CHAPTER 4

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.

____ 1. A substance is a brittle crystal that conducts electricity in molten liquid state only. Which type ofsubstance is it?

a. metallic crystal d. molecular crystalb. ionic crystal e. frozen gasc. covalent crystal

____ 2. A substance is a solid that is ductile and malleable and conducts electricity and heat in the solid state.Which type of substance is it?

a. metallic solid d. molecular solidb. ionic solid e. perfect crystalc. covalent solid

____ 3. A solid is soft and has a low melting point. It does not conduct electricity. What type of solid is it?a. metallic solid d. molecular crystalb. ionic crystal e. plasmac. covalent solid

2____ 4. Which shape and bond angle are predicted by VSEPR theory for H O?a. linear, 180 d. bent, 109.5o o

b. bent, 120 e. bent, less than 109.5o o

c. bent, less than 120o

____ 5. What is the basis of metallic bonding?a. the attraction of metal ions for delocalized electronsb. the attraction between neutral metal ionsc. the neutralization of protons by electronsd. the attraction of oppositely charged ionse. the sharing of two valence electrons between two atoms

____ 6. When is ionic bonding likely to occur between two atoms?a. when both atoms have low ionization energy and low electron affinityb. when both atoms have high ionization energy and high electron affinityc. when both atoms have high ionization energy and low electron affinityd. when one atom has high ionization energy and high electron affinity, while the other has

low ionization energy and low electron affinitye. when one atom has a high ionization energy and low electron affinity, while the other has a

low ionization energy and a high electron affinity

____ 7. Polar covalent bonds occur betweena. atoms which both have equally high electronegativitiesb. atoms which have high but unequal electronegativitiesc. atoms which both have equally low electronegativitiesd. atoms which both have equally low ionization energiese. atoms which have low but unequal ionization energies

____ 8. Which of the following bonds is likely to exhibit the greatest ionic character?a. H-F d. Cl-Clb. F-F e. Cl-Fc. H-Cl

____ 9. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart aspossible?

a. pairs of valence electrons d. mobile electronsb. inner shell electrons e. lone pairs of electronsc. bonding pairs of electrons

____ 10. Four pairs of electrons surrounding a central atom will be arrangeda. pyramidally d. linearlyb. spherically e. trigonallyc. tetrahedrally

____ 11. Diamond and graphite differ in thata. only graphite is composed of carbon atomsb. only graphite conducts electricityc. only graphite burns in oxygen to give carbon dioxide gasd. diamond is less dense than graphitee. diamond is a compound

____ 12. Which of the following is a covalent network solid?a. sodium chloride d. asbestosb. carbon dioxide e. phosphorusc. brass

____ 13. Intermolecular forces area. forces within covalent molecules that hold them togetherb. electrostatic forces between ionsc. bonds between hydrogen and oxygen atoms in water moleculesd. attractive forces between separate covalent moleculese. covalent bonds within a network solid

____ 14. What is the correct order of bond polarity of the bonds F-F, H-F and O-F beginning with the least polar?a. F-F, O-F, H-F d. H-F, F-F, O-Fb. F-F, H-F, O-F e. O-F, H-F, F-Fc. H-F, O-F, F-F

2 2 3 3____ 15. Which of the molecules, CO , H O, NH , and BF , will be polar?

2 3 3 2 2 3a. CO , NH and BF d. CO , H O and NH

2 3 2 3b. H O and NH e. CO and BF

2 3c. H O and BF

____ 16. A molecule consisting of a central atom surrounded by two bonding pairs and two non-bonding (lone)pairs of electrons will be

a. linear d. trigonal pyramidalb. tetrahedral e. trigonal planarc. bent

____ 17. The shape of a BF ion will bea. trigonal pyramidal d. octahedralb. trigonal planar e. tetrahedralc. trigonal bipyramidal

____ 18. The attractive forces that exist between all covalent molecules are known asa. dipole-dipole forces d. hydrogen bondsb. intramolecular forces e. dispersion forcesc. covalent bonds

