.Name:______________________________________________
CHEMISTRY 101 Practice Exam 4 – 100 points
#1: Multiple Choice __________/ 60
#2: Free Response __________/ 40
TOTAL: __________/100
Instructions:
1. Cell phones must be put away and bags punt on the floor.
2. Once we begin the exam, you must ask Dr. Lemieux if you wish to leave and return. 3. Anyone caught cheating in any fashion will be disciplined, as indicated in the syllabus. 4. You will have 1 hr 15 min to complete this exam individually.
1. The pH of a 1.0x10-4 M solution of HNO3 is
A) 4.0 B) 6.0 C) 10.0 D) 12.0
2. In which of the following pairs of salts will both members of the pair hydrolyze in water to give solutions that are basic?
A) NaC2H3O2 and KCN
B) LiNO3 and Na2SO4
C) KI and KCN D) NH4I and NH4NO3
4. Complete the following nuclear equation: 10B + 1n → 4He + ______
A) 42He
B) 115B
C) 7 3Li
D) 126C
3. Which of the following types of radiation is composed of particles with two protons and 2 neutrons?
A) X-rays
B) gamma radiation C) beta particles D) alpha particles
5.
The daughter isotope produced by the beta decay of is A) 234
91Pa B) 230
89Ac C) 230
88Ra D) 234
92U
6. Which of the following lists appropriate shielding for alpha particles and gamma rays, respectively?
A) concrete wall, aluminum foil B) lead barrier, aluminum foil C) skin, concrete wall
D) none, lead barrier
7. In which the following pairs of acids are both members of the pair strong acids? A) HNO2 and H2SO4
B) H2SO4 and HF
C) HCl and HC2H3O2
D) HNO3 and HClO4
8. Which of the following is not a conjugate acid/base pair? A) HCO3–/CO3–
B) NH4+/NH3
C) H3PO4/H2PO4
-D) H2O/OH–
9. Which of following could be used to make up a buffer? A) HCl + NaCl
B) KBr + CaBr2
C) HF + NaF D) H2CO3 + H2O
10. The explanation for how a beta particle is produced in the nucleus of a radionuclide and then ejected involves the conversion (in a complex series of steps) of a
14. Complete the following nuclear equation: 23994Pu → 42He + _____
A) 235U B) 243Cm
C) 237Th D) 241Cf
11. Which of the following types of molecules would be most soluble in water because of hydrogen bonding?
A) ether B) aldehyde C) alkane D) alcohol
12. Which choice correctly lists functional groups present in the aspirin molecule shown? A) amine, ester
B) ester, ether
C) carboxylic acid, alcohol D) carboxylic acid, ester
13. Calcium nitrate would be the salt produced by the neutralization of which acid and base?
A) calcium nitrite and nitrous acid B) calcium hydroxide and nitric acid C) calcium nitride and nitrous acid D) calcium hydroxide and nitrous acid
15. Which of the following is not a strong base? A) Mg(OH)2
B) Ca(OH)2
C) Sr(OH)2
16. What is the correct name for the molecule shown? A) 1,2-chloroethane
B) 2,3-chloropropane C) 1,2-dichloropropane D) 2,3-chlorobutane E) none of the above
17. Which of the following types of molecules is not polar? A) alkane
B) aldehyde C) alcohol D) ester
E) none of the above
18. Which of the following types of radiation is composed only energy? A) positron
B) gamma C) beta D) alpha
E) none of the above
19. Which choice correctly lists the functional groups present in the vitamin A molecule shown?
A) alkene, alcohol B) ketone, amine C) alcohol, aldehyde D) carboxylic acid, alkene
20. The half-life sodium-24 is 15 hours. If a sample emits 120 cpm of radiation. Later, the radiation is measured again and found to be 15 cpm. How much time passed?
Free Answer Section (40 points total)
Important: You must show ALL work to receive full credit. Remember to keep track of your sig figs. Write your answer with units in the box.
1. Draw and name three isomers of C4H9F. (8 points)
2. Consider a 2.0 x 10-4 M HCl solution. Determine the [OH-], pOH, and pH. Is the solution
acidic or basic? (8 points)
[OH-] = _____________
pOH = _____________
3. Phospohorus-32 has a half-life of 14.3 days. How many grams of a phosphorus-32 would remain undecayed in a 20.0 g sample after 42.9 days ? (5 points)
4. Write the name of the molecule.
5. Draw the structure of the molecule
1 atm = 760 mmHg = 760 torr R = 0.0821 (L*atm) / (mol * K)
ΔHvap of water = 40.7 kJ/mol ΔHfus of water = 6.02 kJ/mol
Specific heat capacity of liquid water = 1.00 cal/g 0C = 4.184 J / mol 0C
1 mole gas has volume 22.4 L at STP (00C and 1 atm pressure)
K = 0C + 273.15 Kw = [H3O+][OH-] = 1.0x10-14
