Chapter 7 and chapter 8 Study Guide

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

____ 1. Which ion is this atom most likely to form?

a. Na+ c. Ne-

b. Na- d. Mg+

____ 2. Based on the periodic table shown, elements from columns A and C will combine in which ratio?a. 1 A: 3 C c. 3A:1Cb. 1A:1C d. These elements will not combine.

____ 3. Based on the periodic table shown, elements from columns B and F will combine in which ratio?a. 1B:2F c. 2B:3Fb. 1B:1F d. These elements will not combine.

____ 4. Based on the periodic table shown, elements from columns B and E will combine in which ratio?a. 2B:3E c. 3B:2Eb. 3B:1E d. These elements will not combine.

____ 5. In the equation for the formation of magnesium sulfide shown, which atom gains electrons?

a. A c. Cb. B d. D

____ 6. Which is the correct formula for the ionic compound that results from these two atoms?

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a. X2Y5 c. X2Y3

b. X5Y2 d. X3Y2

____ 7. Which is true of the model of bonding shown in this figure?

a. Metallic atoms are present in a “sea” of negatively charged atoms.b. Valence electrons are able to move easily among the metallic cations.c. It results in the substance being very brittle and not easily deformed.d. Heat and electricity are easily carried by the cations from one region to another.

____ 8. Which is described as the force holding two atoms together?a. cation c. formula unitb. chemical bond d. lattice

____ 9. Which is the charge that results when oxygen becomes an ion?a. +2 c. +3b. -3 d. -2

____ 10. Group 13 elements tend to acquire which charge when they form ions?a. +3 c. +5b. -5 d. -3

____ 11. Which is true of binary ionic compounds?a. They consist of only two atoms.b. They consist of atoms of only two elements.c. They contain two different anions.d. They have bonds that share two valence electrons.

____ 12. A compound has the formula X3Y. For every 15 X atoms present in this compound, how many Y atoms are there?a. 3 c. 45b. 5 d. 15

____ 13. How many total electrons must be transferred to form one formula unit of the compound Al2O3?a. 2 c. 6b. 3 d. 5

____ 14. Which is a physical property of ionic compounds in their solid state?a. good conductor of electricityb. weak attractive forces between ionsc. low boiling pointd. high melting point

____ 15. Which is the correct order of bond strength, from greatest to least, for the compounds MgCl2, MgO, and Mg3N2?a. MgO, MgCl2, Mg3N2 c. MgCl2, MgO, Mg3N2

b. Mg3N2, MgCl2, MgO d. Mg3N2, MgO, MgCl2

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____ 16. Which is a correct statement of bond strength?a. Compounds with smaller atoms have weaker bond strength.b. Compounds with a higher total number of atoms in the compound have greater bond

strength.c. Compounds containing atoms with greater charges have higher bond strength.d. Compounds with a more negative lattice energy have lower bond strength.

____ 17. Which is a property of substances that exhibit metallic bonding?a. high boiling points c. low melting pointsb. rigid and brittle d. poor conductors of electricity

____ 18. Which is the correct formula for the compound formed between beryllium and nitrogen?a. BeN c. Be3N2

b. Be3N d. Be2N3

____ 19. What is the correct formula for the compound formed between magnesium and the phosphate ion?a. MgPO4 c. Mg3(PO4)2

b. Mg3PO2 d. MgP2O8

____ 20. Which is the correct formula for the compound Manganese (III) Fluoride?a. MnF c. MnF3

b. Mn3F d. Mn3F3

____ 21. Which is the correct formula for the compound Chromium (II) Nitrate?a. (Cr)2NO3 c. CrNO2

b. Cr2NO3 d. Cr(NO3)2

____ 22. Which is the correct name for the compound FeS?a. Iron Sulfide c. Iron (II) Sulfideb. Iron (I) Sulfide d. Iron (II) Sulfide (II)

____ 23. Which is the correct name for the compound CaClO2?a. Calcium Chloride c. Calcium Chloriteb. Calcium Chloroxide d. Calcium Chlorate

