Unit 3 Review. Chapter 5 and 6
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1 Unit 3 Review Chapter 5 and 6
2 Which of the following electron configurations belong to an element that is the most chemically reactive? 1. 1s s 2 2s 2 2p s 2 2s 2 2p s 2 2s 2 2p 6 3s 2 3p 6
3 Which of the following electron configurations belong to an element that is the most chemically reactive? 1. 1s s 2 2s 2 2p s 2 2s 2 2p s 2 2s 2 2p 6 3s 2 3p 6
4 An octet is equal to
5 An octet is equal to
6 Which of the following situations will cause the element with the electron configuration 1s 2 2s 2 2p 5 to have an octet configuration? 1. Loss of one electron 2. Gain of one electron 3. Loss of two electrons 4. Gain of three electrons
7 Which of the following situations will cause the element with the electron configuration 1s 2 2s 2 2p 5 to have an octet configuration? 1. Loss of one electron 2. Gain of one electron 3. Loss of two electrons 4. Gain of three electrons
8 The elements of Group _ are able to satisfy the octet rule without forming compounds
9 The elements of Group _ are able to satisfy the octet rule without forming compounds
10 Stable ions of which of the following elements do NOT have octets of valence electrons? 1. F 2. Na 3. Cl 4. Be
11 Stable ions of which of the following elements do NOT have octets of valence electrons? 1. F 2. Na 3. Cl 4. Be
12 An element with the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 will ionize to a(n) 1. anion 2. cation 3. noble gas 4. Both a and b
13 An element with the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 will 1. anion 2. cation 3. noble gas 4. Both a and b ionize to a(n)
14 An ion and its parent atom differ in 1. electron configuration. 2. number of electrons. 3. chemical reactivity. 4. All of the above.
15 An ion and its parent atom differ in 1. electron configuration. 2. number of electrons. 3. chemical reactivity. 4. All of the above.
16 The electrostatic attraction between _ forms an ionic bond. 1. Dipoles 2. Electrons 3. Ions 4. nuclei
17 The electrostatic attraction between _ forms an ionic bond. 1. Dipoles 2. Electrons 3. Ions 4. nuclei
18 Which of the following reactions is NOT a step in the formation of sodium chloride? 1. Na (solid) Na (gas) 2. Cl (gas) + e- Cl- (gas) 3. Na + (gas) + e- Na (gas) 4. Cl 2 (gas) Cl (gas) + Cl (gas)
19 Which of the following reactions is NOT a step in the formation of sodium chloride? 1. Na (solid) Na (gas) 2. Cl (gas) + e- Cl- (gas) 3. Na + (gas) + e- Na (gas) 4. Cl 2 (gas) Cl (gas) + Cl (gas)
20 Which of the following reactions in the formation of sodium chloride is exothermic? 1. Cl (gas) + e- Cl-(gas) 2. Na+ (gas) + Cl- (gas) NaCl (solid) 3. Both (a) and (b) 4. Neither (a) nor (b)
21 Which of the following reactions in the formation of sodium chloride is exothermic? 1. Cl (gas) + e- Cl-(gas) 2. Na+ (gas) + Cl- (gas) NaCl (solid) 3. Both (a) and (b) 4. Neither (a) nor (b)
22 The salts NaCl (solid) and CaCl 2 (solid) 1. Are good conductors of electricity. 2. Are positively charged. 3. Are held together by ionic bonds. 4. Both a and b
23 The salts NaCl (solid) and CaCl 2 (solid) 1. Are good conductors of electricity. 2. Are positively charged. 3. Are held together by ionic bonds. 4. Both a and b
24 Compared with solid ionic compounds, solid molecular compounds 1. Have lower melting points. 2. Are more brittle. 3. Are harder. 4. Conduct electricity as liquids.
25 Compared with solid ionic compounds, solid molecular compounds 1. Have lower melting points. 2. Are more brittle. 3. Are harder. 4. Conduct electricity as liquids.
