution → Water Pollution Acid rain is rain having a pH less than 5.6.

Air pollutants that contribute to acid rain The major industrial and consumer sources of acid rain 13.7 The Inside Story: Indoor Air Pollution Indoor air pollution poses a major health concern The main indoor air pollutants and their sources Where radon comes from and why it is hazardous 13.8 Stratospheric Ozone: Earth’s Vital Shield Ozone shields humans from UV light.

CFCs and depletion of the ozone layer The consequences of stratospheric ozone depletion 13.9 Carbon Dioxide and Climate Change The greenhouse effect trapping of reradiated solar rays by the atmosphere The mechanism and significance of the greenhouse effect Strategies for reducing the amount of CO2 released into the atmosphere

.

13.10 Who Pollutes? Who Pays?

Air pollution causes damage to buildings, clothing, and other objects.

Air quality standards and the seven major air pollutants Demonstrations 1. Dip some filter paper (or white paper toweling) into a solution of cobalt(II) chloride, and let it dry. The paper will be blue when it is dry, but when the atmosphere is humid, it will cause the paper to turn pink. Try holding the paper over a steaming cup of coffee or boiling water.

2. (Air pressure) Pour about 10 mL water into an empty soda can and heat it to boiling.

Then, with tongs, quickly invert the can into a container of cool water. The pressure of the air crushes the can.

.

Chapter 14: Water Overview The chapter begins by discussing the special properties of water in comparison to other substances. Next, the water cycle, biological and chemical contamination, and water treatment methods are introduced.

Lecture Outline 14.1

14.2

14.3

14.4 14.5

14.6 14.7

Water: Some Unique Properties Water has a high dipole moment, a high heat of vaporization, high heat capacity, and a low heat of fusion.

Water in Nature Saltwater constitutes nearly 98% of the water on Earth.

The water cycle and natural contaminants, a dynamic equilibrium that is powered by the Sun. Chemical and Biological Contamination Fewer than 10% of the people of the world have access to sufficient clean water.

Water: Who Uses It and How Much?

Groundwater Contamination → Tainted Tap Water Chemical dumps, garbage dumps, underground storage tanks, and overuse of fertilizers are all potential sources of groundwater contamination.

Making Water Fit to Drink Wastewater Treatment Wastewater treatment plants: primary, secondary, and advanced

Demonstrations 1. (High heat of vaporization of water) Mix ordinary rubbing alcohol with an equal volume of water. Dip a piece of cloth (such as a handkerchief) into the alcohol mixture, gently squeeze out most of the excess liquid, and then, using tongs, brush the cloth past a flame so that it catches fire. Wave the burning cloth slowly through the air to show that it really is burning. When the flame goes out, hold up the cloth to show that it is still intact.

Let a few students feel the cloth to see how cool it is. The heat from the burning alcohol was used up in vaporizing the water.

2. (High surface tension of water) Fill a container several inches deep with water, and float a plastic strawberry basket on the surface. The basket is actually heavier than water, but the surface tension of the water keeps it afloat. Adding a few drops of detergent lowers the surface tension of the water, and the basket sinks. (This demonstration can be done with a floating needle on the stage of an overhead projector.)

.

Chapter 15: Energy Overview Chapter 15 begins by discussing the sources of energy and the laws of thermodynamics.

Next, the chapter discusses the energy requirements and costs of a technologically advanced culture.

Lecture Outline 15.1 15.2

15.3

15.4 15.5 15.6 15.7 15.8 15.9

Energy: Starring Our Sun The Sun is the source of energy on planet Earth.

Energy and Chemical Reactions Chemical reactions depend on several factors and are either endothermic or exothermic.

The Laws of Thermodynamics The first law: energy is conserved The second law: you can’t break even Power: People, Horses, and Fossils Coal: The Carbon Rock of Ages Natural Gas and Petroleum Convenient Energy Nuclear Energy Renewable Energy Sources

Demonstrations 1. Place several tablespoonfuls of calcium oxide (quicklime) in a plastic ziploc bag.

Add water (and some red food color, if desired). The bag will get hot and can be passed around.

2. Place some ammonium nitrate or ammonium acetate in a ziplock bag. Add water (and some blue food color, if desired). The bag will get cold and can be passed around.

.

Chapter 16: Biochemistry Overview Chapter 16 discusses the chemistry of life, from the substances required for energy to the molecules that define the structure of life.

Lecture Outline 16.1

16.2

16.3

16.4

16.5

16.6

16.7

16.8

.

Energy and the Living Cell An introduction to the major parts of the cell Structure and energy production are discussed along with photosynthesis and the sources of energy for animals and metabolism.

Carbohydrates: A Storehouse of Energy Carbon and water (“carbohydrate”) are the basis for the structures of the simple sugars (monosaccharides) to the complex carbohydrates, starches, glycogen, and cellulose.

Fats and Other Lipids Fats are esters of the fatty acids. Fat structures may be saturated, with no carbon-to-carbon double or triple bonds, or unsaturated, with one or more carbon-to-carbon double or triple bond(s).

Proteins: Polymers of Amino Acids Muscle, skin, and hair are all mostly proteins. Here, the structure and properties of amino acids and proteins are discussed.

Structure and Function of Proteins The four levels of proteins are described (primary, secondary, tertiary, and quaternary).

How enzymes work as catalysts Nucleic Acids: Parts, Structure, and Function Four simple base pairs define everything about you.

The two types and function of nucleic acids are described.

Replication is the copying or duplication of DNA molecules.

RNA: Protein Synthesis and the Genetic Code In transcription, the DNA is transcribed to mRNA. The mRNA travels to the ribosome and is then translated into a protein.

The important characteristics of the genetic code are described.

The Human Genome Various topics of recombinant DNA technology, genetic testing, and research are discussed, from DNA profiling and DNA fingerprinting to gene therapy and genetically modified organisms.

Demonstrations 1. (Test for starch) To several mL of a dilute solution of soluble starch, add a drop of iodine in KI solution. The starch–iodine complex is dark blue. (This can be shown on the overhead projector.)

2. (Biuret test for proteins) To 5 mL of 1% albumin or gelatin in a small beaker, add 5 mL of 2 M NaOH, and then add several drops of 0.5% copper sulfate. (Do this on the stage of an overhead projector.) A lavender color confirms the presence of peptide bonds.

3. (Enzyme action) Dissolve a little urea in about 10 mL of water in a small beaker. Add a little neutralized indicator solution (e.g., a yellow-green solution of bromthymol blue).

When a small amount of urease is added, the solution turns blue because of the formation of ammonia.

CO(NH2)2 + H2O → CO2 + 2 NH3 4. (Steroid test) In several mL of CH2Cl2 (in a small beaker on the overhead projector), dissolve a few crystals of cholesterol. Then add 1 mL of acetic anhydride and about 5 drops of concentrated sulfuric acid. The solution will turn pink, then violet; then it will slowly turn blue, and finally green.

.

Chapter 17: Food Overview In this chapter we discuss food, what it’s made of, and the substances added to it. The three main classes of foods are carbohydrates, fats, and proteins. For proper nutrition, our diet should include balanced proportions of these three foods, plus water, vitamins, minerals, and fiber.

Lecture Outline 17.1

17.2

17.3

17.4

17.5 17.6

17.7

Carbohydrates in the Diet Dietary carbohydrates, the sugars and starches, and metabolism are discussed.

Fats and Cholesterol The fats contain abundant calories, but they are harmful in excess. Lipids and their function are described.

Proteins: Muscle and Much More Proteins are built from the amino acids. Here, the essential amino acids are described and the diseases associated with their deficiency.

