Question

How many possible combinations are there for the values of L and ML when n 3?

Answer 1

Answer:

When n = 3, l= 0, 1, 2 (l takes on three values and thus there are three possible subshells)

Answer 2

For the value of n = 3. maximum 9 combinations of orbitals are possible.

l = 0, 1, 2

the value of m will be,

l = 0, m = 0

l = 1, m = -1, 0, 1

l = 2, m = -2, -1, 0, 1, 2

The third shell will have 9 orbitals.

Explanation

QUANTUM NUMBER -  

• The set of numbers of describe the orbital position of electrons in an atom.
• There are four types of quantum numbers as

1. Principle Quantum (n) - describes the electron shell or energy level of an atom.

2. Azimuthal Quantum (l) - It depicts the subshells and ranges from 0 to n-1.  

3. Magnetic Quantum (m) - It specifies the projection of an electron in a subshell and the shape along with the orbital orientation. It ranges from -l to +l.

4. Spin Quantum (s) - It describes the spin of the electron in an orbital. it can be $^+_-\frac{1}{2}$.