Quantum Number Worksheet - Answer Key
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- Principal Quantum Number
- Is represented by – n
- Has values from ranging from – 1 → ∞
- Indicates – the size and energy level in which the electron is housed.
The bigger the n value, the further the electro is from the nucleus.
- Degeneracy is when orbitals have the same value of n.
- Angular Momentum Quantum Number
- Is represented by – l
- Has values from ranging from – 0 → (n-1)
- Indicates – the type of orbital.
- l = 0 → s orbital
- l = 1 → p orbital
- l = 2 → d orbital
- l = 3 → f orbital
- Magnetic Quantum Number
- Is represented by – ml
- Has values from ranging from – ( –l →+ l)
- Indicates – # of orbitals.
- l =0 (the s orbital) → ml =0
This means that there is only one s-orbital.
- l =1 (the p orbital) → ml = (-1, 0, +1)
Because there are 3 values of for ml there would be three p orbitals.
- l =2 (the d orbital) → ml = (-2, -1, 0, 1, 2)
Because there are 5 values for ml there would be five d orbitals.
- l = 3 (the f orbital) → ml = (-3, -2, -1, 0, 1, 2, 3)
Because there are 7 values for ml there would be seven differently orientated f orbitals.
- Spin Quantum Number
- Is represented by – ms
- Has values from ranging from – (+½, - ½)
- Indicates – spin of an electron
- What is the Pauli Exclusion Principle?
Only 2 electrons can be in a particular orbital and they must have opposite spin numbers.
- Which of the following pairing of quantum numbers is invalid, why?
- n=3, l =2, ml =2, ms = ½
This set of quantum numbers is valid. All values fit the required parameters.
- n=4, l =3, ml =4, ms =- ½
This set is invalid. The value of ml cannot equal 4 if l = 3
- n=0, l =0, ml =0, ms = -½
This is an invalid set of quantum numbers because n cannot equal zero.
- n=2, l =-1, ml =1, ms = ½
This is an invalid set of quantum numbers because l cannot equal -1.
- How many electrons can have the following designation?
- 1p – None.
- 6dxy – 2
- 4f – 14
- n=3 – 9