A) first electron shellB) second electron shellC) third electron shellD) fourth electron shell

1. In a calcium atom in the ground state, the electronsthat possess the least amount of energy are located inthe

A) 6 B) 9 C) 3 D) 18

2. What is the maximum number of electrons in the thirdshell of an atom?

A) a compound B) an elementC) a mixture D) a substance

3. The ratio of chromium to iron to carbon varies amongthe different types of stainless steel. Therefore,stainless steel is classified as

A) mass, onlyB) mass and charge, onlyC) mass and energy, onlyD) mass, charge, and energy

4. Given the balanced equation representing a reaction:H+(aq) + OH–(aq) H2O( ) + 55.8 kJIn this reaction there is conservation of

A) number of moles presentB) volume occupied by individual gas moleculesC) temperature measured on the Kelvin scaleD) pressure at standard temperature

5. The average kinetic energy of the molecules of anideal gas is directly proportional to the

A) B) C) D)

6. Which is the correct electron-dot symbol for a boronatom in the ground state?

A) protons, onlyB) neutrons, onlyC) protons and neutronsD) protons and electrons

7. The mass of a calcium atom is due primarily to themass of its

A) 9 B) 10 C) 19 D) 28

8. What is the mass number of 199F?

A) travel in defined circlesB) are most likely found in an excited stateC) have a positive chargeD) are located in orbitals outside the nucleus

9. According to the wave-mechanical model of the atom,electrons in an atom

A) 2-3 B) 2-5 C) 2-8-5 D) 2-8-6

10. Which represents the electron configuration of ametalloid in the ground state?

A) K and Na B) K and ClC) K and Ca D) K and S

11. Which elements have the most similar chemicalproperties?

A) SbO5 B) Sb5OC) Sb2O5 D) Sb5O2

12. Which formula correctly represents antimony (V)oxide?

A) small atomic radii and high ionizationenergies

B) small atomic radii and low ionization energiesC) large atomic radii and low ionization energiesD) large atomic radii and high ionization energies

13. The atoms of the most active nonmetals have

A) low electrical conductivityB) high heat conductivityC) existence as brittle solidsD) existence as molecular solids

14. Which property is generally characteristic ofmetallic elements?

A) They tend to gain electrons easily whenbonding.

B) They tend to lose electrons easily whenbonding.

C) They are poor conductors of heat.D) They are poor conductors of electricity.

15. What is a property of most metals?

A) the same chemical and physical propertiesB) the same chemical properties and different

physical propertiesC) different chemical properties and the same

physical propertiesD) different chemical and physical properties

16. At STP, the element oxygen can exist as either O2 orO3 gas molecules. These two forms of the elementhave

A) B)

C) D)

17. What is the correct Lewis electron-dot structure forthe compound magnesium fluoride?

A) B)

C) D)

18. Which Lewis electron-dot diagram is correct for CO2?

A) 8 protons, 8 neutrons, 10 electronsB) 8 protons, 10 neutrons, 8 electronsC) 8 protons, 10 neutrons, 10 electronsD) 10 protons, 8 neutrons, 8 electrons

19. An oxide ion (O2–) formed from an oxygen-18 atomcontains exactly

A) 8 valence electronsB) 2 electrons in the first shellC) 3 electron shellsD) 22 neutrons

20. An atom of argon rarely bonds to an atom of anotherelement because an argon atom has

A) The nuclear charge of each successive atomdecreases, and the atomic radius decreases.

B) The nuclear charge of each successive atomdecreases, and the atomic radius increases.

C) The nuclear charge of each successive atomincreases, and the atomic radius decreases.

D) The nuclear charge of each successive atomincreases, and the atomic radius increases.

21. What occurs as the atomic number of the elements inPeriod 2 increases?

A) H ® Li ® Na ® KB) I ® Br ® Cl ® FC) O ® S ® Se ® TeD) H ® Be ® Al ® Ga

22. Which sequence correctly places the elements inorder of increasing ionization energy?

A) Energy is absorbed and a bond is formed.B) Energy is absorbed and a bond is broken.C) Energy is released and a bond is formed.D) Energy is released and a bond is broken.

23. The balanced equation below represents a moleculeof bromine separating into two bromine atoms.

What occurs during this change?

