chemistry, science

PLEASE JUST CHECK THE ATTACHMENT IN THE FILES.Why is oxygen reduced in the reaction of hydrogen with oxygen to make water?

Oxygen pulls electrons toward itself.

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Oxygen pushes electrons toward the hydrogens.

Oxygen absorbs a proton.

Which term describes the following process?
2Fe(s) + O2(g) + 2H2O(l) ? 2Fe(OH)2(s)
4Fe(OH)2(s) + O2(g) +2H2O(l) ? 4Fe(OH)3(s)

salt hydrolysis

electrolysis

corrosion

The half-reaction method is particularly useful for balancing redox equations.

true

false

A spontaneous reaction causes current to flow in an electrolytic cell.

true

false

Which of the following chemical equations represents an oxidation-reduction reaction?

Mg(OH)2 + 2HCl ? MgCl2 + 2H2O

BiCl2 + Na2SO4 ? 2NaCl + BiSO4

CH4+2O2?CO2+2H2O

Identify the products formed in the net reaction of the electrolysis of water.

liquid hydrogen and oxygen gas

liquid oxygen and hydrogen gas

hydrogen gas and oxygen gas

The gas produced at the cathode in the electrolysis of brine is _________.

chlorine

oxygen

hydrogen

____ 8.
____ 9.
____ 10.
____ 11.
____ 12.
____ 13.
____ 14.
____ 15.
____ 16.
H is oxidized and Cl is reduced in this reaction.
2ClO- +H2 +2e- ?2Cl- +2OH-

true

false

In which of the following species is the oxidation number of sulfur less than 6?

SO3

NaSO4

SO2

A proton is transferred between a conjugate acid-base pair.

true

false

A Lewis base is a substance that can _________.

accept a pair of electrons

donate a pair of electrons

donate a hydrogen ion

Which combination of acid and salt in aqueous solution would form a buffer?

carbonic acid and sodium carbonate

hydrochloric acid and potassium chloride

sulfuric acid and calcium sulfate

Which type of solution is one with a pH of 7?

acidic

basic

neutral

The formula of the ammonium ion is written as _________.
a.
b.
c.
H3O+
H+
NH4+
A highly active metal is most easily oxidized.

true

false

When an acid reacts with a base, what compounds are formed?

