Introduction to Chemistry Review
Questions
Course Introduction
Introduction to Chemistry provides a comprehensive foundation in the principles and concepts of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and the properties of acids, bases, and solutions. The course emphasizes the application of scientific methods and problem solving, equipping students with the skills necessary to analyze chemical reactions and understand the role of chemistry in everyday life and various scientific fields. Through laboratory exercises and theoretical lessons, students gain practical experience and develop a deeper appreciation for the fundamental role chemistry plays in the natural world and modern technology.
Recommended Textbook
Foundations of College Chemistry 13th Edition by Morris Hein
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Page 2
Chapter 1: An Introduction to Chemistry
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Sample Questions
Q1) Which is a pure substance ?
A)element
B)compound
C)mixture
D)both A and B
Answer: D
Q2) State the four steps of the scientific method.
Answer: The four steps of the scientific method are:
1.Making observations to collect facts or data.
2.Formulating a hypothesis to explain your observations.
3.Designing and performing experiments to test your hypothesis.
4.Using the results of your experiments to reformulate your hypothesis. You then retest your hypothesis and continue on.
Q3) Which is a solution?
A)air
B)liquid water
C)solid iron
D)soil
Answer: A
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Page 3
Chapter 2: Standards for Measurement
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Sample Questions
Q1) The density of copper is 8.96g/mL.The mass of 7.00mL of copper is
A)62.7g
B)1.28g
C)0.781g
D)1.96g
Answer: A
Q2) How many significant figures should be included in the answer to the following calculation? (3.60)(2.489)(5.1110)
A)2
B)3
C)4
D)5
Answer: B
Q3) The density of ethanol is 0.7893g/mL.What is the mass of one pint of ethanol?
Answer: The mass of one pint of ethanol is 373.4g
Q4) If two substances have the same mass,the one with the greater volume will have the greater density.<sup> </sup>
A)True
B)False
Answer: False
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Chapter 3: Elements and Compounds
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Sample Questions
Q1) The majority of the elements are A)metals. B)gases. C)nonmetals.
D)metalloids.
Answer: A
Q2) Which element is a liquid at room temperature? A)fluorine. B)chlorine. C)bromine. D)iodine.
Answer: C
Q3) Consider the chemical formula for one molecule of methane,CH<sub>4</sub>.If instead of one molecule we had 10 molecules of methane,how many carbon atoms would be present?
A)10
B)1 C)4
D)40
Answer: A
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Chapter 4: Properties of Matter
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Sample Questions
Q1) When 20.0g of mercury is heated from 10.0<sup>º</sup>C to 20.0<sup>º</sup>,27.6 J of energy are absorbed.What is the specific heat of mercury?
A)0.725 J/g<sup>º</sup>C
B)0.138 J/g<sup>º</sup>C
C)2.76 J/g<sup>º</sup>C
D)No correct answer is given
Q2) The specific heat of aluminum is 0.900J/g<sup>º</sup>C.A 400.0g sample of aluminum at 20.0<sup>º</sup>C absorbs 2520.J of heat energy.What is the new temperature of the aluminum?
A)7.00<sup>º</sup>C
B)13.0<sup>º</sup>C
C)20.0<sup>º</sup>C
D)27.0<sup>º</sup>C
Q3) When chemical reactions occur,energy is always released.
A)True
B)False
Q4) 4.184 joules are equal to one calorie.
A)True
B)False
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Chapter 5: Early Atomic Theory and Structure
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Sample Questions
Q1) What is the relative electrical charge of a proton?
A)-1
B)+1
C)-2
D)0
Q2) Define in simple terms the concept of natural abundance for the isotopes of any element and how it determines the average atomic masses of the elements.
Q3) Which experiment led to the notion that the atom contains an extremely small,positively charged nucleus?
A)Millikan's oil drop experiment
B)Rutherford's gold foil experiment
C)Thomson's cathode ray experiment
D)Dalton's atomic experiment
Q4) What is the atomic number of magnesium?
