1. 216 mL

2. 30.1 ppm

3. (a) diamagnetic; (b) BO = 3

4. s-MOs:

  p-MOs:

5.  -57 kJ/mol

6.  CF₂Cl₂    CF₂Cl + Cl DH = + 339 kJ

 CF₂Cl₂  CFCl₂ + F  DH = + 485 kJ

7.  CF₂Cl₂    CF₂Cl + Cl DH = + 339 kJ

 8.

9.

H₂O₂    C_2h
O₃       C_2v
HO₂^-    Cs
H₂O    C_2v
O₂^-2    Dooh
H₃O+    C_3v

10.  B₂

11.  doublet

12. Use DE = hc/l to get 650 nm

13.

(a) 1.67 g CH₄ at 100% efficiency
(b) 11.14 g needed at 15% efficiency
(c) 17.0 L CH₄

14.
(a)

15.

(a) SO₂ sulfur dioxide
(b) O₃ ozone
(c) CaSO₄ calcium sulfate
(d) MgCO₃ magnesium carbonate
(e) KO₂ potassium superoxide
(f) Na₂O₂ sodium peroxide
(g) Li₂O lithium oxide
(h) BaO₂ barium peroxide
(i) H₂O₂ hydrogen peroxide
(j) Al₂O₃ aluminum oxide

16.  (b) the bond energies between oxygen and 1st or 2nd row elements are larger (more stable) than bond energies between oxygen and the other elements, even though they have similar electronegativities

17.
(a) MgO has larger coulombic attraction (+2 and -2) between ions compared to NaF which has +1 and -1.
(b) should be intermediate in strength

18.  S-O bond energies are greater than those for O-O; SO₂ has an additional resonance form, O=S=O, unavailable to O₃ because the central atom has 10 e.  This latter rez form also has FC = 0 on all three atoms.

19.  (a) first one must convert to mole fraction:  210,000 ppm O₂
 

X_O2 = 0.21 and X_O3 = 10/1 x 10⁶ = 1 x 10^-5

P_O2 = X_O2 x Ptot and P_O3 = X_O3 x Ptot

K_p = P_O2³/P_O3² = (X_O2 x Ptot)³/(X_O3 x Ptot)²

K_p = (X_O2)³/(X_O3)² x Ptot

K_p = 0.213/(1 x 10^-5)² x P_tot

K_p = 9 X 107 X P_tot

20.  DH = -200 kJ