26 Because strong attractive forces hold the layers in a salt in relatively fixed 1. Are hard. positions, ionic compounds 2. Are brittle. 3. Fracture along cleavage planes. 4. All of the above.
27 Because strong attractive forces hold the layers in a salt in relatively fixed 1. Are hard. 2. Are brittle. positions, ionic compounds 3. Fracture along cleavage planes. 4. All of the above.
28 Differences in which of the following factors might account for a difference in the crystal structures of two different ionic compounds. 1. Cation-ion ratio 2. Sizes of the cations and anions 3. Charges of the cations and anions 4. All of the above
29 Differences in which of the following factors might account for a difference in the crystal structures of two different ionic compounds. 1. Cation-ion ratio 2. Sizes of the cations and anions 3. Charges of the cations and anions 4. All of the above
30 Compounds that have the same number of positive and negative charges are said to be 1. Cationic 2. Anionic 3. Electrically neutral 4. Isoelectronic
31 Compounds that have the same number of positive and negative charges are said to be 1. Cationic 2. Anionic 3. Electrically neutral 4. Isoelectronic
32 An ion of bromine with a single negative charge has the symbol and the name 1. Br +, bromide ion 2. Br -, bromide ion 3. Br +, bromium ion 4. Br -, bromium ion
33 An ion of bromine with a single negative charge has the symbol and the name 1. Br +, bromide ion 2. Br -, bromide ion 3. Br +, bromium ion 4. Br -, bromium ion
34 What is the metallic ion in the compound copper (II) chloride? 1. Cl2-2. Cl - 3. Cu + 4. Cu 2+
35 1. Cl2-2. Cl - 3. Cu + 4. Cu 2+ What is the metallic ion in the compound copper (II) chloride?
36 What is the name of the compound formed by zinc ions, Zn 2+, and fluoride 1. Zinc difluoride 2. Zinc fluorate 3. Zinc fluoride 4. Zinc (II) fluroite ions, F -?
37 What is the name of the compound formed by zinc ions, Zn 2+, and fluoride 1. Zinc difluoride 2. Zinc fluorate 3. Zinc fluoride 4. Zinc (II) fluroite ions, F -?
38 What is the chemical formula of the compound formed by zinc ions,, Zn 2+, 1. ZnF 2. ZnF 2 3. Zn 2 F 4. Zn 2 F 3 and fluoride ions, F -?
39 What is the chemical formula of the compound formed by zinc ions,, Zn 2+, 1. ZnF 2. ZnF 2 3. Zn 2 F 4. Zn 2 F 3 and fluoride ions, F -?
40 What is the chemical formula of the compound formed by tin (IV) ions and 1. SnCl 2 2. Sn 2 Cl 2 3. SnCl 4 4. Sn 4 Cl chloride ions?
41 What is the chemical formula of the compound formed by tin (IV) ions and 1. SnCl 2 2. Sn 2 Cl 2 3. SnCl 4 4. Sn 4 Cl chloride ions?
