Imat Chemistry

IMAT CHEMISTRY

IMAT Chemistry Dr.Bampilis

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IMAT Chemistry Dr.Bampilis

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IMAT CHEMISTRY The constitution of matter   

States of matter Heterogeneous and homogeneous systems Compounds and elements

1.1.

Which name of the following phase changes is NOT correct?

A. Gas to liquid = Condensation B. Solid to liquid = Melting C. Solid to gas = Sublimation D. Gas to solid = Freezing E. Liquid to gas = Evaporation 1.2.

Chemical transformations differ from physical transformations because: A. do not change with temperature.

B. involve changes in volume.

C. involve formation and separation of bonds. D. involve phase transition.

E. proceed at a constant pressure.

1.3.

Which of the following systems is not heterogeneous?

A. Foam B. Suspension C. Sm ok e D. Emulsion E. Solution 1.4.

The -ice-water system is: A. ph ysically the same.

B. physically homogeneous.

C. chemically heterogeneous and physically hom ogeneous.

D. chemically homogeneous and physically heterogeneous.

E. chemically heterogeneous.

1.5. Α compound differs from a mixture in that a compound always has a: Α. homogeneous composition. Β. maximum of two components.

C. minimum of six components.

D. minimum of three components. Ε. fixe and constant composition.

1.6. Which substance cannot be decomposed into simpler substances? Α. Ammonia Β. Aluminum C. Methane D. Methanol Ε. None of them 1.7. Under the same conditions of temperature and pressure, a liquid differs from a gas because the particles of the liquid: Α. are in constant straight-line motion. Β. take the shape of the container they occupy.

C. have no regular arrangement.

D. have stronger forces of attraction between them. Ε. have smaller forces of attraction between them.

1.8. Which statement describes a chemical property? Α. Its crystals are a metallic gray. Β. It dissolves in alcohol.

C. It forms a violet-colored gas.

D. It reacts with hydrogen to form a gas. Ε. All of them.

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The structure of the atom    

Elementary particles Atomic number and mass number Isotopes Electronic structure of atoms of the elements

2.1.

Compared to a sodium atom a sodium cation has: A. one more electron.

B. one more proton.

C. one neutron less.

D. the same mass number.

E. one proton less.

2.2.

Which is the correct way to indicate the electronic configuration of the outermost electron shell for the elements belonging to the second group of the periodic table?

A. ns2 B. np3 C. ns3 D. ns1 E. np2 2.3.

Two atoms of iron that have the same atomic number - but different mass number - 57 and 58 respectively - are: A. diastereomers of iron.

B. isotopes of iron.

C. enantiomers of iron.

D. the first one is iron, the second one is ferrite.

E. isomers of iron.

2.4.

Two isotopes of the same element have same chemical behavior because they have: A. the same number of electrons and neutrons.

B. the same mass number.

C. the same number of protons and neutrons.

D. the same number of neutrons.

E. the same number of electrons in the most outer orbital.

2.5.

Compared to the charge and mass of a proton, an electron has: A. the same charge and a smaller mass.

B. the same charge and the same mass.

C. an opposite charge and a smaller mass.

D. an opposite charge and the same mass.

E. the same charge and a bigger mass.

2.6. Α proton has approximately the same mass as: Α. a neutron. Β. an alpha particle.

C. a beta particle.

D. an electron. Ε. two electrons.

2.7. Α neutron has approximately the same mass as: Α. an alpha particle. Β. a beta particle.

C. an electron.

D. a proton. Ε. a cell.

2.8. Which symbols represent atoms that are isotopes? Α. C-14 and Ν-14 Β. Ο-16 and Ο-18 C. I-131 and Ι-131 D. Rn-222 and Ra-222 Ε. None of them 2.9. Which atom contains exactly 15 protons? Α. Ρ-32 Β. S-32 C. Ο-15 D. Ν-15 Ε. Ρ-15 2.10. An ion with 5 protons, 6 neutrons, and α charge of 3+ has an atomic number of: Α. 5 Β. 6 C. 8 D. 11 Ε. 15 2.11. Which of the following applies to a neutron? Α. Positive charge and located in an orbital. Β. Negligible mass and located in the nucleus.

C. Positive charge and located in the nucleus. D. Uncharged and located in an orbital. Ε. Uncharged and located in the nucleus.

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2.12. Which of the following facts allows you to determine that atom Α and atom Β are isotopes of the same element? Α. They each have 6 protons. Β. They each have 4 neutrons.

C. The sum of the electrons and neutrons in each is 14.

D. They each have 4 valence electrons. Ε. They each have an atomic mass of 14.

2.13. The orbitals composing an atom's valence electron shell: Α. contain the most energetic electrons of the atom. Β. are arranged as concentric spheres.

C. contain the atom's least energetic electrons.

D. never contain more than 1 electron. Ε. may change shape when covalent bonds are formed.

2.14. In a fusion reaction, reacting nuclei must collide. Collisions between two nuclei are difficult to achieve because the nuclei are: Α. both negatively charged and repel each other. Β. both positively charged and repel each other.

C. oppositely charged and attract each other.

D. oppositely charged and repel each other. Ε. none of them.

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The periodic table of elements     

Groups and periods Transition elements Periodic properties of elements: atomic radius, ionization potential, electron affinity Metals and non-metals Relations between electronic structure, position in the periodic table and properties

3.1.

Which o f the following elements does not belong to the group of alkali metals?

A. Li B. Na C. Cs D. Mg E. Fr 3.2.

The loss of a neutron from the nucleous of an atom leads to: A. an increase by one unit of Z for that element.

B. a decrease by one unit of A for that element.

C. an increase in the positive charge of the nucleus.

D. an emission of alpha and beta particles.

E. the ionization of the atom.

3.3.

Which of the following options contains the right sequence of the elements considering an increase in their ionization potential?

A.F, O. N, C B. O, N, C, F C. C, N, O, F D. C, O, N, F E. F, O, N, C 3.4.

Which of the following shows how the atomic radius of the elements changes on crossing from left to right in the row of the Periodic Table from potassium to bromine?

K to Ca

Sc to Zn

Ga to Br

A.

decrease

decrease

decrease

B.

decrease

decrease

increase

C.

decrease

increase

decrease

D.

increase

decrease

increase

E.

increase

increase

increase

3.5.

Which of the following terns of elements show a semimetallic behavior?

A. C, F, Na B. F, As, Fe C. Ca, Al, B D. Si, B, As E. Si, Na, K 3.6.

Which one of the following is correct about the first and second electron affinities of oxygen?

A. first = slightly exothermic, second = very endothermic.

B. first = slightly exothermic, second = very exothermic.

C. first = slightly endothermic, second = very exothermic.

D. first = slightly endothermic, second = very endothermic.

E. first = very exothermic, second = very exothermic.

3.7.

Which three groups of the Periodic Table contain the most elements classified as metalloids (semimetals)? Α. 1, 2 and 13 Β. 2, 13 and 14 C. 14, 15 and 16 D. 16, 17 and 18 Ε. 15, 12 and 29 IMAT Chemistry Dr.Bampilis

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3.8.

Which element's ionic radius is smaller than its atomic radius? Α. Neon B. Nitrogen C. Sodium D. Sulfur E. None of them 3.9.