Minerals, Vitamins, and Other Essentials The minerals are inorganic substances required for life. The roles of vitamins, minerals, and fiber are studied.

Starvation, Fasting, and Malnutrition The effects of starvation, fasting, and malnutrition are discussed.

Food Additives The common food additives and their purpose are studied in detail. The substances that are added to food to make it taste better, look better, prevent spoilage, and add minerals and vitamins to the diet retard spoilage are studied.

Problems with Our Food The main problems with harmful substances in our food are studied.

Carcinogens, contaminants, and how to avoid them are discussed.

Demonstrations 1. Fill a small beaker (100–150 mL) about one-third full of sugar (sucrose). Carefully add 5–10 mL of concentrated sulfuric acid, and step back. A black cylinder of foamed carbon will rise up out of the beaker and there will be smoke and fumes. The demonstration should be done in a hood or in a well-ventilated area.

2. (Cornstarch putty) To 1 cup of corn starch, slowly add about 1/3 cup water and mix.

The gooey mixture has some unusual properties. It can be cut with a knife or with scissors, but it flows like a viscous liquid. It looks wet, but if you rub it between your fingers, it gets powdery. It can be rolled into a ball, but then the ball will flatten. It is a non-Newtonian fluid. .

3. Put several spoonfuls of baking soda into a glass soda bottle. Add about a cupful of vinegar, and then quickly spread the opening of a balloon over the mouth of the bottle.

The balloon will be blown up by the carbon dioxide generated. The balloon can be removed from the bottle at any time.

.

Chapter 18: Drugs Overview Chapter 18 examines the world of pharmaceuticals, from aspirin to opiates. The type and action of the common classes of drugs are discussed. A drug is a chemical substance that affects the functioning of living things and is used to relieve pain, to treat illness, or to improve one’s state of health.

Lecture Outline 18.1

18.2

18.3

18.4

18.5

18.6

18.7

.

Scientific Drug Design Natural and synthetic drugs Chemotherapy (chemical therapy) can be used to treat disease.

Pain Relievers: From Aspirin to Oxycodone The wonder drugs The common OTC analgesics, NSAIDS, and antipyretic drugs are discussed as well as how each works.

The potential for addiction to narcotics Chemistry, allergies, and the common cold Drugs and Infectious Diseases Antibacterial drugs are reviewed—effective against bacteria, not viruses.

Viruses and antiviral drugs are discussed along with AIDS. Structure–function relationship and combinatorial chemistry are discussed.

Chemicals against Cancer Aim of cancer research is to kill the cancerous tissue without killing normal cells.

The type and action of the common anticancer drugs are described.

Hormones: The Regulators Regulate growth, metabolism, and reproduction Hormones, prostaglandins, and steroids are discussed along with how each works.

The types of sex hormones, how each acts, and how birth control drugs work The chemistry and social revolution related to “The Pill” are discussed.

Drugs for the Heart The types of drugs for treating heart disease are discussed along with how they work.

High blood pressure is the most common cardiovascular disease.

Drugs and the Mind How the brain amines norepinephrine and serotonin affect the mind Three classes of drugs: stimulant, depressant, and psychotropic Chemistry of the nervous system and neurotransmitters Brain amines and their effects are discussed.

The importance of chirality PEA could govern emotions of romantic relationships.

18.8

.

Anesthetics and their effects, from general anesthetics to ketamine and PCP Depressant drugs Alcohol is the most used and abused depressant drug.

Barbiturates and antianxiety drugs are discussed.

Stimulant drugs: cocaine, caffeine, and nicotine are discussed.

Amphetamine was once used for weight loss, and it is now used in treating mild depression and narcolepsy. Methamphetamine is inexpensive and widely abused.

Hallucinogenic drugs: these drugs change the way people see things.

From LSD to marijuana to ecstasy Drugs and Society Drug abuse and drug misuse are discussed.

Placebo and nocebo effects

Chapter 19: Fitness and Health Overview Chapter 19 connects the world of fitness and how we feel with the type and quantity of chemical compounds we ingest. The chapter begins by discussing the food categories and how much of each category should be in our diet. Next, vitamins, minerals, and electrolytes are introduced. The chapter concludes with the chemistry of sports materials.

Lecture Outline 19.1

19.2

19.3

19.4 19.5

19.6

.

Calories: Quantity and Quality Most calories should come from carbohydrates. No more than 25% of calories should come from fats.

Vitamins, Minerals, Fluids, and Electrolytes Table 19.1 is a table of recommended daily adult intakes of vitamins.

Sodium, potassium, and chloride ions are the major essential electrolytes.

Water is the best drink when you are thirsty.

Weight Loss: Diets and Exercise To lose a pound, you must burn 3500 kcal.

The healthy way to lose weight is to exercise. Not only will you lose weight, but you will also look and feel better.

Measuring Fitness Men should have more than 3% body fat; women need 10-12%.

Some Muscular Chemistry Muscles consume ATP (adenosine triphosphate) for energy.

Aerobic muscle contraction occurs in the presence of oxygen.

Anaerobic muscle contraction occurs when sufficient oxygen is not available.

Drugs, Athletic Performance, and the Brain Restorative drugs are painkillers and anti-inflammatory drugs.

Stimulant drugs are used in an attempt to improve performance.

Anabolic steroids are used to build muscle mass.

Some runners get a euphoric high during and after a long, hard run.

Smoking is one of the worst things you can do to your physical wellbeing.

Chapter 20: Chemistry Down on the Farm and in the Garden and on the Lawn Overview This chapter discusses modern food production and associated technologies. Fertilizers, pest control, herbicides and defoliants, and sustainable agriculture are all discussed from a conventional, modern farming techniques perspective to modern organic/alternative techniques.

Lecture Outline 20.1

20.2

20.4

20.5

20.6

.

Farming with Chemicals: Fertilizers How we use and produce the three primary plant nutrients— nitrogen, phosphorus, and potassium—is discussed.

The War against Pests How we control substances that kill organisms that we consider pests as well as how to handle pest resistance is discussed.

Pesticides and biological insect controls Herbicides and Defoliants How we control weeds as well as how to handle weed resistance is discussed.

Sustainable Agriculture What is needed to produce food and fiber indefinitely is discussed.

Sustainable agriculture and organic farming Some Malthusian Mathematics Rule of 72 and population growth and its implications Can we feed a hungry world?

Chapter 21: Household Chemicals Overview The modern home is stocked with a variety of chemical products. Chapter 21 introduces the student to the chemistry of soaps, detergents, bleaches, paints, cosmetics, perfumes, and other chemical compounds used in and around the home.

Lecture Outline 21.1

21.2

21.3

21.4

21.5

21.6

.

A History of Cleaning Fat + Lye  Soap. Soap is a substance formed by mixing a base and a fatty acid.

Synthetic Detergents Modern detergents are made in the laboratory.

ABS detergents: nonbiodegradable LAS detergents: biodegradable Laundry detergent formulations Dishwashing detergents Laundry Auxiliaries: Softeners and Bleaches Fabric softeners: quaternary ammonium salts Laundry bleaches: whiter whites Chlorine kills bacteria and whitens clothes.

All-Purpose and Special-Purpose Cleaning Products Hazards of mixing cleaners Special-purpose cleaners Green cleaners Solvents, Paints, and Waxes Solvents Paints Waxes Cosmetics: Personal Care Chemicals Skin creams and lotions Moisturizers and sunscreens Antiaging Creams and Lotions Nanoparticles in cosmetics Lipstick and Eye makeup Deodorants and antiperspirants Toothpaste: soap with grit and flavor It’s the same thing you wash your clothes with!