a salt and water

water only

a salt only
chem_progresstes_2.pdf

Unformatted Attachment Preview

Course Name: Chemistry 2
Student: Omar Hassan
Course ID: SCIH032062
ID: E93324820
Submittal: 52
Progress Test 2
This Progress Test covers the course materials that were assigned in Units 3 and 4. Although the progress test is
similar in style to the unit evaluations, the progress test is a closed-book test. It is important that you do your own work.
Select the response that best completes the statement or answers the question.
You may use a calculator on this progress test. A periodic table has been included for your reference.
____ 1.
Why is oxygen reduced in the reaction of hydrogen with oxygen to make water?
a.
b.
c.
____ 2.
Which term describes the following process?
2Fe(s) + O2(g) + 2H2O(l) ? 2Fe(OH)2(s)
4Fe(OH)2(s) + O2(g) +2H2O(l) ? 4Fe(OH)3(s)
a.
b.
c.
____ 3.
____ 6.
true
false
Which of the following chemical equations represents an oxidation-reduction reaction?
a.
Mg(OH)2 + 2HCl ? MgCl2 + 2H2O
b.
BiCl2 + Na2SO4 ? 2NaCl + BiSO4
c.
CH4 + 2O2 ? CO2 + 2H2O
Identify the products formed in the net reaction of the electrolysis of water.
a.
b.
c.
____ 7.
true
false
A spontaneous reaction causes current to flow in an electrolytic cell.
a.
b.
____ 5.
salt hydrolysis
electrolysis
corrosion
The half-reaction method is particularly useful for balancing redox equations.
a.
b.
____ 4.
Oxygen pulls electrons toward itself.
Oxygen pushes electrons toward the hydrogens.
Oxygen absorbs a proton.
liquid hydrogen and oxygen gas
liquid oxygen and hydrogen gas
hydrogen gas and oxygen gas
The gas produced at the cathode in the electrolysis of brine is _________.
a.
b.
c.
chlorine
oxygen
hydrogen
____ 8.
H is oxidized and Cl is reduced in this reaction.
2ClO- + H2 + 2e- ? 2Cl- + 2OHa.
b.
____ 9.
true
false
In which of the following species is the oxidation number of sulfur less than 6?
a.
SO3
b.
NaSO4
c.
SO2
____ 10. A proton is transferred between a conjugate acid-base pair.
a.
b.
true
false
____ 11. A Lewis base is a substance that can _________.
a.
b.
c.
accept a pair of electrons
donate a pair of electrons
donate a hydrogen ion
____ 12. Which combination of acid and salt in aqueous solution would form a buffer?
a.
b.
c.
carbonic acid and sodium carbonate
hydrochloric acid and potassium chloride
sulfuric acid and calcium sulfate
____ 13. Which type of solution is one with a pH of 7?
a.
b.
c.
acidic
basic
neutral
____ 14. The formula of the ammonium ion is written as _________.
a.
H3O+
b.
H+
c.
NH4+
____ 15. A highly active metal is most easily oxidized.
a.
b.
true
false
____ 16. When an acid reacts with a base, what compounds are formed?
a.
b.
c.
a salt and water
water only
a salt only
____ 17. The pH of a sample of coffee is 5.0. A sample of milk has a pH of 6.0. Compared to the [H+]of milk the [H+]
of the coffee is _________.
a.
b.
c.
1.0 times higher
10 times higher
10 times lower
____ 18. Which of these processes is not an oxidation?
a.
b.
c.
A decrease in oxidation number
A gain of oxygen
A complete loss of electrons
____ 19. Zinc is oxidized in a graphite dry cell battery.
a.
b.
true
false
____ 20. Which of these compounds is an Arrhenius acid?
a.
b.
LiOH
NH3
c.
H3PO4
____ 21. What balances charges that build up as reduction and oxidation occur in a voltaic cell?
a.
b.
c.
the salt bridge
one of the half-cells
the moving electrons
____ 22. In reference to solutions of strong acids and strong bases, the word strong refers to the molarity.
a.
b.
true
false
____ 23. Which of the general types of reactions is not a redox reaction?
a.
b.
c.
single replacement
double replacement
combination
____ 24. If the cell potential for a redox reaction is negative,
a.
b.
c.
the redox reaction is spontaneous.
the redox reaction is not spontaneous.
the reaction only occurs during electrolysis.
____ 25. The electrode in the center of the most common dry cells are made of copper.
a.
b.
true
false
