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Test 4 Review

Total questions: 93

Worksheet time: 3hrs 2mins

Name
Class
Date
1.

What is the shorthand configuration for Lead?

a)

[Xe]6s24f145d106p2

b)

[Xe]6s25d106p2

c)

[Rn]6s25d106p2

d)

[Rn]6s24f145d106p2

2.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
3.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
4.

How many valence electrons does Silicon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

5.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
6.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
7.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
8.

How many valence electrons does Lithium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

9.
What is the total number of energy levels used by an atom of aluminum
(Al, atomic #13) in the ground state?
a)
3
b)
7
c)
13
d)
0
10.
This "rule" of Quantum Chemistry states that it is impossible to know both the position and velocity of an electron at the same time.
a)
Hund's Rule
b)
Heisenberg Uncertainty Principle
c)
Aufbau Principle
d)
Pauli Exclusion Principle
11.
Identify the following element:
1s22s22p63s23p64s23d10
a)
nickel
b)
copper
c)
zinc
d)
gallium
12.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
13.
The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?
a)
0
b)
3
c)
5
d)
7
14.

How many valence electrons does Boron Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

15.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
16.
How many valence electrons are in an atom of sulfur?
a)
2
b)
4
c)
6
d)
8
17.
I am an element in the 3rd row of the periodic table...I have one unpaired electron in my last sublevel...I have 3 valence electrons...who am I?
a)
Na
b)
Al
c)
Cl
d)
Ar
18.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
19.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
20.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 47 oC?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
21.
At 250 k and 1.75 atm, a gas has a mass of 15.3 g and occupies 5.60 L. What is the molar mass of the gas?
M=mRT/PV
a)
32.04
b)
42.15
c)
48.91
d)
54.28
22.
Find the density of Neon gas at .725 atm and 25°C 
D=MP/RT
a)
.35
b)
.47
c)
.60
d)
.79
23.
What volume does 13.6 g of O2 gas at 37°C and 135 kPa occupy?
PV=nRT
a)
6.22 L
b)
8.11 L
c)
10.54 L
d)
12.73 L
24.

Which of the following quantities of substance contain 6 x 1022 molecules?

[Relative atomic mass: H, 1; C, 12; O, 16; Avogadro’s Constant: 6 X 1023 mol -1]

I 1.8 g water

II 1.0 g hydrogen gas

III 3.2 g oxygen gas

IV 4.4 g carbon dioxide

a)

I and II only

b)

III and IV only

c)

I, III, and IV only

d)

I, II, III, and IV

25.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
26.
You have 3.5 L of H2 (g) at STP. How many moles of gas are there?
a)
22.4 mol
b)
22.4 L
c)
0.16 mol
d)
0.16 L
27.

How many liters of NH3 are needed to react completely with 30.0L of NO?

4NH3(g) + 6NO (l)--> 5N2 (g) + 6H2O (l)

a)

5.0 L

b)

20.0 L

c)

7.5 L

d)

120.0 L

28.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

29.

2CO + O2 −-> 2CO2

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

0.0199

30.
Which scientist developed the atomic theory?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
James Chadwick
31.
JJ Thomson's theory was nicknamed _______.
a)
Billiard Ball Theory
b)
Solar System Theory
c)
Electron Cloud
d)
Plum Pudding
32.
Who discovered the proton?
a)
Thomson
b)
Dalton
c)
Bohr
d)
Rutherford
33.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
34.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
35.
James Chadwick discovered the ________.
a)
proton
b)
neutron
c)
electron
d)
nucleus
36.
Who believed that all matter is made up of small particles called atoms?
a)
Dalton
b)
Rutherford
c)
Bohr
d)
Chadwick
37.
What did Thomson discover?
a)
electron
b)
proton
c)
neutron
d)
electron cloud
38.
What does this image represent
a)
Billiard Ball
b)
Solar System
c)
Plum Pudding
d)
Electron Cloud
39.
This scientist believed that electrons orbit the nucleus.
a)
Dalton
b)
Bohr
c)
Rutherford
d)
Chadwick
40.
The Gold Foil experiment was done by __________.
a)
Chadwick
b)
Bohr
c)
Rutherford
d)
Thomson
41.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
Thomson
b)
Rutherford
c)
Dalton
d)
Democritus
42.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
43.
This scientist performed the Cathode Ray Tube experiment and proposed the Plum Pudding Model of the atom
a)
Dalton
b)
Chadwick
c)
Thomson
d)
Democritus
44.
His model of the atom is referred to as the Nuclear atom.
a)
Chadwick
b)
Dalton
c)
Rutherford
d)
Robert Millikan
45.
"Everything is composed of atoms" was stated by:
a)
Democritis
b)
Dalton
c)
Moseley
d)
Einstein
46.
The scientist responsible for the oil drop experiment was:
a)
Democritis
b)
Dalton
c)
Millikin
d)
De Broglie
47.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
48.
The impossibility to know simultaneously the exact position and momentum of a particle is called the:
a)
Einstein Uncertainty Principle
b)
Moseley Uncertainty Principle
c)
Heisenburg Uncertainty Principle
d)
Bohr Uncertainty Principle
49.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
50.
The nucleus of an atom can be described as:
a)
spacious and negatively charged
b)
dense and positively charged
c)
spacious and positively charged
d)
dense and negatively charged
51.
The subatomic particles that factor into atomic mass are:
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
protons, neutrons, and electrons
52.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
53.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
54.

