Electron Configuration (Chapter 5)

Electron Configuration

100

The electron configuration of magnesium.

1s² 2s² 2p⁶ 3s²

200

The electron configuration of ruthenium. 

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d⁶

300

The electron configuration of sodium.

1s² 2s² 2p⁶ 3s¹

400

The electron configuration of manganese. 

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4d⁵

500

The electron configuration of silver.

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d⁹  

More Notations

100

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d⁶ 

Ruthenium

200

[Kr] 5s² 4d¹⁰

Cadmium

300

Noble gas notation for lead.

[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

400

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s¹ 

Antimony

500

Seaborgium

[Rn] 7s² 5f¹⁴ 6d⁴

Noble Gas Notation

100

Noble gas notation for iridium.

[Xe] 6s² 4f¹⁴ 5d⁷

200

Noble gas notation for chlorine. 

[Ne] 3s² 3p⁵

300

Noble gas notation for nobelium. 

[Ne] 3s² 3p⁵

400

Noble gas notation for caesium.

[Xe] 6s¹

500

Noble gas notation for magnesium. 

[Ne] 3s²

Terms

100

Hund's rule. 

All orbitals must have one electron before any in the sublevel (s, p, d, or f) can have two electrons. 

200

Electrons must spin in opposite directions within their orbitals. 

Pauli exclusion principle

300

Principal Quantum Number

Deals with the orbital's size and energy. Tells the relative distance of the electron from the nucleus.

400

"Till the end of the line"

Noble gas notation

500

Aufbau Principle

lowest-energy orbitals fill first