A) attract the electrons in the bond between theatom and another atom

B) repel the electrons in the bond between theatom and another atom

C) attract the protons of another atomD) repel the protons of another atom

24. Electronegativity is a measure of an atom's ability to

A) ionic, because electrons are sharedB) ionic, because electrons are transferredC) covalent, because electrons are sharedD) covalent, because electrons are transferred

25. Two atoms with an electronegativity difference of0.4 form a bond that is

A) A -ionic B -network C -metallic D-molecularB) A -network B -ionic C -molecular D-metallicC) A -metallic B -molecular C-network D-ionicD) A -ionic B -network C -molecular D-metallic

26. The table below contains data for compounds A, B, C, and D.

Which list identifies the type of bonding characteristic of each compound's solid phase?

A) coordinate covalent bondsB) polar covalent bondsC) nonpolar bondsD) ionic bonds

27. The transfer of electrons from sodium atoms tochlorine atoms results in the formation of

A) ionic B) nonpolar covalentC) polar covalent D) metallic

28. Which type of bonding involves positive ionsimmersed in a sea of mobile electrons?

A) H2O B) H2S C) H2Se D) H2Te

29. Which molecule is the most polar?

A) B)

C) D)

30. Which electron-dot structure represents a non-polarmolecule?

A) Potential energy decreases and average kinetic energy increases.B) Potential energy increases and average kinetic energy increases.C) Potential energy increases and average kinetic energy remains the same.D) Potential energy remains the same and average kinetic energy increases.

31. The graph below represents the relationship between temperature and time as heat is added to asample of H2O

Which statement correctly describes the energy of the particles of the sample during interval BC?

A) A releases heat and B absorbs heat.B) A absorbs heat and B releases heat.C) Both A and B absorb heat.D) Both A and B release heat.

32. Solid A at 80ºC is immersed in liquid B at 60ºC.Which statement correctly describes the energychanges between A and B?

A) hydrogen bondingB) covalent bondingC) metallic bondingD) ionic bonding

33. Which intermolecular force of attraction accounts forthe relatively high boiling point of water?

A) atom-atomB) molecule-moleculeC) ion-ionD) molecule-ion

34. When a salt dissolves in water, the water moleculesare attracted by dissolved salt particles. Thisattraction is called

A) attraction by the protons for the neutronsB) attraction by the two nuclei for the electronsC) repulsion by the valence electrons of the

atomsD) repulsion by the protons in the two nuclei

35. A chemical bond between two atoms results from asimultaneous

A) Xe( ) B) Kr( )C) Ne( ) D) He( )

36. Which of the following liquids has the weakest vander Waal's forces of attraction between itsmolecules?

A) only one double bondB) two double bondsC) one triple bondD) all single bonds

37. In the alkane series, each molecule contains

A) C2H2 B) C2H4

C) C4H8 D) C4H10

38. Which compound is an alkyne?

A)

B)

C)

D)

39. Which structural formula represents a member of thealkene series?

A) 2 Na + 2 H2O ® 2 NaOH + H2

B) CaCO3 ® CaO + CO2

C) LiOH + HCl ® LiCl + H2OD) CH4 + 2 O2 ® CO2 + 2 H2O

40. Which equation represents a double replacementreaction?

A) synthesisB) decompositionC) single replacementD) double replacement

41. N2(g) + 3 H2(g) « 2 NH3(g)

What type of reaction is shown above?

A) 3s to 4s B) 3p to 4pC) 3s to 3p D) 4p to 4s

42. Which electron transition would result in theemission of energy?

A) neutron absorption by the nucleusB) gamma ray emission from the nucleusC) movement of electrons to higher energy levelsD) return of electrons to lower energy levels

43. What causes the emission of radiant energy thatproduces characteristic spectral lines?

A) more protons B) fewer protonsC) a larger radius D) a smaller radius

44. A chloride ion differs from a chlorine atom in thatthe chloride ion has

A) 2-7-1 B) 2-8-1 C) 2-8-2 D) 2-8-3

45. Which electron configuration represents an atom inan excited state?

A) 0.05 g B) 0.050 gC) 0.056 g D) 0.0563 g

46. Which measurement contains three significantfigures?

A) 49 electrons, 49 protons, and 85 neutronsB) 49 electrons, 49 protons, and 49 neutronsC) 36 electrons, 36 protons, and 85 neutronsD) 36 electrons, 36 protons, and 49 neutrons

47. What is the structure of a krypton-85 atom?

A) empty space and has a small, negativelycharged nucleus

B) empty space and has a small, positivelycharged nucleus

C) a large, dense, positively charged nucleusD) a large, dense, negatively charged nucleus

48. An experiment in which alpha particles were used tobombard thin sheets of gold foil led to theconclusion that an atom is composed mostly of

A)

B)

C)

D)

