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Quantum Numbers
Quiz 1
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Q.1
How many electrons total are found in the f orbital?
2
6
10
14
Q.2
With each higher energy level, the electrons are
lower in energy
more stable
weaker
farther from the nucleus
Q.3
Is theorbital permitted?
yes
no
Q.4
For a principle quantum number, "n", equal towhat is the total electron capacity of that level?
2
4
8
16
Q.5
A subshell that contains 5 orbitals is ... subshell.
d
s
f
p
Q.6
The proper pair of the L value with the orbital shape.
0; f
3; p
1; s
2; d
Q.7
"Electrons fill equal energy orbitals singly before pairing."
aufbau principle
Hund's Rule
Pauli Exclusion Principle
Uncertainty Principle
Q.8
How many total electrons can the f orbitals in a sublevel hold?
2
14
6
10
Q.9
What is the noble gas configuration for Sulfur?
[Ar] 3p4
[He] 3s2 3p4
[Ne] 3s2 3p4
[Na] 3s2 3p4
Q.10
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
Hund’s Rule
Aufbau Principle
Pauli Exclusion Principle
Q.11
What quantum number describes the energy level of an orbital?
l
m
s
n
Q.12
The major difference between aorbital and a 2 s orbital is that
the 2 s orbital is at a higher energy level.
the 2s orbital has a slightly different shape.
the 1 s orbital can have only one electron.
the 2s orbital can hold more electrons.
Q.13
N=l=3?
4f
4d
3s
3p
Q.14
Which of the following sub levels does not exist
2p
3d
2d
5f
4f
Q.15
What is the maximum number of electrons that contain the values n=4 l=3
2
6
10
14
18
Q.16
A quantum number determining orbital orientation around the atom’s core is called... .
n
l
m
s
Q.17
Below are the examples on how to fill the atomic quantum number, except... .
n = 2, l =1, m = 0, s = -1/2
n = 1, l =3, m = 0, s = +1/2
n = 3, l =1, m = 0, s = -1/2
n = 3, l = 2, m = +2, l = +1/2
Q.18
Properly pair the l-value is with the orbital shape.
0; f
1; s
3; p
2; d
Q.19
The first electron of any element is placed in this orbital
4f
2p
3d
1s
Q.20
Which values can (n) be?
only 0
0, 1, 2, 3...
1,2,3,4...
-2 < n < +2
0 h : 0 m : 1 s
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