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
  `+(1)/(2)` or
  `-(1)/(2)`

Step-by-step 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
`+(1)/(2)` for upward spin and
`-(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
  `+(1)/(2)` or
  `-(1)/(2)`