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WorksheetsCh 4: Modern Atomic Theory
Total questions: 35
Worksheet time: 31mins
Name
Class
Date
1.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency?
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
2.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
3.
Select the correct order of waves on the EMS
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
4.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
5.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
6.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude
7.
What is a photon?
a)
When radiation burst through electric waves
b)
The emission of electrons from a metal caused by light striking the metal
c)
The rate at which a waves energy flows through a given unit of area.
d)
packets of electromagnetic energy
8.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
9.
Certain blue lights have a frequencey of 6.91x1014Hz. What is the wavelength?
a)
4.34x1021
b)
4.34x10-21
c)
4.34x10-7
d)
2.07x1023
10.
What is the wavelength for a quantum of light with energy of 7.56x10-19J?
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
11.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
12.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
13.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
14.
What atom matches this electron configuration?
[Xe] 6s24f145d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
15.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
16.
The electron configuration of an atom is 1s22s22p63s23p64s23d104p3. The number of valence electrons in the atom is
a)
3
b)
5
c)
10
d)
15
17.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
18.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
19.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
20.
_______ carry the greatest amount of energy.
a)
x-rays
b)
gamma rays
c)
infrared rays
d)
visible light
21.
This image is an illustration of
a)
photoelectric effect
b)
Dalton's atomic theory
c)
Bohr model
d)
Quantum mechanical model
22.
In the Bohr model, the orbit closest to the nucleus is
a)
called the ground state and is lowest in energy
b)
called the ground state and is highest in energy
c)
called the excited state and is lowest in energy
d)
called the excited state and is highest in energy
23.
Which of the following was NOT a limitation of the Bohr model of the atom?
a)
It only worked for a single electron atom like Hydrogen
b)
It did not explain the chemical behavior of atoms
c)
It did not show that electrons are allowed to have only certain energy levels.
24.
Both light and electrons have dual nature. That is, they both may have properties of waves and particles.
a)
True
b)
False
25.
Quantized means that only certain values are allowed.
a)
True
b)
False
26.
Which model of the atom said that electrons closest to the nucleus have the highest energy?
a)
Bohr model
b)
Quantum mechanical model
c)
Not true of either model
d)
Both Bohr and Quantum mechanical model
27.
Define "quantized"
a)
The electron's mass is very small.
b)
The electron is actually a wave.
c)
The position & momentum of the electron cannot be known at the same time.
d)
The electron is limited to certain positions in the atom.
28.
"Electrons have particle and wave-like properties."
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
29.
created an equation to treat the electron as a wave and described orbitals
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
30.
"Electrons in the same orbital have opposite spin."
a)
Aufbau principle
b)
Hund's Rule
c)
Pauli Exclusion Principle
d)
Uncertainty Principle
31.
"Electrons fill lower energy orbitals before filling higher energy orbitals."
a)
Aufbau principle
b)
Hund's Rule
c)
Pauli Exclusion Principle
d)
Uncertainty Principle
32.
"Electrons fill equal energy orbitals singly before pairing."
a)
Aufbau principle
b)
Hund's Rule
c)
Pauli Exclusion Principle
d)
Uncertainty Principle
33.
Define "quantized"
a)
The electron's mass is very small.
b)
The electron is actually a wave.
c)
The position & momentum of the electron cannot be known at the same time.
d)
The electron is limited to specific amounts of energy in the atom.
34.
Scientist who proposed the "wave theory" to explain particle behavior.
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
35.
The position & momentum (energy) of the electron cannot be known at the same time.
a)
Planck's constant
b)
Heisenberg Uncertainty Principle.
c)
de Broglie wave equation
d)
Bohr's model of the atom
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