# Question #08502

Apr 16, 2015

Here's what I get.

#### Explanation:

Question 1

Both electrons in the $\text{3s}$ 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 $\text{2s}$ orbital, which is between the $\text{1s}$ and $\text{2p}$ 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 $\text{2p}$ orbital, but none in the other $\text{2p}$ 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 $\text{4d}$ 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 $\text{4d}$ orbitals before you filled the $\text{4p}$ orbitals, which are lower in energy.

This violates the Aufbau Principle.