Question

Question #08502

Answer 1

Here's what I get.

Explanation:

Question 1

Both electrons in the `"3s"` orbital have the same spin.

This violates the Pauli Exclusion Principle: No two electrons in the same orbital can have the same spin.

Question 2

You have no electrons in the `"2s"` orbital, which is between the `"1s"` and `"2p"` levels.

This violates the Aufbau Principle: When adding electrons to an atom, you put them in the lowest-energy orbitals available.

Question 3

You have two electrons in one `"2p"` orbital, but none in the other `"2p"` orbitals.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 4

The electrons in the half-filled `"4d"` orbitals don't all have the same spin.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 5

You filled the `"4d"` orbitals before you filled the `"4p"` orbitals, which are lower in energy.

This violates the Aufbau Principle.