Which element has the highest first ionization energy? Α. Sodium Β. Aluminum C. Calcium D. Phosphorus Ε. All elements have the same first ionization energy.

3.10. Which compound forms a colored aqueous solution? Α. CaCI 2 Β. CrCI 3 C. ΝaΟΗ D. KBr Ε.CaCl 2 and CrCI3 3.11. Which element in Group 15 has the strongest metallic character? Α. Βi Β. As C. Ρ D. Ν Ε. Both Ν and Bi 3.12. Which halogens are gases at STP? Α. Chlorine and fluorine Β. Chlorine and bromine C. Iodine and fluorine D. Iodine and bromine Ε. Iodine and chlorine 3.13. Which set of elements contains a metalloid? Α. Κ, Μn, As, Ar Β. Li, Mg, Ca, Kr C. Βa, Ag, Sn, Xe D. Fr, F, Ο, Rn Ε. None of them 3.14. Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms: Α. number of principal energy levels. Β. number of valence electrons.

C. atomic numbers.

D. atomic masses. Ε. level of similarity.

3.15. Sodium and potassium atoms behave similarly in chemical reactions, because: Α. they have the same number of neutrons. Β. each has a single valence electron.

C. they have the same atomic mass.

D. they have the same number of electrons. Ε. they have the same number of protons.

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The chemical bond      

Ionic bond Covalent bond Bond polarity Electronegativity Metallic bond Intermolecular forces

4.1.

When talκing about the ionic bond, which kind of attraction force is intended?

A. Α force between electrons and protons of any atom.

B. Α force between ions with opposite charge in the compounds.

C. Α force between nucleus and electrons of the atoms in the compounds.

D. Α force between atoms in the elements.

E. Α force between ions of the same – element.

4.2.

Covalent bond is formed when two atoms: A. transfer one or more electrons from an atom to another.

B. share all the valence electrons.

C. transfer all the valence electrons from an atom to another.

D. share all the electrons.

E. share a couple of electrons.

4.3.

Choose the shortest bond among the following: A. double C-C. B. single C-C. C. double C-O. D. single C-N. E. triple C-C. 4.4.

What is the total number of electrons in an ammonium ion, ΝH4+ ?

A. 9 B. 8 C. 11 D.10 E. 12 4.5.

How many nitrogen electrons are involved in bond formation in ΗΟΝO2 A. 4 B. 3 C. 6 D.5 E. 7 4.6.

Which of the following are correct about carbon to carbon bonds?

1. The length of carbon to carbon bonds increases in the order CC, C=C, C-C. 2. The strength of the C=C bond is less than twice the strength of the C-C bond.

3. The carbon atoms are joined by six electrons in the CC bond.

A. 1 and 2 only B. 1 and 3 only C. 2 and 3 only D. 3 only E. 1, 2 and 3 4.7.

Ionic compounds: A. are more easily soluble in polar solvents.

B. are more easily soluble in non polar solvents.

C. are sol ubl e in sol vents that are not capable to form hydrogen bonds.

D. ar e always soluble in gasoline.

E. are never water soluble.

4.8.

What is the total number of electrons in the ions of sodium chloride?

A. sodium ion = 10, chloride ion = 18 B. sodium ion = 8, chloride ion = 8 C. sodium ion = 10, chloride ion = 17 D. sodium ion = 11, chloride ion = 17 E. sodium ion = 11, chloride ion = 18

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4.9.

The positions of some elements in the Periodic Table are shown below.

Which two of the elements shown react most energetically with each other?

A. Νa and Cl B. Ne and Νa C. C and He D. Li and Br E. Li and Kr 4.10. The positions of some elements in the Periodic Table are shown above.

Which one of the following pairs of elements is most likely to form a covalent bond?

A. Beryllium and iodine B. Potassium and chlorine C. Magnesium and bromine D. Strontium and oxygen E. Calcium and chlorine 4.11.When combining with nonmetallic atoms, metallic atoms generally will: Α. lose electrons and form negative ions. Β. lose electrons and form positive ions.

C. lose electrons but don't form any ions.

D. gain electrons and form negative ions. Ε. gain electrons and form positive ions.

4.12.When a metal atom combines with a nonmetal atom, the nonmetal atom will: Α. lose electrons and decrease in size. Β. lose electrons and increase in size.

C. gain electrons and decrease in size.

D. gain electrons and increase in size. Ε. lose energy and decrease in size.

4.13. An atom of which of the following elements has the greatest ability to attract electrons? Α. Silicon Β. Both nitrogen and sulfur C. Sulfur D. Nitrogen Ε. Chlorine 4.14. At STP, which substance is the best conductor of electricity? Α. Nitrogen Β. Neon C. Sulfur D. Silver Ε. Glass 4.15. Which of the following bonds and properties are correctly matched? Α. Ionic bonds - are strong only if the participating ions are hydrated. Β. Covalent bonds - may be single, double or triple.

C. Hydrogen bonds - are responsible for bonding oxygen and hydrogen to form a single water molecule.

D. Polar covalent bonds - can occur between two atoms of the same element. Ε. Hydrogen bonds,- are stronger than covalent bonds.

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4.16. Water has the property of adhesion because: Α. hydrogen bonds form between adjacent water molecules. Β. it has a high specific heat.

C. covalent bonds hold an individual water molecule together.

D. hydrogen bonds form between water molecules and hydrophilic substances. Ε. it has a great deal of kinetic energy.

4.17. Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the van der Waals forces? All the choices are elements in the liquid state. Α. Ar, Kr, Ne, Xe Β. Kr, Xe, Αr, Ne C. Ne, Ar, Kr, Xe D. Ne, Kr, Xe, Ar Ε. Xe, Κr, Ar, Ne

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Fundamentals of inorganic chemistry  

Nomenclature Main properties of inorganic compounds: oxides, hydroxides, acids, salts, position in the periodic table.

5.1.

Which one of the following is NOT the correct formula for a lithium compound?

A. LiCO3 B. LiHSO4 C. CH3CO2Li D. Li3N E. Li2S 5.2.

Which of the following substances is not a compound?

A. Diamond B. Methane C. Limestone D. Quicklime E. Silica 5.3.

One group of elements in the Periodic Table contains, in descending order, boron, aluminum, gallium, indium and thallium. Which of the following are correct about these elements?

1. Indium forms the oxide In2O3.

2. Boron is the least reactive element in the group.

3. Gallium forms the sulphate GaSO4.

A. 1 only B. 1 and 3 C. 2 and 3 D. 1 , 2 and 3 E. 1 and 2 5.4. Which of the following formulas represents aluminium sulfate?

A. AlSO4 B. A l 2 ( S O 4 ) 3 C. Α l2 ( S O3 ) 3 D. Αl3(SO4)2 E. AISO3 5.5. Which formula represents the hypocliorite ion?

A.HClO B. ClO2C. ClOD.ClO2E. C l O 3 5.6.

Which of th e following ionic compounds contains a biv alen t cation?

A. Fe 2(SO 4) 3 B. CaCO3 C. KCI D.ΝaΟΗ E. AlPO4 5 . 7 . W h ich is th e chemical name for Cu(NO3)2?

A. Copp er (Ι) nitrate B. Cop per (ΙΙ) nitrate C. Calciu m nitrate D. Cop p er nitroxid e E. Dicopp er monoxide of nitrogen 5.8.

