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December 15th, 2006 Chemistry 111 150 minutes Final Exam
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Necessary Constants
NA = 6.02 x 10^23 mol-1^ h = 6.626 x 10-34^ J s c = 3.00 x 10^8 m s-
B = 2.178 x 10-18^ J R = 0.0821 L atm mol-1^ K-
Potentially Useful Equations ∆E = q + w w = -P∆V q = m s ∆T q = C ∆T ∆H = ∆E + P∆V
Eph = hν = c = νλ Ee- = -B / n^2 n = 1, 2, … l = 0, 1, … n-
m l = - l , …, + l PTOT = P 1 + P 2 + … Xi = ni / nTOT = Pi / PTOT
urms = (3RT / M)1/2^ [Pobs + a(n / Vobs)^2 ] x [Vobs – n b] = n RT
50 questions, 2 points each
- The operation, (2115 - 2101) x (5.11 x 7.72) = _________.
a. 5.5 x 10^2 b. 552 c. 552.3 d. 552.
- The quantity 1.0 mg cm-3^ is the same as:
a. 1.0 x 10-6^ kg m-3^ b. 1.0 x 10-3^ kg m-3^ c. 1.0 kg m-3^ d. 1.0 x 10^3 kg m-
- A metal cube is 0.161 cm on each side and has a mass of 36 mg. What is the density of this
metal?
a. 6.11 g cm-3^ b. 6.51 g cm-3^ c. 8.63 g cm-3^ d. 8.96 g cm-
- Which of the following has the same number of electrons and neutrons?
a. 1 H b. 40 Ca2+^ c. 14 C d. 19 F-
- Different isotopes of a particular element contain the same number of __________.
a. protons b. neutrons c. electrons d. protons and neutrons
- The systematic name for the compound MoO 3 is:
a. molybdenum(VI) oxide b. molybdenum trioxide c. molybdenum(III) oxide d. molybdenum(III) trioxide
- The empirical formula of the ionic compound that forms from magnesium and fluorine is:
a. Mg 2 F 3 b. MgF c. Mg 3 F 2 d. MgF 2
- When the equation, Al(NO 3 ) 3 + Na 2 S Æ Al 2 S 3 + NaNO 3 , is balanced, the coefficients are:
a. 2, 1, 3, 2 b. 4, 6, 3, 2 c. 2, 3, 1, 6 d. 2, 3, 2, 3
- How many atoms of nitrogen are in 8.5 g of NH 3?
a. 1.4 x 10-23^ b. 0.50 c. 3.0 x 10^23 d. 6.0 x 10^23
- A compound with a molar mass of 60.05 g mol-1^ is 40.0% C, 6.71 % H, and 53.29% O by mass. What is the molecular formula of this compound? a. C 3 H 8 O b. C 2 H 4 O 2 c. C 2 H 2 O 4 d. CH 2 O
- According to the reaction, 2 NH 3 (g) + 2 O 2 (g) Æ N 2 O(g) + 3 H 2 O(g), if 8.0 grams of NH 3 react with
8.0 g O 2 , the limiting reagent is _______ and the theoretical yield of N 2 O is _____. a. NH 3 , 0.24 mol b. O 2 , 0.13 mol c. NH 3 , 0.47 mol d. O 2 , 0.25 mol
- According to the reaction, 2 H 2 (g) + O 2 (g) Æ 2 H 2 O(g), what is the percent yield if 27 g of H2O are
produced from the reaction of 1.5 moles of O 2?
a. 1.5 % b. 25 % c. 50 % d. 66 %
1 3. The concentration of chloride ions in a 0.150 M solution of AlCl 3 is:
a. 0.0500 M b. 0.150 mol c. 0.450 mol d. 3.00 M
1 4. The number of moles of sodium ions in 2.00 L of 0.500 M Na 3 P is:
a. 0.500 mol b. 1.00 mol c. 3.00 mol d. 6.00 mol
1 5. How many grams of NaCl are in 150 mL of a 3.0 M solution?
