Electron Configuration and Orbital Theory

The video tutorial covers the basics of electron orbitals, including the s, p, d, and f sublevels. It explains how electrons are represented in these orbitals using arrows and boxes, adhering to the Pauli exclusion principle and Hund's rule. The tutorial also demonstrates how to draw orbital diagrams for elements like oxygen, chromium, germanium, and bismuth, and concludes with instructions on creating Lewis dot diagrams to represent valence electrons.

What is the maximum number of electrons that can be held in an s orbital?

• 4

• 2

• 1

• 3

According to the Pauli Exclusion Principle, how must electrons in the same orbital be oriented?

• Randomly

• Same direction

• Opposite directions

• Perpendicular

How many orbitals are present in a p sublevel?

• 2

• 3

• 1

• 4

What does Hund's Rule state about electron distribution in orbitals?

• Electrons pair up before filling empty orbitals

• Electrons fill orbitals randomly

• Electrons fill the lowest energy orbital first

• Electrons fill orbitals singly before pairing

How many orbitals are there in a d sublevel?

• 4

• 6

• 3

• 5

In the f sublevel, how many orbitals are available?

• 8

• 7

• 6

• 5

For the element Oxygen, how many electrons are in the 2p sublevel?

• 5

• 4

• 3

• 2

What is the electron configuration shortcut for Chromium?

• [Kr] 5s2 4d10

• [Xe] 6s2 4f14

• [Ne] 3s2 3p6

• [Ar] 4s2 3d4

How many valence electrons does Germanium have?

• 4

• 2

• 8

• 6

In a Lewis dot diagram, how are electrons represented around the element symbol?

• As arrows

• As numbers

• As lines

• As dots