Which of the following chemical formulas is not correct?

A.BaCl2 B. ΚΜnΟ 4 C. RbBr D.Al2F3 E.CaO 5.9. The positions of the main group elements in the Periodic Table are shown below:

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Which one of the following formulae is NOT correct?

A. CsNO3 B. GaCO3 C. Ba(HCO3 ) 2 D. BeSO4 E. SnS2 5.10. All hydrogen halides (or hydrohalic acids) are acids that do not contain oxygen and are formed by hydrogen combined with: A. an element that belongs either to group 1 or to group 2.

B. a transition metal.

C. an alkal i metal.

D. one nonmetal or more.

E. an alkaline earth metal.

5.11. Which one of the following is NOT correct about Fe, Cu and Zn, which are in the first row of the transition metals?

A. They are all reactive metals.

B. Only two of them form coloured ions.

C. They all form basic oxides.

D. All of them form M2+ ions.

E. They all have densities greater than those of Group 1 metals.

5.12. Which of the following is a binary compound? Α. Hydrogen sulfide Β. Hydrogen sulfate C. Ammonium sulfide D. Ammonium sulfate Ε. Potassium chlorate 5.13. Given the unbalanced equation: Αl + Ο2  Αl2O3. When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients? Α. 9 Β. 7 C. 5 D. 4 Ε. 6 5.14. What is the empirical formula of the compound whose molecular formula is Ρ4Ο10? Α. PO Β. PO2 C. Ρ2Ο5 D. Ρ8Ο20 Ε. PO6 5.15. Which of the following is a binary compound? Α. Potassium chloride Β. Ammonium chloride C. Potassium chlorate D. Ammonium chlorate Ε. Hydrogen sulfate 5.16. Indicate the planar molecule between those proposed. Α. CH2O Β. CΗ4 C. Η 2Ο D. NH3 Ε. CCl4 5.17. Which formula represents a molecular substance? Α. CaO Β. CO C. Li2Ο D. Al2O3 Ε. None of them 5.18. Which substance is an example of a network solid? Α. Nitrogen dioxide Β. Sulfur dioxide C. Carbon dioxide D. Silicon dioxide Ε. All of them 5.19. Which combination of atoms can form a polar covalent bond? Α. Η and Η Β. H and Br C. N and N D. N2 and N2 Ε. Na and Br 5.20. A strontium atom differs from a strontium ion in that the atom has a greater: A. number of electrons B. number of protons C. difference D. atomic number E. mass number 5.21. Which element is a monoatomic gas at STP? A. Chlorine B. Fluorine C. Neon D. Nitrogen E. Silver 5.22. Α student investigated the physical and chemical properties of a sample of unknown gas and then investigated the gas. Which statement represents a conclusion rather than an experimental observation? Α. The gas is colorless. Β. The gas is carbon dioxide.

C. When the gas is bubbled in limewater, the liquid becomes cloudy.

D. When placed in the gas, a flaming splint stops burning. Ε. None of them.

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Chemical reactions and stoichiometry      

Atomic and molecular weight Avogadro constant Concept of the mole, conversion from grams to moles and vice versa Elementary stoichiometric calculations Balancing simple reactions Various types of chemical reactions

The Law of Conservation of Mass (or Matter) in a chemical reaction can be stated thus: In a chemical reaction, matter is neither created nor destroyed.

It was discovered by Antoine Laurent Lavoisier (1743-94) about 1785.

6.1.

What does the Lavoisier's law state?

A. When two gases at the same temperature and pressure conditions combine, the volumes of the two gases and the product of their reaction - if this too is a gas - establish a simple numerical relation.

B. In a pure chemical compound elements that formed it are in a definite and constant relation of weight between them.

C. Same volumes of different gases at the same temperature and pressure conditions contain the same number of molecules.

D. If two elements combine to give more than one compound, the relation between the amount - in terms of weights - of the first element combined with a fixed amount of the second element can be expressed with integers, usually small.

E. The sum of the masses of the substances that are reacting is equal to the sum of the masses of the substances obtained by the reaction.

6.2.

In one mole of sodium (atomic number 11, atomic weight 23) there are: A. 11 g of sodium B. 1 mole of protons C. 11 moles of protons D. 1 g of sodium E. 1 mole of electrons 6.3.

Molecular weight of ammonia is 17 a.m.u. What is the weight of 0,02 moles of this compound?

A. 1,7 g B. 340 mg C. 3,4 mg D.0,017 g E. 3,4 g 6.4.

Water molecular weight is 18 a.m.u. How many moles are contained in 2 litres of water at 4 degrees centigrade?

A. Around 111 B. Around 2 C. Around 200 D. Around 22,4 E. Around 18 6.5.

The volume of 22,414 litres is occupied by: A. a mole of liquid nitrogen.

B. a kilogram of water vapor.

C. a mole of whatever gas at the standard temperature and pressure conditions.

D. a gram of whatever gas at the standard temperature and pressure conditions.

E. a mole of whatever gas at 25 degrees centigrade and 1 atmosphere.

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6.6.

Which of the following sentences is correct?

A. Temperature influences volume and pressure of a gas, but not its amount.

B. Volume of a gas depends neither on its temperature nor on its pressure.

C. The pressure applied by a gas depends on its amount and on its volume, but not on its temperature.

D. The amount of a gas influences only its volume, neither its pressure nor its temperature.

E. The amount of a gas influences only its temperature, neither its volume nor its pressure.

6.7.

Ch oose the only one balanced equ ation.

A. 2CaOCa+O2 B. Ν2 + 3 Η2  3 ΝΗ3 C. 4ΝΗ3+5O24ΝΟ+ 6H2O D. 3 ΚΟH + 2 Η3ΡO4 Κ3PΟ4 + 3H2Ο E. 2Ο3 2Ο2+Ο 6.8.

Calculate how many grams of gaseous hydrogen are formed from a reaction between 39 g of metallic potassium (atomic weight: 39 a.m.u.) and water (excess reagent), after balancing the following reaction: Κ + H2O KOH +Η2 A. 0.5 B. 1.0 C. 2.0 D. 4 E. 3,0 6.9.

8.0 g of copper oxide is reduced to 5.6 g of copper using hydrogen gas. [relative atomic mass: Cu = 64, O= 16] CuO + Η 2  Cu + Η 2 O What is the yield of copper as α percentage of the theoretical maximum?

A. 43.9% B. 56.0% C. 14.3% D. 70.0% E. 87.5% 6.10. Ηοw many grams of sodium chloride are obtain ed from a reaction that involves 46 gram s of sod iu m (atomic weigh t: 23) and 80 gram s of chlorine (atom ic weigh t: 35.4)?

