Electron Configurations

How many electrons does Si contain? (click to see image)

• 14
• 28
• 2
• 4

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How many electrons can the first energy level hold?

• 1
• 2
• 8
• 0

The 4 orbitals are

• s, p, d, f

• a, b, c, d

• 2, 4, 6, 8

How many electrons can the d sublevel hold?

• 8
• 10
• 2
• 4

Each row on the periodic table represents:

• an energy level

• a sublevel

• an electron

• an orbital

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What does Hund's rule state?

• An orbital can contain two electrons only if the electrons have opposite spins.

• An orbital can contain two electrons only if all other orbitals at that sublevel are empty.

• An orbital can contain two electrons only if the electrons have different energy levels.

• An orbital can contain two electrons only if all other orbitals in that sublevel contain at least one electron.

Why do electrons enter the 4s orbital before entering the 3d orbital? 

• because the 3d orbital is at a lower energy level

• because both the 4s and 3d orbitals are at the same energy level

• because the 4s orbital is at a lower energy level

• because the 4s orbital is at a higher energy level

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What does the sign represent with respect to electrons?

• opposite spin of two electrons

• different principal energy levels of two electrons

• distances of two electrons from the nucleus

• attraction between two electrons

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According to the Pauli exclusion principle, when can two electrons occupy the same orbital?

• only if there is no place else to put them

• only if they have the same spin

• only if they have opposite spins

• only if they are alike in all their properties

Electron configuration of hydrogen (H)

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