Electron Configuration

Which of the following statements about atomic orbitals is TRUE?

• An atomic orbital can hold any number of electrons.

• An atomic orbital can only hold one electron.

• An atomic orbital defines a region where an electron is most likely to be found.

• An atomic orbital has a specific size and shape.

How many sublevels does the energy level with n = 3 have?

• 1

• 2

• 3

• 4

Which of the following factors is NOT considered when writing electron configuration?

• Principal quantum number (n)

• Azimuthal quantum number (l)

• Spin quantum number (ms)

• Pauli Exclusion Principle

The ground state electron configuration describes the distribution of electrons in an atom at its:

• highest energy level

• lowest energy level

• middle energy level

• specific energy level

What principle states that electrons fill orbitals with the lowest energy levels first?

• Pauli Exclusion Principle

• Aufbau Principle

• Hund's Rule

• Noble Gas Rule

According to the Pauli Exclusion Principle, which of the following statements is FALSE?

• An orbital can hold a maximum of two electrons.

• Two electrons in the same orbital must have opposite spins.

• No two electrons can have the same set of four quantum numbers.

• All orbitals in a subshell must be filled before moving to a higher energy level.

When filling degenerate orbitals, Hund's Rule states that electrons first fill each orbital:

• completely before moving to the next

• halfway before pairing up

• with the same spin

• 1. with the same energy

Which of the following is NOT a type of atomic orbital?

• s

• p

• d

• 1. q

What is the shorthand method used to represent the electron configuration of an element by referencing the configuration of the nearest noble gas?

• Aufbau notation

• Pauli shorthand

• Hund's rule notation

• 1. Noble gas configuration

The electron configuration for nitrogen (N) is 1s²2s²2p³. Which principle is violated by this configuration?

• Aufbau Principle

• Pauli Exclusion Principle

• Hund's Rule

• 1. None of the above