Worksheets2.2 QUANTUM MECHANICAL MODEL
Total questions: 10
Worksheet time: 5mins
How many orbitals make up the d subshell?
1
5
3
7
What orbital is shown in the picture?
s orbital
p orbital
d orbital
f orbital
Which quantum number represents the shape of the orbital?
principal quantum number
azimuthal (angular momentum) quantum number
magnetic quantum number
spin quantum number
What is the purpose of the quantum numbers?
To calculate wavelength associated with the moving electron.
To calculate velocity associated with the moving electron.
To predict the probable location of an electron in the Bohr model.
To predict the probable location of an electron in the quantum mechanical model.
What is the difference in a 1s orbital and a 2s orbital?
The shape of the orbital
The size of the orbital
The number of electrons it can hold
None of the above
Which quantum number represents the orientation of the orbital?
principal quantum number
azimuthal (angular momentum) quantum number
magnetic quantum number
spin quantum number
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), m=(-1/2)
n=(4), l=(2), ml=(-3), ms=(+1/2)
What states that every orbital of a subshell must be singly occupied before any orbital can have a pair?
Pauli exclusion principle
Hund's rule
Aufbau principle
None of the above
This states that no two electrons will have the same 4 quantum numbers in an atom or molecule. The two electrons of the same orbital must have opposite spin states.
Pauli exclusion principle
Hund's rule
Aufbau principle
None of the above
What states that electrons fill the lowest energy orbitals/levels first before occupying higher energy levels?
Pauli exclusion principle
Hund's rule
Aufbau Principle
None of the above
