Electron Configuration Assessment (F24)

The 4 orbitals are

• s, p, d, f

• a, b, c, d

• 2, 4, 6, 8

Each row on the periodic table represents:

• an energy level

• a sublevel

• an electron

• an orbital

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NGSS.HS-PS1-1

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

Tags

NGSS.HS-PS1-1

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

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

Write the electron configuration associated with this orbital diagram

• 1s²2s²2p⁶

• 1s¹2s¹2p³

• 1s²2s²2p⁶3s²

• 1s²2s²2p⁶3s³

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Write the electron configuration for the element identified by this orbital diagram

• 1s¹2s¹2p³3s¹

• 1s²2s²2p⁵3s¹

• 1s2s2p3s

• 1s²2s²2p⁶3s¹

Tags

NGSS.HS-PS1-1

The electron configuration of an atom is 1s²2s²2p⁶.  The number of electrons in the atom is 

• 3
• 6
• 8
• 10

Tags

NGSS.HS-PS1-1

Check all of the following that could actually exist in a correctly written electron configuration.

• 4s³

• 3p⁴

• 2p⁸

• 6d³

• 1s¹

Tags

NGSS.HS-PS1-1