A. 144 B. 126 C. 117 D. 46 E. 132 23 -1 6.11. The Avogadro constant is 6.0 x 10 mol . How many hydrogen atoms are there in 0.420 g of cyclohexane? [Ar: H = 1; C = 12] A. 3.6 x 1022 B. 3.0 x 1021 C .1.8 x 1023 D. 3.0 x 1022 E. 1.8 x 1022 6.12. What is the total number of atoms represented in the formula CuSO4 5 Η2Ο? Α. 8 Β. 13 C. 21 D. 27 Ε. 28 6.13. One molecule of ozone contains how many oxygen atoms? Α. 1 Β. 2 C. 3 D. 4 Ε. 6 6.14. What is the mass of a formula of K2CO3? Α. 138 g Β. 106 g C. 99 g D. 67 g Ε. 78 g 6.15. What is the total number of atoms contained in 2.00 moles of nickel? Α. 58.9 Β. 22 C. 118 D. 6.02 1023 Ε. 1.2  1024 6.16. What is the total number of moles of hydrogen molecules contained in 9.03  10 23 molecules? Α. 1.5 moles B. 2.00 moles C. 6.02 moles D. 9.03 moles Ε. 9.00 moles 6.17. Α compound is 86% carbon and 14% hydrogen by mass. What is the empirical formula for this compound? Α. CH Β. CH2 C. CH3 D. CH4 Ε. CH6 23 6.18. What is the mass in grams of 3.0  10 molecules of CO2? Α. 22 g Β. 44 g C. 3g D. 66 g Ε. 88 g 6.19. What is the percent by mass of water in the hydrate Na2CO3 10 H2Ο (formula mass = 286)? Α. 6.89% Β. 9.99% C. 14.5% D. 26.1% Ε. 62.9% IMAT Chemistry Dr.Bampilis

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6.20. At STP, 32.0 liters of Ο2 contain the same number of molecules as: Α. 22.4 L Αr Β. 28.0 L of Ν2 C. 25.0 L of Ν2 D. 32.0 L of Η2 Ε. 44.8 L of He 6.21. What is the mass of a formula of (NH 4)3ΡΟ4? Α. 113 g Β. 121 g C. 149 g D. 404 g Ε. 77 g 6.22. What Kelvin temperature is equal to 25C A. 248 K B. 298 K C. 100K D. 200K E. 220K 6.23. Consider the ideal-gas equation (P.V=n.R.T) and indicate the answer reporting the correct description of the terms appearing in it.

A. Pressure, volume, number of moles and absolute temperature.

B. Pressure, dm3, number of moles and absolute temperature.

C. Pressure, volume, chemical amount and absolute temperature.

D. Pressure, dm3, number of moles and Kelvin.

E. Pascal, volume, chemical amount and absolute temperature.

6.24. Which measurement contains three significant figures? Α. 0.08 cm Β. 0.080 cm C. 800 cm D. 8.08 cm Ε. 80 cm 6.25. To determine the density of an irregularly shaped object, a student immersed the object in 21.2 milliliters of Η2o in a graduated cylinder, causing the level of the Η2Ο to rise to 27.8 milliliters. If the object had a mass of 22.4 grams, what was the density of the object? Α. 27.8 g/mL, Β. 6.6 g/mL C. 3.0 g/mL D. 3.4 g/mL Ε. 22.8 g/mL 6.26. In a laboratory exercise to determine the volume of a mole of a gas at STP, a student determines the volume to be 2.25 liters greater than the accepted value of 22.4 liters. The percent error in the student's value is: Α. 2.25% Β. 3.3% C. 10.0% D. 20.2% Ε. 24.7% 6.27. The volume of a given mass of an ideal gas at constant pressure is: Α. directly proportional to the Kelvin temperature. Β. directly proportional to the Celsius temperature.

C. inversely proportional to the Kelvin temperature.

D. inversely proportional to the Celsius temperature. Ε. directly proportional to both Kelvin and Celsius.

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Solutions

 Solvent properties of water  Solubility  The main ways of expressing the concentration of solutions Normality is another way to express the concentration of a solution. It is similar in many ways to molarity. The difference is that molarity is way to provide information about the number of molecules in a liter of solution and normality provides information about the number of reactive units in a liter of solution. Molarity is expressed in terms of moles of a compound per liter of solution. (Remember a mole is 6.021023 molecules) Normality is expressed in equivalents per liter. An equivalent can defined as the number of moles of "reactive units" in a compound. One equivalent can either react with or take the place of one mole of hydrogen ions.

Osmotic pressure is the pressure which needs to be applied to a solution to prevent the inward flow of water across a semi permeable membrane The osmotic pressure of a dilute solution is found to obey a relationship of the same form as the ideal gas law:

7.1.

How many grams of NaOH (M. W. = 40) mu st be dissolved in 500 mL of water to obtain an aqueous solution, 1 Μ, of ΝaOH? A. 40 B. 20 C.7 D. 80 E. 2 7.2.

How many grams of H2SO4 (M.W. = 98 a.m .u .} are contained in 250 ml of a 2 M H 2SO4 aqueous solu tion?

A. 98 g B. 57 g C.49 g D. 13 g E. 24,5 g 7.3.

An equivalent of AI(OH)3 is equal to: A. a mole B. a third of a mole C. three moles D. a sixth of a mole E. six moles 7.4.

What does the" normality" of a solution indicate?

A. Grams of solute per litre of solution.

B. The number of equivalent of the solute per litre of solution.

C. The number of equivalent of the solute per kilogram of solution.

D. The number of moles of the solute per litre of solution.

E. The number of moles of the solute per kilogram of solution.

7.5.

Hοw many mL of water must be added to 150 ml of a 0,4 M solution in order to obtain a final concentration of 0,1 M? A. 150 B. 300 C.600 D.250 E. 450 IMAT Chemistry Dr.Bampilis

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7.6.

Sodium chloride (relative molecular mass = 58.5) has a solubility of 36.0 g per 100 g of water.

The density of the solution is 1.13 g/mL. Which of the following calculations would give the solubility in moles per litre?

A. 36.0 1000/(58.5 1.13) B. 36.0  10 1,13/58.5 C. 36.0  1000  1,13/(58.5  136) D. 36.0101.13/(58.5136) E. 36.0 10/58.5 7.7.

At 0°C, which is the osmotic pressure of an urea solution 0.5% w/V, given the M.W. of urea is 60?

A. 1.867 atm B. 0.867atm C.200 mm Η2Ο D. 1870 mm Η2Ο E. 800 mmHg 7.8.

Which of the following statements are correct about the solvent properties of water?

1. All ionic substances dissolve in water.

2. All covalent substances are insoluble in water.

3. The solubility of solids usually increases with a rise in temperature.

A. 3 only B. 1 only C. 2 only D. 2 and 3 only E. none 7.9.

Which solution is the most concentrated? Α. 1 mole of solute dissolved in 1 litre of solution. Β. 2 moles of solute dissolved in 3 litres of solution.

C. 6 moles of solute dissolved in 4 litres of solution.

D. 4 moles of solute dissolved in 8 litres of solution. Ε. All solutions have the same degree of concentration.

7.10. What is the total number of moles of H2SO4 needed to prepare 5.0 litres of a 2.0 Μ solution of H2SO4? Α. 2.5 Β. 5.0 C. 9.0 D. 10 Ε. 20 7.11. What is the molarity of a KF(aq) solution containing 116 grams of KF (Mr = 58) in 1.00 L of solution? Α. 1.00 Μ Β. 2.00 Μ C. 3.00 Μ D. 4.00 Μ Ε. 5.00 Μ 7.12. How are the boiling and freezing points of a sample of water affected when salt is dissolved in the water? Α. The boiling point decreases and the freezing point decreases. Β. The boiling point decreases and the freezing point increases.