A)12
B)24
C)25
D)55
Q5) How are the different isotopes of an element alike;how are they different?
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Chapter 6: Nomenclature of Inorganic Compounds
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Sample Questions
Q1) Which is phosphorous pentachloride?
A)PCl<sub>5</sub>
B)P<sub>5</sub>Cl
C)P<sub>2</sub>Cl<sub>5</sub>
D)P<sub>5</sub>Cl<sub>2</sub>
Q2) Nitrogen and oxygen combine in a number of ways.In these compounds the oxygen atom always carries a -2 charge.What is the charge of the nitrogen atom in each compound?
A.NO
B.NO<sub>2</sub>
C.N<sub>2</sub>O
D.N<sub>2</sub>O<sub>4</sub>
Q3) Which is a cation?
A)A vanadium (II)ion
B)A fluoride ion
C)A hydroxide ion
D)A hydrogen carbonate ion
Q4) The prefix "hepta" means six.
A)True
B)False
Page 8
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Chapter 7: Quantitative Composition of Compounds
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Sample Questions
Q1) What is the percent by mass of hydrogen in sulfuric acid?
A)1.04%
B)2.06%
C)4.03%
D)5.93%
Q2) One mole of magnesium has the same number of atoms but a smaller mass than one mole of sulfur.
A)True
B)False
Q3) What is the molecular formula of a compound with the empirical formula
CHO<sub>2</sub> and molar mass of 90.04g?
A)CHO<sub>2</sub>
B)C<sub>2</sub>H<sub>2</sub>O<sub>4</sub>
C)C<sub>3</sub>H<sub>3</sub>O<sub>6</sub>
D)C<sub>4</sub>H<sub>4</sub>O<sub>8</sub>
Q4) How many grams of carbon are present in 45.0 g of CCl<sub>4</sub>?
A)0.293 g
B)3.51 g
C)5.76 g
D)41.49 g
Page 9
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Chapter 8: Chemical Equations
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Sample Questions
Q1) The following questions refer to a reaction in which sodium and water react to produce sodium hydroxide and hydrogen gas.
A.Write a balanced chemical equation for the reaction.
B.When one mole of hydrogen is produced,how many moles of sodium are consumed?
C.When one mole of hydrogen is produced,how many moles of water are consumed?
D.When one mole of hydrogen is produced,how many moles of sodium hydroxide are produced?
Q2) Change these word equations into balanced chemical equations.
A.Magnesium plus oxygen yields magnesium oxide.
B.Water decomposes to yield hydrogen and oxygen.
C.Sodium sulfate plus barium chloride yields barium sulfate and sodium chloride.
D.Sodium plus iron(III)nitrate yields sodium nitrate plus iron.
Q3) The following reaction: 2H<sub>2</sub> + O<sub>2</sub> \(\rarr\)2H<sub>2</sub>O,is an example of A)combination.
B)decomposition.
C)single-displacement.
D)double-displacement.
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Page 10
Chapter 9: Calculations From Chemical Equations
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Sample Questions
Q1) What mass of carbon monoxide is produced when 1.50 moles of oxygen react completely in the following equation? 2C + O<sub>2</sub> \(\rarr\)2CO
A)84.0g
B)42.0g
C)28.0g
D)21.0g
Q2) In every chemical reaction the number of moles of reactant must equal the number of moles of product.
A)True
B)False
Q3) Two solutions are combined in a beaker.One solution contains 500.0g of potassium phosphate and the other contains 500.0g of calcium nitrate.A double-displacement reaction occurs.What mass of each of the following substances is present when the reaction stops.
A.Potassium phosphate
B.Calcium nitrate
C.Calcium phosphate
D.Potassium nitrate
Q4) Nitrogen gas to water
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Chapter 10: Modern Atomic Theory and the Periodic Table
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Sample Questions
Q1) The third principal energy level can hold a maximum of 18 electrons. A)True
B)False
Q2) Each horizontal row on the periodic table is called a A)period B)family
C)group
D)cohort
Q3) The electron configuration,[Ne] 3s<sup>2</sup> 3p<sup>4</sup>,is the ground state electron configuration of A)sodium. B)neon.
