Electrons and Waves Test Review

How many orbitals are there in a "2p" electron subshell?

• 2

• 3

• 6

• 10

How many orbitals are in a "4d" electron subshell?

• 4

• 5

• 10

• 15

Which of the following does NOT apply to electron orbitals?

• An orbital can only hold 2 electrons

• Electrons in an orbital must have opposite spin

• Orbitals hold one electron each before they pair up

• An orbital can only hold 1 electron

The Pauli Exclusion Principle says:

• Each orbital only holds 2 electrons and they must have opposite spin

• Electrons fill in closest to the nucleus first, then fill higher energy levels

• Each orbital in a subshell holds 1 electron before electrons can pair up

Hund's Rule says:

• Each orbital in a subshell is singly occupied with 1 electron before any orbital is doubly occupied

• Electrons fill from lowest energy to highest energy levels

• Electrons in an orbital must have opposite spin

Aufbau Principle says:

• Electrons fill in lower energy levels first

• Electrons in an orbital must have opposite spin

• Only 2 electrons fit in one orbital

What do the subshell letters s, p, d, and f represent?

• Number of electrons a subshell can hold

• Shape of the subshell

• Name of the person that discovered them

For an electron to change from the ground state to the excited state:

• Energy is absorbed

• Energy is emitted

• Radiation is emitted

Tags

NGSS.HS-PS4-3

If electrons in atom have the lowest possible energies, we say they are in:

• Excited State

• Ground State

• State of Texas

How many electrons fit in each subshell?

• s: 2 p: 6 d: 10 f: 14

• s: 2 p: 2 d: 6 f: 10

• s: 1 p: 3 d: 5 f: 7

Tags

NGSS.HS-PS1-1