Perfumes, colognes, and aftershaves Aromatherapy Some hairy chemistry Shampoo, hair coloring, permanent waving, hair sprays, hair removers, and hair restorers The well-informed consumer

Demonstrations 1. Into a tall glass place some baking soda, some liquid detergent, and a few drops of red food color. Adding vinegar to this mixture will cause it to bubble up and look somewhat like a strawberry ice cream soda.

2. Add several drops of food color to each of two beakers about half-full of water. Add a little liquid chlorine bleach to one of the beakers, and watch the color disappear.

.

Chapter 22: Poisons Overview Many compounds are toxic to humans. Chapter 22 discuses many toxic substances that are known, giving priority to those that are more likely to be encountered in everyday life, their effects, detection, identification, and their antidotes.

Lecture Outline 22.1

22.2

22.3

22.4 22.5 22.6

22.7

.

Natural Poisons Natural poisons and their sources are given such as oleanders, hydrangeas, holly berries, irises, azaleas, and wisteria seeds.

Poisons and How They Act Understanding corrosive poisons, metabolic poisons, and heavy metal poisons and how each acts Antidotes for some common metabolic poisons and heavy metal poisons More Chemistry of the Nervous System Nerve poisons: stopping the acetylcholine cycle (various substances interfere with the action of neurotransmitters) Nerve poisons are the most deadly killing agents developed for military use.

The Lethal Dose How much does it take to kill? The concept of the LD50 value.

The Liver as a Detox Facility How the body is able to detoxify some substances Carcinogens and Teratogens Substances shown to cause cancer are known as carcinogens. Cancers and how they develop are discussed Three ways to test for carcinogens: The Ames test uses bacteria, animal testing uses test animals, and epidemiological studies are a statistical approach.

A teratogen is a substance that causes birth defects.

Hazardous Wastes Industrial waste, reactive wastes, flammable wastes, toxic wastes, and corrosive wastes What is the price we pay for these wastes/poisons?

Appendix A – Reagent List

Chemical Name A Acetic acid

Form/Concentration Formula

Labs

15 M Glacial (conc.)

6M 1M 0.5 M

28, 29, 50, 52, 55

[CH3COOH]

46, 65 4, 24, 25, 47 51

Acetic anhydride

[(CH3CO)2O]

55

Acetone Alcohol (isopropyl)

[CH3COCH3] [CH3CH(OH)CH3]

23, 28, 31, 44 (when noted in lab as alternative to ethanol)

Aluminum sulfate

1M

[Al2(SO4)3]

45

Ammonia (ammonium hydroxide)

18 M (conc.)

[NH3] or [NH4OH]

20, 50

2M 1% solution

52, 58 52

Ammonium chloride

solid

[NH4Cl]

3

Ammonium nitrate

solid

[NH4NO3]

42

Ammonium sulfide

solid

[(NH4)2S]

12

Ammonium phosphate B Barfoed's reagent Barium chloride

solid

[(NH4)3PO4]

58

0.1 M 5% solution

[BaCl2]

8 58

Barium nitrate Benedict's reagent Benzaldehyde

5% solution

[Ba(NO3)2]

58 57

[C6H5C(O)H]

28

Benzyl alcohol Buffer solution (pH=7) Butanol

[C6H5CH2OH]

29 57, 65

[CH3(CH2)3OH]

52

Butyric acid C Calcium metal Calcium acetate

[CH3(CH2)2COOH]

29

[Ca] [Ca(C2H3O2)2]

26

57

solid solid

44

Calcium chloride

solid 1M

[CaCl2]

3, 34 14

Calcium hydroxide

saturated solution

[Ca(OH)2]

36

Calcium nitrate

solid

[Ca(NO3)2]

61

218 .

Appendix A – Reagent List

Calcium oxide Cellulose Cerric(IV) nitrate (in 2 M HNO3) Chromatography paper Cobalt(II) nitrate

1M 5% solution solid 1% solution

[CaO] [Ce(NO3)6]2-

solution

9, 13, 14, 26 60 47 57 28 52

0.4 M strips and wire (sm. gauge) turnings

[Co(NO3)2]

11

[Cu]

26, 28, 45, 46, 64, 66

Copper(II) acetate

solid

[Cu(C2H3O2)2]

57

Copper(II) carbonate

solid

[CuCO3]

12

Copper(II) chloride

solid 1M 0.1 M

[CuCl2]

66 9 8

Copper(II) nitrate Copper oxide Copper(II) sulfate

1M fine powder

[Cu(NO3)2] [CuO] [CuSO4]

13, 26 49

crystals

[CuSO4.5H2O]

16

95% (denatured)

[CH3CH2OC2H3O2] [CH3CH2OH]

54, 55 10, 17, 23, 28, 29, 38, 39, 40, 41, 44, 47, 49, 50, 52, 55

Ethyl ether

[C2H5OC2H5]

50

Ethylene glycol

[HO(CH2)2OH]

30

solid

[Eu2O3]

8

40% solution

53 29

1% solution

HCHO [HCOOH] [C6H12O6]

1% solution

[C6H12O6]

57, 65

Copper

Copper(II) sulfate pentahydrate D E Ethyl acetate Ethyl alcohol (ethanol)

Europium oxide F Formaldehyde Formic acid Fructose G Glucose

12, 35

crystals 0.1% solution 1.0 M

219 .

57 47, 50 12, 13, 14, 25, 45

57

Appendix A – Reagent List

[HOCH2CHOH CH2OH]

30, 40, 56

[CaSO4.2H2O]

6

H Hexamethylenediamine

[H2N(CH2)6NH2]

30

Hexane Hydrochloric acid

[C6H14] [HCl]

28, 30, 55, 56 9, 11, 20, 58 21, 35, 48, 58 58 3, 9, 19, 24, 26 3, 13, 51 22, 64

3% solution 30% solution

[H2O2]

43, 48, 49 43

crystals 1% solution 5% solution tincture small pieces filings

[I2]

57, 65 57, 65 46, 56 25 26 4

0.2 M

[Fe(NH4)2(SO4)2]

11

1M

[FeCl3]

47, 48, 65

Glycerol (or glycerin) Gypsum

Hydrogen peroxide I Iodine

Iron metal Iron(II) ammonium sulfate Iron(III) chloride (Ferric chloride)

powdered

12 M (conc. ) 6M 3M 1M 0.5 M 0.1 M

[Fe]

0.1 M 1% solution

11 28

Iron(II) nitrate

1M

[Fe(NO3)2]

26, 47

Iron(II) sulfate

0.2 M 1M

[FeSO4]

58 9

Isobutyl alcohol

[CH3CH(CH3)CH2OH] 29

Isobutylamine

[(CH3)2CHCH2NH2]

28

Isopropyl alcohol

75% solution

[CH3CH(OH)CH3]

2, 17, 34, 58

L Lead Lead(II) acetate

sheet

[Pb] [Pb(C2H3O2)2]

32

Lead(II) nitrate Lithium chloride

1M 1M

[Pb(NO3)2] [LiCl]

13, 48 9

220 .

65

Appendix A – Reagent List

Litmus paper

0.1 M red blue

Luminol M Magnesium chloride Magnesium Magnesium sulfate heptahydrate

1M ribbon

[MgCl2]

4 8, 15, 26

(Epsom Salt)

[MgSO4.7H2O]

16

8 22, 35, 47, 58 22, 35 49

10% solution

58

Magnesium nitrate

1M 5% solution

[Mg(NO3)2]

26 60

Manganese dioxide

0.012 M

[MnO2]

38

[CH3OH]

29, 53, 54

Methanol N Nitrate/Nitrite test strips Nitric Acid

59 15 M (conc.)

