Part A What is the only possible value of m? for an electron in an s orbital?

What are the possible values of m? for an electron in a d orbital?

Part B

Which of the following set of quantum numbers (ordered n, ?, m?, ms) are possible for an electron in an atom?

Check all that apply.

5, 3, 0, 1/2

3, 3, 1, -1/2

3, 2, -3, 1/2

4, 2, 3, -1/2

3, 2, 1, -1

4, 2, -1, -1/2

-2, 1, 0, -1/2

3, 1, 0, -1/2

A) For an electron in s orbital, the value of the azimuthal quantum number ? is 0. The magnetic quantum number, m_? can have values from –? through 0 to +?. Since ? = 0, the only value of m_? is 0.

For an electron in d orbital, the value of ? is 2. m_? can assume values from –? through 0 to +?; hence the possible values of m_? are -2, -1, 0, +1, +2.

B) The general rule for an electron to have an agreeable set of quantum numbers is that

a) n can have any positive integral value like 1,2,3,etc.

b) ? can have values 0 to (n-1).

c) m_? can have values –? through 0 to +?.

d) m_S can have value either +1/2 or -1/2.

Hence, (i) 5,3,0,1/2 is allowed.

(ii) 3,3,1,-1/2 isn’t allowed since n = 3 and ? can have values 0, 1 or 2.

(iii) 3,2,-3,1/2 isn’t allowed as ? = 2 and m_? can be -2, -1, 0, +1, +2.

(iv) 4,2,3,-1/2 isnt allowed since ? =2 and the permissible values of m_? are -2, -1, 0, +1, +2.

(v) 3,2,1,-1 isn’t allowed as m_s can have value only +1/2 or -/12.

(vi) 4,2,-1,-1/2 is an allowed combination.

(vii) -2,1,0,-1/2 isn’t allowed since the principal quantum number n can have only positive integer values.

(viii) 3,1,0/-1/2 is an allowed set.