____ 19. Why does a central atom surrounded by 4 atoms have a tetrahedral shape instead of a square planarshape?

a. orbitals are never at right angles to each otherb. the lone pairs around the central atom push the 4 atoms into this configurationc. the angle in a tetrahedron is larger than in a square planar arrangementd. the 4 atoms want to be as close together as possiblee. none of the above

____ 20. What would be the shape of a molecule containing a central atom attached to two other atoms with onelone pair of electrons?

a. linear d. tetrahedralb. bent e. trigonal bipyramidalc. trigonal planar

____ 21. What would be the shape of a molecule containing a central atom attached to two other atoms with nolone pairs of electrons?

a. linear d. trigonal planarb. bent e. see-sawc. trigonal pyramidal

____ 22. What would be the shape of a molecule containing a central atom attached to two other atoms with threelone pairs of electrons?

a. linear d. trigonal planarb. bent e. see-sawc. trigonal pyramidal

____ 23. What would be the shape of a molecule containing a central atom attached to three other atoms with onelone pair of electrons?

a. linear d. trigonal planarb. bent e. see-sawc. trigonal pyramidal

____ 24. What would be the shape of a molecule containing a central atom attached to two other atoms with twolone pairs of electrons?

a. bent d. see-sawb. trigonal pyramidal e. square planarc. trigonal planar

____ 25. What would be the shape of a molecule containing a central atom attached to four other atoms with onelone pair of electrons?

a. trigonal planar d. square pyramidalb. see-saw e. octahedralc. square planar

____ 26. What would be the shape of a molecule containing a central atom attached to four other atoms with twolone pairs of electrons?

a. trigonal planar d. square pyramidalb. trigonal pyramidal e. octahedralc. square planar

____ 27. What would be the shape of a molecule containing a central atom attached to five other atoms with onelone pair of electrons?

a. trigonal pyramidal d. square pyramidalb. trigonal planar e. octahedralc. square planar

____ 28. What would be the shape of a molecule containing a central atom attached to six other atoms?a. trigonal planar d. square pyramidalb. trigonal pyramidal e. octahedralc. square planar

3____ 29. What would be the shape of BF ?a. trigonal planar d. square planarb. trigonal pyramidal e. none of the abovec. tetrahedral

____ 30. Which of the following substances would be polar?a. carbon dioxide d. ammonium ionb. boron trifluoride e. sulfate ionc. ammonia

____ 31. Which of the following substances would not be polar?a. hydrogen chloride d. sulfur dioxideb. ammonia e. carbon dioxidec. water

____ 32. Which of the following is not a property of ionic solids.a. conduct electricity in solution d. contain positive and negative ionsb. brittle e. ductilec. form a lattice

3____ 33. Which forces exist between ammonia, NH , particles?I. Van der Waals

II. metallic bondingIII. hydrogen bondingIV. dipole

a. I only d. I, III and IV onlyb. I and IV only e. I, II and III onlyc. I and II only

4____ 34. Which forces exist between methane, CH particles?I. Van der Waals

II. metallic bondingIII. hydrogen bondingIV. dipole

a. I only d. I, III and IV onlyb. I and IV only e. I, II and III onlyc. I and II only

____ 35. Which forces exist between hydrogen chloride, HCl, particles?I. Van der Waals

II. metallic bondingIII. hydrogen bondingIV. dipole

a. I only d. I, III and IV onlyb. I and IV only e. I, II and II onlyc. I and II only

____ 36. Which forces exist between iron, Fe, particles?I. Van der Waals

II. metallic bondingIII. hydrogen bondingIV. dipole

a. I only d. I, III and IV onlyb. I and IV only e. I, II and III onlyc. I and II only

____ 37. What causes high surface tension in water?a. the high boiling point of water d. the low density of iceb. the bent shape of the molecule e. none of the abovec. hydrogen bonding

____ 38. When do ionic compounds conduct electricity?I. when warm

II. when moltenIII. when dissolvedIV. when gaseous

a. II only d. I and II onlyb. I, II and III only e. II and III onlyc. IV only

____ 39. Which statement is the best description of hydrogen chloride, HCl?a. polar molecule d. ionic compoundb. polar bonds, non polar molecule e. none of the abovec. non polar molecule

