How many electrons in an atom can have each of the following quantum number or sublevel designations?

(a) 2s

(b) n = 3, l = 2

(c) 6d

(a) Number of electrons in an atoms is, 2

(b) Number of electrons in an atoms is, 10

(c) Number of electrons in an atoms is, 10

Explanation:

There are 4 quantum numbers:

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. The value of this quantum number ranges from. When l = 2, the value of

Spin Quantum number : It describes the direction of electron spin. This is represented as. The value of this is for upward spin and for downward spin.

Number of electrons in a sublevel = 2 (2l+1)

(a) 2s

n = 2

Value of 'l' for 's' orbital : l = 0

Number of electrons in an atoms = 2 (2l+1) = 2 (2*0+1) = 2

(b) n = 3, l = 2

Number of electrons in an atoms = 2 (2l+1) = 2 (2*2+1) = 10

(c) 6d

n = 2

Value of 'l' for 'd' orbital : l = 2

Number of electrons in an atoms = 2 (2l+1) = 2 (2*2+1) = 10