____ 26. Positive ions move to the cathode in which which of the following processes?
a.
b.
c.
Electrolysis
Oxidation
Hydrolysis
____ 27. In the following unbalanced reaction, which atom is reduced?
HNO3 + HBr ? NO2 + Br2 + H2O
a.
b.
c.
hydrogen
nitrogen
bromine
____ 28. What is the oxidizing agent in the following reaction?
CH4 + 2O2 ? CO2 + 2H2O
a.
CH4
b.
O2
c.
CO2
____ 29. In the reaction of hydrogen with iodine, which is the reducing agent?
a.
b.
c.
hydrogen
iodine
hydrogen ion
____ 30. Hydrogen is reduced in a hydrogen-oxygen fuel cell.
a.
b.
true
false
____ 31. The oxidation number of hydrogen when it is in a compound other than a hydride is _________.
a.
b.
c.
–1
+1
0
____ 32. SO2 is the reducing agent in the following reaction.
MnO4- + SO2 ? Mn+2 + SO4-2
a.
b.
true
false
____ 33. Which of the following is an oxidation half-reaction?
a.
Cl2 + 2e- ? 2Cl-
b.
Na ? Na+ + 1e-
c.
2H+ + 2e- ? H2
____ 34. If an atom is oxidized in a redox reaction, what must happen to another atom in the system?
a.
b.
c.
It must be oxidized.
It must be reduced.
It must be neutralized.
____ 35. The first electrochemical cell was invented by Benjamin Franklin.
a.
b.
true
false
____ 36. Acids are considered nonelectrolytes.
a.
b.
true
false
____ 37. Why can’t a lead storage battery be recharged indefinitely?
a.
b.
c.
A direct current must pass through the cells.
The electrodes lose lead sulfate.
It is difficult to reverse the direction of current flow.
____ 38. What is the standard cell potential of this cell? This cell is built using two electrodes:
Zn2+ + 2e ? Zn
E° = -0.76V
Ba2+ + 2e ? Ba
E° = -2.90V
a.
b.
c.
E°cell = -3.66V
E°cell = -2.14V
E°cell = +2.14V
____ 39. A strong acid or base can be described as an indicator.
a.
b.
true
false
____ 40. Hydrogen is produced at the anode and oxygen at the cathode when a current is applied to two electrodes
immersed in pure water.
a.
b.
true
false
____ 41. Which of the following is the name of a process in which electrical energy causes a chemical reaction?
a.
b.
c.
hydrolysis
electrolysis
oxidation
____ 42. What is the best description for a solution with a hydrogen-ion concentration equal to 1 x 10-5 M?
a.
b.
c.
acidic
basic
neutral
____ 43. Mercury’s ions are easily oxidized.
a.
b.
true
false
____ 44. How much H2SO4 is needed to neutralize 1 liter of a 0.50M solution of NaOH ?
a.
b.
c.
0.25 mol
0.50 mol
1.0 mol
____ 45. In which of the following types of reaction are electrons gained?
a.
b.
c.
decomposition
oxidation
reduction
____ 46. Which pH value could represent the equivalence point of the titration of a strong base and a strong acid?
a.
b.
c.
pH 9
pH 7
pH 5
____ 47. Which ion or molecule is the conjugate base of the ammonium ion, NH4+
a.
H3O+
b.
NH3
c.
OH-
____ 48. Which of these solutions is closest to neutral?
a.
[H+] = 1 x 10-6M
b.
[OH-] = 1 x 10-3M
c.
[H+] = 1 x 10-9M
____ 49. Titration is the process of adding a known amount of solution of known concentration to determine the
concentration of another solution called?
a.
b.
true
false
____ 50. What is the formula for nitric acid?
a.
HNO3
b.
H3NO
c.
H3N
Carefully review your answers on this progress test and make any corrections you feel are necessary. When
you are satisfied that you have answered the questions to the best of your ability, transfer your answers to the
online test submission page in the presence of your proctor.
The University of Nebraska is an equal opportunity educator and employer. ©2018, The Board of Regents of the
University of Nebraska. All rights reserved.
1
2
8
18
18
8
1
2
8
18
8
1
2
8
8
1
2
8
1
2
1
1
(223)
Fr
87
2
8
18
32
18
8
Francium 1
Cesium
132.91
Cs
55
Rubidium
85.468
Rb
37
Potassium
39.098
K
19
Sodium
22.990
Na
11
Lithium
6.941
Li
3
Hydrogen
1.0079
H
1
1A
Be
Mg
Ca
Sr
Radium
(226)
Ra
88
Barium
137.33
Ba
56
Strontium
87.62
38
Calcium
40.08
20
2
8
8
2
2
8
2
2
2
2
8
18
32
18
8
2
2
8
18
18
8
2
2
8
18
8
2
Magnesium
24.305
12
Beryllium
9.0122
4
2A
2
Sc
Y
Lu
(262)
Lr
2
8
18
32
9
2
2
8
18
9
2
2
8
18
32
