Download 2008 Periodic Table of the Elements Instructions: Read carefully all

FIUDepartment of Chemistry
CHM 1033 Survey of Chemistry Dr. Kavallieratos
Exam No 2
July 2010
Form 2
Name (print) _____________________________(Sign and Date) _______________________PID# _____-____-______
By signing above , I acknowledge that I am aware of the rules regarding academic honesty and of the penalties which may
result from academic misconduct. Such penalties may range from an “F” grade in the class to suspension or permanent
expulsion from the university with concurrent notation of the misconduct in my permanent records. I also understand that in
the event, I fail to return to the instructor this signed original along with my answer sheet I will be graded with an “F” for the
class.
IA
1
1
IIA
2
IIIB
3
IVB
4
VB
5
2008 Periodic Table of the Elements
VIB
6
VIIB
7
VIIIB
8
VIIIB
9
VIIIB
10
IB
11
IIB
12
IIIA
13
IVA
14
VA
15
VIA
16
VIIA
17
VIIIA
18
2
H
He
1.008
3
4
5
6
7
8
9
4.003
10
Li
Be
B
C
N
O
F
Ne
6.94
9.01
10.81
12.01
14.01
16.00
19.00
20.18
22.99
24.31
26.98
28.09
30.97
32.07
35.45
39.95
K
Ca
Sc
39.10
40.08
Rb
Sr
85.47
87.62
Cs
11
Na
19
12
Mg
←
23
V
Cr
Mn
44.96
47.88
50.94
51.97
Y
Zr
Nb
88.91
91.22
Ba
La
132.91
137.33
Fr
(223)
55
87
Cu
Zn
Ga
Ge
As
Se
Br
Kr
54.94
55.85
58.93
58.69
63.55
65.39
69.72
72.59
74.92
78.96
79.90
83.80
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
92.91
95.94
(98)
101.07
102.91
106.42
107.87
112.41
114.82
118.71
121.75
127.60
126.90
131.29
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
138.91
178.49
180.95
183.85
186.21
190.2
192.22
195.08
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Unn
Uuu
Uub
?
Uuq
?
Uuh
?
Uuo
226.03
227.03
266
269
272
277
?
289
?
289
?
293
56
88
57
89
72
104
(261)
58
73
105
(262)
59
42
74
106
(263)
60
43
75
107
(262)
61
44
76
108
(265)
62
45
77
109
63
46
78
110
64
47
79
111
65
30
48
80
112
66
31
49
81
113
67
32
50
82
114
68
33
51
83
115
69
34
35
18
Ar
Ni
41
29
17
Cl
Co
40
26
16
S
Fe
39
25
15
P
28
Ti
24
14
Si
27
38
21
→
22
37
20
13
Al
52
84
53
85
116
117
70
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140.12
140.91
144.24
(145)
150.36
151.96
157.25
158.92
162.50
164.93
167.26
168.93
173.04
174.97
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
232.04
231.04
238.03
237.05
(244)
(243)
(247)
(247)
(251)
(252)
91
92
93
94
95
96
97
98
99
100
(257)
101
(258)
102
54
86
71
Ce
90
36
(259)
103
Lr
(260)
Instructions: Read carefully all answers before selecting the best one for each question!
1)
In a solution of 20mg of sugar in 100 mL of water, sugar is the
a) solution
b) solute
c) solvent
2)
The molar mass of 2-methylpropane is:
a) 30g/mol b) 44 g/mol c) 58 g/mol d) None of the above
3)
The molar volume of any gas (in L) under Standard Temperature and Pressure is:
a) 6.02 x 1023
b) 44.8
c) 22.4
d) 273.15
4)
Which of the following has the same number of atoms as 32g of Methane?
a) 115g of Sodium b) 391g of Potassium
c) 32 g of Ethane d) 48g of Magnesium
5)
At Standard Temperature and Pressure 22.4 L of Chlorine gas Cl2 will have a mass of:
a) 35.45g
b) 22.4g
c) 28.0g
d) 70.9g
6)
What is the intermolecular force that makes the molecules of iodine interact and is responsible for the fact
that iodine is solid at room temperature?
a) Covalent Bond b) Ionic Bond c) Hydrogen Bond d) London Induced Dipole-Induced Dipole Forces
d) suspension
118
7)
25 g of methanol are disolved in 100.0 mL of water. What is the w/v % concentration of the solution?
a) 20%
b) 25%
c) 75%
d) 80%
8)
The molecular shape of the methane molecule (CH4) is best described as:
a) linear
b) trigonal planar
c) trigonal pyramidal
9)
How many grams of AgNO3 are required to make 1.00 L of a 0.100 M solution?
a) 0.100 g
b) 85.0 g
c) 8.50 g
d) 17.0 g
10)
Which substance has non-polar covalent bonds, and is overall non-polar?
