Unit Test Study Guide

How many electrons can occupy an orbital in any sublevel?

• two, if they have opposite spins

• two, if they have the same spin

• one

• depends on the sublevel

How many electrons are needed to completely fill the fourth energy level?

• 2

• 4

• 18

• 32

# of ORBITALS for the four sublevels?

• s:2, p:6, d:10, f:14

• s:1, p:3, d:5, f:7

• s:4, p:12, d:20, f:28

• s:14, p:10, d:5, f:2

What are the MAX # of ELECTRONS for the four sublevels?

• s:2, p:6, d:10, f:14

• s:1, p:3, d:5, f:7

• s:4, p:12, d:20, f:28

• s:14, p:10, d:6, f:2

Which orbital below can never exist according to quantum theory?

• 3d

• 3f

• 4s

• 2p

Which sublevel is associated with a spherical (ball shaped) electron cloud?

• s

• p

• d

• f

Electrons fill the lowest energy level

• Hund's Rule

• Aufbau Principle

• Pauli's Exclusion Principle

Complete orbitals with single electrons before pairing up electrons in a single orbital

• Hund's Rule

• Aufbau Principle

• Pauli's Exclusion Principle

What part of electron configuration does the Pauli Exclusion Principle govern?

• Lowest energy level is filled first

• Complete orbitals with single electrons before pairing

• 2 electrons can share an orbital if they have opposite spin.

The following orbital notations are incorrect.

Identify the Principle or Rule broken because the 3p^4 electron should show an opposite spin.

• Pauli Exclusion Principle

• Hund's rule

• Aufbau Principle