h8 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. n ionic bond is. a. attraction of an atom for its electrons. b. attraction of atoms for electrons they share. c. a force that holds together atoms that are oppositely charged. d. the movement of electrons from one atom to another. 2. The formula unit of an ionic compound shows the a. total number of each kind of ion in a sample. b. simplest ratio of the ions. c. numbers of atoms within each molecule. d. number of nearest neighboring ions surrounding each kind of ion. 3. The overall charge of a formula unit for an ionic compound. a. is always zero. c. is always positive. b. is always negative. d. may have any value. 4. How many chloride (l ) ions are present in a formula unit of magnesium chloride, given that the charge on a Mg ion is 2+? a. one-half c. two b. one d. four 5. Ionic bonds generally occur between. a. metals.. c. a metal and a nonmetal b. nonmetals. d. noble gases. 6. Salts are examples of. a. nonionic compounds. c. nonmetals. b. metals. d. ionic compounds. 7. three-dimensional arrangement of particles in an ionic solid is called a(n). a. crystal lattice. c. formula unit. b. sea of electrons. d. electrolyte. 8. In a crystal lattice of an ionic compound,. a. ions of a given charge are clustered together, far from ions of the opposite charge. b. ions are surrounded by ions of the opposite charge. c. a sea of electrons surrounds the ions. d. neutral molecules are present. 9. What is the relationship between lattice energy and the strength of the attractive force holding ions in place? a. The more positive the lattice energy is, the greater the force. b. The more negative the lattice energy is, the greater the force. c. The closer the lattice energy is to zero, the greater the force. d. There is no relationship between the two quantities. 10. The formation of a stable ionic compound from ions. a. is always exothermic. b. may be either exothermic or endothermic. c. is always endothermic. d. neither absorbs nor releases energy. 11. In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct?
a. The metallic atom gains electrons from the nonmetallic atom. b. The nonmetallic atom gains electrons from the metallic atom. c. oth atoms gain electrons. d. Neither atom gains electrons. 12. What is the electron configuration for the noble gases other than helium? a. ns 2 np 6 c. ns 2 np 3 b. ns 2 d. ns 2 np 2 13. How many outermost d electrons are there in an ion that has achieved a pseudo-noble gas configuration? a. none c. eight b. five d. ten 14. The anion that has the formula lo is called the. a. chloride ion. c. hypochlorite ion. b. chlorate ion. d. perchlorate ion. 15. Where does a subscript that indicates the number of atoms appear, relative to a chemical symbol in a formula? a. to the upper left c. to the upper right b. to the lower left d. to the lower right 16. What is the formula of calcium phosphate, which is made up of the ions a 2+ and PO 4 3? a. a 3 PO 4 c. a 3 (PO 4 ) 2 b. a 6 PO 4 d. a2(po 4 ) 3 17. Which of the following is an example of an interstitial alloy? a. brass c. carbon steel b. 14-carat gold d. sterling silver 18. The electron configuration of Na is [Ne]3s 1 and that of l is [Ne]3s 2 3p 5. What is the formula of the compound when these elements react? a. Na l c. Nal b. Nal d. Na l 19. formula unit of calcium bromide has two bromide ions corresponding to each calcium ion in the compound. What is the formula of calcium bromide? a. ar c. a r b. ar d. a r Matching 20. lo 2 21. lo 4 22. lo 23. l 24. lo 3 Match the terms below with their correct definitions. a. chlorate d. perchlorate b. hypochlorite e. chlorite c. chloride Match the terms below with their correct definitions. a. alloy j. ionic bond b. anion k. lattice energy c. cation l. metallic bond
