Question

The correct set of quantum numbers to the
unpaired electron of fluorine atom -
(A)n=3, l = 0, m = 0 (B) n = 3, l = 1, m = 1
(C) n=2, l = 0, m=0
(D) nr 2, l = 1, m= 1​

Answer 1

Explanation:

♦ The unpaired electron of fluorine atom have configuration 2p^5

♦So, n=2, p=1=l

♦Hence option D is correct.

Answer 2

Answer:

The answer is D) n= 2, l = 1, m= 1​

Explanation:

As we all know the electronic configuration of the Fluorine atom is $1s^22s^22p^5$.

• So the electron in the outermost shell enters the p shell.

• The number of electrons in the outermost shell decides the principal quantum number, therefore n=2
• When n=2 the values of l are 0 and 1 which means they have two subshells, 2s and 2p

The magnetic quantum gives the orientation of the orbital. It is denoted by the letter m and has (2l+1) values, i.e the values from +1 through 0 to -1.

• when l=0 m=0 and l=1 m=+1,0,-1
• It is given the hint of unpaired electron of fluorine atom. So in the p subshell, it has 1 unpaired electron as per the Paulis Exclusion principle.
• Hence l=1 the value of m=+1, 0, -1

Therefore the correct set of quantum numbers to the unpaired electron of fluorine atom - (D) n= 2, l = 1, m= 1​