Which of the following set of quantum number is not possible?
Answers
Answer:
Where are the sets??
Explanation:
The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on. The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on. The angular quantum number (l) can be any integer between 0 and n - 1.
Answer:
This set of quantum numbers is not possible as the value of n is 2, and the value of l is also 2. The value of n and l cannot be same....
Explanation:
State which of the following set of quantum number would be possible and which would be permissible for an electron in an atom. a) n=3, l=3, m l =+3 , m s = +1/2 b) n=3, l=0, m l =+1 , m s = - 1/2 c) n=5, l=4, m l =+3 , m s = 1 d) n=0 ,l=0, m l = 0 , m s = +1/2 e) n=4, l=3, m l = - 2 , m s = - 1/2.