42 Sodium hydrogen carbonate, NaHCO 3 1. Contains four different ions 2. Contains a polyatomic cation 3. Is not a salt 4. Contains only a monatomic cation and a polyatomic anion
43 Sodium hydrogen carbonate, NaHCO 3 1. Contains four different ions 2. Contains a polyatomic cation 3. Is not a salt 4. Contains only a monatomic cation and a polyatomic anion
44 What is the formula for the compound formed by aluminum, Al 3+, and the sulfate ion, SO 4 2-? 1. AlSO 4 2. Al 3 SO 4 3. Al 2 (SO 4 ) 3 4. Al(SO 4 ) 3
45 What is the formula for the compound formed by aluminum, Al 3+, and the sulfate ion, SO 4 2-? 1. AlSO 4 2. Al 3 SO 4 3. Al 2 (SO 4 ) 3 4. Al(SO 4 ) 3
46 Which statement is true about a molecule of H 2? 1. Each atom has an electron configuration like that of helium. 2. It is less stable than either of the hydrogen atoms by itself. 3. The electron from both atoms are shared. 4. Both (a) and (c )
47 Which statement is true about a molecule of H 2? 1. Each atom has an electron configuration like that of helium. 2. It is less stable than either of the hydrogen atoms by itself. 3. The electron from both atoms are shared. 4. Both (a) and (c )
48 A single covalent bond involves the 1. Only one electron 2. Two electrons 3. Three electrons 4. A variable number of electrons, which depends on the bonding atoms. sharing of
49 A single covalent bond involves the 1. Only one electron 2. Two electrons 3. Three electrons 4. A variable number of electrons, which depends on the bonding atoms. sharing of
50 The electrons involved in the formation of a covalent bond are 1. Transferred from one atom to another 2. Found only in the s-orbitals 3. Valence electrons 4. In filled orbitals
51 The electrons involved in the formation of a covalent bond are 1. Transferred from one atom to another 2. Found only in the s- orbitals 3. Valence electrons 4. In filled orbitals
52 Nonpolar covalent bonds are not common because 1. One atom usually attracts electrons more strongly that the other. 2. Ions always form when atoms join. 3. The electrons usually remain equally distant from both atoms. 4. Dipoles are rare in
53 Nonpolar covalent bonds are not common because 1. One atom usually attracts electrons more strongly that the other. 2. Ions always form when atoms join. 3. The electrons usually remain equally distant from both atoms. 4. Dipoles are rare in nature.
54 Which of the following substances has the lowest boiling point? 1. CuF 2. H 2 O 3. CO 4. NaCl
55 Which of the following substances has the lowest boiling point? 1. CuF 2. H 2 O 3. CO 4. NaCl
56 To draw a Lewis structure, it is NOT necessary to know 1. The length of the bonds. 2. The types of atoms in the molecule. 3. The number of valence electrons for each atom. 4. The number of atoms in each molecule.
57 To draw a Lewis structure, it is NOT 1. The length of the bonds. necessary to know 2. The types of atoms in the molecule. 3. The number of valence electrons for each atom. 4. The number of atoms in each molecule.
58 The Lewis structure that represents atom in Group 16 of the periodic tale has 1. One pair of valence electrons and three single valence electrons 2. Two pairs of valence electrons and two single valence electrons 3. Three pairs of valence electrons and 1 single valence electron. 4. Four pairs of valence electrons.
59 The Lewis structure that represents atom in Group 16 of the periodic tale has 1. One pair of valence electrons and three single valence electrons 2. Two pairs of valence electrons and two single valence electrons 3. Three pairs of valence electrons and 1 single valence electron. 4. Four pairs of valence electrons.
60 Which of the following atoms should be placed at the center of the Lewis structure of the compound ClF 2 HC? 1. Cl 2. F 3. H 4. C
61 Which of the following atoms should be placed at the center of the Lewis structure of the compound ClF 2 HC? 1. Cl 2. F 3. H 4. C
62 The stubstance whose Lewis structure shows 3 sinlge covalent bonds is 1. H 2 O 2. CH 2 Cl 2 3. NH 3 4. CCl 4
63 The stubstance whose Lewis structure shows 3 sinlge covalent bonds is 1. H 2 O 2. CH 2 Cl 2 3. NH 3 4. CCl 4
64 In a double covalent bond 1. One atom has more than eight valence electrons. 2. One atom loses a pair of electrons. 3. Two atoms share eight valence electrons. 4. Two atoms share two pairs of electrons.
65 In a double covalent bond 1. One atom has more than eight valence electrons. 2. One atom loses a pair of electrons. 3. Two atoms share eight valence electrons. 4. Two atoms share two pairs of electrons.