Which electron configuration belongs to Cl-?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3s2 3p4

55.

What is the short hand configuration for silicon?

a)

[Ar]2s22p2

b)

[Ne]2s22p2

c)

[Ne]3s23p2

d)

[Ne]3s23p4

56.

How many electrons does iron have in the 3rd energy level?

a)

2

b)

6

c)

8

d)

14

57.

What is the short hand configuration for iodine?

a)

[Ar]4s23d6

b)

[Ne]4s23d6

c)

[Kr]5s24d105p5

d)

[Kr]4s24d104p5

58.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

59.

Each orbital can hold how many electrons?

a)

5

b)

4

c)

8

d)

2

60.

In an electron configuration, what follows 4s?

a)

4p

b)

3d

c)

4s

d)

2f

61.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
62.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
63.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
64.

Choose the Noble Gas that you would use to begin the shorthand configuration of the following element.

Plutonium (Pu)

a)

[Xe]

b)

[Ne]

c)

[Rn]

d)

[Kr]

65.

What is the shorthand configuration for Tin?

a)

[Xe]5s24d105p2

b)

[Xe]5s24d105p2

c)

[Kr]5p2

d)

[Kr]5s24d105p2

66.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

67.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
68.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
69.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
70.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

71.

The characteristic color bands that a hot, dilute gas emits when viewed with a spectroscope are called...

a)

emission spectra

b)

absorption spectra

c)

continuous spectra

d)

black body radiation

72.
The shortest wavelength in visible light is______.
a)
violet
b)
red
c)
blue
d)
yellow
73.
_____ have the longest wavelengths and lowest frequencies of all electromagnetic waves.
a)
microwaves
b)
radio waves
c)
gamma rays
d)
ultraviolet
74.
_______ carry the greatest amount of energy. 
a)
x-rays
b)
gamma rays
c)
infrared rays
d)
visible light
75.

The _____ determines the color of visible light.

a)

wavelength

b)

speed

c)

amplitude

d)

light

76.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
77.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
78.

An electron transitions from n = 6 to n = 3. Which wavelength is released?

a)

410 nm

b)

1875 nm

c)

1282 nm

d)

1094 nm

79.

An electron in n=4 has more _______ than an electron in n=2

a)

Stability

b)

Energy

c)

Spin

d)

Wave nature

80.

What color visible light is released when an electron transitions from n = 3 to n = 2?

a)

Red

b)

Blue

c)

Violet

d)

Green

81.

Which electron transition is associated with a higher energy wave?

a)

n = 4 to n = 3

b)

n = 4 to n = 2

c)

n = 4 to n = 1

82.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
83.

Four gas spectra are given. What gases are in the unknown mixture?

a)

Gas B & Gas D

b)

Gas C & Gas B

c)

Gas A & Gas D

d)

Gas D & Gas C

84.
As the wavelength of a wave increases, which is also true?
a)
The energy of the wave will increase.
b)
The speed of the wave will increase.
c)
The frequency of the wave will decrease.
d)
Planck's constant will decrease.
85.
Radio station A broadcasts a signal with a frequency of 98.7 MHz, and radio station B broadcasts a signal with a frequency of 100.3 MHz.  What can be said about the relationship of signal A to signal B?
a)
Signal A and signal B have the same energy.
b)
Signal A has more energy than signal B.
c)
Signal A has a shorter wavelength than signal B.
d)
Signal A has a longer wavelength than signal B.
86.
Which two factors of the electromagnetic radiation have an inverse relationship?
a)
amplitude and nodes
b)
energy and frequency
c)
frequency and wavelength
d)
wavelength and energy
87.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
88.
What happens to the energy of a photon as the frequency of the wave increases? 
a)
The energy increases
b)
The energy decreases
c)
The energy stays the same 
89.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
90.
What is the wavelength for a quantum of light with energy of 7.56x10-19J? (λ=hc/E) 
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
91.
What is the frequency of a light that has the Energy of 2.84x10-19. (v=E/h)
a)
4.30x1014Hz
b)
4.30x10-14Hz
c)
4.30x10-54Hz
d)
4.30x1054Hz
92.
What is the frequency of a light that has the Energy of 2.84x10-19. (v=E/h)
a)
4.30x1014Hz
b)
4.30x10-14Hz
c)
4.30x10-54Hz
d)
4.30x1054Hz
93.
What is the Energy of a blue light with the frequency of 6.91x1014Hz? (E=hv)
a)
4.56x1049J
b)
9.55x10-49J
c)
4.56x10-19J
d)
5.82x1019J

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