4____ 40. Which statement is the best description of carbon tetrachloride, CF ?a. polar molecule d. ionic compoundb. polar bonds, non polar molecule e. none of the abovec. non polar molecule

2____ 41. Which statement is the best description of water, H O?a. polar molecule d. ionic compoundb. polar bonds, non polar molecule e. none of the abovec. non polar molecule

2____ 42. Which statement is the best description of chlorine, Cl ?a. polar molecule d. ionic compoundb. polar bonds, non polar molecule e. none of the abovec. non polar molecule

____ 43. Which statement is the best description of potassium chloride, KCl?a. polar molecule d. ionic compoundb. polar bonds, non polar molecule e. none of the abovec. non polar molecule

____ 44. What type of substance is potassium chloride, KCl?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

2____ 45. What type of substance is carbon dioxide, CO ?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

____ 46. What type of substance is graphite?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

____ 47. What type of substance is sodium, Na?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

2____ 48. What type of substance is hydrogen sulfide, H S?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

4____ 49. What type of substance is methane, CH ?a. ionic d. metallicb. molecular e. none of the abovec. covalent network

____ 50. Identify the incorrect set of information about the shapes of molecules with single bonds only.

Set Lone pairs oncentral atom

Bonding pairs oncentral atom

Shape

A 0 3 trigonal bipyramidal

B 0 4 tetrahedral

C 0 6 octahedral

D 1 3 trigonal pyramidal

E 2 2 V shaped

a. set A d. set Db. set B e. set Ec. set C

____ 51. Which gaseous molecule is non polar?

3 3a. ozone, O d. NH

4b. HCl e. CH

2c. H O

____ 52. Which species is square planar?

4 4a. CF d. SF

44b. BF 1- e. XeF

4c. PF 1-

____ 53. How would Dr. Richard Bader probably describe a double bond?a. an electron density that is twice as high as a single bondb. a higher electron density than a single bondc. four electrons shared between two atomsd. all of the abovee. none of the above

____ 54. What types of things does Dr. Robert J. LeRoy use computer simulations to study?a. behaviour of small molecules d. all of the aboveb. decomposition of small molecules e. none of the abovec. intermolecular forces

____ 55. Why are diamonds so hard?a. because they are made of carbonb. because they are made of a three dimensional array of particlesc. because it is able to conduct electricityd. because there are covalent bonds between particlese. none of the above

____ 56. What is the shape of hydrogen cyanide, HCN?a. linear d. octahedralb. trigonal planar e. trigonal pyramidc. tetrahedral

4____ 57. What is the shape of ammonium, NH 1+?

linear d. octahedrala.

b. trigonal planar e. trigonal pyramidalc. tetrahedral

3____ 58. What is the shape of the nitrate ion, NO 1-?

linear d. octahedrala.

b. trigonal planar e. trigonal pyramidalc. tetrahedral

6____ 59. What is the shape of sulfur hexahydride, SH ?a. linear d. octahedralb. trigonal planar e. trigonal pyramidalc. tetrahedral

____ 60. Which species would have the biggest attraction with a proton, H ?+

3a. sodium ion, Na d. nitrate ion, NO 1-+

b. neon, Ne e. fluoride ion, F1-

4c. methane, CH

____ 61. How will four pairs of electrons surrounding a central atom be arranged?a. pyramidally d. linearlyb. spherically e. trigonallyc. tetrahedrally

____ 62. Six pairs of electrons surrounding a central atom will be arrangeda. tetrahedrally d. octahedrallyb. spherically e. hexagonallyc. trigonal bipyramidally

____ 63. "A partial positive charge at one end of a molecule combined with a partial negative charge at the otherend of a molecule" describes...

a. an orbital d. a photonb. an absorption spectrum e. a dipolec. a quantum

____ 64. What is the bond angle in a bent molecule, such as water?a. 90°b. 104.5°c. 107.3°d. 109.5°e. 120°

____ 65. What is the bond angle in a trigonal pyramidal molecule?a. 90°b. 104.5°c. 107.3°d. 109.5°e. 120°

____ 66. What is the bond angle in a trigonal planar molecule?a. 90°b. 104.5°c. 107.3°d. 109.5°e. 120°

4____ 67. What is the shape of a molecule of carbon tetrachloride, CCl ?a. linearb. trigonal planarc. trigonal pyramidald. tetrahedrale. angular

