Orbital Notation and Pauli, Hund's and Aufbau

“An electron should occupy the lowest energy level first before the higher energy level” is stated in what rule?

• Hund's rule

• Pauli Exclusion Principle

• Aufbau Principle

• All of the above.

What rule states that single electrons must occupy each equal-energy orbital before additional electrons can occupy the same orbitals.

• Hund's rule

• Pauli Exclusion Principle

• Aufbau Principle

• None of the choices.

Which of the following statement is wrong?

• Two electrons must occupy each equal energy orbital before additional electrons can occupy the same orbitals.

• A maximum of two electrons may occupy the same orbitals.

• In filling up orbitals, electron occupies the lowest energy orbital first before the higher energy orbitals.

• None of the choices.

Tags

NGSS.HS-PS1-1

Which orbital shows a violation of Hund's Rule?

• A

• B

• C

• D

Tags

NGSS.HS-PS1-1

Which orbital shows a violation of the Pauli Exclusion Principle?

• A

• B

• C

• D

Which is associated with more energy? 

• 2p

• 2s

• 3p

• 1s

Tags

NGSS.HS-PS1-1

Why do we use the three electron configuration rules: Hund's Rule, Aufbau Principle, and Pauli Exclusion Principle?

• to know where electrons are located

• to know how electrons are oriented in space

• to know how electrons are used in chemical reactions

• all of these

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which principle states that no two electrons in an atom can have the same set of four quantum numbers?

• Pauli Exclusion Principle

• Hund's Rule

• Aufbau Principle

• Heisenberg Uncertainty Principle

In orbital notation, which rule requires that electrons fill orbitals starting with the lowest energy level first?

• Hund's Rule

• Pauli Exclusion Principle

• Aufbau Principle

• Bohr's Model

According to Hund's Rule, how should electrons be distributed in orbitals of the same energy?

• Pair up in each orbital before moving to the next

• Fill each orbital singly before pairing up

• Fill the highest energy orbital first

• None of the above