Unit 2 Chemistry Energy, Light, & Electron Structure Exam Review

Place the following list of energy levels and sublevels in order from lowest to highest energy. 3s, 4p, 2s, 2p, 1s, 3d, 4s, 3p

• 3s, 4p, 2s, 2p, 1s, 3d, 4s, 3p

• 1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p

• 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p

• 1s, 2s, 3s, 4s, 2p, 3p, 4p, 3d,

17. What does n designate in the Bohr Model?

• Orbitals

• Sublevels

• Energy levels

19. What is the maximum number of electrons an orbital may hold? __________________

• 1

• 2

• 3

• 4

20. How many s sublevels are there in the third energy level? ___________________________

• 1

• 2

• 3

• 4

22. How many "p" orbitals can there be in the 2nd energy level? ____________________________

• 1

• 2

• 3

• 4

Indicate the maximum number of electrons in the following.

n=3 energy level _____

• 2

• 8

• 18

• 32

Indicate the maximum number of electrons in the following.

3p orbital _____

• 2

• 4

• 6

• 8

Indicate the maximum number of electrons in the following.

2p sublevel _____

• 2

• 4

• 6

• 8

Apply Hund's Rule, the Pauli Exclusion Principle, and the Aufbau Principle. In the space below, using your electron fill diagram write the unabbreviated electron configurations of the following elements:

iron Fe:________________________________________________

In the space below, write the abbreviated electron configurations of the following elements:

silver Ag: ________________________________________________