C. The boiling point increases and the freezing point decreases.

D. The boiling point increases and the freezing point increases. Ε. The boiling point increases and the freezing point doesn't change.

7.13. Α solution in which the crystallizing rate of the solute equals the dissolving rate of the solute must be: Α. Saturated Β. Unsaturated C. Concentrated D. A gas Ε. Dilute 7.14. Under which conditions are gases most soluble in water? Α. Hight weight and high temperature. Β. High pressure and high temperature.

C. High pressure and low temperature.

D. Low pressure and high temperature. Ε. Low pressure and low temperature.

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Thermochemistry 8.1.

How many joules are equivalent to 35 kilojoules? Α. 0.035 joules Β. 0.35 joules C. 3,500 joules D. 35,000 joules Ε. 22,000 joules 8.2.

What occurs as potassium nitrate is dissolved in a beaker of water, indicating that the process is endothermic? Α. The temperature of the solution decreases. Β. The temperature of the solution increases.

C. The solution changes color.

D. The solution gives off a gas. Ε. The solution changes density.

8.3.

Salt Α and salt Β were dissolved separately in 100 mL beakers of water. The water temperatures were measured and recorded as shown in the table below: Salt Α: initial water temp. 25.1oC final water temp. 30.2oC. Salt Β: initial water temp. 25.1oC final water temp. 20.0oC. Which statement is a correct interpretation of these data? Α. The dissolving of only salt A was endothermic. Β. The dissolving of both salt Α and salt B was exothermic.

C. The dissolving ;of only salt Β was exothermic.

D. The dissolving of both salt Α and salt Β was endothermic. Ε. The dissolving of salt Α was exothermic and the dissolving of salt Β was endothermic.

8.4. The high heat of vaporization of water accounts for: Α. the fact that ice floats. Β. evaporative cooling.

C. the fact that heat is liberated when ice forms.

D. the cohesive properties of water. Ε. capillary action.

8.5. Α solid is dissolved in a beaker of water. Which observation suggests that the process is endothermic? Α. The solution gives off a gas. Β. The temperature of the solution doesn't change.

C. The solution changes color.

D. The temperature of the solution decreases. Ε. The temperature of the solution increases.

8.6.

The heat of fusion of a compound is 30 joules per gram. What is the total number of joules of heat that must be absorbed by a 15.0 gram sample to change the compound from a solid to a liquid at its melting point? Α. 15 cal Β. 45 cal C. 150 cal D. 189 cal Ε. 450 cal 8.7. Α student determined the heat of fusion of water to be 366.9 J/g. If the accepted value is 333.3 J/g, what is the student's percent error? Α. 8.0% Β. 10.0% C. 15% D. 30.0% Ε. 7.0% 8.8.

The phase change represented by the equation I2 (S)  I2 (g) is called: A. sublimation B. Condensation C. Melting D. Boiling E. icing

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8.9.

The heat of fusion is defined as the energy required at constant temperature to change 1 unit mass of a: A. gas to a liquid B. gas to a solid C. solid to a gas D. solid to a liquid E. liquid to a solid 8.10. Solid Χ is placed in contact with solid Υ. Heat will flow spontaneously from Χ to Υ when: Α. Χ is 20°C and Υ is 20°C Β. Χ is 10°C and Υ is 5°C C. Χ is -25°C and Υ is -10°C D. Χ is 25°C and Υ is 30°C Ε. Χ is 2°C and Υ is 3°C

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Rate of reaction - Equilibrium 9.1.

With increasing temperature the value of the equilibrium constant for a reaction: A. always increases.

B. always decreases.

C. increases if the reaction is exothermic, decreases if the reaction is endotermic.

D. increases if the reaction is endothermic, decreases if the reaction is exothermic.

E. remains constant.

9.2.

In chemistry Le Chatelier's principle can be used to predict the effect of different conditions on a chemical equilibrium.

Which of the following statements are true when a reaction is already at equilibrium?

1. If temperature is increased, the endothermic direction of a reaction will be disfavoured.

2. If temperature is decreased, the endothermic direction of a reaction will be disfavoured.

3. If the volume of a container is reduced in a gas-phase reaction, it will favour the side of the reaction with fewer moles of gas.

A. 1 only B. 2 and 3 C. 2 only D. 3 only E. 1 and 3 9.3.

The following reaction is carried out until equilibrium is reached: N2O4 ⇄ 2ΝΟ2. Based on Le Chatelier's principle, what happens if the volume of the container is then decreased?

A. It cannot be predicted.

B. The reaction will go to the left.

C. Only direct changes in pressure have an effect on gas phase reactions, not changes in volume.

D. The reaction will go to the right.

E. None of the above.

9.4. Α reaction begins with only its reactants and moves into eventual equilibrium. Which of the following options is happening during the reaction until equilibrium is reached?

Rate of forward reaction Rate of reverse reaction A.

Decreases

Decreases

B.

Increases

Increases

C.

Decreases

Increases

D.

Increases

Decreases

9.5.

Which of the following is true of a catalysed reaction?

A. At equilibrium, a catalyst drives the forward reaction and so more product is produced.

B. At equilibrium, a catalyst drives the back reaction and so more reactants are produced.

C. The catalysed reaction pathway has a lower energy of activation than the uncatalysed reaction pathway.

D. Α catalyst may be the limiting reagent.

E. None of the above.

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9.6.

Sulphur dioxide reacts with oxygen to produce sulphur trioxide according to the following equilibrium: 2SO 2(g) + Ο 2(g) ⇄ 2SO 3(g)

ΔΗ =-390 kJ.

Which one of the following changes moves the equilibrium most in favour of sulphur trioxide? Α. Increase temperature and increase pressure. Β. Increase temperature and increase reactant concentrations.

C. Increase temperature and add a catalyst.

D. Decrease temperature and add a catalyst. Ε. Decrease temperature and increase pressure.

9.7. When a catalyst is added to a system at equilibrium, a decrease occurs in the: Α. activation energy. Β. heat of reaction.

C. potential energy of the reactants.

D. potential energy of the products. Ε. weight.

9.8. Which is a property of a reaction that has reached equilibrium? Α. The amount of products is greater than the amount of reactants. Β. The amount of products is equal to the amount of reactants.

C. The rate of the forward reaction is greater than the rate of the reverse reaction.

D. The rate of the forward reaction is equal to the rate of the reverse reaction. Ε. None of them.

9.9. Which procedure will increase the solubility of KCI, an endothermic process, in water? Α. Stirring the solute and solvent mixture. Β. Increasing the surface area of the solute.

C. Reducing the temperature of the solvent.

D. Increasing the pressure on the surface of the solvent. Ε. Raising the temperature of the solvent.

9.10. Given the equilibrium system at 25°C: NH4CI(s) ⇄ ΝΗ4+(aq) + CI-(aq) that occur with absorption of thermic energy, what change will shift the equilibrium to the right? Α. Decreasing the temperature to 15°C. Β. Increasing the temperature to 35°C. C. Dissolving NaCI crystals in the equilibrium mixture.

