Question

Summarize the rules for the allowable values of the four quantum numbers of an electron in an atom.

Answer 1

Answer : Rules for the allowable values of the four quantum numbers are:

• 'n' must be positive integer that means n > 0
• The value of 'l' must be from 0 to (n-1)
• The value of 'ml' must be from $(-l\text{ to }+l)$
• The value of 'ms' must be $+\frac{1}{2}$ or $-\frac{1}{2}$

Explanation:

Principle Quantum Numbers : It describes the size of the orbital. It is represented by n. n = 1,2,3,4....

Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...

Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as $m_l$. The value of this quantum number ranges from $(-l\text{ to }+l)$. When l = 2, the value of

Spin Quantum number : It describes the direction of electron spin. This is represented as $m_s$. The value of this is $+\frac{1}{2}$ for upward spin and $-\frac{1}{2}$ for downward spin.

Rules for the allowable values of the four quantum numbers are:

• 'n' must be positive integer that means n > 0
• The value of 'l' must be from 0 to (n-1)
• The value of 'ml' must be from $(-l\text{ to }+l)$
• The value of 'ms' must be $+\frac{1}{2}$ or $-\frac{1}{2}$