1. Unit 6 Review

2.  How many valence electrons does sulfur have? a.1 b.2 c.6 d.16 Question 1

3.  How many valence electrons does sulfur have? a.1 b.2 c.6 d.16 Question 1

4.  How many fluorine atoms can form covalent bonds with one silicon atom? a.1 b.2 c.3 d.4 Question 2

5.  How many fluorine atoms can form covalent bonds with one silicon atom? a.1 b.2 c.3 d.4 Question 2

6.  Why do atoms share electrons in covalent bonds? a.To become ions and attract each other b.To attain a noble-gas electron configuration c.To become more polar d.To increase their atomic numbers Question 3

7.  Why do atoms share electrons in covalent bonds? a.To become ions and attract each other b.To attain a noble-gas electron configuration c.To become more polar d.To increase their atomic numbers Question 3

8.  Covalent molecular compounds are usually _____________. a.Composed of two or more transition metals b.Composed of positive and negative ions c.Composed of two or more nonmetals d.Exceptions to the law of conservation of mass Question 4

9.  Covalent molecular compounds are usually _____________. a.Composed of two or more transition metals b.Composed of positive and negative ions c.Composed of two or more nonmetals d.Exceptions to the law of conservation of mass Question 4

10.  What is the name for N 2 H 4 ? a.Dinitrogen tetrahydride b.Nitrogen hydride c.Mononitrogen dihydride d.Pentahydride dinitride Question 5

11.  What is the name for N 2 H 4 ? a.Dinitrogen tetrahydride b.Nitrogen hydride c.Mononitrogen dihydride d.Pentahydride dinitride Question 5

12.  How many valence electrons does chlorine have? a.1 b.2 c.7 d.8 Question 6

13.  How many valence electrons does chlorine have? a.1 b.2 c.7 d.8 Question 6

14.  How many pairs of electrons must two nitrogen atoms share in order for each atom to have eight valence electrons? a.Zero b.One c.Two d.Three Question 7

15.  How many pairs of electrons must two nitrogen atoms share in order for each atom to have eight valence electrons? a.Zero b.One c.Two d. Three Question 7

16.  Which of the following molecules contain polar covalent bonds? a.Phosphorus, P 4 b.Ozone, O 3 c.Oxygen, O 2 d.Hydrogen Fluoride, HF Question 8

17.  Which of the following molecules contain polar covalent bonds? a.Phosphorus, P 4 b.Ozone, O 3 c.Oxygen, O 2 d.Hydrogen Fluoride, HF Question 8

18.  Which of the following molecules contain nonpolar covalent bonds? a.Cl 2 b.CCl 4 c.SiBr 4 d.H 2 O Question 9

19.  Which of the following molecules contain nonpolar covalent bonds? a.Cl 2 b.CCl 4 c.SiBr 4 d.H 2 O Question 9

20.  What is the formula for diphosphorous pentoxide? a.P 2 O 5 b.P 5 O 2 c.P 3 O 2 d.P 2 O 3 Question 10

21.  What is the formula for diphosphorous pentoxide? a.P 2 O 5 b.P 5 O 2 c.P 3 O 2 d.P 2 O 3 Question 10

22.   Which type of covalent bond is found in Carbon Monoxide? a.Single bond b.Double bond c.Triple bond d.Not enough information Question 11

23.   Which type of covalent bond is found in Carbon Monoxide? a.Single bond b.Double bond c.Triple bond d.Not enough information Question 11

24.  How many electrons are being shared in carbon monoxide? a.1 b.2 c.3 d.6 Question 12

25.  How many electrons are being shared in carbon monoxide? a.1 b.2 c.3 d.6 Question 12

26.  What is a property of covalent molecules? a.Low melting point b.Only exists as a solid at room temperature c.Malleability d.Brittle (easy to break) Question 13

27.  What is a property of covalent molecules? a.Low melting point b.Only exists as a solid at room temperature c.Malleability d.Brittle (easy to break) Question 13

28.  Which of the following correctly shows a prefix used in naming molecular compounds with its corresponding number? a. hexa-, 8 b. octa-, 4 c. deca-, 7 d. nona-, 9 Question 14

29.  Which of the following correctly shows a prefix used in naming molecular compounds with its corresponding number? a. hexa-, 8 b. octa-, 4 c. deca-, 7 d. nona-, 9 Question 14