d. chemical bond m. monatomic ion e. delocalized electrons n. oxidation number f. electrolyte o. oxyanion g. electron sea model p. polyatomic ion h. formula unit q. salts i. interstitial alloy 25. Electrons that are free to move in metals 26. For a monatomic ion, is equal to the charge 27. The force that holds two atoms together 28. charged particle containing more than one atom 29. positively charged ion 30. negatively charged ion 31. n ionic compound whose aqueous solution conducts electricity 32. The name for most ionic compounds other than oxides 33. Represents the way electrons exist in metals 34. charged particle containing only one atom 35. The energy needed to separate the ions of an ionic compound 36. The electrostatic force that holds oppositely charged particles together 37. mixture of elements that has metallic properties 38. mixture formed when small atoms fill holes in a metallic crystal 39. polyatomic ion composed of an element bonded to at least one oxygen atom 40. Shows the simplest ratio of ions in an ionic compound 41. The attraction of a metallic cation for delocalized electrons h9 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. In what form do elements such as hydrogen, nitrogen, and oxygen normally occur? a. as single atoms c. as molecules containing three atoms b. as molecules containing two atoms d. as molecules containing four atoms 2. How many electrons are shared in a double covalent bond? a. none c. two b. one d. four 3. ond length is the distance between. a. two molecules of the same substance. c. the nuclei of two attached atoms. b. the electrons in two attached atoms. d. the orbitals of two attached atoms. 4. Which of the following relationships relating to bond length is generally correct? a. the shorter the bond, the stronger the bond b. the shorter the bond, the weaker the bond c. the shorter the bond, the fewer the electrons in it d. the shorter the bond, the lower the bond dissociation energy 5. The VSEPR model is used mainly to. a. determine molecular shape.. c. determine ionic charge b. write resonance structures. d. measure intermolecular distances. 6. The bond angle is the angle between.
a. the sigma and pi bonds in a double bond. c. two terminal atoms and the central atom. b. the nucleus and the bonding electrons. d. the orbitals of a bonding atom. 7. The VSEPR model is based on the idea that. a. there is always an octet of electrons around an atom in a molecule. b. electrons are attracted to the nucleus. c. molecules repel one another. d. shared and unshared electron pairs repel each other as much as possible. 8. The shape of a molecule whose central atom has four pairs of bonding electrons is. a. tetrahedral. c. trigonal pyramidal. b. trigonal planar. d. linear. 9. The shape of a molecule that has two covalent single bonds and no lone pairs on the central atom is. a. tetrahedral. c. trigonal pyramidal. b. trigonal planar. d. linear. 10. The shape of a molecule that has three single covalent bonds and one lone pair on the central atom is. a. tetrahedral. c. trigonal pyramidal. b. trigonal planar. d. linear. 11. Unequal sharing of electrons between two bonded atoms always indicates. a. a nonpolar covalent bond. c. a polar covalent bond. b. an ionic bond. d. a polar molecule. 12. When electronegativities of two bonded atoms differ greatly, the bond is. a. polar covalent. c. polar covalent. b. coordinate covalent. d. ionic. 