Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2006
Name Date
The last page of each examination should be a periodic table.
c = 3.00 x 108 m/sec
h = 6.63 x 10-34 Js
mp = 1.67 x 10-24 g (mass of proton)
Rydberg Constant (RH) = 2.18 x 10-18 J
Metal Activity Table
(easiest to oxidize at top)
Lithium
Potassium
Barium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cobalt
Nickel
Tin
Lead
HYDROGEN
Copper
Silver
Mercury
Platinum
Gold
1. What is the mass of H2SO4 in a 125 cm3 sample of sulfuric acid that has a density of 1.55 g/cm3 and consists of 65.0% (by mass) H2SO4?
a) 126 g
b) 152 g
c) 181 g
d) 194 g
e) 2-3 g
2. All of the following statements are correct except
a) The conversion of compounds into elements is a chemical change.
b) The conversion of liquid water into gaseous water is a chemical change.
c) The conversion of sugar to carbon and water is a chemical change.
d) The evaporation of water is a physical change.
e) The conversion of elements into compounds is a chemical change.
3. Which of the following statements is/are correct?
A solid crystalline sample of an ionic compound:
I. is held together by electrostatic forces (Couloumb's Law).
II. is composed of cations and anions.
III. is a regular three-dimensional array of positively and negatively charged particles.
IV. contains cations, which are repelled by the anions and attracted to the other cations.
a) II, III, and IV
b) I, II, and III
c) I, II, and IV
d) II and IV
e) I and II
4. Which of the following two statements is/are correct?
I. The formula for ammonium hydroxide is NH4(OH)2.
II. The formula for Manganese (II) Phosphate is Mn3(PO4)2.
a) I
b) II
c) I and II
d) Neither is correct
5. The following is the reaction for the Ostwald Process to produce nitric acid:
2 NO2(g) + H2O(l) ------> 2 HNO3(aq) + NO(g)
If a sample of NO2 produces 15.0 g HNO3, how many grams of the byproduct NO are produced?
a) 14.3 g
b) 10.7 g
c) 7.14 g
d) 4.76 g
e) 3.57 g
6. How many atoms of hydrogen are contained in 1.27 g water?
a) 4.25 x 1022
b) 8.50 x 1022
c) 4.25 x 1023
d) 8.50 x 1023
e) 1.70 x 1024
7. Visiting a planet in a parallel universe you find a chemistry textbook that describes an element with three naturally occurring isotopes and the following values of their masses and abundances:
Isotopic Mass (amu) Fractional Abundance
100.0 amu 0.2000
102.0 amu 0.3333
104.0 amu 0.4667
The atomic weight of this element is
a) 100.5 amu
b) 101.0 amu
c) 101.5 amu
d) 102.0 amu
e) 102.5 amu
8. The composition of oxalic acid is 26.7% carbon, 2.2 % hydrogen and 71.1% oxygen, by mass. What is the empirical formula of oxalic acid?
a) CHO2
b) CHO
c) C2HO4
d) C2HO2
e) none of the above.
9. Which of the following chemical reactions is an oxidation-reduction reaction?
a) NH3 + HCl ------> NH4Cl
b) H2SO4 + Ba(OH)2 ------> BaSO4 + 2 H2O
c) Pb(NO3)2 + 2 HCl ------> PbCl2 + 2 HNO3
d) Mg + CO2 ------> MgO + CO
e) CO2 + H2O ------> H2CO3
10. Which net ionic equation best represents the reaction that occurs when an aqueous solution of barium chloride is mixed with an aqueous solution of sulfuric acid?
a) Ba2+(aq) + 2 Cl-(aq) + 2 H+(aq) + SO42-(aq) ------> BaSO4(s) + 2 HCl(g)
b) Ba2+(aq) + SO42-(aq) ------> BaSO4(s)
c) BaCl2 + H2SO4 ------> BaSO4 + 2 HCl
d) 2 H+(aq) + 2 Cl-(aq) ------> HCl(g)
e) No net reaction occurs.
11. How many milliliters of 0.126 M HClO4 (perchloric acid) are required to give 0.00752 mol HClO4?
a) 0.0948 mL
b) 94.8 mL
c) 0.0597 mL
d) 59.7 mL
e) none of the above.
12. The reaction Ca(OH)2(s) ------> Ca2+(aq) + 2 OH--(aq) indicates that the Ca(OH)2 is a weak base.
a) true
b) false
13. Determine the number of liters of 0.250 M HNO3 required to neutralize a solution by dissolving 17.5 g of NaOH in 350 ml of solution
a) 50.0
b) 0.44
c) 1.75
d) 0.070
e) none of these
14. The value of DHo for the following reaction is -126 kJ.
2 Na2O2 (s) + 2 H2O (l) à 4 NaOH (s) + O2 (g)
How much heat will be evolved when 2.00 moles of NaOH (s) are formed in the reaction?
a) 252 kJ
b) 63 kJ
c) 3.9 kJ
d) 7.8 kJ
e) none of these
15. A 1.96 g sample of titanium was burned in a bomb calorimeter that had a heat capacity of 9.84 kJ/oC. The temperature of the calorimeter increased from 36.84 oC to 98.82oC. Calculate the amount of heat that would be released from the combustion of one mole of titanium.
a) 62.0 kJ
b) 610 kJ
c) 1.49 x 104 kJ
d) 311 kJ
e) 1200 kJ
16. For which one of the following is DH°f zero?
a) O2(s)
b) diamond(s)
c) N2(g)
d) F2(s)
e) none of the above
17. Under constant volume conditions, the heat of combustion of propane (C3H8) is 2220 kJ/mole. A 2.500 g sample if burned and the temperature increased from 20.55° C to 28.25°C. What is the total heat capacity of the calorimeter?
a) 126.1 kJ °C-1
b) 16.4 kJ °C-1
c) 720.8 kJ °C-1
d) 6.55 kJ °C-1
e) none of the answers are within 10% of the correct value.
