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Material Type: Exam; Professor: Sharpless; Class: General Chem I, w/lab; Subject: Chemistry; University: University of Mary Washington; Term: Fall 2006;
Typology: Exams
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December 15th, 2006 Chemistry 111 150 minutes Final Exam
Name ________________________________________
Sign here to acknowledge that you have abided by the UMW Honor Code in taking this exam.
Signature: _____________________________________________________
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
a. 5.5 x 10^2 b. 552 c. 552.3 d. 552.
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-
metal?
a. 6.11 g cm-3^ b. 6.51 g cm-3^ c. 8.63 g cm-3^ d. 8.96 g cm-
a. 1 H b. 40 Ca2+^ c. 14 C d. 19 F-
a. protons b. neutrons c. electrons d. protons and neutrons
a. molybdenum(VI) oxide b. molybdenum trioxide c. molybdenum(III) oxide d. molybdenum(III) trioxide
a. Mg 2 F 3 b. MgF c. Mg 3 F 2 d. MgF 2
a. 2, 1, 3, 2 b. 4, 6, 3, 2 c. 2, 3, 1, 6 d. 2, 3, 2, 3
a. 1.4 x 10-23^ b. 0.50 c. 3.0 x 10^23 d. 6.0 x 10^23
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
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
a. b.
c. d.
energy than sodium.
l
b. 1 c. 2 d. 3
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
a. -1 b. 0 c. +
B d: C≡C C-C H-I C-I C-H
d. + 160 kJ
a. b. c. d.
2 only^ b. SCl 2 and SCl^4 c. SCl 4 only^ d. All are polar
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
a. square planar b. see-sa
Which of the concerning hybrid orbital theory?
4 s formed. ecules. e forms.
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
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SCORE 50 #^ CORRECT 10D (^) % CORRECT (^) NAME .:Dr. E~ Flj \ \
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MARKING INSTRUCTIONS
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