13. What is the electronegativity difference that usually is the dividing line between covalent and ionic bonds? a. 1.0 c. 2.7 b. 1.7 d. 4.0 14. The symbol is placed next to which of the following? a. the less electronegative atom in a polar covalent bond b. the more electronegative atom in a polar covalent bond c. a positive ion d. the nucleus 15. nonpolar covalent bond is one in which. a. electrons are transferred. b. electrons are shared unequally. c. electrons are shared equally. d. both electrons are provided by the same atom. 16. Molecules containing only polar covalent bonds. a. are always polar. c. are always ionic. b. may or may not be polar. d. are always nonpolar. 17. What factor other than electronegativity determines whether a molecule as a whole is polar or not? a. temperature c. its physical state b. its geometry d. its mass 18. Which of the following correctly describes the compound water, H 2 O? a. ionic b. nonpolar overall, with polar covalent bonds c. polar overall, with nonpolar covalent bonds d. polar overall, with polar covalent bonds 19. Which of the following correctly describes the compound carbon tetrachloride, l 4? a. ionic
b. nonpolar overall, with polar covalent bonds c. polar overall, with nonpolar covalent bonds d. polar overall, with polar covalent bonds 20. molecule of ammonia, NH 3, is. a. nonpolar because it is linear. b. polar because it is linear. c. nonpolar because there is no electronegativity difference. d. polar because there is an electronegativity difference and the molecule is trigonal pyramidal. 21. Which of the following compounds is an exception to the octet rule? a. H c. NH b. H d. H O 22. compound el uses sp hybrid orbitals of e atom. Which of the following is the correct bond angle in the compound? a. 104.5 c. 120 b. 109.5 d. 180 23. In the formation of a covalent bond, electrons are. a. shared. c. gained. b. lost. d. transferred. 24. Which of the following elements normally exists in the form of diatomic molecules? a. helium c. iron b. argon d. nitrogen 25. Four electrons are shared in a. a. single covalent bond. c. triple covalent bond. b. double covalent bond. d. quadruple covalent bond. 26. Which of the following molecules contains only sigma bonds? a. methane c. carbon dioxide b. oxygen d. nitrogen 27. Which of the following molecules contains a triple bond? a. methane c. carbon dioxide b. oxygen d. nitrogen 28. How many pi bonds are there in a triple bond? a. none c. two b. one d. three 29. Which of the following molecules would be expected to have the greatest bond dissociation energy? a. F 2 c. N 2 b. O 2 d. l 2 30. Fluorine belongs to group 7. How many covalent bonds are formed between two fluorine atoms? a. 1 c. 3 b. 2 d. 4 31. How many pi bonds are there in a triple covalent bond? a. 1 c. 3 b. 2 d. 4 32. The name of an oxyacid has the suffix -ic acid. What is the suffix of the oxyanion? a. ic c. ate b. ite d. ous 33. How many bond pairs of electrons exist in a molecule of ammonia? a. 1 c. 8
b. 4 d. 10 34. If the electronegativity of H is 2.20 and of l is 3.55, which type of bond is formed between H and l, when they form hydrogen chloride? a. Ionic c. ovalent b. Polar ionic d. Polar covalent Matching 35. O 36. O 2 37. H 2 O 3 38. NH 3 39. N 2 O 4 40. HNO 2 41. HNO 3 42. Hr 43. HrO 3 Match the terms below with their correct definitions. a. hydrobromic acid f. nitric acid b. dinitrogen tetroxide g. carbonic acid c. carbon monoxide h. bromic acid d. nitrous acid i. carbon dioxide e. ammonia Match the terms below with their correct definitions. a. O 3 c. NO b. F 3 d. SF 6 44. Odd number of valence electrons 45. Fewer than 8 electrons around an atom 46. More than 8 electrons around central atom 47. More than one valid Lewis structure Match the terms below with their correct definitions. a. structural formula h. sigma bond b. molecule i. polar covalent c. VSEPR model j. pi bond d. coordinate covalent bond k. covalent bond e. hybridization l. resonance f. oxyacid m. endothermic g. electronegativity n. exothermic 48. The tendency of an atom in a compound to attract electrons 49. kind of bond in which there is unequal sharing of electrons 50. ny bond in which there is electron sharing 51. The particle formed when two or more atoms bond covalently 52. Reactions that occur when more energy is released forming new bonds than is required to break bonds in the initial reactants
