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WorksheetsChem Mod 4 Electrons in the Atom Test Review
Total questions: 36
Worksheet time: 25mins
Name
Class
Date
1.
Lowest allowable energy state of an atom
a)
Excited state
b)
Ground state
c)
Bohr Model
d)
Photon
2.
d sublevel
a)
l = 0
b)
l = 1
c)
l = 2
d)
l = 3
3.
Minimum amount of energy that can be lost or gained by an atom
a)
Photon
b)
Quantum
c)
Excited State
d)
Ground State
4.
The highest energy color of visible light
a)
Red
b)
Violet
c)
Blue
d)
Green
5.
Lowest energy color of light
a)
Violet
b)
Red
c)
Blue
d)
Green
6.
s sublevel
a)
l = 0
b)
l = 1
c)
l = 2
d)
l = 3
7.
All moving particles have wavelike characteristics
a)
de Broglie Equation
b)
Heisenberg Uncertainty Principle
c)
Schrodinger Equation
d)
Pauli Exclusion Principle
8.
Impossible to know the position and particle of a particle
a)
de Broglie Equation
b)
Heisenberg Uncertainty Principle
c)
Schrodinger Equation
d)
Pauli Exclusion Principle
9.
p sublevel
a)
l = 0
b)
l = 1
c)
l = 2
d)
l = 3
10.
3.00 x 108 m/s
a)
Speed of light
b)
Planck's Constant
c)
de Broglie Equation
d)
Schrodinger Equation
11.
f sublevel
a)
l = 0
b)
l = 1
c)
l = 2
d)
l = 3
12.
6.626 x 10-34 J⋅s
a)
Speed of light
b)
Planck's constant
c)
Schrodinger Equation
d)
de Broglie Equation
13.
Electrons fill the lowest energy orbital available
a)
Aufbau Principle
b)
Heisenberg Uncertainty
c)
Pauli Exclusion Principle
d)
Hund's Rule
14.
Carries a quantum of energy
a)
Atomic orbital
b)
Electron
c)
Photon
d)
Speed of light
15.
Electrons are emitted from a metals surface when it is struck by a specific frequency of light
a)
Aufbau Principle
b)
Photoelectric effect
c)
Pauli exclusion principle
d)
Hund's Rule
16.
There can only be a maximum of 2 electrons in an orbital
a)
Atomic orbital
b)
Pauli exclusion principle
c)
de Broglie Equation
d)
Hund's rule
17.
When an atom gains energy
a)
Excited state
b)
Ground state
c)
Bohr Model
d)
Photon
18.
An electrons probable location
a)
Atomic Orbital
b)
Bohr Model
c)
Quantum
d)
Heisenberg Uncertainty Principle
19.
Lowest energy color of visible light
a)
Violet
b)
Red
c)
Green
d)
Blue
20.
Identify the element with the following quantum numbers (4, 2, -2, +1/2)
a)
Yttrium
b)
Ruthenium
c)
Scandium
d)
Manganese
21.
The maximum number of electrons in the 6th energy level is
a)
72
b)
36
c)
8
d)
18
22.
[Ar]4s23d8
a)
Ni
b)
Cu
c)
Pd
d)
Does not exist
23.
Wavelength and frequency have a(n) ______ relationship
a)
Inverse
b)
Direct
24.
Energy and frequency have a(n) _____ relationship
a)
inverse
b)
direct
25.
Select the correct set of quantum numbers for Eu
a)
(4,3,2,+1/2)
b)
(4,2,2,-1/2)
c)
(4,3,-2,+1/2)
d)
4,2,-2,-1/2)
26.
What does the quantum number n represent?
a)
energy level
b)
sublevel
c)
orbital
d)
spin
27.
What does the quantum number l represent?
a)
energy level
b)
sublevel
c)
orbital
d)
spin
28.
What does the quantum number ml represent?
a)
energy level
b)
sublevel
c)
orbital
d)
spin
29.
What does the quantum number ms represent?
a)
energy level
b)
sublevel
c)
orbital
d)
spin
30.
Which of the following is a Noble gas?
a)
Rn
b)
Cd
c)
Sr
d)
Lu
31.
Calculate the energy of a violet light photon with a frequency of 6.6x1014 Hz
a)
4.4x10-19 J
b)
4.4 J
c)
4.5x10-14 J
d)
4.5 J
32.
What is the wavelength of a ray with a frequency of 8.89x1021 Hz?
a)
3.37x10-14 m
b)
3.4x10-14 m
c)
5.89x10-12 m
d)
5.9x10-12 m
33.
The photoelectric effect says that sodium metal requires light with an energy of 4.41x10-19 J in order to eject an electron. Does blue light (wavelength = 471 nm) have enough energy to eject the electron from the metal?
a)
Yes, its energy is 4.41x10-19 J
b)
No, its energy is 4.22x10-19 J
c)
No, its energy is 3.46x10-19 J
d)
No, its energy is 3.10x10-19 J
34.
What is the energy level the valence electrons in F are found in?
a)
1
b)
2
c)
3
d)
Need more information
35.
The electrons found in the outermost energy level
a)
valence electrons
b)
ground state electrons
c)
excited electrons
d)
de Broglie Equation
36.
How many valence electrons does Se have?
a)
4
b)
6
c)
5
d)
3
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