30.  Which of the following formulas represents a covalent molecular compound? a.ZnO b.Xe c.SO d.BeF Question 15

31.  Which of the following formulas represents a covalent molecular compound? a.ZnO b.Xe c. SO d.BeF Question 15

32.  What is the molecular formula for the following structure? a.OH b.HO 2 c.H 2 O d.HO Question 16

33.  What is the molecular formula for the following structure? a.OH b.HO 2 c.H 2 O d.HO Question 16

34.  What is the formula for sulfur hexachloride? a.SCl 6 b.S 6 Cl c.SCl 2 d.S 2 Cl Question 17

35.  What is the formula for sulfur hexachloride? a.SCl 6 b.S 6 Cl c.SCl 2 d.S 2 Cl Question 17

36.  When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial ________________ charge. a.Positive b.Negative c.Neutral d.Not enough information Question 18

37.  When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial ________________ charge. a.Positive b.Negative c.Neutral d.Not enough information Question 18

38.  Polarity is determined by ___________________. a.Atomic Number b.Atomic Radius c.Electronegativity d.Atomic Mass Question 19

39.  Polarity is determined by ___________________. a.Atomic Number b.Atomic Radius c. Electronegativity d.Atomic Mass Question 19

40.  What is the name of NO? a.Nitrogen oxide b.Mononitrogen oxide c.Mononitrogen monoxide d.Nitrogen monoxide Question 20

41.  What is the name of NO? a.Nitrogen oxide b.Mononitrogen oxide c.Mononitrogen monoxide d.Nitrogen monoxide Question 20

42.  What do the two dots between the “N” and “H” represent? a.Bonded pairs of electrons b.Lone pairs of electron c.Ionic bonds d.Not enough information Question 21

43.  What do the two dots between the “N” and “H” represent? a.Bonded pairs of electrons b.Lone pairs of electron c.Ionic bonds d.Not enough information Question 21

44.  What is the formula for tetraphosphorus hexoxide? a.P 6 O 4 b.P 5 O 7 c.P 4 O 6 d.P 3 O 7 Question 22

45.  What is the formula for tetraphosphorus hexoxide? a.P 6 O 4 b.P 5 O 7 c.P 4 O 6 d.P 3 O 7 Question 22

46.  What is the electronegativity of an atom? a.Ability to attract electrons b.Ability to attract neutrons c.Ability to repel electrons d.Ability to attract protons Question 23

47.  What is the electronegativity of an atom? a.Ability to attract electrons b.Ability to attract neutrons c.Ability to repel electrons d.Ability to attract protons Question 23

48.  What element on the periodic table has the highest electronegativity? a.Francium b.Oxygen c.Bromine d.Fluorine Question 24

49.  What element on the periodic table has the highest electronegativity? a.Francium b.Oxygen c.Bromine d.Fluorine Question 24

50.  Which is more polar: a carbon-oxygen bond or a carbon-nitrogen bond? a.Carbon-oxygen bond because it has a lower electronegativity difference. b.Carbon-nitrogen bond because it has a lower electronegativity difference. c.Carbon-oxygen bond because it has a higher electronegativity difference. d.Carbon-nitrogen bond because it has a higher electronegativity difference. Question 25

51.  Which is more polar: a carbon-oxygen bond or a carbon-nitrogen bond? a.Carbon-oxygen bond because it has a lower electronegativity difference. b.Carbon-nitrogen bond because it has a lower electronegativity difference. c.Carbon-oxygen bond because it has a higher electronegativity difference. d.Carbon-nitrogen bond because it has a higher electronegativity difference. Question 25

52.  What is the name of S 2 O 3 ? a.Sulfur trioxide b.Disulfur trioxide c.Sulfur oxide d.Trisulfur dioxide Question 26

53.  What is the name of S 2 O 3 ? a.Sulfur trioxide b.Disulfur trioxide c.Sulfur oxide d.Trisulfur dioxide Question 26

54.  Which atom carries the negative partial charge (- δ ) in Br-F? a.Bromine b.Fluorine c.They are equal d.Not enough information Question 27

55.  Which atom carries the negative partial charge (- δ ) in Br-F? a.Bromine b.Fluorine c.They are equal d.Not enough information Question 27

56.  Which pair of elements listed below is likely to form a covalent bond? a.Lithium and oxygen b.Sodium and copper c.Calcium and neon d.Sulfur and chlorine Question 28

57.  Which pair of elements listed below is likely to form a covalent bond? a.Lithium and oxygen b.Sodium and copper c.Calcium and neon d.Sulfur and chlorine Question 28

58.  What is the name for the H 2 O? a.Dihydrogen monoxide b.Hydrogen dioxide c.Hydrogen oxide d.Dihydrogen oxide Question 29

59.  What is the name for the H 2 O? a.Dihydrogen monoxide b.Hydrogen dioxide c.Hydrogen oxide d.Dihydrogen oxide Question 29

60.  What is the name of IF 7 ? a.Heptaiodine fluoride b.Heptaiodine monofluoride c.Iodine heptafluoride d.Monoiodine heptafluoride Question 30

