WorksheetsQuantum Mechanical Model - Basics
Total questions: 28
Worksheet time: 19mins
How many orbitals make up the "d" sublevel?
1
3
5
7
How many orbitals make up the "s" sublevel?
1
3
5
7
How many orbitals make up the "p" sublevel?
1
3
5
7
How many orbitals make up the "f" sublevel?
1
3
5
7
How many electrons can occupy the f-sublevel?
14
10
6
4
Which main energy level, n, is furthest from the nucleus ?
1
2
3
What is the maximum number of orbitals on the 2nd main energy level (n=2)
8
9
4
2
A 3-D region of space around a nucleus where there is a high likelihood of locating an electron is called a(n)
spectral line.
electron path.
orbital
Pauli exclusion.
Which of the following values does NOT represent a valid electron?
n=(2), l=(1), ml=(1), ms=(+1/2)
n=(4), l=(2), ml=(-1), ms=(-1/2)
n=(2), l=(0), ml=(0), ms=(-1/2)
n=(4), l=(2), ml=(-3), ms=(+1/2)
Which quantum number represents the main energy level?
Principal Quantum Number (n)
Angular Momentum Quantum Number (l)
Magnetic Quantum Number (ml)
Spin Quantum Number (ms)
Which quantum number represents the shape of the orbital?
Principal Quantum Number (n)
Angular Momentum Quantum Number (l)
Magnetic Quantum Number (ml)
Spin Quantum Number (ms)
When n = 2, what are the possible values for the angular momentum?
1
0, 1
0, 1, 2
2
Draw an s-orbtial.
What is the difference between an (n = 1) s-orbital and an (n = 2) s-orbital?
The size.
The shape.
The number of electrons.
All of the above.
According to the Heisenberg Uncertainty Principle, it is impossible to know both the (a) and the (b) of an electron simultaneously.
Orbitals are regions of space around the nucleus where a(n) __________ likely to be located.
proton
neutron
nucleon
electron
Of the following transitions in the Bohr hydrogen atom, the _________ transition results in the emission of the highest-energy photon.
n = 6 --> n = 1
n = 1 --> n = 6
n = 3 --> n = 6
n = 6 --> n = 4
The quantum mechanical model of the atom:
was proposed by Niels Bohr and explains electrons as being found in discrete, fixed paths of energy.
expresses the probability of finding electrons in certain orbitals based on Schrodinger's wave equation.
was the cumulative effort of Ernest Rutherford and his gold-foil experiment.
displays an atom as mostly positive with tiny, negatively charged particles scattered throughout.
How many electrons can each orbital contain?
1
2
3
5
What are the possible values for the angular momentum (l) if n = 3?
0
0, 1
1, 2
0, 1, 2
Match each angular momentum quantum number to the shape it represents:
s
l = 0
p
l = 1
d
l = 2
f
l = 3
How many possible orientations are there for the d-sublevel?
1
3
5
7
What element is displayed in the Bohr model shown?
Oxygen
Neon
Argon
Magnesium
According to the Bohr model, does the atom for the represented element have a neutral charge?
Yes
No
True or False: According to the quantum mechanical model, electrons can only have a positive magnetic spin (ms = +1/2) or a negative magnetic spin (ms = -1/2).
True
False
True or False: An s-orbital has a dumbbell shape.
True
False
An electron has the following "address": 1s2
What four quantum numbers would represent this electron?
n = 1, l = 0, ml = 0, ms = -1/2
n = 1, l = 1, ml = 1, ms = 1
n = 2, l = 0, ml = 0, ms = 1