6M

[HNO3]

35, 47, 50 1, 9, 12, 46, 47, 58, 64, 65, 66

n-octanol

[CH3(CH2)7OH]

29

n-octene

[CH3(CH2)5CH2]

28

[CH3(CH2)4OH]

29

n-pentanol (n-amyl alcohol) P Parafilm® pH test paper (or strips) wide range

30 23, 24, 28, 38, 47, 48, 52, 56, 57, 59, 60, 64, 65, 66

Phenolphthalein Phenol red indicator Phosphorus/Phosphate test strips

13, 21, 30, 44, 49 47 59

Phthalic anhydride

[C8H4O3]

30

Polyvinyl alcohol Potassium chloride

[(CH2CHOH)x] [KCl]

31 58 8 9

[K3Fe(CN)6]

64 11

Potassium ferricyanide

solid 0.1 M 1M 0.3M 0.1 M 221 .

Appendix A – Reagent List

Potassium ferrocyanide Potassium ferrioxalate trihydrate Potassium hydrogen sulfate Potassium iodide

Potassium permanganate Potassium thiocyanate Potassium sulfate Potassium test strips Propane, 2-chloro, 2methyl

0.1 M solid solid

[K4Fe(CN)6] [K3Fe(C2O4)3.3H2O]

11 12 64

solid

[KHSO4]

56

solid 0.1 M 1M 1% solution

[KI]

57, 65 65 12, 13 28

0.1 M

[KSCN] [K2SO4]

11

[CH3CCH3ClCH3]

28

[CH3CH2COOH]

29

[KMnO4]

Propanoic acid R Radiation sources Resorcinol

(alpha, beta, gamma)

45 59

32 [C6H4(OH)2]

28

S Salicylic acid

[C7H6O3]

29, 55

Sebacoyl chloride

[ClCO(CH2)8COCl]

30

Silver nitrate

1M 0.1 M

[AgNO3]

9, 66 64

Sodium acetate

solid 1M

[NaC2H3O2]

30 24 12

[NaHSO4]

Sodium bisulfate (Sodium hydrogen sulfate) Sodium carbonate

[Na2CO3]

Sodium chloride

solid 1M solid 0.1 M 1M

[NaCl]

23, 47, 48, 61, 65 13, 45 27, 34, 60 8 9, 13, 25

Sodium citrate

solid

[NaC6H7O6]

55, 65

[Na4FeCN6]

11

[NaHCO3]

4, 13, 19, 27, 38, 51

Sodium ferrocyanide Sodium hydrogen carbonate (sodium bicarbonate)

solid 222 .

Appendix A – Reagent List

[Na2HPO4]

57, 65

[NaOH]

[NaClO] [NaI] [NaPO3]

3, 21, 30, 49 35 1, 12, 38, 44, 47, 48, 50, 56, 57 47 60 58 13 3, 4, 9, 24, 64, 66 22 42 43 61

[NaNO3]

58

[Na3PO4]

35

Sodium pyrophosphate

[Na4P2O7]

23

Sodium silicate

[Na2SiO3]

23

[Na2SO4]

58 14

[Na2S]

48 47, 65

[Na2SO3]

42, 65 65 42

[Na2S2O3] [Na5P3O10]

56, 57 23

Sodium hydrogen phosphate Sodium hydroxide

Sodium hypochlorite Sodium iodide Sodium metaphosphate Sodium nitrate Sodium phosphate

Sodium sulfate Sodium sulfide Sodium sulfite

Sodium thiosulfate Sodium tripolyphosphate Starch Strontium chloride

pellets 8M 6M 3M 20% solution 10% solution 1.5 M 1M 0.1 M 0.1 M 0.1 M 0.1M

monobasic, 1 M

solid 1M 3M solid solid 1% solution 1.5 M 50% solution 50% solution 1% solution

46, 57, 65

0.1 M

[SrCl2]

8

Sucrose

1% solution

[C12H22O11]

Sulfuric acid

18 M (conc.)

[H2SO4]

57 3, 9, 30, 45, 53, 55, 56, 58 29 38, 56, 57 35

6M 3M 2M T Thioacetamide

6M

[CH3CSNH2] 223 .

27

Appendix A – Reagent List

Tin metal Tin (II) nitrate TLC plates U Urea Urease W Water

Z Zinc metal

Zinc nitrate

[Sn] [Sn(NO3)2]

26

2% solution 1% solution

[H2NCONH2]

47 47

distilled

[H2O]

6, 10, 20, 21, 30, 35, 46, 47, 54, 55, 61, 64, 66

small pieces powdered mossy

[Zn]

26 1, 49 25, 35

solid

[Zn(NO3)2]

26

fluorescent

224 .

26 54, 55

Appendix B – Common Materials List Material A

Specification

Acrylic, clear spray Aftershave Ajax® laundry detergent (liquid) Almonds, sliced Aluminum cans

1 23 2 50 38 10 10, 25, 27, 30, 32, 45 22, 23, 63 53

lids Aluminum foil Ammonia cleaning product Anise seeds Antacid tablets

Alka-Seltzer® Tums

Anti-freeze Aspirin Astringent B Baby oil Baking powder Baking soda Balloons, large party Battery Beets Bleach, chlorine Bloodstains Borax®

Brake fluid Bread, white Butter Butter beans C Cabbage, red Can lids Candle

Investigations

®

21, 51

21

Rolaids®

21, 51 2

aged commercial fresh commercial

55 55 62 62 51 51 5 6 22 23, 25, 27, 63 49

9V

powdered 4% solution 8% solution

emergency size small birthday

Cardboard for lid to Styrofoam® cup

61 31 31 2 50 56 50 22 10 8 36 3

225 .

Appendix B – Common Materials List

Castille soap (or Ivory Snow®) Charcoal, activated Cheese, Swiss Cheesecloth Cigar, little Cigarettes Citrus fruits Clay (soil) Cleansing cream Cloth Coffee, instant granules Coins Cologne Container with lid (plastic) Copper Cork Corn syrup Cotton balls Cotton swabs Cottonseed oil D "Dirty" water Dish washing detergent

filtered non-filtered orange, lemon, or grapefruit juices

different metals pennies (or inexpensive perfume) at least 200 mL capacity tokens (coins) wire, insulated small ground pieces 1% solution

machine hand

®

Downy fabric softener Drain cleaner Drinking Straws Drink mixes (fruit) Dry ice E Egg, raw Elmer's Glue®

61 38 50 50, 59 37 37

37 45 46 59 62 17 54 25, 45 33 23, 62 33 1 6 2 4 57 44, 45, 62 20, 49 60 38 23

18, 23 2 22, 23 19, 36 13 38, 39, 40 47, 65 31

®

Excedrine (extra strength) F Fabric dyes

54 38 226 .

Appendix B – Common Materials List

Fertilizer (inorganic) Food to test for proteins Food colors

FD&C food dyes Fritos® Fruit juices with vitamin C

common 4 blue green red common seven

58 50 28, 30, 38, 52 63 2, 20 61 52

apple orange

56 46 46

G Gelatin, unflavored Grape juice, concentrate Gum, chewing H Hair Hair spray

47 22 17

Handi-Tak® (or other removable gum adhesive)

or modeling clay

Honey

pure 1% solution

Hot air dryer I Ice Incandescent bulb (with socket) Isopropyl alcohol (rubbing) Ivory Snow® (or castille soap) K Karo® syrup Ketchup Knives L Lead samples (at least 1%) Lemon juice Lipstick M Magnet Marbles, glass Margarine

47, 63 23, 62 49

18 57 43, 54 2, 20, 34, 55

8 18 61

dark light

2 2 18 22 65 22 62

handheld

liquid solid 227 .

