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Chemistry Exam (Fall, 2009) - Version 1 - Prof. Francis M. Burns, Exams of Chemistry

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

2009/2010

Uploaded on 12/09/2010

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Test #2 (Fall, 2009) -version 1
Chemistry 114 (Burns)
____
,/100
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
18
lA
8A
r--
1
H 2
1.0079
2A
3 4
2
Li
Be
6.941 9.0122
II
12
3
Na
Mg 3 4 5
22.989 24.305 3B
4B
5B
19
20
21
22
23
K
Ca
Sc
Ti
V
Sandil.Lm
4
39.098 40.08 47.87
50942
37 38 39
40
41
5
Rb
Sr
Y
Zr
Nb
85.468
8762
88905
91.22 92.906
55 56 57
72
73
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
(223) (226) (227) (26 1) (262)
13
3A
5
B
10.811
13
6 8 9
10
Al
7
8B
II
12
6B 7B
IB
2B
26.981
24
25
26 27 28 29 30
31
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
51996
54.938 55.847 58.933
5869
63 .546 65.39 69.723
42 43 44 45 46 47
48
49
Mo
Tc
Ru
Rb
Pd
Ag
Cd
In
95.94 (98) 101.07 102.905 106.4 107861 112.411 114.82
74 75
76
77 78 79 80
81
W
Re
Os Ir
Pt
Au
Hg
Tl
183.85 186.2 190.2
1922
195.09 196.967 200.59
20438
106
10
7
108
109 110
III
112
Sg
Bh
Hs
Mt
...
•••
...
(263) (262) (265) (2 66) (269) (272) (277)
14 15
4A
5A
6 7
C N
12.011
[4006
14 15
Si
P
28.086 30.973
32 33
Ge
As
72.6 1 74 .922
50
5 1
Sn
Sb
118.71 121.75
82 83
Pb
Bi
20719
20898
16
6A
8
0
15.9994
16
S
32.066
34
Se
78.96
52
Te
127.60
84
Po
(209)
17
7A
9
F
18
984
17
Cl
35.453
35
Br
79904
53
r
12690
85
At
(210)
'2""
He
4.0026
10
Ne
20 180
18
Ar
39.948
36
Kr
83.80
54
Xe
131.29
86
Rn
(222)
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, Hg2
C1
2PbCI2, AgBr, HgBr2. Hg2Br
2,
PbBr
2,
AgI, HgIz, Hgzlz, PbIz
CaS04.
SrS0
4,
BaS0
4, AgzS0 4, HgZ
S0
4,
PbS0
4
Group IA carbonates,
(NH
4)ZC03
Group IA phosphates, (NH4)3P04
Group IA sulfides. (
NH
4)zS
Group IA hydroxides, Ca(OH)z, Sr(OH)z,
Ba(OH)2
pf3
pf4

Partial preview of the text

Download Chemistry Exam (Fall, 2009) - Version 1 - Prof. Francis M. Burns and more Exams Chemistry in PDF only on Docsity!

Test #2 (Fall, 2009) - version 1

Chemistry 114 (Burns)

____,/

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

  1. 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)

  1. 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.

  1. 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

  1. 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

  1. 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¥

  1. Classify each of the following bonds as nonpolar covalent, polar covalent, or ionic: (2 points each)

a) C-O

b) K - CI

  1. 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)

  1. What is the formula for the following ions? (3 points each)

a) Phosphate

b) calcium

  1. 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~

  1. 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