Explanation
m = -l to l.
n is called as principal quantum no. and l is the azimuthal quantum No.
So, any sub-orbit is represented as nl
Value of l<n l: 0 1 2 3 4
Value of m -l,……, 0,…… +l.
Value of s +1/2 or -1/2
For 4f : n = 4, l = 3, m = any value between -3 to +3.
When n = 3, value of L are 0 to (n-1) i.e 0,1,2.
s- subshell has only one orbital and that is spherical. So s-orbitals are non-directional.
When n = 3, then l = 3 does not exist.
(I)1s (II)2s (III)2s
(IV)3d (V)3d
3d in (IV) and (V) will be of equal energy, in the absence of any field.
Hydrogen atom is in 1sˈ state. So, 3s, 3p and 3d orbitals will have same energy.
Possible values of n,l,m and s are
n = 1 to ∞(all whole numbers)
l = 0 to (n-1) for every value of n
m = -l to l
s = 1/2 and -1/2
(C) n = 4, l = 4, m = 1
The value of l can have maximum (n-1) value i.e 3. So this option is non-permissible.
Options (a), (b) and (d) are permissible.
Higher the value of (n+l), higher the energy. If (n+l) are same, sub-orbit with lower value of n has lower energy.
Thus, 3p<4s<3d<4p
(4)<(2)<(3)<(1)
Hund’s rule of maximum multiplicity states that during filling of electron in a subshell, pairing of electrons cannot take place until there is any empty orbital available.
Pauli Exclusion principle states that, in any orbital, maximum two electrons can exist, having opposite spin.
X(19):- k = 2, L = 8, M = 8, N = 1
Y(21):- k = 2, L = 8, M= 9, N = 2
Z (25):- k=2, L = 8, M = 13, N = 2
Order of number of electrons in M shell is Z>Y>X
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