1. Review Problems Lecture
CHM1111 Section 04
Instructor: Dr. Jules Carlson
Wednesday, November 30th

2. Problem 2.24
Oxygen gas can be generated by heating KClO3 in the presence of a catalyst:
KClO3 (s)  KCl(s) + O2(g)
What volume of O2 gas will be generated at T = 25 °C and p = Torr from 1.57 g of KClO3?

3. Problem 2.24 Solution

4. Problem 5.16c
Write the complete electron configuration, and list a correct set of values of the quantum numbers for each of the valence electrons in the ground-state configurations of (a) Li, (b) C, (c) F, and (d) Mg.

5. Problem 5.60
Arrange the following in order of decreasing ionization energy: Br, Ar, Ar+, and Cl.

6. Problem 6.28
Determine the Lewis structure of (a) PBr5; (b) O2SCl2; (c) AsCl3; and (d) KrF4. Also, note geometric shapes, dipoles, orbital overlap, hybridization, bond angles.

7. Problem 6.29b
Determine the Lewis structure of each of the following polyatomic ions. Include all resonance structures and formal charges, where appropriate: (b) HSO4-

8. Problem 6.54
Arrange the following bonds in order of increasing bond length (shortest first). List the factors responsible for each placement
Cl-Cl Br-Br O-Cl P=O H-F

9. Problem 7.30 (a)
In each of the following pairs, which has the stronger bond? Use orbital configurations to justify your selections:
(a) O2 or O2+

10. Problem 8.14
Draw molecular pictures of Ne and Xe showing the relative amount of polarizability of each.

11. Problem 8.16
List n-propanol (CH3CH2CH2OH), dimethyl ether (CH3OCH3), and diethyl ether (CH3CH2OCH2CH3) in order of increasing boiling point and explain what features determine this order.

12. Problem 8.20b
Draw Lewis structures that show the hydrogen-bonding interactions for one HF molecule and one acetone molecule.
(CH3)2C = O

13. Problem 9.10
Aqueous ammonia at a concentration of 6.69 M has a density of g/mL. Calculate the mole fractions, mass fraction, and molality of this solution.

14. Problem 9.10 Solution

15. Problem 9.10 Solution

16. Problem 9.10 Solution

17. Problem 4.18
The binding energy of electrons to a chromium metal surface is 7.21 × 10−19 J. Calculate (a) the longest wavelength of light that will eject electrons from chromium metal; (b) the frequency required to give electrons with kinetic energy of 2.5 × 10−19 J; and (c) the wavelength of the light in part (b).

18. Problem 4.18 Solution

19. Problem 4.18 Solution

20. Ch 8-9 Review Problem
Which of the following are polar, somewhat polar or non-polar? What is the phase of each at STP? Identify the types of solids. Which liquids are miscible? Arrange the liquids in order of lowest to highest boiling point. Determine the relative freezing point depression of a 0.1 molal solution of each non-network solid. Kf = 1.86 C kg/mol
CCl4
CH2Cl2
Br2
NH4Cl
Ca3(PO4) 2
H2O
Brass
Graphite (Carbon)
SiO2

21. Problem 5.28
Arrange the following atoms in order of increasing size: Cl, F, P, and S.