49. A student found the boiling point of a liquid to be . If the liquid's actual boiling point is ,

the experimental percent error is equal to

A) a polar covalent bond with an electronegativitydifference of zero

B) polar covalent bond with an electronegativitydifference between zero and 1.7

C) a nonpolar covalent bond with anelectronegativity difference of zero

D) a nonpolar covalent bond with anelectronegativity difference between zero and1.7

50. What type of bond exists in a molecule of hydrogeniodide?

A) HCl(g) B) NaCl(s)C) NH4Cl(s) D) CCl4( )

51. Which compound contains both ionic and covalentbonds?

A) HF( ) B) H2( )C) CH4( ) D) NH3( )

52. In which liquid is hydrogen bonding strongest?

A) 25.0 J/g B) 1376 J/gC) 2,260 J/g D) 34,400 J/g

53. At 1 atmosphere of pressure, 25.0 grams of acompound at its normal boiling point is converted toa gas by the addition of 34,400 Joules. What is theheat of vaporization for this compound, in Joules pergram?

A) It is endothermic.B) It is exothermic.C) The potential energy of the reactants is lower

than the potential energy of the product.D) The potential energy of the reactants is the

same as the potential energy of the product.

54. Given the reaction:

Fe + S ® FeS + energy

Which statement about this reaction is true?

A) alpha particles B) beta particlesC) gamma rays D) neutrons

55. Which radioactive emanations have a charge of 2+?

A) alpha decay B) beta decayC) fission D) fusion

56. Given the reaction:

This reaction is best described as

A) H2O ® H+ + OH–

B) UF6 + 6 Na ® 6 NaF + UC) 23892U ® 23490Th + 42HeD) 2713Al + 42He ® 3015P + 10n

57. Which equation represents artificial transmutation?

A) single replacement B) analysisC) transmutation D) synthesis

58. The reaction:

Is an example of

A) atomic mass B) atomic weightC) mass number D) atomic number

59. All atoms of a given element must have the same

A) the same mass number and the same atomicnumber

B) the same mass number but different atomicnumbers

C) different mass numbers but the same atomicnumber

D) different mass numbers and different atomicnumbers

60. All the isotopes of a given atom have

A) 9 B) 10 C) 19 D) 28

61. What is the total number of neutrons in an atom ofan element that has a mass number of 19 and anatomic number of 9?

A) an atomic number of 3B) 3 valence electronsC) 3 occupied principal energy levels (shells)D) an oxidation number of +3

62. All elements in Period 3 have

A) C2H4 B) C2H6

C) C3H8 D) C4H10

63. Which represents an unsaturated hydrocarbon?

A) electrons and protonsB) electrons and positronsC) neutrons and protonsD) neutrons and electrons

64. Which subatomic particles are found in the nucleusof an atom of beryllium?

A) electrons and protonsB) electrons and positronsC) neutrons and protonsD) neutrons and positrons

65. The stability of isotopes is related to the ratio ofwhich particles in the atoms?

A) 1735Cl B) 2037ClC) 3520Cl D) 3717Cl

66. Chlorine-37 can be represented as

A) total mass of all the protons and neutrons in anatom of Ti

B) total mass of all the protons, neutrons, andelectrons in an atom of Ti

C) weighted average mass of the most abundantisotope of Ti

D) weighted average mass of all the naturallyoccurring isotopes of Ti

67. The atomic mass of titanium is 47.88 atomic massunits. This atomic mass represents the

A) an electron B) a neutronC) a nucleus D) a proton

68. An orbital is defined as a region of the mostprobable location of

A) atomic number B) atomic radiusC) mass number D) neutron number

69. The elements in the Periodic Table are arranged inorder of increasing

A) high ionization energy and poor electricalconductivity

B) high ionization energy and good electricalconductivity

C) low ionization energy and poor electricalconductivity

D) low ionization energy and good electricalconductivity

70. Most nonmetals have the properties of

A) neon B) oxygenC) chlorine D) nitrogen

71. Which substance at STP exists in the form of amonatomic gas?

A) Ge and As B) Bi and PoC) B and C D) Si and P

72. Which elements are both classified as metalloids?

A) Group 1 B) Group 2C) Group 13 D) Group 17

73. Element X reacts with copper to form thecompounds and . In which group on thePeriodic Table is element X found?

A) its densityB) its colorC) its effect on litmusD) the effect on phenolphthalein