D. Dissolving NH4ΝΟΝΗ3 crystals in the equilibrium mixture. Ε. Increasing the temperature to 26°C. 9.11. Given the reaction at equilibrium: 2 CO(g) + Ο2(g) ⇄ 2 CO2(g). When the reaction is subjected to stress, a change will occur in the concentration of: Α. reactants, only. Β. products, only.

C. both reactants and products.

D. neither reactants nor products.

E. Equilibrium.

9.12. In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased? Α. C(s) + Ο2(g) ⇄ CO2(g) Β. CaCO3(s) ⇄ CaO(s) + CO2(g) C. 2 Mg(s) + Ο2(g) ⇄ 2 MgO(s) D. 2 Η2(g)+O2(g) ⇄ 2 Η2Ο(g) Ε. In none of those reported.

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9.13. Given the reaction at equilibrium: 2 SO2(g) + Ο2(g) ⇄ 2 SO3(g) + heat. Which change will shift the equilibrium to the right? Α. Adding a catalyst. Β. Adding more Ο2(g).

C. Decreasing the pressure.

D. Increasing the temperature. Ε. None of them.

9.14. Which statement explains why the speed of some chemical reactions is increased when the surface area of the reactant is increased? Α. This change increases the density of the reactant particles. Β. This change increases the concentration of the reactant.

C. This change exposes more reactant particles to a possible collision.

D. This change alters the electrical conductivity of the reactant particles. Ε. This change exposes less reactant particles to a possible collision.

9.15. Which conditions will increase the rate of chemical reaction? Α. Decreased temperature and decreased concentration of reactants. Β. Decreased temperature and increased concentration of reactants.

C. Increased temperature and decreased concentration of reactants.

D. Temperature and concentrations of reactants are not connected. Ε. Increased temperature and increased concentration of reactants.

9.16. In a chemical reaction, a catalyst changes the: Α. potential energy of the products. Β. direction of movement.

C. potential energy of the reactants. D. heat of reaction. Ε. activation energy.

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Oxidation and reduction  

Oxidation number The concepts of oxidising and reducing agents

10.1. What value does C need to be so th at the following equation can be balanced ?

KΜηO4 + a H2SO4 + 5C2H 5OH  4M nSO4 + b K2SO4 + 5CH3CO2H + c H2O A.11 B. 16 C. 17 D. 26 E. 21 10.2. The following are some compounds of nitrogen; NOCl, KNO2, NO2, NO2Cl, Ca(NO3)2 What oxidation numbers are shown by nitrogen in these compounds?

A. 2, 3, 4, 5 B. 3. 4, 5 C. 3, 4, 5, 6, D. 4,5,6 E. 2.3,4,5,6 10.3. Which is the oxidation number of sulfur in the sulphate ion?

A. -2 B. +6 C. -6 D. +8 E. +4 10.4. The oxidation number of oxygen in the Ο2 molecuie is: A. 0 B. -2 C. +2 D. -4 E. +6 10.5. Α redox reaction ends up with an equal number of: A. atoms that oxidize and atoms that reduce B. relesead electrons and negative charges C. electrons relesead and electrons gained D. electrons relesead and positive charges E. positive and negative valences 10.6. Given the reaction: Ζn + Cu2+  Ζn2+ + Cu say which of the following is correct: A. Ζn gains electrons B. Ζn is the oxidizing agent C. Cu 2+ is the oxidizing agent D. Ζn is reducedCu2+ loses electrons 10.7. Which one of the following is not an oxidation/ reduction reaction?

A. Cl 2 + H 2OHCl + HClO B. NaCl + H2SO4  NaHSO4 C. KClO4  KCl + 2O2 D. 2Fe+3Cl22FeCl3 E. The electrolysis of sodium chloride solution.

10.8. How does the chromium oxidation number vary in the following redox reaction?

(NΗ4)2Cr2O7  Cr2O3 + 4 Η2O + N2 A. From +5 to +2 B. From +4 to +3 C. From +6 to +3 D. From +7 to +2 E. From +7 to +4 10.9. In the functioning of an electrochemical cell: A. only a reduction reaction occurs B. only an oxidation reaction occurs C. a reduction-oxidation reaction occurs D. an acid-base reaction occurs E. a neutralization reaction occurs 10.10. In the following reactions, which substances are acting as oxidizing agents?

C(s) + O2(g)  CO2(g) 2Fe3+(aq) + 2I-(aq)  Fe2+(aq) + I2(aq) Mg(s) + 2H+(aq)  Mg2+(aq) + H2(g) A. O2(g), Fe3+(aq), H+(aq) B. C(s), Fe3+(aq), H+(aq) C. O2(g), I (aq), Mg(s) D. O2(g), I-(aq), H+(aq) 3+ E. C(s), Fe (aq), Mg(s)

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10.11. Consider the following reactions: C2H5Br + OH-  C2H5OH + BrBa2+(aq) + SO42-(aq)  BaSO4(s) Mg(s) + Cu2+(aq)  Mg2+(aq) + Cu(s) Which one of the following types of reaction is NOT included in this list?

A. Elimination B. Substitution C. Displacement D. Precipitation E. Oxidation/reduction 10.12. In a redox reaction: Α. an oxiding agent accepts a proton. Β. a reducing agent becomes oxidized as it accepts an electron.

C. electron is transferred from a reducing agent to an oxidizing agent.

D. a reducing agent donates a proton. Ε. the electrons in an atom move from its valence shell to a shell closer to its nucleus.

10.13. What is the oxidation number of carbon in NaHCO3? Α. +6 Β. +2 C. -4 D. +4 Ε. -2 10.14. Which statement correctly describes a redox reaction? Α. The oxidation half-reaction and the reduction-half reaction occur simultaneously. Β. The oxidation half-reaction occurs before the reduction half reaction.

C. The oxidation half-reaction occurs after the reduction half-reaction.

D. The oxidation half-reaction occurs spontaneously but the reduction half-reaction does not. Ε. The redox reaction is spontaneous in both directions.

10.15. Which metal is obtained commercially by the electrolysis of salt? Α. Ζn Β. Κ C. Fe D. Ag Ε. Au 10.16. Which element can be found in nature in the free (uncombined) state? Α. Ca Β. Βa C. Au D. Αl Ε. Ag

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Acids and bases   

Concepts of acids and bases Acidity, neutrality and basicity of aqueous solutions pH

11.1. When reacting with water, sodium oxide forms: A. a salt.

B. a hydroxide.

C. a hydroxy acid.

D. an acid.

E. sodium peroxide.

11.2. Choose the correct beheaviour of an acid in an aqueous solution: A. it releases electrons.

B. it accepts protons.

C. it releases protons.

D. it releases hydroxide ions. E. it accepts electrons.

11.3. Which one of the following is not an acid/base reaction?

A. FeCI3+6 Η2ΟFe(H2O)6 3+ + 3 CIB. 2ΝΗ3 NH2- + ΝΗ4C. ΑΙ(Η2Ο)63+ + Η2ΟAI(H2O)5(OH)2+ + H3O+ D. CH4 + H(SbF 6)CH 5+ + SbF6E. HNO3 + HCIO4H 2NO 3+ + ClO411.4. Indicate the pH value of a 1 M, HClO4 solution, at 25°C: A. 1 B. 10 C. 0 D. -1 E. 7 11.5. If an acqueous solution of a monoprotic acid has pH = 3 and contains 0.001 moles of acid per litre, then it is sure that the solution: A. contains a weak acid.

