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The following quantum numbers are possib...

The following quantum numbers are possible for how many orbital (s) n = 3, l = 2 and m = +2 ?

A

1

B

2

C

3

D

4

Text Solution

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The correct Answer is:
A
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The following quantum numbers are possible for how many orbitals (s) n = 3, l = 2, m = + 2 ?

How many orbitals are possible for n = 3, l=2 ?

Explain , giving reason , which of the following sets of quantum number are not possible {:(a,n= 0 ,l = 0, m_(1) = 0, m_(s) = +1//2),(b,n= 1 ,l = 0, m_(1) = 0, m_(s) = -1//2),(c,n= 1 ,l = 1, m_(1) = 0, m_(s) = +1//2),(d,n= 2 ,l = 1, m_(1) = 0, m_(s) = -1//2),(e,n= 3 ,l = 3, m_(1) = -3, m_(s) = +1//2),(f,n= 3 ,l = 1, m_(1) = 0, m_(s) = +1//2):}

Two electrons A and B in an atom have the following set of quantum numbers , what is true for A and B: For A, n=3,l=2,m=-2, s=pm1/2 , For B,n=3,l=0,m=0, s=pm1/2

using s, p, d notations describe the orbtal with the following quantum numbers . (a) n = 2 l=1, (b) n = 4 , l = 0, (c) n= 5 , l=3 , (d) n = 3 , l = 2

Given the notation for the sub-shell deotected by the following quantum number a. n = 5, l = 2 b. n = 6 , l= 3 c. n = 4 ,l = 0 d n = 5,l = 4

Explain giving reasons, which of the following sets of quantum numbers are not possible? (a) n=0, l=0, m_(l)=0, m_(s)=+1/2 (b) n=1, l=0, m_(l)=0, m_(s)=-1/2 (c) n=1, l=1, m_(l)=0, m_(s)=+1/2 (d) n=2, l=1, m_(l)=0, m_(s)=-1/2 (e) n=3, l=3, m_(l)=-3, m_(s)=+1/2 (f) n=3, l=1, m_(l)=0, m_(s)=+1/2

Using s, p and d notations, describe the orbitals with following quantum numbers : (a) n=1, l=0 , (b) n=2, l=0 (c) n=3, l=1 , (d) n=4, l=2

Given below are the sets of quantum numbers for given orbitals .Name these orbitals a. n = 2 l = 1 m = -1 b. n = 4 l = 2 m = 0 c. n = 3 l = 1 m = +- 1 d. n = 4 l = 0 m = 0 e. n = 3 l = 2 m = +- 2

Which of the following sets of quantum numbers are correct? n l m n l m

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