C)argon. D)sulfur.
Q4) Atoms of which two elements in the ground state contain the same number of valence electrons?
A)Al and Si
B)Al and B
C)Al and Zn
D)Al and Ge
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Chapter 11: Chemical Bonds: the Formation of Compounds
From Atoms
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Sample Questions
Q1) Using Lewis electron dot symbols,show how magnesium chloride forms from its elements.
Q2) Which of the following statements is false?
A)In order for a covalent bond to form,the atomic orbitals of the atoms must overlap.
B)The most common ions for the representative elements can be predicted based on their tendency to attain the same electron configuration of the closest noble gas.
C)Ionization energies show a large decrease when electrons are removed from a noble gas-like configuration.
D)Ionic compounds exist as large aggregates of positive and negative ions.
Q3) Which does not have a noble gas electron configuration?
A)Sc<sup>+3</sup>
B)Ar
C)O<sup>-2</sup>
D)K
Q4) The Ca<sup>+2</sup> ion is larger than the Ca atom.
A)True
B)False
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Chapter 12: The Gaseous State of Matter
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Sample Questions
Q1) What is the volume of 1.40 moles of chlorine gas at STP?
A)31.4 L
B)16.0 L
C)0.316 L
D)3.17 L
Q2) How many moles of hydrogen are consumed when 40.0 L of hydrogen chloride gas are produced in the following equation?
H<sub>2</sub>(g)+ Cl<sub>2</sub>(g)\(\rarr\)2 HCl(g)
A)0.446 moles
B)0.893 moles
C)1.79 moles
D)3.57 moles
Q3) Under which set of conditions will a real gas be most likely to act as an ideal gas?
A)High temperature and high pressure
B)High temperature and low pressure
C)Low temperature and high pressure
D)Low temperature and low pressure
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14
Chapter 13: Liquids
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Sample Questions
Q1) Which substance contains molecules that will not form hydrogen bonds?
A)Hydrogen
B)Hydrogen fluoride
C)Water
D)Ammonia
Q2) Which phase change corresponds to condensation?
A)Liquid to gas
B)Solid to liquid
C)Solid to gas
D)Gas to liquid
Q3) Which has the lowest vapor pressure?
A)25 mL of water at 283 K
B)10 mL of water at 298 K
C)50 mL of water at 293 K
D)5 mL of water at 323 K
Q4) A 3.000 g sample of hydrated calcium chloride was heated to drive off all the water of crystallization.The remaining anhydrous sample had a mass of 2.2646 g.What is the formula of the hydrate?
Q5) A hydrated sample of cobalt(II)chloride was analyzed and found to consist of 45.44% water.What is the formula of the hydrate?
Page 15
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Chapter 14: Solutions
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Sample Questions
Q1) As particle size increases,surface area increases,and the rate of dissolving increases.
A)True
B)False
Q2) One liter of 2.0 M KCl solution and two liters of 1.0 M KCl solution have the same A)Density
B)Concentration
C)Volume
D)Moles of solute
Q3) What is the mass percent of the solution formed when 5.0 g of solute is dissolved in 40.g of water?
A)8.0 %
B)11 %
C)13 %
D)14 %
Q4) A sulfuric acid solution that is 34.0 % by mass has a density of 1.25 g/mL. What is the molarity of the solution?
Q5) Explain why the solubility of gases decreases with increasing temperature.
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Page 16
Chapter 15: Acids, Bases, and Salts
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Sample Questions
Q1) Which is a strong base?
A)CuOH
B)HCl
C)KOH
D)CH<sub>3</sub>OH
Q2) The pH of a solution can be calculated from the expression
A)pH = - log [OH<sup> -1</sup>]
B)pH = log [OH<sup> -1</sup>]
C)pH = - log [H<sup> +1</sup>]
D)pH = log [H<sup> +1</sup>]
Q3) A 50.0 mL aliquot of a 1.0 M aqueous nitric acid solution is added to a solution prepared from 0.50 g of sodium hydroxide dissolved in enough water to make 500.0 mL of solution.Will the resulting solution be acidic or basic? Support your answer by showing theappropriate calculations.