66 How many double bonds are in the Lewis structure for hydrogen fluoride, 1. None 2. One 3. Two 4. three HF?
67 How many double bonds are in the Lewis structure for hydrogen fluoride, 1. None 2. One 3. Two 4. three HF?
68 To draw the Lewis structure of the polyatomic ion, NO 3 - you would have to those in the structures of N,O,O, and O. 1. Add one electron to 2. Subtract one electron from 3. Add a proton to 4. Subtract a proton from
69 To draw the Lewis structure of the polyatomic ion, NO 3 - you would have to those in the structures of N,O,O, and O. 1. Add one electron to 2. Subtract one electron from 3. Add a proton to 4. Subtract a proton from
70 Which compound s name includes the numerical prefixes di- and tri-? 1. Pb(NO 3 ) CO SO 3 4. N 2 O 3
71 Which compound s name includes the numerical prefixes di- and tri-? 1. Pb(NO 3 ) CO SO 3 4. N 2 O 3
72 VSEPR theory 1. Predicts the shape of some molecules 2. Is limited to polar molecules 3. Assumes that pairs of valence electrons surrounding an atom repel each other. 4. Both (a) and ( c )
73 VSEPR theory 1. Predicts the shape of some molecules 2. Is limited to polar molecules 3. Assumes that pairs of valence electrons surrounding an atom repel each other. 4. Both (a) and ( c )
74 According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of AB2? 1. Linear 2. Bent 3. Trigonal pyramidal 4. Both (a) and (b)
75 According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of AB2? 1. Linear 2. Bent 3. Trigonal pyramidal 4. Both (a) and (b)
76 The shape of molecules that contain only two atoms is 1. Linear. 2. Bent. 3. Trigonal planar. 4. Both (a) and (b)
77 The shape of molecules that contain only two atoms is 1. Linear. 2. Bent. 3. Trigonal planar. 4. Both (a) and (b)
78 VSEPR applied to the unshared pairs of electrons around the central atoms of which compound would suggest that 1. CO 2 2. H 2 O 3. CS 2 4. HF the molecule has a bent shape?
79 VSEPR applied to the unshared pairs of electrons around the central atoms of which compound would suggest that 1. CO 2 2. H 2 O 3. CS 2 4. HF the molecule has a bent shape?
80 VSEPR theory predicts that the shape of carbon tetrachloride, CCl 4, is 1. Linear. 2. Bent. 3. Trigonal planar. 4. Tetrahedral.
81 VSEPR theory predicts that the shape of carbon tetrachloride, CCl 4, is 1. Linear. 2. Bent. 3. Trigonal planar. 4. Tetrahedral.
82 VSEPR theory predicts that the shape of which of the following compounds is not trigonal pyramidal. 1. PBr 3 2. NCl 3 3. BF 3 4. NH 3
83 VSEPR theory predicts that the shape of which of the following compounds is not trigonal pyramidal. 1. PBr 3 2. NCl 3 3. BF 3 4. NH 3
84 Which of the following molecules is 1. C 2 H 2 2. H 2 O 3. BF 3 4. CO 2 polar?
85 Which of the following molecules is 1. C 2 H 2 2. H 2 O 3. BF 3 4. CO 2 polar?
86 Which of the following molecules is 1. NF 3 2. H 2 O 3. C 2 H 4 4. H 3 P nonpolar?
87 Which of the following molecules is 1. NF 3 2. H 2 O 3. C 2 H 4 4. H 3 P nonpolar?
88 The structure of which of the following compounds suggests that it has the highest boiling point? 1. BF 3 2. CO 2 3. H 2 O 4. O 2
89 The structure of which of the following compounds suggests that it has the 1. BF 3 2. CO 2 3. H 2 O 4. O 2 highest boiling point?
90 The structure of which of the following compounds suggests that it has the 1. CO 2. CO 2 3. H 2 S 4. O 2 highest boiling point?
91 The structure of which of the following compounds suggests that it has the 1. CO 2. CO 2 3. H 2 S 4. O 2 highest boiling point?
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