Explain why the quantum number set (3, 3, -2, +½) is not possible for an electron in a ground-state atom.

- It's not correct because the values of n and l are same.

Explanations:- The four quantum numbers are n, l, ml and ms where n stands for Principal quantum number and has values like 1, 2, 3 and so on.

l stands for azimuthal quantum number and has values from 0 to (n-1) where n is principal quantum number.

For the given set of quantum numbers, value of n is 3. So, the possible values of l would be 0,1 and 2.

The value of l for the given set of quantum numbers is 3 which is the reason why the given set is not possible.

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

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