53. kind of bond in which electrons are shared in an area centered between the two atoms 54. kind of bond formed by overlap of parallel orbitals 55. ny acidic compound that contains oxygen 56. model that shows how the atoms are arranged in a molecule 57. Reactions that occur when more energy is required to break existing bonds in reactants than is released when new bonds form in the product molecules 58. condition that occurs when more than one valid Lewis structure can be drawn for a molecule 59. kind of bond in which one of the atoms provides both electrons for sharing 60. model used to determine molecular shape 61. The combining of orbitals in an atom to form new, identical orbitals
h8 Test nswer Section MULTIPLE HOIE 1. NS: PTS: 1 2. NS: PTS: 1 3. NS: PTS: 1 4. NS: PTS: 1 5. NS: PTS: 1 6. NS: PTS: 1 7. NS: PTS: 1 8. NS: PTS: 1 9. NS: PTS: 1 10. NS: PTS: 1 11. NS: PTS: 1 12. NS: PTS: 1 13. NS: PTS: 1 14. NS: PTS: 1 15. NS: PTS: 1 16. NS: PTS: 1 17. NS: PTS: 1 18. NS: To acquire a stable electron configuration, Na loses one electron, thereby forming Na. l gains the electron, making l. There is transfer of only one electron in the entire process. The metal loses only one electron from its outer orbital. The halogen gains only one electron in the process. orrect! The formula should state the simplest ratio of ions. PTS: 1 IF: 2 REF: Page 216 OJ: 8.2.1 escribe the formation of ionic bonds. NT:.1.4 TOP: escribe the formation of ionic bonds. KEY: Ionic bond MS: 2 19. NS: Two atoms of the halogen ion, each with one negative charge, will be required to balance the +2 charge on the metal ion. The charge on the metal ion is +2 and that on the halogen ion is -1. orrect! Two ions of the metal with +2 charge each result into 4 positive charges, while 2 halogen ions neutralize only two positive charges. There will be an overall charge on the species formed, because the charge on each metal ion is double that on each halogen ion.
PTS: 1 IF: 1 REF: Page 221 OJ: 8.3.1 Write formulas for ionic compounds and oxyanions. NT:.1 UP.1 TOP: Write formulas for ionic compounds and oxyanions. KEY: Formula unit MS: 2 MTHING 20. NS: E PTS: 1 21. NS: PTS: 1 22. NS: PTS: 1 23. NS: PTS: 1 24. NS: PTS: 1 25. NS: E PTS: 1 26. NS: N PTS: 1 27. NS: PTS: 1 28. NS: P PTS: 1 29. NS: PTS: 1 30. NS: PTS: 1 31. NS: F PTS: 1 32. NS: Q PTS: 1 33. NS: G PTS: 1 34. NS: M PTS: 1 35. NS: K PTS: 1 36. NS: J PTS: 1 37. NS: PTS: 1 38. NS: I PTS: 1 39. NS: O PTS: 1 40. NS: H PTS: 1 41. NS: L h9 Test nswer Section MULTIPLE HOIE 1. NS: PTS: 1 2. NS: PTS: 1 3. NS: PTS: 1 4. NS: PTS: 1 5. NS: PTS: 1 6. NS: PTS: 1 7. NS: PTS: 1 8. NS: PTS: 1 9. NS: PTS: 1 10. NS: PTS: 1
11. NS: PTS: 1 12. NS: PTS: 1 13. NS: PTS: 1 14. NS: PTS: 1 15. NS: PTS: 1 16. NS: PTS: 1 17. NS: PTS: 1 18. NS: PTS: 1 19. NS: PTS: 1 20. NS: PTS: 1 21. NS: The number of electrons around atom is less than eight. orrect! There are four covalent bonds formed by with H atoms, making the total number of electrons around to eight. There is a lone pair of electron in N, in addition to three bond pairs. There are two lone pairs of electrons around oxygen. PTS: 1 IF: 1 REF: Page 256 OJ: 9.3.3 Explain three exceptions to the octet rule, and identify molecules in which these exceptions occur. NT:.1.4 TOP: Explain three exceptions to the octet rule, and identify molecules in which these exceptions occur. KEY: Octet rule MS: 3 22. NS: There is maximum repulsion between