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Dr. Sean Clapham
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2. Which of the following ionic solids would have the largest

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2. Which of the following ionic solids would have the largest lattice energy?

a. SrO
b. NaF
c. CaBr2
d. CsI
e. BaSO4
3. Which of the following ionic solids would have the largest lattice energy?

a. KF
b. KI
c. LiF
d. LiI
e. NaF

4.Which of the elements listed below has the greatest electronegativity?

a. Na
b. As
c. Ga
d. Cs
e. Sb

5.The number of lone electron pairs in the NO2– ion is ___.

a. 4
b. 5
c. 6
d. 7
e. 8

6. The total number of bonding electrons in a molecule of formaldehyde (H2CO) is

a. 3
b. 4
c. 6
d. 8
e. 18

7.Assuming the octet rule is obeyed, how many covalent bonds will a nitrogen atom form to give a formal charge of zero?

a. 0
b. 1
c. 2
d. 3
e. 4

8.Which of the following is a useful guideline for the application of formal charges in neutral molecules?

a. A Lewis structure in which there are no formal charges is preferred.
b. Lewis structures with large formal charges (e.g., +2,+3 and/or -2,-3) are preferred.
c. The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.

9.Which of the following substances will display an incomplete octet in its Lewis structure?

a. CO2
b. Cl2
c. ICl
d. NO
e. SO2
10.Which one of the following molecules has an atom with an incomplete octet?

a. NF3
b. H2O
c. AsCl3
d. GeH4
e. BF3
11. Which one of the following molecules has an atom with an expanded octet?

a. HCl
b. AsCl5

c. ICl
d. NCl3
e. Cl2
12.Give the number of lone pairs around the central atom and the molecular geometry of IF5.

a. 0 lone pairs, square pyramidal
b. 0 lone pairs, trigonal bipyramidal
c. 1 lone pair, octahedral
d. 1 lone pair, square pyramidal
e. 2 lone pairs, pentagonal

13.Consider the species N2–, N2, and N2+. Which of these species will be paramagnetic?

a. N2 and N2–
b. N2+ and N2
c. N2+ and N2–
d. only N2–
e. none are paramagnetic

14.Which of the following is not true of molecular orbitals?

a. The number of molecular orbitals formed is always equal to the number of atomic orbitals combined.
b. A molecular orbital can accommodate up to two electrons.
c. When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule.
d. Low-energy molecular orbitals fill before high-energy molecular orbitals fill.
e. For any substance, the number of electrons in molecular orbitals is equal to the sum of all the valence electrons on the bonding atoms.

15. Which of the following correctly lists species in order of increasing bond length?

a. C2– < C2 < C2+
b. C2 < C2+ < C2–
c. C2– < C2+ < C2
d. C2+ < C2 < C2–
e. C2+ < C2– < C2

16. Which of the following correctly lists species in order of increasing bond order?

a. C2 < Li2 < Be2 < N2
b. Be2 < Li2 < C2 < N2
c. N2 < Be2 < Li2 < C2
d. N2 < C2 < Li2 < Be2
e. Be2 < C2 < N2 < Li2
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