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Test #2 (Fall, 2009) - version 1
Chemistry 114 (Burns)
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Name·-----I-Ktwif=-==--A---
Time Finished: (1 point)
- Record the clock time, such as 18:53 or 6:53, when you are ready to hand in your test. Failure to do so will result in a
"0" for this "question.")
DON'T OPEN THIS TEST UNTIL
YOU ARE INSTRUCTED TO DO
SO!!
Periodic Table of the Elements
lA 8A
r- 1
H
1.0079 2A
2 Li^ Be
II 12
3 Na^ Mg^3 4
22.989 24.305 3B 4B 5B
K Ca Sc Ti V
(^4) Sandil.Lm 39.098 40.08 47.87 50942 37 38 39 40 41
Rb Sr Y Zr Nb
6 Cs^ Ba^ La^ Hf^ Ta 1 3290, 13734 13891 178.49 180948 87 88 89 104 10 5
7 Fr Ra Ac Rf Db
3A
B
Al
7 8B II 12
6B 7B IB 2B 26.
Cr Mn Fe Co Ni Cu Zn Ga
Mo Tc^ Ru^ Rb^ Pd^ Ag^ Cd^ In
95.94 (98) 101.07 102.905^ 106.4^ 107861 112.411 114.
W Re Os Ir Pt Au Hg Tl
106 107 108 109 110 III 112
Sg Bh Hs Mt^ ...^ ••• ... (263) (262) (265) (266) (269) (272) (277)
4A 5A
C N
12.011 [
Si P
Ge As
Sn Sb
Pb Bi
6A
S
Se
Te
Po
7A
F
Cl
35
Br
r
12690 85
At
'2""
He
Ne
Ar
Kr
Xe
86
Rn
Solubility Rules for Ionic Compounds:
1 Lithium, sodium, potassium, and ammonium (^2) acetate and nitrate 3 Chloride, bromide, and iodide 4 sulfate 5 carbonate
6 ' ' phosphate
7 sulfide 8 hydroxide
Group IA and ammonium compounds are soluble. Acetates and nitrates are soluble. Most chlorides, bromides and iodides are soluble. Most sulfates are soluble. Most carbonates are insoluble. Most phosphates are insoluble. Most sui fides are insoluble. Most hydroxides are insoluble.
AgCl, Hg2C1 (^) 2• PbCI 2 , AgBr, HgBr2. Hg2Br 2, PbBr 2, AgI, HgIz, Hgzlz, PbIz CaS04. SrS0 4, BaS0 (^) 4, AgzS0 (^) 4 , HgZS04, PbS0 (^4) Group IA carbonates, (NH 4 )ZC0 3 Group IA phosphates, (NH4)3P Group IA sulfides. ( NH 4 )zS Group IA hydroxides, Ca(OH)z, Sr(OH)z, Ba(OH)
Electronegativity values:
Electronegativity of the Elements
18 lA 8A . H 2 2.1 (^) 2A
2 Li^ Be 1.0 1.
3 N.^ Mg
0 .9 (^) ,-1.
4 K^ I^ ~^ C.
0.8 1.
16 17 6A 7A
0 F 3.5 4.
S^ CI 2.5^ 3.
Se Br I 2.4^ 2. ,
Rb Sf In So Sb Te I I (^5) 1.8 1.9 2.1 2. 0 .8 1. I
6 Cs^ I^ Ba^ TI 't Pb Bi Po^ At 0.7 0.9 1.8^ 1.9 1.9^ 2.0 2.
,
13 14 15 3A 4A 5A
B N I C 2.0 2.5 3.
AI Si P 1.5 1.8 2.
Ga Ge As 1.6 1.8^ 2.
Conversion Factors: 1 kg = 2.205 Ib 1 m = 3.280 ft 1 m^3 = 264.2 gallon 1 ton = 2000 lb
1 g = 0.03527 ounce 1 cm = 0.3937 in
1 km =0.6214 mile
1 gallon = 4 quarts
1 meter = 1.0936 yards
1 liter = 1.057 quart
1 pound = 454 grams
Physical Constants:
1 amu = 1.660Sx W 24 g N. = 6.0221 X 10 23
- The primary compound in natural gas is methane which is commonly used to heat homes. Methane burns in the air according to the following reaction:
How many grams of O 2 are needed to produce 3.50 g of CO 2? (6 points)
- A student makes the following observations (^) BaCl! ( Pb(NOlh ~,^ ~ with she mix.ed aqueous solutions of the salts Yellow Yellow-^ No reaction^ No reaction listed in the table. She mixed her unknown with (^) brownish precipitate NaOH and CUS04, observing a white precipitate precipitate for all of them. However, Pb(N0 3 )2 produced White White White no precipitate with the unknown. Identify the (^) precipitate precipitate precipitate ,
salt, which is one of the six used. Write balanced chemical equations for each of White (^) White reactions, including states of matter. (6 points) (^) precipitate (^) precipitate
White precipitate
6-1 fb(lJo.:)L..0 ~tJ.,.
-He-
No reaction
\I/hite precipitate
No reaction
No reaction
No reaction
-J<;,i.
Pb(NOlh
euso,
~
NaOH
fb (1JO!-)1-. ~).,. J.lJtt(jH(~) --i> Pb ([)(.f)z..^ ~)^ r^ ;)^ AJa.^ IJq^ (~^
)
Ph(,u
3
)2. (~) (- CIASO,( Li) ---P Pb ;X;7{~).I- CAL VCI)2- ('1)
SHORT ANSWER: Try to limit your answer to the space provided. However, you may use the blank portion of page 2
for your answer, if necessary.
- Fill in the blanks to complete the following table (1 point each):
Chemical Symbol Ion Formed Number of electrons in Ion Number of Protons in Ion
I
F p-^ /0 4
S $2^ -^ 18 I~
r!>tA. Ba^
5tt^56
- Indicate whether each of the following compounds is a ionic compound, an acid, or a molecular compound (2 points each):
a) ZnF^ I^ o-vtL.
~,so, 40f 6
- Write chemical formulas for the following compounds? (2 points each)
a) Aluminum sulfide (^) 4~S
b) Iron(IU) hydroxide (iCOI+)
c) Carbonic acid (^) If;> ~
d) Dinitrogen tetroxide (sometimes elToneously spelled tetraoxide) (^) AJ.;...t¥
- Classify each of the following bonds as nonpolar covalent, polar covalent, or ionic: (2 points each)
a) C-O
b) K - CI
- Identify the following chemical reactions (Some answers have more than one possible answer, but only one answer is required): (2 points each) 0
a) 3 CuS04(aq) + 2 AI(s) -t Ah(S04Maq) + 3 Cu(s).
H 20 b) H 2 (g) + Oz(g) -t HzOiaq).
1l. Detennine the oxidation number in each of the following (2 points each):
a) 0 in 0 3 o
b) NinN0 (^2)
- What is the formula for the following ions? (3 points each)
a) Phosphate
b) calcium
- What is the rooJ geometry of the following molecules at the indicated atom (see alTow):
(2 points each)
~.. .. :F-C=N a. ..^ ..^ fn--T+~~ f _ra.WJvV
b. (^) kJra-'J~
- The following Lewis symbols for ions have their charges omitted. Determine the number of extra
electrons that each ion is showing and its charge. (1 point each) Extra Electrons (^) Ion's Charge
[ :r.: J a) ~ ,3 -
b)
[:~~: J -J.
50f 6