4 18, 33 56 56

Appendix B – Common Materials List

Marker, permanent Marshmallow, puffs Matches Meat, lean white (chicken or turkey) Metal pellets M&M's® candies Milk Mineral oil Molasses Motor oil (30 wt.)

Mulch or other humus N Nailclippers Nail polish remover Notebook paper O Oil, Olive Oil, cooking (vegetable) Oven cleaner P Paint thinner Paper clips

10

50 23, 37, 44 50, 56 41 52 47, 50 2, 44 2 2 59 47 23 9 56 17, 18 23

large metal aluminum plastic

Paper towels Paper, white sheets Paraffin Paring knife Peanut butter Peanut oil Pencil Plaster of Paris Plastic wrap

23 30, 52, 54, 55, 59 2, 31, 45

2 25, 27, 28, 40, 45, 64 11, 13, 32, 64 2 48 17 56 52, 54, 55 6

(or foil for covering beaker)

Plastic sleeve, clear, letter size Poppy seeds Potato, raw Potato chip Power steering fluid R

52, 54, 55 11, 13 53 48 56 2 1, 15, 19, 20, 30, 31, 43, 54

Ruler, metric 228 .

Appendix B – Common Materials List

Radish Rice Rubber bands Rubber, small pieces S Sand Sandpaper Scented oil Scissors Shampoo, clear or white Silver piece (tarnished) Skittles® candies Smoke detector Soap Soft drink, clear Soil samples (three) Stapler and staples Starch, soluble Steel wool, fine Storage bags, plastic zippered Straw, drinking Styrofoam® cups

Sugar, table

Sunglasses Sunscreens, 3 differenrt SPF Syrup T Tape, clear Tea bags (standard dark tea) Thumbtacks Thread Tide® Toilet bowl cleaner Transmission fluid V

50, 56 50 3, 44, 50, 59

(stopper, rubber band, eraser)

2 4, 59 15 60 7 22, 63 27

bar liquid, softsoap, bodywash

10-oz 8.5-oz 6.4-oz powdered, 1% solution granulated 1% solution

52 32 62 17, 27, 62 22 59 52 18 12, 45 33 32 3, 31, 41 42 42 57

4, 50 57 64 64 17

metal

7, 49, 62 54 2, 15 61 23 2

229 .

Appendix B – Common Materials List

Vanilla extract Vegetable cooking oil Vick's Vapoinhaler® Vinegar Vitamin C tablets Vivarin® (or No-Doze®) tablets W Wire to form a stirrer Wool, undyed or natural color

23 2, 56

250 mg

53 22, 23, 63 46 54

yarn or fabric

230 .

3 52

Appendix C - Laboratory Equipment

Apparatus A B Balance

Size/Type

Investigations

centigram

1, 5, 6, 14, 15, 16, 17, 21, 46, 54, 55, 65, 66 35, 37, 43, 58 15, 19, 20 45 9, 12, 13, 14, 17, 23, 24, 25, 44, 54, 57, 58, 59, 65, 66 22, 40, 46, 50, 54, 59 30, 31, 35, 38, 44, 48, 49, 52, 53, 55, 60 2, 20, 22, 29, 35, 36, 46, 47, 48, 54, 55, 58, 59, 61 6, 9, 30, 41, 48, 50, 51, 55, 63 19, 34, 36, 39, 48, 51, 61, 66 27 62 19

analytical Barometer Beakers

30-mL 50-mL (five)

100-mL 150-mL (two) 250-mL (three)

600-mL or 400-mL 1000-mL (1-L) (three) 2000-mL (2-L) Boiling stones (or marble chips) Burette C Caliper Centrifuge Clamps D Darkbox Desiccator (w/desiccant) Diffraction gratings Discharge Tubes (w/apparatus)

Buret Utility (incl. test tube)

49 6, 16 8 8 8 8 8 13

Helium

Hydrogen Neon Mercury Dropper bottles E Earth light Erlenmeyer flasks

1 38, 65 15 6, 29, 30, 37, 48, 51

8 5, 21 5, 19, 39, 55 36

500-mL 250-mL 100-mL 231 .

Appendix C - Laboratory Equipment

150-mL 125-mL

21 38, 46, 50, 61 15 1, 4, 6, 10, 16, 23, 38, 58 12, 16, 17, 22, 35, 37, 40, 47, 49, 50, 61, 64, 65, 66

9-cm Buchner funnel, filter flasks, stoppers, tubing to fit 9-cm Buchner or glass funnel

14, 35, 37, 38, 50, 55, 58, 66 9, 12, 14, 35, 37, 38, 46, 47, 50, 55, 58, 60, 61, 65, 66 55, 64 8, 9, 58 37 1, 9, 27, 30, 35 38, 65 2, 36, 37 44, 60, 61, 65

Eudiometer tube Evaporating dish Eye dropper

F Filter apparatus Filter paper

Flame test wires Flask Forceps Fume hood Funnel G Geiger counter Glass, cobalt Glass tube Gloves, lab Graduated cylinders

large, for drying platinum or nichrome 250-mL

long stem glass

1" ID with 2 1-holed stoppers generic Acetone resistant 10-mL

25-mL 50-mL 100-mL

1000-mL (1-L) Grease or wax pencil H Hose clamps

32 58 20 (all labs) 31 4, 12, 13, 14, 15, 17, 19, 24, 35, 38, 40, 41, 44, 45, 47, 48, 51, 52, 58, 60, 64, 65, 66 6 2, 21, 43 2, 3, 13, 19, 22, 31, 36, 38, 39, 44, 45, 46, 48, 51, 58, 59, 60, 63 15 20, 36, 39, 59, 64 36

232 .

Appendix C - Laboratory Equipment

Hot plate

Hot water bath L Laboratory burner M Metal cutters Mortar and pestle P Petri dishes Pipette with safety bulb R Radiation sources Ring, wire and ceramic coated pad Ringstand S Spatula Spectrophotometer Squeeze bottle Stirring rod, glass

Stoppers

Stopwatch

1, 10, 12, 16, 18, 21, 22, 27, 29, 35, 38, 39, 41, 46, 47, 48, 49, 50, 52, 54, 55, 57, 58, 59, 60, 61, 62, 65 65 (w/flint striker or matches)

9, 23, 30, 47, 56, 58 38 21, 53, 54, 55

10-mL volumetric 50-mL volumetric

64 46, 66 21

(alpha, beta, gamma)

32 48, 51 6, 15, 30, 37, 48, 51

100-mL

(with rubber policeman) solid to fit 500-mL Erlenmeyer flask solid to fit 500-mL Volumetric flask solid to fit small test tube solid to fit large test tube solid to fit extra-large test tube 1 hole to fit 100-mL graduated cylinder 1 hole to fit 100-mL Erlenmeyer flask 1 hole to fit 250-mL Erlenmeyer flask 1 hole to fit large test tube 1 hole to fit filter flask 2 hole to fit 100-mL Erlenmeyer flask #1 1-holed with glass tube insert (or watch with second hand)

233 .

