Quantum Numbers and Electron Configurations Review

Identify the following element:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

• nickel
• copper
• zinc
• gallium

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What is the name of the element whose electron configuration is 1s²2s²2p³?

• magnesium

• nitrogen

• carbon

• phosphorous

Tags

NGSS.HS-PS1-1

Which electron configuration belongs to Copper (Cu)?

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸
• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹
• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

How many d orbitals are there in a given sublevel?

• 1
• 3
• 5
• 7

How many p orbitals are there in a sublevel?

• 2
• 1
• 4
• 3

4. Below are the examples on how to fill the atomic quantum number, except... .

• n = 2, l =1, m = 0, s = -1/2

• n = 1, l =3, m = 0, s = +1/2

• n = 3, l =1, m = 0, s = -1/2

• n = 3, l = 2, m = +2, l = +1/2

13. A theory stating that it is forbidden for 2 electrons having the same value of atomic quantum numbers is explained by... .

• Hund

• Aufbau

• Pauli

• Schrodinger

Electrons will not pair up in a subshell until all other subshells (orientations) are full. This describes which theory of the quantum atomic model?

• Hund’s Rule

• Aufbau Principle

• Pauli Exclusion Principle

• Heisenberg's Uncertainty Principle

How many electrons can the d sublevel hold?

• 8
• 10
• 2
• 4

Identify the subshell in which electrons with the following quantum numbers are found:

n = 3, l = 2

• 3s

• 3p

• 3d