3____ 68. What is the shape of a molecule of antimony(III) fluoride, SbF ?a. linearb. trigonal planarc. trigonal pyramidald. tetrahedrale. angular

4____ 69. What is the shape of a molecule of selenium tetrachloride, SeCl ?a. T-shapedb. seesawc. trigonal bipyramidald. square pyramidale. square planar

4____ 70. What is the shape of a molecule of krypton tetraiodide, KrI ?a. T-shapedb. seesawc. trigonal bipyramidald. square pyramidale. square planar

4____ 71. Predict the shape of a phosphate ion, PO 3-.a. seesawb. trigonal planarc. trigonal pyramidald. tetrahedrale. square planar

3____ 72. Predict the shape of OF +.

seesawa.

b. trigonal planarc. trigonal pyramidald. tetrahedrale. T-shaped

____ 73. Which compound has polar covalent bonds?

2a. AgCl

4b. CH

2c. Cl

4d. CF

2 8e. B H

____ 74. Which compound is truly covalent?

2a. SOb. MgO

3c. NH

3d. PCl

2 3e. P S

____ 75. Which molecule has a molecular dipole?

4a. CCl

3b. NF

2c. BeF

4d. CF

2e. CO

____ 76. Metals can be rolled into sheets and stamped into various forms. In contrast, diamond is very hard andbrittle. Which explanation for these different properties is correct?

a. Metals have semi-ionic bonds, whereas diamond has covalent bonds.b. The electrons that surround a metal atom are free to move through the metal. The bonding

electron pairs in a diamond are held tightly between two carbon atoms in an overalltetrahedral pattern.

c. The electrons of a metal are held more tightly to the parent atom than the electrons ofcarbon. Hence, the bonds in a metal are stronger than the bonds in diamond.

d. Diamond has strong double bonds between carbon atoms. Metal bonds are normally singlecovalent bonds, which bend easily.

e. Metals are made of metal atoms, whereas diamond is made of non-metal carbon atoms.

____ 77. Which bond is most polar?a. C¾Ob. C¾Nc. B¾Od. B¾Ne. S¾O

____ 78. Which compound is the best example of a molecular solid held together by London dispersion forces?a. KI

2b. Na O

2c. H O

2d. CO

3e. NH

____ 79. Which compound is a network solid?a. NaCl (table salt)

25 52b. C H (paraffin wax)

8c. S (sulfur)d. mixture of C and Fe (steel)

2e. SiO (quartz)

____ 80. A pure substance melts at 113°C and does not conduct electricity in either the solid or liquid state. Howwould you classify this substance?

a. ionic solidb. network solidc. molecular solidd. metallic solide. atomic solid

____ 81. A solid compound consists of ions bound in a crystal lattice. Which property would you not expect thissolid to have?

a. high melting pointb. good conductivity in the solid statec. hardd. soluble in a polar solvente. brittle

____ 82. A substance is a white powder, which melts at 660°C to give a transparent liquid. The substance does notconduct electricity in its solid state, but it does conduct electricity in its liquid state. How would youclassify the substance?

a. ionicb. networkc. moleculard. metallice. atomic

____ 83. A substance is a white solid, which melts at a temperature greater than 700°C. The substance isextremely hard and not workable. It is a poor conductor of heat and electricity in both its solid and liquidstates. How would you classify the substance?

a. ionicb. networkc. moleculard. metallice. atomic

____ 84. A substance is a silvery white solid, which melts at 675°C to give a silvery liquid. The substanceconducts electricity in both its solid and liquid states. How would you classify the substance?

a. ionicb. networkc. moleculard. metallice. atomic

____ 85. A substance has an extremely low boiling point of 4 K. It is a clear, colourless gas at room temperature,and it does not conduct electricity in its liquid or solid state. How would you classify this substance?

a. ionicb. networkc. moleculard. metallice. atomic