32
9
Lawrencium 2
103
Lutetium
174.97
71
Yttrium
88.906
39
Scandium
44.956
21
Ti
Zr
Hf
(227)
Ac
89
2
8
18
32
18
9
Actinium 2
Actinide Series
Lanthanum
138.91
La
57
2
8
18
18
9
2
V
23
Nb
Ta
2
8
11
2
2
8
18
32
11
2
2
8
18
12
1
232.04
Th
2
8
18
20
8
2
2
8
18
32
18
10
Thorium 2
90
Cerium
140.12
Ce
58
(262)
Db
105
2
8
18
32
32
11
Dubnium 2
Tantalum
180.95
73
Niobium
92.906
41
Vanadium
50.941
Lanthanide Series
(261)
Rf
2
8
18
32
10
2
2
8
18
10
2
2
8
10
2
2
8
18
32
32
10
Rutherfordium 2
104
Hafnium
178.49
72
Zirconium
91.22
40
Titanium
47.90
22
4
4B
3
3B
2
8
9
2
Noble Gases
Nonmetals
Metalloids
5B
Cr
Mo
2
8
18
13
1
2
8
13
1
W
Pr
231.04
Pa
2
8
18
21
8
2
2
8
18
32
20
9
Protactinium 2
91
140.91
Praseodymium
59
(263)
Sg
2
8
18
32
12
2
2
8
18
32
32
12
Seaborgium 2
106
Tungsten
183.85
74
Molybdenum
95.94
42
Chromium
51.996
24
6B
6
Mn
Tc
2
8
18
14
1
2
8
13
2
Re
Nd
2
8
18
22
8
2
238.03
U
2
8
18
32
21
9
Uranium 2
92
Neodymium
144.24
60
(264)
Bh
2
8
18
32
13
2
2
8
18
32
32
13
Bohrium 2
107
Rhenium
186.21
75
Technetium
(98)
43
Manganese
54.938
25
7B
7
Inner transition metals
Alkaline Earth Metals
Other Metals
Transition Metals
5
Transition Elements
Alkali Metals
Representative Elements
Ru
Os
Pm
(237)
Np
2
8
18
23
8
2
2
8
18
32
22
9
Neptunium 2
93
Promethium
(145)
61
(265)
Hs
2
8
18
32
14
2
2
8
18
15
1
2
8
18
32
32
14
Hassium 2
108
Osmium
190.2
76
Ruthenium
101.07
44
Iron
55.847
Fe
2
8
14
2
Rh
Ir
Sm
(244)
Pu
2
8
18
24
8
2
2
8
18
32
24
8
Plutonium 2
94
Samarium
150.4
62
(268)
Mt
2
8
18
32
15
2
2
8
18
16
1
2
8
15
2
2
8
18
32
32
15
Meitnerium 2
109
Iridium
192.22
77
Rhodium
102.91
45
Cobalt
58.933
Co
27
8B
9
Not found
in nature
Tc
26
8
Gas
Liquid
Solid
He
Br
C
Si
Pd
Pt
2
8
18
32
17
1
2
8
18
18
2
8
16
2
Eu
(243)
Am
2
8
18
25
8
2
2
8
18
32
25
8
Americium 2
95
Europium
151.96
63
(269)
Ds
110
2
8
18
32
32
17
Darmstadtium 1
Platinum
195.09
78
Palladium
106.4
46
Nickel
58.71
Ni
28
10
Silicon
28.086
14
2
8
18
32
18
1
2
8
18
18
1
2
8
18
1
*
12
Cd
Hg
Ununbium
(277)
Gd
Curium
(247)
Cm
96
Gadolinium
157.25
64
2
8
18
32
25
9
2
2
8
18
25
9
2
Tb
(247)
Bk
2
8
18
27
8
2
2
8
18
32
32
18
2
2
8
18
32
18
2
2
8
18
18
2
2
8
18
2
2
8
18
32
27
8
Berkelium 2
97
Terbium
158.93
65
* Name not officially assigned.
(272)
112
Mercury
200.59
80
Cadmium
112.41
48
Zinc
65.38
Zn
30
2B
Uuu Uub
111
Gold
196.97
Au
79
Silver
107.87
Ag
47
Copper
63.546
Cu
29
1B
11
Average
atomic mass
Element name
Element symbol
Electrons in each
energy level
2
8
18
32
32
18
Unununium 1
*
2
8
4
Atomic number
Figure 6.9 Periodic Table of the Elements
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
68
2
3
Al
In
Tl
Dy
(251)
Cf
2
8
18
28
8
2
2
8
18
32
18
3
2
8
18
18
3
2
8
18
3
2
8
3
2
8
18
32
28
8
Californium 2
98
Dysprosium
162.50
66
Thallium
204.37
81
Indium
114.82
49
Gallium
69.72
Ga
31
Aluminum
26.982
13
*
Si
Ge
Ho
2
8
18
32
18
4
2
8
18
18
4
(252)
Es
2
8
18
29
8
2
2
8
18
32
29
8
Einsteinium 2
99
Holmium
164.93
67
2
8
4
2
4
2
8
18
4
Ununquadium
114
Uuq
Lead
207.2
Pb
82
Tin
118.69
Sn
50
Germanium
72.59
32
Silicon
28.086
14
C
Carbon
12.011
B
6
Boron
10.81
5
14
4A
13
3A
15
N
P
As
Sb
Bi
Er
(257)
Fm
2
8
18
30
8
2
2
8
18
32
18
5
2
8
18
18
5
2
8
18
5
2
8
5
2
5
2
8
18
32
30
8
Fermium 2
100
Erbium
167.26
68
Bismuth
208.98
83
Antimony
121.75
51
Arsenic
74.922
33
Phosphorus
30.974
15
Nitrogen
14.007
7
5A
16
O
S
Se
Te
Po
(258)
Md
2
8
18
31
8
2
2
8
18
32
18
6
2
8
18
18
6
2
8
18
6
2
8
6
2
6
2
8
18
32
31
8
Mendelevium 2
101
Thulium
168.93
Tm
69
Polonium
(209)
84
Tellurium
127.60
52
Selenium
78.96
34
Sulfur
32.06
16
Oxygen
15.999
8
6A
17
F
Cl
Br
At
Yb
(259)
No
2
8
18
32
8
2
2
8
18
32
18
7
2
8
18
18
7
2
8
18
7
2
8
7
2
7
2
8
18
32
32
8
Nobelium 2
102
Ytterbium
173.04
70
Astatine
(210)
85
Iodine
126.90
I
53
Bromine
79.904
35
Chlorine
35.453
17
Fluorine
18.998
9
7A
18
Kr
Radon
(222)
Rn
86
Xenon
131.30
Xe
54
Krypton
83.80
36
Argon
39.948
Ar
18
Neon
20.179
Ne
10
Helium
4.0026
He
2
8A
2
8
18
32
18
8
2
8
18
18
8
2
8
18
8
2
8
8
2
8
2
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