47 38 46 4, 6, 11, 12, 17, 22, 23, 31, 38, 39, 54, 56, 59, 61, 63 1, 55, 60 21 21 54, 60, 64 18, 48 42 51 36 19 34 37 36 19 18, 20, 43, 48

Appendix C - Laboratory Equipment

T Test tubes

disposable very small (7.5 cm) small (about 10 cm long)

large (about 15 cm long) (eight)

Test tube holder Test tube rack Thermometer

Tubing

Tongs U Ultraviolet light V Vials (three) Voltmeter Volumetric flask, with stopper

30 19, 22 2, 5, 9, 10, 11, 12, 13, 26, 28, 29, 38, 41, 53, 54, 55, 56, 60, 62, 64 11, 12, 18, 34, 39, 40, 46, 47, 48, 65

extra-large (about 25 mm x 200 mm) (see also clamps)

40, 42, 57 29 11, 18 3, 6, 13, 15, 19, 20, 34, 39, 40, 41, 42, 48, 50, 55

rubber, assorted lengths clear vacuum

36, 37, 48 19, 45 44 6, 16 8, 49, 54, 55, 64

25-mL, with stoppers or caps standard microscale conductivity tester 250-mL 500-mL 1000-mL (1-L)

W Wash bottles (two) Waste container (inorganics) Watch glasses (two)

59, 62 25, 45 10 46 21 65, 66 13, 15, 21, 55 38 6, 11, 14, 16, 28, 30, 39, 44, 47, 49, 50, 52, 56, 62, 63

Weighing paper or boats

3, 4

234 .

Appendix A – Reagent List

Chemical Name A Acetic acid

Form/Concentration Formula

Labs

15 M Glacial (conc.)

6M 1M 0.5 M

28, 29, 50, 52, 55

[CH3COOH]

46, 65 4, 24, 25, 47 51

Acetic anhydride

[(CH3CO)2O]

55

Acetone Alcohol (isopropyl)

[CH3COCH3] [CH3CH(OH)CH3]

23, 28, 31, 44 (when noted in lab as alternative to ethanol)

Aluminum sulfate

1M

[Al2(SO4)3]

45

Ammonia (ammonium hydroxide)

18 M (conc.)

[NH3] or [NH4OH]

20, 50

2M 1% solution

52, 58 52

Ammonium chloride

solid

[NH4Cl]

3

Ammonium nitrate

solid

[NH4NO3]

42

Ammonium sulfide

solid

[(NH4)2S]

12

Ammonium phosphate B Barfoed's reagent Barium chloride

solid

[(NH4)3PO4]

58

0.1 M 5% solution

[BaCl2]

8 58

Barium nitrate Benedict's reagent Benzaldehyde

5% solution

[Ba(NO3)2]

58 57

[C6H5C(O)H]

28

Benzyl alcohol Buffer solution (pH=7) Butanol

[C6H5CH2OH]

29 57, 65

[CH3(CH2)3OH]

52

Butyric acid C Calcium metal Calcium acetate

[CH3(CH2)2COOH]

29

[Ca] [Ca(C2H3O2)2]

26

57

solid solid

44

Calcium chloride

solid 1M

[CaCl2]

3, 34 14

Calcium hydroxide

saturated solution

[Ca(OH)2]

36

Calcium nitrate

solid

[Ca(NO3)2]

61

218 .

Appendix A – Reagent List

Calcium oxide Cellulose Cerric(IV) nitrate (in 2 M HNO3) Chromatography paper Cobalt(II) nitrate

1M 5% solution solid 1% solution

[CaO] [Ce(NO3)6]2-

solution

9, 13, 14, 26 60 47 57 28 52

0.4 M strips and wire (sm. gauge) turnings

[Co(NO3)2]

11

[Cu]

26, 28, 45, 46, 64, 66

Copper(II) acetate

solid

[Cu(C2H3O2)2]

57

Copper(II) carbonate

solid

[CuCO3]

12

Copper(II) chloride

solid 1M 0.1 M

[CuCl2]

66 9 8

Copper(II) nitrate Copper oxide Copper(II) sulfate

1M fine powder

[Cu(NO3)2] [CuO] [CuSO4]

13, 26 49

crystals

[CuSO4.5H2O]

16

95% (denatured)

[CH3CH2OC2H3O2] [CH3CH2OH]

54, 55 10, 17, 23, 28, 29, 38, 39, 40, 41, 44, 47, 49, 50, 52, 55

Ethyl ether

[C2H5OC2H5]

50

Ethylene glycol

[HO(CH2)2OH]

30

solid

[Eu2O3]

8

40% solution

53 29

1% solution

HCHO [HCOOH] [C6H12O6]

1% solution

[C6H12O6]

57, 65

Copper

Copper(II) sulfate pentahydrate D E Ethyl acetate Ethyl alcohol (ethanol)

Europium oxide F Formaldehyde Formic acid Fructose G Glucose

12, 35

crystals 0.1% solution 1.0 M

219 .

57 47, 50 12, 13, 14, 25, 45

57

Appendix A – Reagent List

[HOCH2CHOH CH2OH]

30, 40, 56

[CaSO4.2H2O]

6

H Hexamethylenediamine

[H2N(CH2)6NH2]

30

Hexane Hydrochloric acid

[C6H14] [HCl]

28, 30, 55, 56 9, 11, 20, 58 21, 35, 48, 58 58 3, 9, 19, 24, 26 3, 13, 51 22, 64

3% solution 30% solution

[H2O2]

43, 48, 49 43

crystals 1% solution 5% solution tincture small pieces filings

[I2]

57, 65 57, 65 46, 56 25 26 4

0.2 M

[Fe(NH4)2(SO4)2]

11

1M

[FeCl3]

47, 48, 65

Glycerol (or glycerin) Gypsum

Hydrogen peroxide I Iodine

Iron metal Iron(II) ammonium sulfate Iron(III) chloride (Ferric chloride)

powdered

12 M (conc. ) 6M 3M 1M 0.5 M 0.1 M

[Fe]

0.1 M 1% solution

11 28

Iron(II) nitrate

1M

[Fe(NO3)2]

26, 47

Iron(II) sulfate

0.2 M 1M

[FeSO4]

58 9

Isobutyl alcohol

[CH3CH(CH3)CH2OH] 29

Isobutylamine

[(CH3)2CHCH2NH2]

28

Isopropyl alcohol

75% solution

[CH3CH(OH)CH3]

2, 17, 34, 58

L Lead Lead(II) acetate

sheet

[Pb] [Pb(C2H3O2)2]

32

Lead(II) nitrate Lithium chloride

1M 1M

[Pb(NO3)2] [LiCl]

13, 48 9

220 .

65

Appendix A – Reagent List

Litmus paper

0.1 M red blue

Luminol M Magnesium chloride Magnesium Magnesium sulfate heptahydrate

1M ribbon

[MgCl2]

4 8, 15, 26

(Epsom Salt)

[MgSO4.7H2O]

16

8 22, 35, 47, 58 22, 35 49

10% solution

58

Magnesium nitrate

1M 5% solution

[Mg(NO3)2]

26 60

Manganese dioxide

0.012 M

[MnO2]

38

[CH3OH]

29, 53, 54

Methanol N Nitrate/Nitrite test strips Nitric Acid

59 15 M (conc.)

6M

[HNO3]

35, 47, 50 1, 9, 12, 46, 47, 58, 64, 65, 66

n-octanol

[CH3(CH2)7OH]

29

n-octene

[CH3(CH2)5CH2]

28

[CH3(CH2)4OH]

29

n-pentanol (n-amyl alcohol) P Parafilm® pH test paper (or strips) wide range

30 23, 24, 28, 38, 47, 48, 52, 56, 57, 59, 60, 64, 65, 66

Phenolphthalein Phenol red indicator Phosphorus/Phosphate test strips

13, 21, 30, 44, 49 47 59

Phthalic anhydride

[C8H4O3]

30

Polyvinyl alcohol Potassium chloride

[(CH2CHOH)x] [KCl]

31 58 8 9

[K3Fe(CN)6]

64 11

Potassium ferricyanide

solid 0.1 M 1M 0.3M 0.1 M 221 .