B. is a buffer system. C. contains α strong acid.

D. contains an organic acid.

E. contains an acid not entirely dissociated..

11.6. If the pH value of a solution changes from 4 to 6 what happens to the concentration of hydrogen ions that are in the solution?

A. It decreases by 100 times. B. It halves.

C. It increases by 100 times.

D. It decreases by 2 times.

E. It increases by 2 times.

11.7. Calculate the pH of a solution obtained by adding 100 ml of a 0,1 M, ΗCl solution to 50 ml of a 0,2 M, ΝaOH solution.

A. 1.00 B. 5.00 C. 14,00 D.7,00 E. 8.00 11.8. What is the pΗ of an aqueous solution of HClO4 0,040 Μ? Α. 4.0 Β. 2.7 C. 3.1 D. 1.4 Ε. 7.2 11.9. Α basic substance is weak in aqueous solution only if it: Α. is a dilute base. Β. is conjugated with a strong acid.

C. is only partially ionized.

D. is an organic base. Ε. is a derivative of NH3.

11.10. An acid substance is weak in aqueous solution if it: Α. is a dilute acid. Β. is only partially ionized.

C. is conjugated with a strong base.

D. is an organic acid. Ε. is a non-oxoacid.

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Fundamentals of organic chemistry             

Bonds between carbon atoms, molecular Structural and displayed formulae Concept of isomers Aliphatic, alicyclic and aromatic hydrocarbons functional groups: alcohols ethers amines aldehydes ketones carboxylic acids esters amides

The fat-soluble vitamins A, D, E, and K. Making halogenoalkanes from alcohols using hydrogen halides.

The general reaction looks like this:

Dehydrogenation reaction of a alcohol When the vapours of an alcohol are passed over copper catalyst heated at 573K. It undergoes dehydrogenation (loss of hydrogen or oxidation). The product formed depends on the alcohol and hence this reaction is also used to distinguish the three classes of alcohols.

When the vapours of a primary alcohol are passed over copper heated at 573K, the corresponding aldehyde is formed.

When the vapours of a secondary alcohol are passed over copper heated at 573K, the corresponding ketone is formed.

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Tertiary alcohol when reacted with copper catalyst at 573K are not dehydrogenated but undergoes dehydration to give the corresponding alkene.

Saponification is the hydrolysis of a carboxylic acid ester under basic conditions. The direct products are a carboxylic acid salt and an alcohol.

Electrophoresis is the motion of dispersed particles relative to a fluid under the influence of a spatially uniform electric field Biotin, also known as vitamin H or coenzyme R, is a water-soluble B-vitamin (vitamin B7).

Myoglobin is an iron- and oxygen-binding protein found in the muscle tissue of vertebrates in general and in almost all mammals. It is related to hemoglobin, which is the iron- and oxygen-binding protein in blood, specifically in the red blood cells.

Distinguishing tests for primary, secondary and tertiary amines

R-CONH2 + HNO2 == (HEAT) == >R-COOH + N2 (evolved)+H2O

12.1. Which one of the following could NOT be the formula of an aldehyde?

A. C5H12O B. C6H12O C. C6H12O2 D. C5H10O E. C5H10O2 11.2. What does it occurs during the combustion of a candle?

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12.3. "According to some theories on the origin of life, the first organic compounds derived from reaction of water vapour, methan, ammonia and other substances typical of the primitive atmosphere. The energy needed by these reactions might come from thunder and volcanic activity".

Which of the following statements can be gathered from this reading?

A. Reactions among water and other constituents of the primitive atmosphere required energy.

B. Reactions among water and other constituents of the atmosphere released a great amount of energy.

C. The first organic compounds might derive from the reaction between water and ammonia.

D. Many organic compounds were already part of the primitive atmosphere.

E. First living organisms derived from reactions in the primitive atmosphere.

12.4. Which is the general formula of alkanes? (η = 1, 2, 3, 4...)

A. CnH2n-2 B. CnH2n C. CnH2n+2 D.CnH2n-6 E. CnH4n 12.5. Which is the molecular formula of cyclohexane?

A. C6H8 B. C6H10 C. C6H14 D. C6H12 E. C6H6 12.6. The compound (CH3)2CHCH2NH2 can be synthesized by the following route.

1 2 3 CH3CH= CH2 CH3CHBrCH3  (CH3 )2CHCN (CH3)2CHCH2NH2 What types of reaction are used in stages 1, 2 and 3?

A. 1 = addition; 2 = substitution: 3 = hydrolysis B. 1 = addition: 2 = addition; 3 = reduction C. 1 = addition: 2 = substitution; 3 = reduction D. 1 = substitution; 2 = addition; 3 = hydrolysis E. 1 = substitution; 2 = addition: 3 = reduction 12.7. Which is the molecular formula of ethanal?

A. C2H3O B. C3H 2 O 2 C. C3HO2 D. C2H4O E. C3H2O 12.8. Which of the following compounds can be obtained by adding water to an alkene?

A. Alcohol B. Ether C. Aldehyde D. Ketone E. Alkane 12.9. Which one of t he following compounds can be made from ethanol by using only a substitution reaction?

A. Ethanal B. Bromoethane C. Ethanoic acid D. Ethoxyethane E. Ethene 12.10. Which is the formula of calcium acetate?

A. Ca2C2H3O 2 B. Ca2(C2H3O2)4 C. CaC2H3O2 D.Ca(C2H3O2)3 E. Ca(C2H3O2)2 12.11. Carboxylic acids: A. usually show low values of dissociation constant.

B. form esters reacting with other carboxylic acids.

C. do not form salts.

D. are obtained by aldehyde reduction.

E. form amines reacting with ammonia.

12.12. What can be obtained through a dehydrogenation reaction of a secondary alcohol?

A. an aldehyde B. an amide C. an ether D. an alkene E. none of the previous options 12.13. An organic compound represented by the chemical formula C6H6 may be: A. benzene B. glucose C. cyclohexane D. dimethylbutane E. hexane IMAT Chemistry Dr.Bampilis

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12.14. An aromatic compound consists of two benzene rings joined together.

Which of the following could be its formula?

1. C10H8 2. C10H10 3. C10Η12 4. C12H10 5. C12H12 A. 2 and 4 B. 3 and 4 C. 2 and 5 D.3 and 5 E. 1 and 4 12.15. Natural soaps are: A. Potassium or sodium salts of fatty acids B. monounsaturated fatty acids C. saturated fatty acids D. polyunsaturated fatty acids E. triglycerides 12.16. The nucleobases in ribonucleic acids are: A. adenine-thymine-uracil-cytosine.

B. adenine-guanine-thymirιe-cytosine.

C. adenine-guanine-pirimidina-cytosine.

D. adenine-guanine-uracil-cytosine.

E. adenine-guanine-uraci!-cytosine.

12.17. The most abundant inorganic not soluble compound in the skeleton is: A. KF B. ΝaF C. CaF2 D.CaCO3 E. Ca3(ΡΟ4)2 12.18. Wh ich of th e following sen ten ces is correct?