____ 24. Which is the correct name for the compound Na3P?a. Sodium Phosphide c. Sodium Phosphateb. Sodium Phosphite d. Sodium (III) Phosphide

____ 25. Which is the correct name for the compound CoCO3?a. Carbon Oxygen Carbonate c. Cobalt Carbonateb. Cobalt (II) Carbonate d. Cobalt Carbonoxide

____ 26. Which is the correct name for the compound NH4SO4?a. Nitrogen Hydrogen Sulfate c. Ammonium (II) Sulfateb. Nitrogen Hydrosulfate d. Ammonium Sulfate

____ 27. How many valence electrons are in an atom of phosphorus?a. 2 c. 4b. 3 d. 5

____ 28. How many valence electrons are in an atom of magnesium?a. 2 c. 4b. 3 d. 5

____ 29. How many valence electrons does a helium atom have?a. 2 c. 4b. 3 d. 5

____ 30. How many valence electrons are in a silicon atom?a. 2 c. 6b. 4 d. 8

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____ 31. What is the name given to the electrons in the highest occupied energy level of an atom?a. orbital electrons c. anionsb. valence electrons d. cations

____ 32. How does calcium obey the octet rule when reacting to form compounds?a. It gains electrons.b. It gives up electrons.c. It does not change its number of electrons.d. Calcium does not obey the octet rule.

____ 33. What is the maximum charge an ion is likely to have?a. 2 c. 4b. 3 d. 5

____ 34. What is the electron configuration of the calcium ion?a. 1s 2s 2p 3s 3p c. 1s 2s 2p 3s 3p 4sb. 1s 2s 2p 3s 3p 4s d. 1s 2s 2p 3s

____ 35. What is the electron configuration of the gallium ion?a. 1s 2s 2p 3s 3p c. 1s 2s 2p 3s 3p 4s 4pb. 1s 2s 2p 3s 3p 4s d. 1s 2s 2p 3s 3p 3d

____ 36. What is the charge on the strontium ion?a. 2– c. 1b. 1– d. 2

____ 37. How many electrons does silver have to give up in order to achieve a pseudo-noble-gas electron configuration?a. 1 c. 3b. 2 d. 4

____ 38. How many electrons does barium have to give up to achieve a noble-gas electron configuration?a. 1 c. 3b. 2 d. 4

____ 39. What is the formula of the ion formed when potassium achieves noble-gas electron configuration?a. K c. Kb. K d. K

____ 40. Which of the following ions has a pseudo-noble-gas electron configuration?a. Fe c. Cub. Mn d. Ni

____ 41. Which of the following elements does NOT form an ion with a charge of 1 ?a. fluorine c. potassiumb. hydrogen d. sodium

____ 42. What is the formula of the ion formed when tin achieves a stable electron configuration?a. Sn c. Snb. Sn d. Sn

____ 43. What is the formula of the ion formed when cadmium achieves a pseudo-noble-gas electron configuration?a. Cd c. Cdb. Cd d. Cd

____ 44. Which of the following is a pseudo-noble-gas electron configuration?a. 1s 2s 2p 3s 3d c. 1s 2s 2p 3s 3p 3d

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b. 1s 2s 2p 3s 3p d. 1s 2s 2p 3s 3d 4s____ 45. How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?

a. 1 c. 3b. 2 d. 4

____ 46. What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?a. P c. Pb. P d. P

____ 47. How does oxygen obey the octet rule when reacting to form compounds?a. It gains electrons.b. It gives up electrons.c. It does not change its number of electrons.d. Oxygen does not obey the octet rule.