61.  What is the name of IF 7 ? a.Heptaiodine fluoride b.Heptaiodine monofluoride c.Iodine heptafluoride d.Monoiodine heptafluoride Question 30

62.  How many hydrogen atoms does it take for the carbon atom to form a stable octet? a.1 b.2 c.3 d.4 Question 31

63.  How many hydrogen atoms does it take for the carbon atom to form a stable octet? a.1 b.2 c.3 d.4 Question 31

64.  The bonds between carbon and oxygen atoms shown in the figure below would be best classified as: a.Nonpolar covalent bonds b.Polar covalent bonds c.Ionic bonds d.Metallic bonds Question 32

65.  The bonds between carbon and oxygen atoms shown in the figure below would be best classified as: a.Nonpolar covalent bonds b.Polar covalent bonds c.Ionic bonds d.Metallic bonds Question 32

66.  For the diatomic molecule Cl 2, how many electrons does each chlorine atom contribute to the sharing? a.1 b.2 c.3 d.4 Question 33

67.  For the diatomic molecule Cl 2, how many electrons does each chlorine atom contribute to the sharing? a.1 b.2 c.3 d.4 Question 33

68.  What is the formula for carbon monoxide? a.CO b.CO 2 c.C 2 O d.C 2 O 4 Question 34

69.  What is the formula for carbon monoxide? a.CO b.CO 2 c.C 2 O d.C 2 O 4 Question 34

70.  How many total electrons are shared between two oxygen atoms in a covalent double bond? a.2 b.4 c.6 d.8 Question 35

71.  How many total electrons are shared between two oxygen atoms in a covalent double bond? a.2 b.4 c.6 d.8 Question 35

72.  Nitrogen and oxygen can form a covalent compound. In this example, electrons are: a.Lost b.Gained c.Shared d.Unchanged Question 36

73.  Nitrogen and oxygen can form a covalent compound. In this example, electrons are: a.Lost b.Gained c.Shared d.Unchanged Question 36

74.  What does this symbol represent? a.Dipole b.Electronegativity c.Nonpolar bond d.Transfer of electrons Question 37

75.  What does this symbol represent? a.Dipole b.Electronegativity c.Nonpolar bond d.Transfer of electrons Question 37

76.  How many double bonds are in the molecule SiO 2 ? a.0 b.1 c.2 d.3 Question 38

77.  How many double bonds are in the molecule SiO 2 ? a.0 b.1 c.2 d.3 Question 38

78.  Water has a higher boiling point than carbon dioxide because attractions between polar molecules are _________________ than attractions between nonpolar molecules. a.Weaker b.Stronger c.The same d.Not enough information Question 39

79.  Water has a higher boiling point than carbon dioxide because attractions between polar molecules are _________________ than attractions between nonpolar molecules. a.Weaker b.Stronger c.The same d.Not enough information Question 39

80.  Which atom carries the positive partial charge (+ δ ) in H-Cl? a.Hydrogen b.Chlorine c.They are equal d.Not enough information Question 40

81.  Which atom carries the positive partial charge (+ δ ) in H-Cl? a.Hydrogen b.Chlorine c.They are equal d.Not enough information Question 40

82.  Which of the following is an example of an intramolecular force? a.Covalent bonding b.Ionic bonding c.Hydrogen bonding d.Both a & b Question 41

83.  Which of the following is an example of an intramolecular force? a.Covalent bonding b.Ionic bonding c.Hydrogen bonding d.Both a & b Question 41

84.  What is a polar covalent bond? a.A covalent bond where the protons are shared equally. b.A covalent bond where the protons are shared unequally. c.A covalent bond where the electrons are shared equally. d.A covalent bond where the electrons are shared unequally. Question 42

85.  What is a polar covalent bond? a.A covalent bond where the protons are shared equally. b.A covalent bond where the protons are shared unequally. c.A covalent bond where the electrons are shared equally. d.A covalent bond where the electrons are shared unequally. Question 42

86.  Which of the following is not an example of a diatomic molecule? a.Hydrogen b.Sulfur c.Oxygen d.Bromine Question 43

87.  Which of the following is not an example of a diatomic molecule? a.Hydrogen b.Sulfur c.Oxygen d.Bromine Question 43

88.  What is the name given to the pairs of valence electrons not involved in bonding? a.Lone pair b.Shared pair c.Bonded pair d.Paired electrons Question 44

89.  What is the name given to the pairs of valence electrons not involved in bonding? a.Lone pair b.Shared pair c.Bonded pair d.Paired electrons Question 44

90.  What forces are between 2 different molecules? a.Intramolecular forces b.Dipole forces c.Intermolecular forces d.Bonding forces Question 45

91.  What forces are between 2 different molecules? a.Intramolecular forces b.Dipole forces c.Intermolecular forces d.Bonding forces Question 45