Point out the differences and similarities in the orbitals represented by following sets of quantum numbers- n l m

(i) 3 2 +2
(ii) 3 2 –1

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Solution

Dear Student,
The principal quantum number 'n' of both orbitals is 3. This represents the third shell .
The azimuthal quantum number 'l' of both orbitals is 2 . This shows that both are d-subshell.
Differences

Quantum number I electron II electron

Magnetic quantum number +2 -1

The first electron will be in 5^thorbital and the second electron will be in 2^nd orbital.
Regards!

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Similar questions

n = 4, l = 0, m_{l} = 0, m_{s} = + \frac{1}{2}

n = 3, l = 1, m_{l} = 1, m_{s} = - \frac{1}{2}

n = 3, l = 2, m_{l} = 0, m_{s} = + \frac{1}{2}

n = 3, l = 0, m_{l} = 0, m_{s} = - \frac{1}{2}

n = 4, l = 0, m = 0, s = + \frac{1}{2}

n = 3, l = 1, m = 1, s = - \frac{1}{2}

n = 3, l = 2, m = 0, s = + \frac{1}{2}

n = 3, l = 0, m = 0, s = - \frac{1}{2}

n = 4, l = 0, m = 0, s = + \frac{1}{2}

n = 3, l = 1, m = 1, s = - \frac{1}{2}

n = 3, l = 2, m = 0, s = + \frac{1}{2}

n = 3, l = 0, m = 0, s = - \frac{1}{2}

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Quantum number	I electron	II electron
Magnetic quantum number	+2	-1