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