____ 48. What is the electron configuration of the oxide ion (O )?a. 1s 2s 2p c. 1s 2sb. 1s 2s 2p d. 1s 2s 2p

____ 49. What is the electron configuration of the iodide ion?a. 1s 2s 2p 3s 3p 3d 4s 4p 4d 5s 5pb. 1s 2s 2p 3s 3p 3d 4s 4p 4dc. 1s 2s 2p 3s 3p 3d 4s 4p 4d 5sd. 1s 2s 2p 3s 3p 3d 4s 4p

____ 50. What is the charge on the cation in the ionic compound sodium sulfide?a. 0 c. 2b. 1 d. 3

____ 51. Which of the following occurs in an ionic bond?a. Oppositely charged ions attract.b. Two atoms share two electrons.c. Two atoms share more than two electrons.d. Like-charged ions attract.

____ 52. What is the net charge of the ionic compound calcium fluoride?a. 2– c. 0b. 1– d. 1

____ 53. Which of the following is true about an ionic compound?a. It is a salt. c. It is composed of anions and cations.b. It is held together by ionic bonds. d. all of the above

____ 54. How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?a. 0 c. 2b. 1 d. 3

____ 55. How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide?a. 0 c. 2b. 1 d. 3

____ 56. What is the formula unit of sodium nitride?a. NaN c. Na N

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b. Na N d. NaN____ 57. What is the formula unit of aluminum oxide?

a. AlO c. AlOb. Al O d. Al O

____ 58. What is the name of the ionic compound formed from lithium and bromine?a. lithium bromine c. lithium bromiumb. lithium bromide d. lithium bromate

____ 59. What is the formula for sodium sulfate?a. NaSO c. Na(SO )b. Na SO d. Na (SO )

____ 60. What is the formula for potassium sulfide?a. KS c. KSb. K S d. K S

____ 61. Which of the following compounds has the formula KNO ?a. potassium nitrate c. potassium nitriteb. potassium nitride d. potassium nitrogen oxide

____ 62. Which of the following pairs of elements is most likely to form an ionic compound?a. magnesium and fluorine c. oxygen and chlorineb. nitrogen and sulfur d. sodium and aluminum

____ 63. Ionic compounds are normally in which physical state at room temperature?a. solid c. gasb. liquid d. plasma

____ 64. What does the term coordination number in ionic crystals refer to?a. the total number of valence electrons in an atomb. the number of oppositely charged ions surrounding a particular ionc. the number of atoms in a particular formula unitd. the number of like-charged ions surrounding a particular ion

____ 65. Under what conditions can potassium bromide conduct electricity?a. only when meltedb. only when dissolvedc. only when it is in crystal formd. only when melted or dissolved in water

____ 66. Which of the following is NOT a characteristic of most ionic compounds?a. They are solids.b. They have low melting points.c. When melted, they conduct an electric current.d. They are composed of metallic and nonmetallic elements.

____ 67. Which of the following particles are free to drift in metals?a. protons c. neutronsb. electrons d. cations

____ 68. What is the basis of a metallic bond?a. the attraction of metal ions to mobile electronsb. the attraction between neutral metal atomsc. the neutralization of protons by electronsd. the attraction of oppositely charged ions

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____ 69. What characteristic of metals makes them good electrical conductors?a. They have mobile valence electrons.b. They have mobile protons.c. They have mobile cations.d. Their crystal structures can be rearranged easily.

____ 70. Which metallic crystal structure has a coordination number of 8?a. body-centered cubic c. hexagonal close-packingb. face-centered cubic d. tetragonal

____ 71. How many single covalent bonds are elements in Column F likely to form?

a. 1 c. 3b. 2 d. 4

____ 72. Which combination of bonds is present in this molecule?

O = O

a. 1 sigma bond only c. 2 pi bondsb. 1 sigma bond and 1 pi bond d. 1 sigma bond and 2 pi bonds

____ 73. Which is true of the bond length of these covalent molecules?a. The bonds in A are longer than the bonds in B or Cb. The bonds in C are the same length as the bonds in Bc. The bonds in B are longer than the bonds in A or Cd. The relative bond length of these compounds cannot be determined

____ 74. Which covalent molecule has the strongest bond?a. A c. Cb. B d. They are all equally strong

____ 75. Which exception to the octet rule is shown by this molecule?

a. uneven number of valence electronsb. suboctet

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c. expanded octetd. coordinate covalent bond