a. 3.00 b. 26.3 c. 58.5 d. 176
- If all the following were made into 0.1 M solutions, which solution would have the highest concentration of particles? a. AlCl 3 b. K 2 CO 3 c. NaF d. Na 2 S 2 O 3
- When aqueous BaI 2 and K 2 SO 4 are combined, a precipitate forms. Which are the spectator ions in this reaction? a. Ba2+^ and SO 4 2-^ b. K+^ and I-^ c. Ba2+^ and I-^ d. K+^ and SO 4 2-
- The balanced net ionic equation for the reaction that occurs when aqueous AgNO 3 and NaI are mixed is: a. Ag+(aq) + I-(aq) Æ AgI(s) b. Ag+(aq) + NO 3 - (aq) Æ AgNO 3 (s) c. Na+(aq) + NO 3 - (aq) Æ NaNO 3 (s) d. AgNO 3 (aq) + NaI(aq) Æ AgI(aq) + NaNO 3 (s)
- A 50.0 mL sample of NaOH was neutralized by titration with 50.0 mL of 0.150 M H 2 SO 4. What was the NaOH concentration? a. 0.0750 M b. 0.150 M c. 0.300 M d. 0.750 M
- Which is a correct orbital diagram for a ground state nitrogen atom?
a. b.
c. d.
- ments generally decreases across a period because:
- much more apt to exist as an anion than is sodium. This is because:
energy than sodium.
- Which isoelectronic series is correctly arranged in order of increasing radius?
l
- re of PF 3 is drawn, how many lone pairs of electrons are there on
b. 1 c. 2 d. 3
- following is true concerning the N to O bonds in the nitrite ion, NO 2 -^?
the other is a single bond. but shorter than a double bond.
1s
2 s
2 p
1s
2 s
2 p
1s
2 s
2 p
1s
2 s
2 p
The atomic radius of main group ele a the effective nuclear charge increases across a period. b. the effective nuclear charge decreases across a period. c. the principal quantum number increases across a period. d. the principal quantum number decreases across a period.
Chlorine is a. chlorine is bigger than sodium. b. chlorine has a greater ionization c. chlorine has a greater electron affinity than sodium. d. chlorine is a gas and sodium is a solid.
a. K+^ < Ca 2+^ < Ar < Cl -^ b. Cl-^ < Ar < K+^ < Ca 2+ c. Ca 2+^ < Ar < K+^ < Cl-^ d. Ca2+^ < K+^ < Ar < C -
When the Lewis structu phosphorous?
a. 0
Which of the a. Both bonds are single bonds. b. Both bonds are double bonds. c. One bond is a double bond and d. Both bonds are the same and are longer than a single bond
- rogen in nitric acid (shown below) is:
a. -1 b. 0 c. +
- ergies given below to determine the enthalpy of the reaction,
H-C≡C-H + 2 H-
B d: C≡C C-C H-I C-I C-H
d. + 160 kJ
- For which of the following is the central atom sp hybridized?
a. b. c. d.
2 only^ b. SCl 2 and SCl^4 c. SCl 4 only^ d. All are polar
- The molecular
The formal charge on nit
d. +
O
HO N O
Use the table of bond en H H I Æ I-C-C-I H H on ∆H (kJ mol -1): 839 348 299 240 413
a. - 160 kJ b. - 217 kJ c. - 63 kJ
H
H C H
H
H N H
H O
O C OH
H
Of the following compounds, which is/are polar?
N C H
Cl S Cl
a. SCl
geometry of BrF 4 +^ is:
w c. octahedral d. tetrahedral
- following is incorrect
a. square planar b. see-sa
Which of the concerning hybrid orbital theory?
4 s formed. ecules. e forms.
- mple of an ideal gas is originally at 25.0 C and 0.100 atm. It is heated to 300 C at
c. 0.192 atm d. 1.20 atm
a. Hybrid orbital theory explains the equivalence of the bonds in CH b. The number of orbitals hybridized equals the number of hybrid orbital c. Except for bonds to H, overlap of hybrid orbitals forms the sigma network of mol d. According to hybrid orbital theory, all electrons are localized in species with no resonanc
A 3.00 L sa o^ o constant volume. The new pressure of the gas is:
a. 0.0520 atm b. 0.101 atm
Cl S Cl Cl
Cl
S
Cl Cl Cl (^) Cl Cl
Cl
l
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