18. An important reaction of alkenes is the addition of bromine to the double bond. Given the following information, calculate the DH for the bromination of ethylene.
Bond Type Bond Dissociation Energies (kJ mol-1)
C - C 348
C = C 614
O - O 146
C - O 358
O - H 463
C- H 413
Br - Br 193
C - Br 276
a) -276 kJ mol-1
b) 54 kJ mol-1
c) -93 kJ mol-1
d) 183 kJ mol-1
e) None of the answers are within 10% of the correct value.
19. Which orbital diagram represents a violation of the Pauli Exclusion Principal for an atom in its ground state?
a) w b) x c) y d) z e) both w and y
20. Which quantum number defines the energy of an orbital?
a) spin
b) magnetic
c) principal
d) azimuthal
e) angular momentum
21. Which of the following electron configurations is incorrect ?
a) Br [Ar] 5s24d105p5
b) Ar [Ne] 3s23p6
c) Ge+4 [Ar] 3d10
d) Zn+2 [Ar] 3d10
e) all of the above are correct configuration
22. Arrange the following species: K, Mg, Mg+2 , and Na in order of decreasing radii.
a) Mg+2 > Mg > Na . K
b) K > Na > Mg+2 > Mg
c) K > Mg > Na > Mg+2
d) K > Na > Mg > Mg+2
e) None of the preceding answers is correct
23. The molecule of propenol has the bond structure shown below. The hybridization on the three carbon atoms, from left to right, is:
a) sp3, sp3, sp
b) sp2, sp2, sp3
c) sp, sp2, sp
d) sp2, sp, sp3
e) sp2, sp3, sp3
24. For the ClF4+ ion, how many (total) valence electrons should be in the Lewis structure?
a) 32
b) 33
c) 34
d) 35
e) 36
25. The nitrogen atom is central in laughing gas, N2O, dinitrogen oxide, which has the following characteristics
a) linear, polar
b) bent, polar
c) trigonal planar, nonpolar
d) bent, non polar
e) linear, nonpolar
26. Based on molecular orbital theory, which of the following diatomic molecules is predicted to be paramagnetic?
a) B2
b) N2
c) Li2
d) C2
e) F2
27. All of the following statements concerning a sample of oxygen at 1.00 atm pressure are true except:
a) collisions between the gaseous molecules are elastic
b) the molecules are in constant rapid randon motion
c) the average kinetic energy of the gaseous oxygen is inversely proportional to the absolute temperature of the gas.
d) the pressure exerted by gaseous is due to the impact of the molecules with the walls of the container.
e) the volume occupied by the oxygen molecules is negligible compared with the size of the container.
28. What is the density of ammonia gas, NH3, at 31° C (304.2 K) and 0.988 atm pressure? (The molar mass of NH3 is 17.03 g/mol and R = 8.314 J mol-1 K-1 = 0.08206 L atm mol-1 K-1)
a) 0.0396 g/L
b) 0.674 g/L
c) 0.691 g/L
d) 6.61 g/L
e) 16.8 g/L
29. What is the partial pressure of oxygen in a container that contains 2.0 mol of oxygen, 3.0 mol of nitrogen, and 1.0 mol of carbon dioxide when the total pressure is 900 mm Hg?
a) 150 mm Hg
b) 200 mm Hg
c) 300 mm Hg
d) 450 mm Hg
e) 600 mm Hg
30. Write a Lewis structure for the ion AlF63-. (Al will have more than an octet around it) How many non-bonding valence-shell electrons are there in all?
a) 24
b) 30
c) 36
d) 42
e) 48
31. For which of the following pairs is the element with the larger second ionization listed first?
I. Na and Mg
II. Al and Mg
III. Ca and K
IV. Ne and F
a) I and II
b) I, II, and III
c) I, II, and IV
d) IV only
e) For none
32. Which one of the following substances would be the most soluble in water?
a) CH3CH2CH3
b) KOH
c) BF3
d) CBr4
e) toluene (CH3C6H6)
33. The electronic configuration of Mn+3 is (with the orbitals written in order of increasing energy):
a) 1s22s23s23p64s23d5
b) 1s22s22p63s23p63d64s1
c) 1s22s22p63s23p64s13d3
d) 1s22s22p63s23p64s23d2
e) 1s22s22p63s23p63d4
34. When NaCl dissolves in water, the force of attraction that exists between Na+ and H2O is called:
a) dipole-dipole
b) ion-ion
c) hydrogen bonding
d) ion-dipole
e) none of the above
35. Which liquid will have the highest boiling point? ( all have the same kb value )
a) aqueous 0.050 M NaI
b) aqueous 0.050 M glucose
c) aqueous 0.050 M CoI2
d) aqueous 0.025 M AlI3
e) aqueous 0.030 M Na3PO4