____ 76. Which exception to the octet rule is shown by this molecule?

a. uneven number of valence electrons c. expanded octetb. suboctet d. coordinate covalent bond

____ 77. Which type of molecular shape is shown by this molecule?

a. trigonal pyramidal c. bentb. tetrahedral d. trigonal planar

____ 78. Which type of molecular shape is shown by this molecule?

a. trigonal pyramidal c. trigonal bipyramidalb. tetrahedral d. octahedral

____ 79. Which is NOT a diatomic molecule?a. Fluorine c. Bromineb. Nitrogen d. Boron

____ 80. Which type of bond has one pair of electrons shared between atoms?a. single covalent c. double covalentb. coordinate covalent d. metallic

____ 81. How many single covalent bonds can carbon form?a. 1 c. 3b. 2 d. 4

____ 82. How many single covalent bonds can halogens form?a. 1 c. 3b. 2 d. 4

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____ 83. Multiple covalent bonds consist of which of these?a. 1 sigma bond only c. three pi bonds onlyb. 1 or 2 sigma bonds and a pi bond d. 1 sigma bond and 1 pi bond

____ 84. In the compound PCl3, how many total valence electrons are present?a. 4 c. 24b. 8 d. 26

____ 85. How many valence electrons are available in the ion NO3-?

a. 16 c. 22b. 9 d. 24

____ 86. Which type of bond has an electronegativity difference greater than 1.7?a. ionic c. nonpolar covalentb. metallic d. polar covalent

Element Electronegativity Element ElectronegativityCarbon 2.55 Nitrogen 3.04Oxygen 3.44 Phosphorous 2.19Sulfur 2.58 Aluminum 1.61Fluorine 3.98 Chlorine 3.16

____ 87. What is the electronegativity difference in the compound Aluminum Chloride, AlCl3?a. 4.77 c. 7.87b. 3.16 d. 1.55

____ 88. Based on its electronegativity difference, which kind of bond is present in the compound OF2?a. ionic c. polar covalentb. metallic d. nonpolar covalent

____ 89. Covalent compounds display which of these properties?a. They are hard, brittle solidsb. They have high melting and boiling pointsc. They display luster.d. Their intermolecular forces are relatively weak.

____ 90. How many pairs of bonding electrons are in a molecule that displays sp2 hybridization?a. 2 c. 4b. 3 d. 5

____ 91. How many pairs of bonding electrons are present in a molecule that displays trigonal bipyramidal molecular shape?a. 3 c. 5b. 4 d. 6

____ 92. What molecular shape does the compound CCl4 have?a. trigonal planar c. octahedralb. tetrahedral d. bent

____ 93. Which is the correct name for the compound N2O3?a. dinitro trioxide c. trinitrogen dioxideb. nitrogen (II) oxide (III) d. dinitrogen trioxide

____ 94. Which is the correct name for the compound PCl5?a. monophosphorus tetrachloride c. phosphorus pentachlorideb. phosphorus chloride d. pentaphosphorus chloride

____ 95. Which is the correct name for the compound N2O4?a. tetranitrogen dioxide c. dinitrogen quadoxide

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b. dinitrogen tetroxide d. nitrogen oxide____ 96. Which is the correct formula for the compound dinitrogen monoxide?

a. NO2 c. N2O1

b. (NO)2 d. N2O____ 97. Which is the formula for the compound sulfur hexachloride?

a. S6Cl c. SCl5

b. SCl6 d. S2Cl3

____ 98. Which is the correct name for the compound HClO3?a. hydrogen chlorate c. hydrogen chloride trioxideb. chloric acid d. hydrochloric acid

____ 99. Which is the correct name for the compound HNO2?a. hyponitrous acid c. nitrous acidb. hydronitrogen dioxide d. hydronitric acid

____ 100. Which is the correct formula for the compound phosphoric acid?a. H3P c. H3PO4

b. HPO3 d. H3PO3

____ 101. Identify the correct structure of NO .a. c.

b. d.