74. Which physical characteristic of a solution mayindicate the presence of a transition element?

A) 1+ B) 2+ C) 1- D) 2-

75. What is the net charge of an ion that has 8 protons, 9neutrons, and 10 electrons?

A) Be, Mg, Ca B) Ca, Mg, BeC) Ba, Ra, Sr D) Sr, Ra, Ba

76. Which list of elements from Group 2 on the PeriodicTable is arranged in order of increasing atomicradius?

A) decrease in size as it forms a positive ionB) increase in size as it forms a positive ionC) decrease in size as it forms a negative ionD) increase in size as it forms a negative ion

77. An atom with the electron configuration2-8-2 would most likely

A) Cl atom B) F atomC) O atom D) S atom

78. Which atom has the weakest attraction for theelectrons in a bond with an H atom?

A) first ionization energyB) activation energyC) conductivityD) electronegativity

79. The amount of energy required to remove theoutermost electron from a gaseous atom in theground state is known as

A) physically mixed in a fixed proportionB) physically mixed in a variable proportionC) chemically combined in a fixed proportionD) chemically combined in a variable proportion

80. A compound is a substance composed of two ormore elements that are

A) Al B) Ar C) Mg D) Na

81. In the formula XSO4, the symbol X could representthe element

A) sodium sulfite B) sodium sulfateC) sodium sulfide D) sodium thiosulfate

82. What is the chemical name for Na2SO3?

A) F B) Fr C) Cl D) Cr

83. Which element has the lowest electronegativityvalue?

A) a metallic elementB) a radioactive elementC) a molecular compoundD) an ionic compound

84. A sample of a substance has these characteristics:

• melting point of 984 K• hard, brittle solid at room temperature • poor conductor of heat and electricity as a solid• good conductor of electricity as a liquid on in anaqueous solution

This sample is classified as

A) a monatomic moleculeB) a diatomic moleculeC) a heterogeneous mixtureD) a homogeneous mixture

85. What is formed when two atoms of bromine bondtogether?

A) metallicB) hydrogen bondC) network bondD) coordinate covalent bond

86. What kind of bond is formed in the reaction shownbelow?

A) B)C) D)

87. Which formula represents a nonpolar moleculecontaining polar covalent bonds?

Base your answers to questions 88 and 89 on the information below.

A student investigated heat transfer using a bottle of water. The student placed the bottle in a roomat 20.5°C. The student measured the temperature of the water in the bottle at 7 a.m. and again at 3p.m. The data from the investigation are shown in the table below.

88. State the direction of heat transfer between the surroundings and the water in the bottle from 7 a.m. to3 p.m.

89. Show a numerical setup for calculating the change in the thermal energy of the water in the bottlefrom 7 a.m. to 3 p.m.

90. Base your answer to the following question on the following information.

Carbon and oxygen are examples of elements that exist in more than one form in the same phase. Graphite and diamond are two crystalline arrangements for carbon. The crystal structure ofgraphite is organized in layers. The bonds between carbon atoms within each layer of graphite arestrong. The bonds between carbon atoms that connect different layers of graphite are weakbecause the shared electrons in these bonds are loosely held by carbon atoms. The crystalstructure of diamond is a strong network of atoms in which the shared electrons are strongly heldby the carbon atoms. Graphite is an electrical conductor, but diamond is not. At 25°C, graphite hasa density of 2.2 g/cm3 and diamond a density of 3.51 g/cm3. The element oxygen can exist as diatomic molecules, O2, and as ozone, O3. At standard pressurethe boiling point of ozone is 161 K.

Calculate the volume, in cm3, of a diamond at 25°C that has a mass of 0.200 gram. Your responsemust include both a correct numerical setup and the calculated result.

Answer KeyBM3 Practice

1. A2. D3. C4. D5. C6. B7. C8. C9. D10. A11. A12. C13. A14. B15. B16. D17. C18. C19. C20. A21. C22. B23. B24. A25. C26. D27. D28. D29. A30. B31. C32. A33. A34. D35. B36. D

37. D38. A39. D40. C41. A42. D43. D44. C45. A46. D47. D48. B49. A50. B51. C52. A53. B54. B55. A56. B57. D58. C59. D60. C61. B62. C63. A64. C65. C66. D67. D68. A69. A70. A71. A72. A

73. D74. B75. D76. A77. A78. D79. A80. C81. C82. A83. B84. D85. B86. D87. B88. –Heat was

transferred from thesurroundings to thewater in the bottle.–The water absorbedenergy from thesurroundings.

89. q = (800. g)(4.18 J/g• ºC)(20.5ºC –12.5ºC)(800)(4.18)(8)

90.