Final Review - Part 2 Ch 6: Thermochemistry | Ch 7: The Quantum Mechanical Model of the Atom

Ch 8: Periodic Properties of the Elements| Ch 9: Chemical Bonding: Lewis Theory

Ch 10: Molecular Geometry and Bonding| Ch 5: Gases

DisclaimerThis is a student made review, it reflects what I believe will be on the final but you should not rely solely on this review.

20. Calculate ∆ H rxn for the reaction:

CaO (s) + CO2 (g) → CaCO3 (s)

Use the following ∆ H ’s.

Ca (s) + CO2 (g) + 1/2O2 (g) → CaCO3 (s) ∆ H=−812.8 kJ

1Ca (s) + 2O2 (g) → 2CaO (s) ∆ H=−12 69.8kJ

21. 12.0 moles of gas are in a 5.00 L tank a 24ᵒC. Calculate the difference in pressure using the van der Waals equation and ideal gas law under these conditions. The van der Waals constants for this gas are:

a= 2.300 L2 atm/ mol2 b= 0.0430 L/mol

22. Which of the following transitions results in absorption of the of the highest-

energy photon?

a. n=6 → n=2

b. n=2 → n=5

c. n=4 → n=3

d. n=3 → n=4

e. n=5 → n=6

22. A system releases 622 kJ of heat and does 105 kJ of work on the surroundings. What is the change in internal energy of the system?

23. Determine the shortest frequency of light that is required to remove an

electron from a sample of metal if the binding energy of the sample of metal is

4.08 x 104 kJ/mol.

24. A gas occupies 11.2 liters under a pressure of 0.860 atm. What pressure will the gas be under if the volume decrease to 9000. mL?

25. Which of the following statements is/are true?

I. When forming cations, electrons closer to the nucleus are easier to remove

II. The effective nuclear charge (Zeff) for O is -2III. Valence electrons are the easiest to removeIV. The electrons closest to the nucleus shield those further

from the nucleusV. When the effective nuclear charge increases, atomic radius

decreases

26. Which of the following molecules is nonpolar (does not have a net dipole moment)?

f. HF b. CBr4 c. H2S d. NCl3 e. CHCl3

27. How many grams of water would be produced if 20.0 liters of oxygen were burned at a temperature of -10.0ᵒC and a pressure of 1.3 atm?

2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g)

28. Use the chemical equation from #67. If you burned one gallon of gas (C8H18) (approximately 4000. grams), how many liters of carbon dioxide would be produced at a temperature of 21.0ᵒC and a pressure of 1.00 atm?

29. Arrange the following gases at 300K in order of decreasing rate of effusion:

F2 SF6 CO Kr

30. Draw the correct Lewis structure for the following and determine the mg and eg for each around each central atom:

a. IF5

b. XeCl4

31. Which of the following symbols describing an orbital is incorrect and why?

b. 6s1

c. 4f8

d. 4p8

e. 2p5

f. 2d3

32. Which of the following statements is/are false?

g. As wavelength increases, energy decreases

h. As frequency increases, energy decreases

i. The product of wavelength and frequency is a constant

j. As the amplitude of a wave increases, the intensity of light decreases

k. Emission of light results from a transition from lower n to higher n

33.Arrange the following ions in order of decreasing radius:Br - Na + Rb +

34. Which of the following has the highest first ionization energy?

K, Sr, Fr, Co, Nb