____ 102. Which of the following compounds is an exception to the octet rule?a. BH c. NHb. CH d. H O

____ 103. A compound BeCl uses sp hybrid orbitals of Be atom. Which of the following is the correct bond angle in the compound?a. 104.5° c. 120°b. 109.5° d. 180°

____ 104. Which is a typical characteristic of an ionic compound?a. Electron pairs are shared among atoms.b. The ionic compound has a low solubility in water.c. The ionic compound is described as a molecule.d. The ionic compound has a high melting point.

____ 105. What is shown by the structural formula of a molecule or polyatomic ion?a. the arrangement of bonded atoms c. the number of metallic bondsb. the number of ionic bonds d. the shapes of molecular orbitals

____ 106. Which of these elements does not exist as a diatomic molecule?a. Ne c. H

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b. F d. I____ 107. How do atoms achieve noble-gas electron configurations in single covalent bonds?

a. One atom completely loses two electrons to the other atom in the bond.b. Two atoms share two pairs of electrons.c. Two atoms share two electrons.d. Two atoms share one electron.

____ 108. Why do atoms share electrons in covalent bonds?a. to become ions and attract each otherb. to attain a noble-gas electron configurationc. to become more polard. to increase their atomic numbers

____ 109. Which of the following elements can form diatomic molecules held together by triple covalent bonds?a. carbon c. fluorineb. oxygen d. nitrogen

____ 110. Which noble gas has the same electron configuration as the oxygen in a water molecule?a. helium c. argonb. neon d. xenon

____ 111. Which elements can form diatomic molecules joined by a single covalent bond?a. hydrogen onlyb. halogens onlyc. halogens and members of the oxygen group onlyd. hydrogen and the halogens only

____ 112. Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?a. unvalenced pair c. inner pairb. outer pair d. unshared pair

____ 113. Which of the following electron configurations gives the correct arrangement of the four valence electrons of the carbon atom in the molecule methane (CH )?a. 2s 2p c. 2s 2p 3sb. 2s 2p 3s d. 2s 2p

____ 114. Which of the following diatomic molecules is joined by a double covalent bond?a. c.b. d.

____ 115. A molecule with a single covalent bond is ____.a. CO c. COb. Cl d. N

____ 116. Once formed, how are coordinate covalent bonds different from other covalent bonds?a. They are stronger. c. They are weaker.b. They are more ionic in character. d. There is no difference.

____ 117. When H forms a bond with H O to form the hydronium ion H O , this bond is called a coordinate covalent bond because ____.a. both bonding electrons come from the oxygen atomb. it forms an especially strong bondc. the electrons are equally sharedd. the oxygen no longer has eight valence electrons

____ 118. Which of the following bonds is the least reactive?

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a. C—C c. O—Hb. H—H d. H—Cl

____ 119. How many valid electron dot formulas—having the same number of electron pairs for a molecule or ion—can be written when a resonance structure occurs?a. 0 c. 2 onlyb. 1 only d. 2 or more

____ 120. In which of the following compounds is the octet expanded to include 12 electrons?a. H S c. PClb. PCl d. SF

____ 121. How many electrons can occupy a single molecular orbital?a. 0 c. 2b. 1 d. 4

____ 122. Molecular orbital theory is based upon which of the following models of the atom?a. classical mechanical model c. quantum mechanical modelb. Bohr model d. Democritus’s model

____ 123. How is a pair of molecular orbitals formed?a. by the splitting of a single atomic orbitalb. by the reproduction of a single atomic orbitalc. by the overlap of two atomic orbitals from the same atomd. by the overlap of two atomic orbitals from different atoms

____ 124. The side-by-side overlap of p orbitals produces what kind of bond?a. alpha bond c. pi bondb. beta bond d. sigma bond

____ 125. Where are the electrons most probably located in a molecular bonding orbital?a. anywhere in the orbitalb. between the two atomic nucleic. in stationary positions between the two atomic nucleid. in circular orbits around each nucleus

