WorksheetsQuantum Mechanical Model
Total questions: 39
Worksheet time: 29mins
Name
Class
Date
1.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
2.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
3.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
4.
What is this element?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
5.
What shape are P Orbitals?
a)
Cloverleaf shaped
b)
Spherical shaped
c)
Hybrid structure
d)
Dumbell shaped
6.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
7.
What is the electron configuration of Ag?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9
b)
[Kr] 5s2 4d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d9
d)
1s2 2s2 2p6
8.
What shape are S orbitals?
a)
Dumbell shaped
b)
Cloverleaf shaped
c)
Spherical shaped
d)
Hybrid structure
9.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
10.
There are 4 different types of sublevels: s,p,d,f
a)
true
b)
false
11.
How many electrons can each p orbital hold?
a)
6
b)
3
c)
2
d)
4
12.
How many orbitals are there in the "d" sublevel?
a)
1
b)
3
c)
5
d)
7
13.
How many orbitals are there in a "p" sublevel?
a)
2
b)
1
c)
4
d)
3
14.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
15.
Which is associated with more energy?
a)
2p
b)
2s
c)
3p
d)
1s
16.
How many total electrons can the orbitals in the "f" sublevel hold?
a)
2
b)
14
c)
6
d)
10
17.
Which orbital has the least amount of energy?
a)
p orbital
b)
d orbital
c)
s orbital
d)
What is an orbital?
18.
Oxygen (O) has an electron configuration of:
a)
1s2, 2s2, 2p6, 3s2, 3p6
b)
1s2, 2s2, 2p4
c)
1s2, 2s2, 2p6
d)
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
19.
An area of high probability of finding an electron 90% of the time is called a(n)
a)
nucleus
b)
sublevel
c)
orbital
d)
energy level
20.
The exponent or superscript in an electron configuration tells us
a)
the number of positions of that orbital.
b)
the distance from the nucleus or level.
c)
the number of electrons in that orbital.
d)
the number of electrons in the atom.
21.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
22.
How many total electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
23.
How many valance electrons are in 1s22s22p63s2
a)
4 ve
b)
2 ve
c)
8 ve
d)
6 ve
24.
The Quantum Mechanical Model is the most recent/modern atomic model.
a)
True
b)
False
25.
Electron configuration is based on ___.
a)
Quantum Mechanical Model
b)
Science
c)
Thomson's Model
d)
Borh's Model
26.
What is this element?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
27.
What shape are D Orbitals?
a)
Hybrid structure
b)
Spherical shaped
c)
Dumbell shaped
d)
Cloverleaf shaped
28.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
29.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
30.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
31.
What is the highest occupied energy level?
a)
1
b)
2
c)
3
d)
4
32.
What is the highest occupied energy level?
a)
4
b)
5
c)
6
d)
7
33.
How many quantum numbers are there in the Quantum Mechanical Model?
a)
3
b)
2
c)
4
d)
6
34.
The quantum number "n" represents:
a)
spin
b)
orbital
c)
sublevel
d)
energy level
35.
The quantum number "l" represents:
a)
spin
b)
orbital
c)
sublevel
d)
energy level
36.
The quantum number ml represents:
a)
spin
b)
orbital
c)
sublevel
d)
energy level
37.
The quantum number ms represents:
a)
spin
b)
orbital
c)
sublevel
d)
energy level
38.
Which scientist developed the Uncertainty Principle:
a)
E. Schroedinger
b)
W. Heisenberg
c)
J. Dalton
d)
N. Bohr
39.
The Heisenberg Uncertainty Principle states:
a)
You cannot measure the momentum and exact position of an electron at the same time
b)
electrons occupy the orbitals of lowest energy first
c)
an atomic orbital may describe at most 2 electrons
d)
No two electrons can have the same set of quantum numbers
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