Please explain this question briefly and then the answer.....
 
  1. = 2, = ?, ml = +1; name: 2p

Asked by ppratim02 | 5th Sep, 2015, 05:35: PM

Expert Answer:

  • 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. If n = 3, for example, l can be either 0, 1, or 2.
  • The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.

As per above rule, the only combination for n=1 is as follows,

The orbital having quantum number combination n=1, l=0 and l=0 is 1s.

Also, only 2p orbital has values of quantum numbers n=2, l= 1 and m having three values such as -1, 0, +1.

Thus, for n= 2, ml=0 then, l should also be 0 as per above table.

Hence, when n = 2, ml= +1 then l must be 1.

Answered by Prachi Sawant | 6th Sep, 2015, 04:21: PM