Q4) What is the pH of a 0.020 M nitric acid solution?
A)0.020
B)-2.0
C)1.7
D)4.0
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Chapter 16: Chemical Equilibrium
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Sample Questions
Q1) The value of the equilibrium constant is temperature dependent.
A)True
B)False
Q2) The equilibrium constant can change significantly with a change in A)concentration.
B)catalyst.
C)temperature. D)pressure.
Q3) Equilibrium is reached in a chemical reaction when
A)the reactants are completely consumed.
B)the concentrations of all reactants and products become equal.
C)the rates of the opposing reactions become equal.
D)the forward and reverse reactions stop.
Q4) What is the pH of a 0.140 M HCl solution?
A)0.854
B)13.2
C)0.140
D)3.66
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Chapter 17: Oxidationreduction
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Sample Questions
Q1) In this chemical process,the oxidation numbers of aluminum on the reactant and the product are: 2 Al<sub>2</sub>O<sub>3</sub> \(\rarr\) 4 Al + 3 O<sub>2</sub>
A)+2,+3
B)+3,0
C)+2,+4
D)0,+4
Q2) Which species is the reducing agent in the following equation?
2 Al<sub>2</sub>O<sub>3</sub>\(\rarr\) 4 Al + 3O<sub>2</sub>
A)Al<sup>+3</sup>
B)O<sup>-2</sup>
C)Al
D)O<sub>2</sub>
Q3) In an electrolytic cell
A)a chemical reaction occurs spontaneously and releases energy as electricity.
B)electricity causes a chemical reaction to occur.
C)a physical change occurs spontaneously and releases energy as electricity.
D)electricity causes a physical change to occur.
Q4) During a redox reaction,the reducing agent is oxidized.
A)True
B)False
Page 19
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Chapter 18: Nuclear Chemistry
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Sample Questions
Q1) Part of a radioactive decay series begins with U-238 emitting in succession a(n)
A.Alpha particle
B.Beta particle
C.Beta particle
D.Alpha particle
E.Alpha particle
Predict the product of each successive emission.
Q2) The instrument used to measure ionizing radiation is a
A)radioactive counter.
B)Curie counter.
C)Roentgen counter.
D)Geiger counter.
Q3) A beta particle has
A)a mass of 4 amu.
B)a charge of +4.
C)a charge of -1.
D)neither mass nor charge.
Q4) U-232 represents a uranium isotope with 92 protons and 146 neutrons.
A)True
B)False
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Chapter 19: Introduction to Organic Chemistry Online Only
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Sample Questions
Q1) How many pairs of electrons are shared in a single covalent bond?
A)One
B)Two
C)Three
D)Four
Q2) What is the total number of carbon atoms in a molecule of 2-methyl-4-ethyloctane?
A)8
B)11
C)14
D)17
Q3) How many pairs of electrons are shared in a double covalent bond?
A)One
B)Two
C)Three
D)Four
Q4) Write the balanced molecular formulas for the incomplete combustion of the first three members of the alkane series.The products are carbon monoxide and water.
Q5) Name and write the formulas for the three structural isomers of pentane.
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Chapter 20: Introduction to Biochemistry Online Only
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Sample Questions
Q1) The end product of the digestion of starch is A)cellulose.
B)glucose.
C)glycogen.
D)glucagon.
Q2) A fatty acid which contains many double covalent bonds between carbon atoms is saturated.
A)True
B)False
Q3) Animals store food energy as A)glycogen.
B)cellulose.
C)enzymes.
D)glucagon.
Q4) Carbohydrates supply about 17 kJ of energy per gram.What mass of glucose would yieldapproximately 340 kJ of energy?
A)5800 g
B)0.050 g
C)20.g
D)357 g
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