____ 126. Sigma bonds are formed as a result of the overlapping of which type(s) of atomic orbital(s)?a. s only c. d onlyb. p only d. s and p

____ 127. Which of the following bond types is normally the weakest?a. sigma bond formed by the overlap of two s orbitalsb. sigma bond formed by the overlap of two p orbitalsc. sigma bond formed by the overlap of one s and one p orbitald. pi bond formed by the overlap of two p orbitals

____ 128. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?a. pairs of valence electrons c. mobile electronsb. inner shell electrons d. the electrons closest to the nuclei

____ 129. What causes water molecules to have a bent shape, according to VSEPR theory?a. repulsive forces between unshared pairs of electronsb. interaction between the fixed orbitals of the unshared pairs of oxygenc. ionic attraction and repulsiond. the unusual location of the free electrons

____ 130. Which of the following theories provides information concerning both molecular shape and molecular bonding?a. molecular orbital theory c. orbital hybridization theory

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b. VSEPR theory d. Bohr atomic theory

____ 131. Experimental evidence suggests that the H—C—H bond angles in ethene, C H , are ____.a. 90 c. 120b. 109.5 d. 180

____ 132. What type of hybrid orbital exists in the methane molecule?a. sp c. spb. sp d. sp d

____ 133. What is the shape of a molecule with a triple bond?a. tetrahedral c. bentb. pyramidal d. linear

____ 134. What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom?a. c.b. d.

____ 135. How many pi bonds are formed when sp hybridization occurs in ethene, C H ?a. 0 c. 2b. 1 d. 3

____ 136. Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen?a. C c. Ob. Na d. S

____ 137. Which of the following covalent bonds is the most polar?a. H—F c. H—Hb. H—C d. H—N

____ 138. What is thought to cause the dispersion forces?a. attraction between ions c. sharing of electron pairsb. motion of electrons d. differences in electronegativity

____ 139. Which of the forces of molecular attraction is the weakest?a. dipole interaction c. hydrogen bondb. dispersion d. single covalent bond

____ 140. What causes dipole interactions?a. sharing of electron pairsb. attraction between polar moleculesc. bonding of a covalently bonded hydrogen to an unshared electron paird. attraction between ions

____ 141. What are the weakest attractions between molecules?a. ionic forces c. covalent forcesb. Van der Waals forces d. hydrogen forces

____ 142. What causes hydrogen bonding?a. attraction between ionsb. motion of electronsc. sharing of electron pairsd. bonding of a covalently bonded hydrogen atom with an unshared electron pair

____ 143. Why is hydrogen bonding only possible with hydrogen?a. Hydrogen’s nucleus is electron deficient when it bonds with an electronegative atom.b. Hydrogen is the only atom that is the same size as an oxygen atom.c. Hydrogen is the most electronegative element.

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d. Hydrogen tends to form covalent bonds.____ 144. Which type of solid has the highest melting point?

a. ionic solid c. metalb. network solid d. nonmetallic solid

____ 145. What is required in order to melt a network solid?a. breaking Van der Waals bonds c. breaking hydrogen bondsb. breaking ionic bonds d. breaking covalent bonds

____ 146. What type of ions have names ending in -ide?a. only cations c. only metal ionsb. only anions d. only gaseous ions

____ 147. When Group 2A elements form ions, they ____.a. lose two protons c. lose two electronsb. gain two protons d. gain two electrons

____ 148. What is the correct name for the N ion?a. nitrate ion c. nitride ionb. nitrogen ion d. nitrite ion

____ 149. When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.a. prefix c. Roman numeral following the nameb. suffix d. superscript after the name

____ 150. Aluminum is a group 3A metal. Which ion does A1 typically form?a. Al c. Alb. Al d. Al

____ 151. In which of the following are the symbol and name for the ion given correctly?a. Fe : ferrous ion; Fe : ferric ionb. Sn : stannic ion; Sn : stannous ionc. Co : cobalt(II) ion; Co : cobaltous iond. Pb : lead ion; Pb : lead(IV) ion

