WorksheetsNMAT MASTERCLASS - EXAM 3
Total questions: 15
Worksheet time: 3hrs 30mins
What does the principal quantum number (n) indicate?
The shape of the orbital
The orientation of the orbital
The size and energy of the shell
The spin of the electron
Which quantum number determines the shape of an atomic orbital?
Principal quantum number (n)
Azimuthal quantum number (l)
Magnetic quantum number (ml)
Spin quantum number (ms)
What is the maximum number of electrons that can occupy a single orbital
2
4
6
8
For which value of n is it possible to have a d subshell?
n=1
n=2
n=3
n=0
Which of the following describes the magnetic quantum number (ml)?
It specifies the size of the orbital.
It specifies the shape of the orbital.
It specifies the orientation of the orbital in space.
It specifies the spin of an electron.
If n = 4 and l = 3, what type of subshell is being referred to?
s
p
d
f
How many total electrons can be held in all orbitals within n=3 shell?
2
8
18
24
In which subshell would you find an electron with l=1?
s
p
d
f
For which principal quantum number would you find f orbitals present?
n=1
n=2
n=3
n=4
When considering multiple electrons in an atom, what principle governs their arrangement based on their spins?
Hund's rule
Aufbau Principle
Dalton's Law
Pauli's Exclusion Principle
Consider the photo of orbital diagrams shown here. Which of the following correctly follows Hund's rule?
B
C
D
E
How many protons and electrons are present in O2- ion?
6 electrons and
8 protons
8 electrons and
8 protons
10 electrons and
8 protons
8 electrons and
10 protons
How many protons are there in Li+ cation?
two protons
three protons
four protons
zero protons
If n=3, which of the following is not a possible angular momentum quantum number value?
0
1
2
3
What is the magnetic quantum number (ml) value for 3d6?
-2
-1
0
1