Appendix A – Reagent List

Potassium ferrocyanide Potassium ferrioxalate trihydrate Potassium hydrogen sulfate Potassium iodide

Potassium permanganate Potassium thiocyanate Potassium sulfate Potassium test strips Propane, 2-chloro, 2methyl

0.1 M solid solid

[K4Fe(CN)6] [K3Fe(C2O4)3.3H2O]

11 12 64

solid

[KHSO4]

56

solid 0.1 M 1M 1% solution

[KI]

57, 65 65 12, 13 28

0.1 M

[KSCN] [K2SO4]

11

[CH3CCH3ClCH3]

28

[CH3CH2COOH]

29

[KMnO4]

Propanoic acid R Radiation sources Resorcinol

(alpha, beta, gamma)

45 59

32 [C6H4(OH)2]

28

S Salicylic acid

[C7H6O3]

29, 55

Sebacoyl chloride

[ClCO(CH2)8COCl]

30

Silver nitrate

1M 0.1 M

[AgNO3]

9, 66 64

Sodium acetate

solid 1M

[NaC2H3O2]

30 24 12

[NaHSO4]

Sodium bisulfate (Sodium hydrogen sulfate) Sodium carbonate

[Na2CO3]

Sodium chloride

solid 1M solid 0.1 M 1M

[NaCl]

23, 47, 48, 61, 65 13, 45 27, 34, 60 8 9, 13, 25

Sodium citrate

solid

[NaC6H7O6]

55, 65

[Na4FeCN6]

11

[NaHCO3]

4, 13, 19, 27, 38, 51

Sodium ferrocyanide Sodium hydrogen carbonate (sodium bicarbonate)

solid 222 .

Appendix A – Reagent List

[Na2HPO4]

57, 65

[NaOH]

[NaClO] [NaI] [NaPO3]

3, 21, 30, 49 35 1, 12, 38, 44, 47, 48, 50, 56, 57 47 60 58 13 3, 4, 9, 24, 64, 66 22 42 43 61

[NaNO3]

58

[Na3PO4]

35

Sodium pyrophosphate

[Na4P2O7]

23

Sodium silicate

[Na2SiO3]

23

[Na2SO4]

58 14

[Na2S]

48 47, 65

[Na2SO3]

42, 65 65 42

[Na2S2O3] [Na5P3O10]

56, 57 23

Sodium hydrogen phosphate Sodium hydroxide

Sodium hypochlorite Sodium iodide Sodium metaphosphate Sodium nitrate Sodium phosphate

Sodium sulfate Sodium sulfide Sodium sulfite

Sodium thiosulfate Sodium tripolyphosphate Starch Strontium chloride

pellets 8M 6M 3M 20% solution 10% solution 1.5 M 1M 0.1 M 0.1 M 0.1 M 0.1M

monobasic, 1 M

solid 1M 3M solid solid 1% solution 1.5 M 50% solution 50% solution 1% solution

46, 57, 65

0.1 M

[SrCl2]

8

Sucrose

1% solution

[C12H22O11]

Sulfuric acid

18 M (conc.)

[H2SO4]

57 3, 9, 30, 45, 53, 55, 56, 58 29 38, 56, 57 35

6M 3M 2M T Thioacetamide

6M

[CH3CSNH2] 223 .

27

Appendix A – Reagent List

Tin metal Tin (II) nitrate TLC plates U Urea Urease W Water

Z Zinc metal

Zinc nitrate

[Sn] [Sn(NO3)2]

26

2% solution 1% solution

[H2NCONH2]

47 47

distilled

[H2O]

6, 10, 20, 21, 30, 35, 46, 47, 54, 55, 61, 64, 66

small pieces powdered mossy

[Zn]

26 1, 49 25, 35

solid

[Zn(NO3)2]

26

fluorescent

224 .

26 54, 55

Appendix B – Common Materials List Material A

Specification

Acrylic, clear spray Aftershave Ajax® laundry detergent (liquid) Almonds, sliced Aluminum cans

1 23 2 50 38 10 10, 25, 27, 30, 32, 45 22, 23, 63 53

lids Aluminum foil Ammonia cleaning product Anise seeds Antacid tablets

Alka-Seltzer® Tums

Anti-freeze Aspirin Astringent B Baby oil Baking powder Baking soda Balloons, large party Battery Beets Bleach, chlorine Bloodstains Borax®

Brake fluid Bread, white Butter Butter beans C Cabbage, red Can lids Candle

Investigations

®

21, 51

21

Rolaids®

21, 51 2

aged commercial fresh commercial

55 55 62 62 51 51 5 6 22 23, 25, 27, 63 49

9V

powdered 4% solution 8% solution

emergency size small birthday

Cardboard for lid to Styrofoam® cup

61 31 31 2 50 56 50 22 10 8 36 3

225 .

Appendix B – Common Materials List

Castille soap (or Ivory Snow®) Charcoal, activated Cheese, Swiss Cheesecloth Cigar, little Cigarettes Citrus fruits Clay (soil) Cleansing cream Cloth Coffee, instant granules Coins Cologne Container with lid (plastic) Copper Cork Corn syrup Cotton balls Cotton swabs Cottonseed oil D "Dirty" water Dish washing detergent

filtered non-filtered orange, lemon, or grapefruit juices

different metals pennies (or inexpensive perfume) at least 200 mL capacity tokens (coins) wire, insulated small ground pieces 1% solution

machine hand

®

Downy fabric softener Drain cleaner Drinking Straws Drink mixes (fruit) Dry ice E Egg, raw Elmer's Glue®

61 38 50 50, 59 37 37

37 45 46 59 62 17 54 25, 45 33 23, 62 33 1 6 2 4 57 44, 45, 62 20, 49 60 38 23

18, 23 2 22, 23 19, 36 13 38, 39, 40 47, 65 31

®

Excedrine (extra strength) F Fabric dyes

54 38 226 .

Appendix B – Common Materials List

Fertilizer (inorganic) Food to test for proteins Food colors

FD&C food dyes Fritos® Fruit juices with vitamin C

common 4 blue green red common seven

58 50 28, 30, 38, 52 63 2, 20 61 52

apple orange

56 46 46

G Gelatin, unflavored Grape juice, concentrate Gum, chewing H Hair Hair spray

47 22 17

Handi-Tak® (or other removable gum adhesive)

or modeling clay

Honey

pure 1% solution

Hot air dryer I Ice Incandescent bulb (with socket) Isopropyl alcohol (rubbing) Ivory Snow® (or castille soap) K Karo® syrup Ketchup Knives L Lead samples (at least 1%) Lemon juice Lipstick M Magnet Marbles, glass Margarine

47, 63 23, 62 49

18 57 43, 54 2, 20, 34, 55

8 18 61

dark light

2 2 18 22 65 22 62

handheld

liquid solid 227 .

4 18, 33 56 56

Appendix B – Common Materials List

Marker, permanent Marshmallow, puffs Matches Meat, lean white (chicken or turkey) Metal pellets M&M's® candies Milk Mineral oil Molasses Motor oil (30 wt.)

Mulch or other humus N Nailclippers Nail polish remover Notebook paper O Oil, Olive Oil, cooking (vegetable) Oven cleaner P Paint thinner Paper clips

10

50 23, 37, 44 50, 56 41 52 47, 50 2, 44 2 2 59 47 23 9 56 17, 18 23

large metal aluminum plastic

Paper towels Paper, white sheets Paraffin Paring knife Peanut butter Peanut oil Pencil Plaster of Paris Plastic wrap

23 30, 52, 54, 55, 59 2, 31, 45

2 25, 27, 28, 40, 45, 64 11, 13, 32, 64 2 48 17 56 52, 54, 55 6

(or foil for covering beaker)

Plastic sleeve, clear, letter size Poppy seeds Potato, raw Potato chip Power steering fluid R

52, 54, 55 11, 13 53 48 56 2 1, 15, 19, 20, 30, 31, 43, 54

Ruler, metric 228 .

