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A chemistry exam from fall, 2009, focusing on topics such as the periodic table, solubility rules, electronegativity values, conversion factors, and various chemical reactions. Students are required to answer multiple-choice questions, fill in the blanks, and draw lewis structures.
Typology: Exams
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r- 1
(^4) Sandil.Lm 39.098 40.08 47.87 50942 37 38 39 40 41
6 Cs^ Ba^ La^ Hf^ Ta 1 3290, 13734 13891 178.49 180948 87 88 89 104 10 5
Sg Bh Hs Mt^ ...^ ••• ... (263) (262) (265) (266) (269) (272) (277)
Cl
35
r
12690 85
'2""
Xe
86
1 Lithium, sodium, potassium, and ammonium (^2) acetate and nitrate 3 Chloride, bromide, and iodide 4 sulfate 5 carbonate
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)
18 lA 8A . H 2 2.1 (^) 2A
2 Li^ Be 1.0 1.
0 .9 (^) ,-1.
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 gallon = 4 quarts
1 pound = 454 grams
Physical Constants:
How many grams of O 2 are needed to produce 3.50 g of CO 2? (6 points)
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
No reaction
\I/hite precipitate
No reaction
No reaction
No reaction
-J<;,i.
Pb(NOlh
euso,
~
NaOH
)
3
for your answer, if necessary.
Chemical Symbol Ion Formed Number of electrons in Ion Number of Protons in Ion
F p-^ /0 4
5tt^56
~,so, 40f 6
a) Aluminum sulfide (^) 4~S
b) Iron(IU) hydroxide (iCOI+)
c) Carbonic acid (^) If;> ~
d) Dinitrogen tetroxide (sometimes elToneously spelled tetraoxide) (^) AJ.;...t¥
a) C-O
b) K - CI
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)
a) Phosphate
b) calcium
(2 points each)
~.. .. :F-C=N a. ..^ ..^ fn--T+~~ f _ra.WJvV
b. (^) kJra-'J~
electrons that each ion is showing and its charge. (1 point each) Extra Electrons (^) Ion's Charge
[ :r.: J a) ~ ,3 -
b)
[:~~: J -J.