Which of the following orbitals are not possible?Group of answer choices2d4f6d3g

The possible orbitals are determined by the quantum numbers in quantum mechanics. The principal quantum number (n) can be any positive integer. The azimuthal quantum number (l) can be any integer from 0 to n-1. The magnetic quantum number (ml) can be any integer from -l to +l.

1. 2d: Here, n=2 and l is represented by 'd' which corresponds to l=2. But for n=2, the maximum value of l can be 1 (n-1). So, 2d is not possible.

2. 4f: Here, n=4 and l is represented by 'f' which corresponds to l=3. For n=4, the maximum value of l can be 3 (n-1). So, 4f is possible.

3. 6d: Here, n=6 and l is represented by 'd' which corresponds to l=2. For n=6, the maximum value of l can be 5 (n-1). So, 6d is possible.

4. 3g: Here, n=3 and l is represented by 'g' which corresponds to l=4. But for n=3, the maximum value of l can be 2 (n-1). So, 3g is not possible.

So, the orbitals that are not possible are 2d and 3g.