A. Some proteins don't contain n itrogen.

B. Every protein contains ph osp horous.

C. Every protein contains nitrogen.

D. Some proteins don 't contain carb on .

E. E very pr otein contains nitrogen sulfur.

12.19. One mole of a certain protein weighs 60 kg; this mole contains: A. 60 amino acids B. 6.000 amino acids C. 60.000 molecules 23 D. 6,023 10 molecules of proteins E. 6,0231023 molecules of amino acids 12.20. Among the following options, choose the one that represents the class of compounds that give the highest energy to an organism: A. carb ohydrates B. proteins C. lipids D. fat soluble vitam ins E. nucleic acids 12.21. Which of th e following represents a fat-soluble vitamin?

A. B1 B. Β2 C. C D. Biotin E. Κ 12.22. Which of th e following compounds contains iron ?

A. Tryglycerid es B. Myoglobin C. Chlorophyll D. Caroten e E. Insulin 12.23. How many atoms of hydrogen are there in 3.0 kg of ethane? [rel ative atomic mass: Η = 1, C = 12; Avogadro con stan t = 6.0 1 0 2 3 per mol] A. 3.6  1023 B. 3.9 1026 C. 6.01022 D.3.6  1026 E. 6.0  1025 12.24. Which of the following must be correct about organic isomers?

1. They have the same molecular formulae.

2. Their physical properties are very similar.

3. They have different structural formulae.

A. 1 only B. 1 and 3 only C. 1 and 2 only D. 2 and 3 only E. 1,2 and 3

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12.25. Which rows of the table correctly describe the reactions of the aqueous acids with amines and amides?

Amines Amides Row 1 Ethanoic acid Reacts Does not react Row 2 Nitrous acid Reacts Reacts A. Rows 1 and 2 B. None of the rows C. Rows 1 and 3 D. Rows 2 and 3 E. All of the rows 12.26. Electrophoresis is a process that separates compounds according to their: A. electric charge B. mass C. density D. magnetic moment E. electronegativity 12.27. In which pair of hydrocarbons does each compound contain only one double bond per molecule? Α. C2H2 and C 2H6 Β. C 2H2and C 3H6 C. C 4H8 and C2H4 D. C6H6 and C7H8 Ε. C6H9 and C7H12 12.28. The products of the fermentation of sugar are ethanol and: Α. water Β. hydrogen C. oxygen D. carbon dioxide Ε. sulfur dioxide 12.29. Which property is generally characteristic of an organic compound? Α. Low melting point Β. High melting point C. Medium melting point D. Soluble in polar solvents Ε. Insoluble in nonpolar solvents 12.30. The synthetic process by which monomers are covalently linked is: Α. hydrolysis Β. condensation C. isomerization D. glycosidic linkage Ε. ester linkage 12.31. Which element is present in all organic compounds? Α. Carbon B. Nitrogen C. Nitric acid D. Oxygen Ε. Phosphorous 12.32. Which of the following functional groups normally acts as an acid?

A. Amino Β. Phosphate C. Hydroxyl D. Carbonyl Ε.Sulfhydryl 12.33. Which polymers occur naturally? Α. Starch and nylon Β. Starch and plastic C. Starch and cellulose D. Protein and nylon Ε. Protein and plastic 12.34. Petroleum is classified chemically as: Α. a substance Β. a compound C. a mineral D. an element Ε. a mixture 12.35. Fatty acids in phospholipids and triacylglycerols interact with one another by: Α. disulfide bridges Β. van der Waals interactions C. covalent bonds D. hydrogen bonds

Ε. fatty acids do not interact with one another

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Answers

1.1. D , 1.2. C , 1.3. E , 1.4. D , 1.5. A , 1.6. B , 1.7. D , 1.8. D .

2.1. D , 2.2. B , 2.3. B , 2.4. E , 2.5. C , 2.6. A , 2.7. D , 2.8. B , 2.9. A , 2.10. A , 2.11. E , 2.12. A , 2.13. E , 2.14. B .

3.1. D , 3.2. B , 3.3. D , 3.4. A , 3.5. D , 3.6. A , 3.7. C , 3.8. C , 3.9. D , 3.10. B , 3.11. A , 3.12. A , 3.13. A , 3.14. B , 3.15. B .

4.1. B, 4.2. E, 4.3. E, 4.4. B, 4.5. D , 4.6. E , 4.7. A , 4.8. A , 4.9. A , 4.10. A , 4.11. B , 4.12. D , 4.13. E , 4.14. D , 4.15. B , 4.16. D , 4.17. E .

5.1. A , 5.2. A , 5.3. E , 5.4. B , 5.5. C , 5.6. B , 5.7. B , 5.8. D , 5.9. B, 5.10. D, 5.11. A , 5.12. A , 5.13. A , 5.14. C , 5.15. A , 5.16. A , 5.17. B , 5.18. D , 5.19. B , 5.20. A , 5.21. C , 5.22. B .

6.1. E , 6.2. C , 6.3. B , 6.4. A , 6.5. C, 6.6. C , 6.7. C, 6.8. B , 6.9. E , 6.10. C , 6.11. A , 6.12. C , 6.13. C , 6.14. A , 6.15. E , 6.16. A , 6.17. B , 6.18. A , 6.19. E , 6.20. D , 6.21. C , 6.22. B , 6.23. C , 6.24. D , 6.25. D , 6.26. C , 6.27. A .

7.1. B , 7.2. C , 7.3. B , 7.4. B , 7.5. E , C, 7.13. A , 7.14. C .

7.6. C , 7.7. A , 7.8. A , 7.9. C , 7.10. D , 7.11. B , 7.12.

8.1. D , 8.2. A , 8.3. E , 8.4. B , 8.5. D , 8.6. E , 8.7. B , 8.8. A , 8.9. D , 8.10.

B.

9.1. D , 9.2. B, 9.3. B, 9.4.C , 9.5. C , 9.6. E, 9.7. A , 9.8. D , 9.9. E , 9.10. B , 9.11. C , 9.12.

B , 9.13. B , 9.14. C , 9.15. E , 9.16. E .

10.1. A , 10.2. B, 10.3. B , 10.4. A , 10.5. C , 10.6. C , 10.7. B, 10.8. C , 10.9. C , 10.10. A , 10.11. A, 10.12. C, 10.13. D , 10.14. A , 10.15. B , 10.16. C .

11.1. B , 11.2. C , 11.3. A , 11.4. C , 11.5. C , 11.6. A , 11.7. D , 11.8.D , 11.9.C , 11.10. B .

12.1. A , 12.2. A , 12.3. A , 12.4. C , 12.5. D , 12.6. A , 12.7. D , 12.8. A , 12.9. B , 12.10. E , 12.11. A , 12.12. A , 12.13. A , 12.14. E , 12.15. A , 12.16. D , 12.17. E , 12.18. C , 12.19. D , 12.20. C , 12.21. E , 12.22. B , 12.23. D , 12.24. B , 12.25. A , 12.26. A , 12.27. C , 12.28. D , 12.29. A , 12.30. B , 12.31. A , 12.32. B , 12.33. C , 12.34. E , 12.35. B .

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