Quantum numbers

Question 1

These are a set of four numbers (n, l, ml, ms) that describe the properties of atomic orbitals and the electrons within them, specifying their energy, shape, orientation, and spin

Answer 1

Quantum numbers

Question 2

This number, denoted by ‘n’, determines the energy level and general size of an atomic orbital. It can take integer values (1, 2, 3, …) and represents the electron shell. Higher values of ‘n’ correspond to higher energy levels and larger orbitals

Answer 2

Principal Quantum Number (n):

Question 3

This number, denoted by ‘l’, describes the shape of the atomic orbital. It can take values from 0 to n-1 (0, 1, 2, … n-1). Values of ‘l’ are often represented by letters (l=0 is ‘s’, l=1 is ‘p’, l=2 is ‘d’, l=3 is ‘f’, and so on

Answer 3

Azimuthal or Angular Momentum Quantum Number (l)

Question 4

This number, denoted by ‘ml’, describes the orientation of an atomic orbital in space relative to other orbitals in the same energy level. It can take values from -l to +l, including 0 (-l, -l+1, … 0, … l-1, l).

Answer 4

Magnetic Quantum Number (ml):

Question 5

This number, denoted by ‘ms’, describes the intrinsic angular momentum or “spin” of an electron, which is quantized and can be either spin up (+1/2) or spin down (-1/2).

Answer 5

Spin Quantum Number (ms):