Question #08502

1 Answer
Ernest Z. · Media Owl
Apr 16, 2015

Here's what I get.

Explanation:

Question 1

enter image source here

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

enter image source here

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

enter image source here

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

enter image source here

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

enter image source here

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

This violates the Aufbau Principle.

www.ck12.org

Related questions
See all questions in Electron Configuration
Impact of this question
74191 views around the world
You can reuse this answer
Creative Commons License