two lone pairs when they are diametrically opposite to each other. The bond angle is 104.5, when the hybridization is sp3, and there are two lone pairs of electrons. The bond angle is 109.5, when there are no lone pairs of electrons in the sp3 hybridized central atom. The bond angle is 120 for the sp2 hybridized atom. orrect! PTS: 1 IF: 1 REF: Page 259 OJ: 9.4.2 Predict the shape of and the bond angles in a molecule. NT:.1.4 TOP: Predict the shape of and the bond angles in a molecule. KEY: Molecular shape MS: 1 23. NS: PTS: 1 24. NS: PTS: 1 25. NS: PTS: 1 26. NS: PTS: 1 27. NS: PTS: 1 28. NS: PTS: 1 29. NS: PTS: 1 30. NS:
Fluorine can acquire the configuration of a stable octet by sharing one electron with another fluorine atom, forming only one covalent bond. orrect! There are seven valence electrons in fluorine. Each fluorine atom requires one more electron to fulfill the octet. To form three covalent bonds with another fluorine atom, each atom needs three unpaired electrons. To form four covalent bonds with another fluorine atom, each atom needs four unpaired electrons which it does not have. PTS: 1 IF: 2 REF: Page 243 OJ: 9.1.2 escribe the formation of single, double, and triple covalent bonds. NT:.1 TOP: escribe the formation of single, double, and triple covalent bonds. KEY: ovalent bond MS: 2 31. NS: triple covalent bond has one sigma and two pi bonds. One pi bond and one sigma between two atoms results in a double bond. orrect! ll the three bonds in a triple covalent bond cannot be pi as there has to be one sigma bond. The total number of bonds is three in case of a triple bond. PTS: 1 IF: 2 REF: Page 245 OJ: 9.1.3 ompare and contrast sigma and pi bonds. NT:.1 TOP: ompare and contrast sigma and pi bonds. KEY: Sigma bond pi bond MS: 2 32. NS: ccording to the rules of the nomenclature, if the oxyanion has the suffix -ate, the oxyacid will have suffix -ic. ic is the suffix of oxyacid, not of oxyanion. When the suffix of oxyanion is -ite, the suffix of oxyacid will be -ous. orrect! -ous is the suffix given to oxyacid, not to oxyanion. PTS: 1 IF: 1 REF: Page 250 OJ: 9.2.2 Name acidic solutions. NT: UP.1 TOP: Name acidic solutions. KEY: Oxyanion Oxyacid MS: 1 33. NS: The total number of bond pairs is the number of bonding electrons divided by two. There is one lone pair of electrons on a nitrogen atom. orrect! The total number of bonding electrons is 8.
The total number of electrons in a molecule of ammonia is 10. PTS: 1 IF: 1 REF: Page 252 OJ: 9.3.1 List five basic steps used in drawing Lewis structures. NT:.1 TOP: List five basic steps used in drawing Lewis structures. KEY: Structural formula MS: 2 34. NS: Since the electronegativities between the two atoms are different, the atom with higher electronegativity will have a greater tendency to share the electrons. This results in a polar covalent bond. The bond formed between H and l is by sharing electron. In case of ionic bond, the electron is completely transferred from one atom to another. The difference in the electronegativities between the two atoms is such that l has a higher share of electrons. orrect! PTS: 1 IF: 1 REF: Page 263 OJ: 9.5.1 escribe how electronegativity is used to determine bond type. NT:.1.4 TOP: escribe how electronegativity is used to determine bond type. KEY: Electronegativity MS: 2 MTHING 35. NS: PTS: 1 36. NS: I PTS: 1 37. NS: G PTS: 1 38. NS: E PTS: 1 39. NS: PTS: 1 40. NS: PTS: 1 41. NS: F PTS: 1 42. NS: PTS: 1 43. NS: H PTS: 1 44. NS: PTS: 1 45. NS: PTS: 1 46. NS: PTS: 1 47. NS: PTS: 1 48. NS: G PTS: 1 49. NS: I PTS: 1 50. NS: K PTS: 1 51. NS: PTS: 1 52. NS: N PTS: 1 53. NS: H PTS: 1 54. NS: J PTS: 1 55. NS: F PTS: 1 56. NS: PTS: 1
57. NS: M PTS: 1 58. NS: L PTS: 1 59. NS: PTS: 1 60. NS: PTS: 1 61. NS: E PTS: 1