____ 152. Which of the following correctly provides the name of the element, the symbol for the ion, and the name of the ion?a. fluorine, F , fluoride ion c. copper, Cu , cuprous ionb. zinc, Zn , zincate ion d. sulfur, S , sulfurous ion

____ 153. The nonmetals in Groups 6A and 7A ____.a. lose electrons when they form ionsb. have a numerical charge that is found by subtracting 8 from the group numberc. all have ions with a –1 charged. end in -ate

____ 154. What determines that an element is a metal?a. the magnitude of its charge c. when it is a Group A elementb. the molecules that it forms d. its position in the periodic table

____ 155. What is the Stock name for chromic ion?a. chromium(I) ion c. chromium(III) ionb. chromium(II) ion d. chromium(IV) ion

____ 156. Which of the following is NOT a cation?a. iron(III) ion c. Ca

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b. sulfate d. mercurous ion____ 157. In which of the following are the symbol and name for the ion given correctly?

a. NH : ammonia; H : hydride c. OH : hydroxide; O : oxideb. C H O : acetate; C O : oxalite d. PO : phosphate; PO : phosphite

____ 158. Which of the following correctly provides the names and formulas of polyatomic ions?a. carbonate: HCO ; bicarbonate: COb. nitrite: NO ; nitrate: NOc. sulfite: S ; sulfate: SOd. chromate: CrO ; dichromate: Cr O

____ 159. An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.a. fewer electrons than protons c. only two elementsb. neutral molecules d. a polyatomic anion

____ 160. Why are systematic names preferred over common names?a. Common names do not provide information about the chemical composition of the

compound.b. Common names are derived from the method used to obtain the compound.c. Common names were assigned by the scientist who discovered the compound.d. Common names are not very descriptive.

____ 161. Which of the following compounds contains the Mn ion?a. MnS c. Mn Ob. MnBr d. MnO

____ 162. How are chemical formulas of binary ionic compounds generally written?a. cation on left, anion on rightb. anion on left, cation on rightc. Roman numeral first, then anion, then cationd. subscripts first, then ions

____ 163. Which of the following is true about the composition of ionic compounds?a. They are composed of anions and cations.b. They are composed of anions only.c. They are composed of cations only.d. They are formed from two or more nonmetallic elements.

____ 164. Which of the following formulas represents an ionic compound?a. CS c. N Ob. BaI d. PCl

____ 165. Which element, when combined with fluorine, would most likely form an ionic compound?a. lithium c. phosphorusb. carbon d. chlorine

____ 166. Which of the following shows correctly an ion pair and the ionic compound the two ions form?a. Sn , N ; Sn N c. Cr , I ; CrIb. Cu , O ; Cu O d. Fe , O ; Fe O

____ 167. In which of the following are the formula of the ionic compound and the charge on the metal ion shown correctly?a. UCl , U c. IrS , Ir

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b. ThO , Th d. NiO, Ni____ 168. Which of the following correctly represents an ion pair and the ionic compound the ions form?

a. Ca , F ; CaF c. Ba , O ; Ba Ob. Na , Cl ; NaCl d. Pb , O ; Pb O

____ 169. In which of the following is the name and formula given correctly?a. sodium oxide, NaO c. cobaltous chloride, CoClb. barium nitride, BaN d. stannic fluoride, SnF

____ 170. Which of the following compounds contains the lead(II) ion?a. PbO c. Pb2Ob. PbCl4 d. Pb2S

____ 171. Which set of chemical name and chemical formula for the same compound is correct?a. iron(II) oxide, Fe O c. tin(IV) bromide, SnBrb. aluminum fluorate, AlF d. potassium chloride, K Cl

____ 172. What is the correct formula for potassium sulfite?a. KHSO c. K SOb. KHSO d. K SO

____ 173. Which set of chemical name and chemical formula for the same compound is correct?a. ammonium sulfite, (NH ) S c. lithium carbonate, LiCOb. iron(III) phosphate, FePO d. magnesium dichromate, MgCrO

