MID-TERM EXAMINATION II
1. Which of the following is an example of a precipitation reaction?
A. 2 C6H6(l) + 15 O2(g) = 12 CO2(g) + 6 H2O(l) B. H3PO4 + 3 NaOH = Na3PO4 + 3 H2O C. H2O(l) = H2O(g) D. Ag+(aq) + Cl-(aq) = AgCl(s)
2. Consider the following reaction
SnCl2(s) + Cl2(g) = SnCl4(l) delta H = -1861 J
A. This is a neutralization reaction. B. "delta H" is the specific heat of the reaction. C. The reaction is endothermic. D. The reaction is exothermic.
3. The net ionic equation for
Al(NO3)3(aq) + NaOH(aq) = Al(OH)3(s) + NaNO3(aq)
is:
A. Al3+(aq) + 3 OH-(aq) = Al(OH)3(s) B. Al(NO3)3(aq) + 3 NaOH(aq) = Al(OH)3(s) + 3 NaNO3(aq) C. NO3-(aq) + 3 OH-(g) = Al3+(aq) + 3 Na+(aq) D. 3 NO3-(aq) + 3 Na+(aq) = 3 NaNO3(aq)
4. How many grams of solute is required to make 150.0 mL of a 0.100 M solution of potassium chloride?
A. 1.12 g B. 1.12 kg C. 0.0150 g D. 1.65 g
5. Sodium tripolyphosphate, Na5P3O10, was a common ingredient in laundry detergents. How many moles of sodium ions are there in 0.30 L of 0.10 M Na5P3O10?
A. 0.030 mol B. 0.10 mol C. 0.15 mol D. 0.30 mol
6. Concentrated hydrochloric acid from a chemical supply company is about 12 M in concentration. How many milliliters of this would be needed to make 1.0 L of a solution that is 0.20 M in HCl?
A. 2.4 mL B. 17 mL C. 60 mL D. 200 mL
7. According to the following equation,
2 CO(g) + O2(g) = 2 CO2(g) delta H = -566 kJ
what is delta H for the combustion of 14.0 g CO(g) in excess oxygen?
A. -142 kJ B. -283 kJ C. -566 kJ D. -1132 kJ
8. It requires 37.51 mL of a hydrochloric acid solution to completely neutralize 0.3150 g of pure sodium carbonate, Na2CO3. Calculate the concentration of the hydrochloric acid.
A. 0.07923 M B. 0.1182 M C. 0.1585 M D. 0.125 M
9. When 440 J of heat is added to 253 g of mercury, the temperature increases from 25 C to 37.5 C. Compute the specific heat and the molar heat capacity of mercury.
A. 0.139 J/g K, 27.9 J/mol K B. 35.2 J/g K, 7.06 J/mol K C. 0.0464 J/g K, 9.31 J/mol K D. -0.139 J/g K, -27.9 J/mol K
10. Given the following reactions and their associated enthalpy changes:
H2(g) + Br2(g) = 2 HBr(g) delta H = -72 kJ H2(g) = 2 H(g) delta H = 436 kJ Br2(g) = 2 Br(g), delta H = 224 kJ
calculate the enthalpy change for the reaction
H(g) + Br(g) = HBr(g)
A. -366 kJ B. -732 kJ C. +366 kJ D. +732 kJ
11. On the following diagram of a wave, the unit labeled (A) is
A. frequency B. wavelength C. measured in hertz D. both (B) and (C) are correct
12. In an H-atom emission tube there is a transition with a wavelength of 486 nm. What is the energy, in Joules, of this photon from this transition?
A. 4.09 x 10-19 J B. 4.09 x 10-28J C. 2.44 x 1018 J D. 9.66 x 10-23 J
13. Green light in the visible portion of the electromagnetic spectrum has a wavelength of about 525 nm. What is its frequency in Hz?
A. 1.58 x 1011 Hz B. 5.71 x 1014 Hz C. 1.75 x 10-15 Hz D. 1.58 x 1020 Hz
14. Which of the following has the longest de Broglie wavelength?
A. A bus traveling at 95 mph. B. A golf ball traveling at 95 mph. C. A 95 mph football. D. An electron traveling at 95 mph.
15. Important information provided by the principal quantum number, n, is that it
A. tells you how many neutrons there are in the nucleus. B. tells you exactly how many electrons a particular element has. C. provides information on the masiumum number of unpaired electrons a particular element has. D. provides information about the energy of the atom and the average distance of the electron from the nucleus.
16. Which of the following is the correct ground state orbital diagram for a nitrogen atom?
17. Arrange the following subshells in order of increasing energy in a
multi-electron
1s, 2s, 3s, 2p, 3p, 4p, 3d
A. 1s < 2s < 2p < 3s < 3p < 4p < 3d B. 1s < 2s < 2p < 3s < 3p < 3d < 4p C. 3d < 4p < 3p < 3s < 2p < 2s < 1s D. 4p < 3d < 3p < 3s < 2p < 2s < 1s
18. Give the values of the n and l quantum numbers for the 3d subshell.
A. n = 3 l = 0 B. n = 3 l = 3 C. n = 0 l = 3 D. n = 3 l = 2
19. The total number of orbitals with principal quantum number n = 3 is:
A. 2 B. 6 C. 9 D. 18
20. The number of unpaired electrons in a fluorine atom is:
A. 0 B. 1 C. 2 D. 3
21. Which of the following are isoelectronic?
Ne, Cl-, Al3+, Na, O2-
A. Na, Ne, O2- B. Na, Cl-, O2- C. Cl-, Al3+, Ne D. Ne, Al3+, O2-
22. The ground state electron configuration for the Ca atom is
A. 4s2 B. [Ar]4s2 C. [Kr]4s2 D. [K]4s2
23. What is the ground state electron configuration of the Mn2+ ion?
A. [Ar]4s23d5 B. [Ar]4s23d3 C. [Ar]3d5 D. [Ar]4s13d4
24. Which of the following series of atoms are arranged correctly in order of increasing size?
A. H < Li < Be B. Na < Mg < Ca C. Cl < Br < As D. K < Ga < In
25. Arrange the following species in order of increasing size:
Kr, Se-, Br, Se2-, Se
A. Kr < Br < Se2- < Se- < Se B. Br < Kr < Se2- < Se- < Se C. Kr < Br < Se < Se- < Se2- D. Se < Se- < Se2- < Br < Kr