a) O2
b) CCl4
c) NaCl
d) CO
11)
When red blood cells are placed into deionized water they will undergo ____since deionized water is ____
a) hemolysis/hypertonic b) hemolysis/hypotonic c) crenation/hypertonic d) crenation/hypotonic
12)
Unsaturated hydrocarbons have:
a) only C-C bonds
c) no C=C bonds
13)
The formula CnH2n corresponds to:
a) Alkanes
b) Alkenes
14)
Alcohol vaporization is a(n)___________process
a) Exothermic
b) Endothermic
d) tetrahedral
b) one or more C=C bonds or C≡C bonds
d) an odd number of carbon atoms
c) Alkynes
c) Chemical
d) Alcohols
d) all of the above
15)
When a given quantity of gas is kept at stable temperature and the pressure is increased
a) Volume will increase b) Volume will decrease c) Volume will be always 22.4Ld)number of moles changes
16)
Which one of the following compounds is an isomer of heptane
a) cyclohexane
b) 2,2-dimethylbutane
c) 2,2-dimethylpentane
17)
The following structures could be described as:
H
H
C
H 3C
a) isomers
18)
CH3
H
C
C
CH2 CH3
d)methylcyclopentane
C
H
H 3C
b) different conformations of the same compound
c) alkynes
d) None of the above
What is the correct name for the following structure:
a) 2-ethyl butane
b) 2-methyl pentane
c) 3-methyl pentane
d) 3-methyl hexane
19)
Which of the following substances is an electrolyte?
a) HCl
b) NaCl
c) NH4NO3
20)
A general statement concerning the solubility of organic compounds is _____
a) the larger molecules dissolve best in a solvent with a low molecular weight.
b) those compounds that have only covalent bonds dissolve well in water.
c) the polar organic compounds dissolve best in non-polar solvents.
d) the nonpolar compounds can dissolve well in non-polar polar solvents.
21)
What is the approximate F-B-F angle observed in the BF3 molecule?
a) 90°
b) 105°
c) 120°
d) 180°
22)
The least electronegative element of the following is
a) Sodium
b) Hydrogen
23)
The electronic structure of SO3 is __________and the molecular structure is _____________
a) tetrahedral, bent
b) tetrahedral, pyramidal
c) trigonal planar, bent
d) trigonal planar, trigonal planar
24)
Two identical gas containers containing N2 and O2 have the exact same number of moles, but the O2 is stored
at 20°C while the N2 container is stored at 40°C. Which of the following statements is true?
a) The molecules of the two gases have the same kinetic energy
b) P(for N2) = 2 x P(for O2)
c) The two gases are different so we cannot apply gas laws to compare their pressures
d) The oxygen container is heavier
c) Carbon
d) All are electrolytes
d) Chlorine
25)
How much sodium chloride do you need to prepare 740 mL of a 0.9% saline (m/v) NaCl solution for IV
therapy?
a) 3g
b) 7g
c) 20g
d) 40g
26)
Which of the following statements is NOT true concerning organic chemistry?
a) Some organic compounds can be made from inorganic compounds.
b) Organic chemistry is the chemistry of chemicals originating from living organisms.
c) Organic chemistry is the chemistry of carbon-containing compounds.
d) Of the more that 20 million known chemical compounds, the vast majority are organic compounds.
27)
Hydrocarbons with only single bonds are called _____. Those with a triple bond are called _____, and those
with a double bonds are called _____.
a) alkanes, alkenes, alkynes
b) alkenes, alkynes, alkanes
c) alkanes, alkynes, alkenes
d) alkenes, alkanes, alkynes
28)
Name the compound, CH3CH=CHCH3.
a) Butane
b) 1-Butene
c) 2-Butene
29)
Hydrogen in hydrocarbons:
a) forms ionic compounds
c) bonds to carbon and forms chains
b) forms 1 covalent bond to a C atom
d) bonds to hydrogen by covalent bonds
30)
Propene, benzene, acetylene, and 2-butene are all examples of
a) alkenes
b) alkanes
c) unsaturated hydrocarbons
31)
A molecular formula of an alkene is
a) C7H16
b) C9H18
32)
Calculate the Pressure of 15L of gas, at the temperature of 20oC, if its pressure at 50oC is 2.00 Atm.
a) 2.20 Atm
b) 1.81 Atm
c) 5.00 Atm
d) 0.80 Atm
33)
2-methylbutane and 2,2’-dimethyl-propane are:
a) Conformations
b) Isotopes
34)
Which of the following is the formula for 1-butyne?
a) CH3CH2CH2CH3
b) CH2=CHCH2CH3
35)
What would be the proper name for the following compound? Identify and number the longest chain
correctly!
c) C5H8
c) Isomers
d) CH2=CHCH3
d) 2-Butyne
d) aromatic compounds
d) C6H6
d) None of the above
d) None of the above
CH3
CH2 CH3
H 2C
H 3C
CH
C
H2
CH
CH
CH3
CH3
a) 2,4,6-trimethyl-undecane b) 3,5,7-trimethyl-decane c) 2,4,6-trimethyl-octane d) 2-ethyl,4,6-dimethylheptane
36)
What would the following equation can be described as: PV = nRT
a) the law of conservation of matter
b) The ideal gas law
c) the periodic law of the elements
d) Boyle’s law
37)
The main component(s) of gasoline is (are):
a) hydrocarbons
b) carbohydrates
38)
Standard Temperature and Pressure is
a) 37oC and 1.01 Atm
b) 25oC and 1 Atm
39)
To prepare 5.00 mL of a 0.200 M solution of Potassium Chloride in water you will need to dissolve
a) 7.46 mg
b) 74.6 mg
c) 746 mg
d) None of the above
40)
Dienes have to contain
a) Triple bonds
b) At least two double bonds
This is an EASY EXAM! GOOD LUCK:)
c) elemental carbon
d) ionic compounds
c) 100oC and 1 Atm d) 0oC and 1 Atm
c) Single bonds only
d) The benzene ring