____ 174. What type of compound is CuSO ?a. monotomic ionic c. polyatomic ionicb. polyatomic covalent d. binary molecular

____ 175. Which polyatomic ion forms a neutral compound when combined with a group 1A monatomic ion in a 1:1 ratio?a. ammonium c. nitrateb. carbonate d. phosphate

____ 176. Sulfur hexafluoride is an example of a ____.a. monatomic ion c. binary compoundb. polyatomic ion d. polyatomic compound

____ 177. Molecular compounds are usually ____.a. composed of two or more transition elementsb. composed of positive and negative ionsc. composed of two or more nonmetallic elementsd. exceptions to the law of definite proportions

____ 178. What is the ending for the names of all binary compounds, both ionic and molecular?a. -ide c. -adeb. -ite d. -ate

____ 179. Which of the following correctly shows a prefix used in naming binary molecular compounds with its corresponding number?a. deca-, 7 c. hexa-, 8b. nona-, 9 d. octa-, 4

____ 180. Which of the following is a binary molecular compound?a. BeHCO c. AgI

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b. PCl d. MgS

____ 181. Which of the following formulas represents a molecular compound?a. ZnO c. SOb. Xe d. BeF

____ 182. Consider a mystery compound having the formula M T . If the compound is not an acid, if it contains only two elements, and if M is not a metal, which of the following is true about the compound?a. It contains a polyatomic ion. c. Its name ends in -ic.b. Its name ends in -ite or -ate. d. It is a binary molecular compound.

____ 183. Which of the following shows both the correct formula and correct name of an acid?a. HClO , chloric acid c. H PO , phosphoric acidb. HNO , hydronitrous acid d. HI, iodic acid

____ 184. What is the name of H SO ?a. hyposulfuric acid c. sulfuric acidb. hydrosulfuric acid d. sulfurous acid

____ 185. What is the formula for sulfurous acid?a. H SO c. H SOb. H SO d. H S

____ 186. What is the formula for phosphoric acid?a. H PO c. HPOb. H PO d. HPO

____ 187. What is the formula for hydrosulfuric acid?a. H S c. HSOb. H SO d. H S

____ 188. Which of the following are produced when a base is dissolved in water?a. hydronium ions c. hydrogen ionsb. hydroxide ions d. ammonium ions

____ 189. How are bases named?a. like monatomic elements c. like ionic compoundsb. like polyatomic ions d. like molecular compounds

____ 190. Which of the following pairs of substances best illustrates the law of multiple proportions?a. H and O c. CaCl and CaBrb. P O and PH d. NO and NO

____ 191. Select the correct formula for sulfur hexafluoride.a. S F c. F Sb. F SO d. SF

____ 192. What is the correct name for the compound CoCl ?a. cobalt(I) chlorate c. cobalt(II) chlorateb. cobalt(I) chloride d. cobalt(II) chloride

____ 193. Suppose you encounter a chemical formula with H as the cation. What do you know about this compound immediately?a. It is a polyatomic ionic compound. c. It is a base.

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b. It is an acid. d. It has a 1 charge.____ 194. What is the correct formula for barium chlorate?

a. Ba(ClO) c. Ba(ClO )b. Ba(ClO ) d. BaCl

____ 195. What is the correct formula for calcium dihydrogen phosphate?a. CaH PO c. Ca(H PO )b. Ca H PO d. Ca(H HPO )

____ 196. What does an -ite or -ate ending in a polyatomic ion mean?a. Oxygen is in the formula. c. Nitrogen is in the formula.b. Sulfur is in the formula. d. Bromine is in the formula.

____ 197. Which of the following is the correct name for N O ?a. nitrous oxide c. nitrogen dioxideb. dinitrogen pentoxide d. nitrate oxide

____ 198. What is the correct name for Sn (PO ) ?a. tritin diphosphate c. tin(III) phosphateb. tin(II) phosphate d. tin(IV) phosphate

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