Appendix B – Common Materials List

Radish Rice Rubber bands Rubber, small pieces S Sand Sandpaper Scented oil Scissors Shampoo, clear or white Silver piece (tarnished) Skittles® candies Smoke detector Soap Soft drink, clear Soil samples (three) Stapler and staples Starch, soluble Steel wool, fine Storage bags, plastic zippered Straw, drinking Styrofoam® cups

Sugar, table

Sunglasses Sunscreens, 3 differenrt SPF Syrup T Tape, clear Tea bags (standard dark tea) Thumbtacks Thread Tide® Toilet bowl cleaner Transmission fluid V

50, 56 50 3, 44, 50, 59

(stopper, rubber band, eraser)

2 4, 59 15 60 7 22, 63 27

bar liquid, softsoap, bodywash

10-oz 8.5-oz 6.4-oz powdered, 1% solution granulated 1% solution

52 32 62 17, 27, 62 22 59 52 18 12, 45 33 32 3, 31, 41 42 42 57

4, 50 57 64 64 17

metal

7, 49, 62 54 2, 15 61 23 2

229 .

Appendix B – Common Materials List

Vanilla extract Vegetable cooking oil Vick's Vapoinhaler® Vinegar Vitamin C tablets Vivarin® (or No-Doze®) tablets W Wire to form a stirrer Wool, undyed or natural color

23 2, 56

250 mg

53 22, 23, 63 46 54

yarn or fabric

230 .

3 52

Appendix C - Laboratory Equipment

Apparatus A B Balance

Size/Type

Investigations

centigram

1, 5, 6, 14, 15, 16, 17, 21, 46, 54, 55, 65, 66 35, 37, 43, 58 15, 19, 20 45 9, 12, 13, 14, 17, 23, 24, 25, 44, 54, 57, 58, 59, 65, 66 22, 40, 46, 50, 54, 59 30, 31, 35, 38, 44, 48, 49, 52, 53, 55, 60 2, 20, 22, 29, 35, 36, 46, 47, 48, 54, 55, 58, 59, 61 6, 9, 30, 41, 48, 50, 51, 55, 63 19, 34, 36, 39, 48, 51, 61, 66 27 62 19

analytical Barometer Beakers

30-mL 50-mL (five)

100-mL 150-mL (two) 250-mL (three)

600-mL or 400-mL 1000-mL (1-L) (three) 2000-mL (2-L) Boiling stones (or marble chips) Burette C Caliper Centrifuge Clamps D Darkbox Desiccator (w/desiccant) Diffraction gratings Discharge Tubes (w/apparatus)

Buret Utility (incl. test tube)

49 6, 16 8 8 8 8 8 13

Helium

Hydrogen Neon Mercury Dropper bottles E Earth light Erlenmeyer flasks

1 38, 65 15 6, 29, 30, 37, 48, 51

8 5, 21 5, 19, 39, 55 36

500-mL 250-mL 100-mL 231 .

Appendix C - Laboratory Equipment

150-mL 125-mL

21 38, 46, 50, 61 15 1, 4, 6, 10, 16, 23, 38, 58 12, 16, 17, 22, 35, 37, 40, 47, 49, 50, 61, 64, 65, 66

9-cm Buchner funnel, filter flasks, stoppers, tubing to fit 9-cm Buchner or glass funnel

14, 35, 37, 38, 50, 55, 58, 66 9, 12, 14, 35, 37, 38, 46, 47, 50, 55, 58, 60, 61, 65, 66 55, 64 8, 9, 58 37 1, 9, 27, 30, 35 38, 65 2, 36, 37 44, 60, 61, 65

Eudiometer tube Evaporating dish Eye dropper

F Filter apparatus Filter paper

Flame test wires Flask Forceps Fume hood Funnel G Geiger counter Glass, cobalt Glass tube Gloves, lab Graduated cylinders

large, for drying platinum or nichrome 250-mL

long stem glass

1" ID with 2 1-holed stoppers generic Acetone resistant 10-mL

25-mL 50-mL 100-mL

1000-mL (1-L) Grease or wax pencil H Hose clamps

32 58 20 (all labs) 31 4, 12, 13, 14, 15, 17, 19, 24, 35, 38, 40, 41, 44, 45, 47, 48, 51, 52, 58, 60, 64, 65, 66 6 2, 21, 43 2, 3, 13, 19, 22, 31, 36, 38, 39, 44, 45, 46, 48, 51, 58, 59, 60, 63 15 20, 36, 39, 59, 64 36

232 .

Appendix C - Laboratory Equipment

Hot plate

Hot water bath L Laboratory burner M Metal cutters Mortar and pestle P Petri dishes Pipette with safety bulb R Radiation sources Ring, wire and ceramic coated pad Ringstand S Spatula Spectrophotometer Squeeze bottle Stirring rod, glass

Stoppers

Stopwatch

1, 10, 12, 16, 18, 21, 22, 27, 29, 35, 38, 39, 41, 46, 47, 48, 49, 50, 52, 54, 55, 57, 58, 59, 60, 61, 62, 65 65 (w/flint striker or matches)

9, 23, 30, 47, 56, 58 38 21, 53, 54, 55

10-mL volumetric 50-mL volumetric

64 46, 66 21

(alpha, beta, gamma)

32 48, 51 6, 15, 30, 37, 48, 51

100-mL

(with rubber policeman) solid to fit 500-mL Erlenmeyer flask solid to fit 500-mL Volumetric flask solid to fit small test tube solid to fit large test tube solid to fit extra-large test tube 1 hole to fit 100-mL graduated cylinder 1 hole to fit 100-mL Erlenmeyer flask 1 hole to fit 250-mL Erlenmeyer flask 1 hole to fit large test tube 1 hole to fit filter flask 2 hole to fit 100-mL Erlenmeyer flask #1 1-holed with glass tube insert (or watch with second hand)

233 .

47 38 46 4, 6, 11, 12, 17, 22, 23, 31, 38, 39, 54, 56, 59, 61, 63 1, 55, 60 21 21 54, 60, 64 18, 48 42 51 36 19 34 37 36 19 18, 20, 43, 48

Appendix C - Laboratory Equipment

T Test tubes

disposable very small (7.5 cm) small (about 10 cm long)

large (about 15 cm long) (eight)

Test tube holder Test tube rack Thermometer

Tubing

Tongs U Ultraviolet light V Vials (three) Voltmeter Volumetric flask, with stopper

30 19, 22 2, 5, 9, 10, 11, 12, 13, 26, 28, 29, 38, 41, 53, 54, 55, 56, 60, 62, 64 11, 12, 18, 34, 39, 40, 46, 47, 48, 65

extra-large (about 25 mm x 200 mm) (see also clamps)

40, 42, 57 29 11, 18 3, 6, 13, 15, 19, 20, 34, 39, 40, 41, 42, 48, 50, 55

rubber, assorted lengths clear vacuum

36, 37, 48 19, 45 44 6, 16 8, 49, 54, 55, 64

25-mL, with stoppers or caps standard microscale conductivity tester 250-mL 500-mL 1000-mL (1-L)

W Wash bottles (two) Waste container (inorganics) Watch glasses (two)

59, 62 25, 45 10 46 21 65, 66 13, 15, 21, 55 38 6, 11, 14, 16, 28, 30, 39, 44, 47, 49, 50, 52, 56, 62, 63

Weighing paper or boats

3, 4

234 .