Navigating Quantum Numbers and Electron Configurations

The video tutorial by Professor Dave explains quantum numbers and their role in determining electron arrangements in atoms. It covers the four quantum numbers: principal (n), angular momentum (l), magnetic (m_l), and spin (m_s), detailing their significance and how they describe atomic orbitals. The tutorial also explains the Pauli exclusion principle, electron configurations, and how to use the periodic table to determine these configurations. Key principles like the Aufbau principle and Hund's rule are discussed to help understand electron distribution in orbitals.

What is an atomic orbital?

• A specific path an electron follows around the nucleus

• A region of probability where an electron can be found

• A type of particle that makes up an electron

• A fixed point in space where an electron is located

Which quantum number represents the energy level of an electron?

• Principal quantum number (n)

• Angular momentum quantum number (l)

• Magnetic quantum number (m sub l)

• Spin quantum number (m sub s)

What shape is associated with an s orbital?

• Clover-shaped

• Complex and varied

• Spherical

• Dumbbell-shaped

How many p orbitals are there per energy level?

• 1

• 3

• 7

• 5

What values can the magnetic quantum number (m sub l) take if l is 2?

• -3, -2, -1, 0, 1, 2, 3

• 0, 1, 2

• -1, 0, 1

• -2, -1, 0, 1, 2

What is the spin quantum number (m sub s) for an electron?

• 0 or 1

• 1 or -1

• 1/2 or -1/2

• 2 or -2

According to the Pauli exclusion principle, how many electrons can occupy the same orbital?

• 4

• 3

• 2

• 1

Which principle tells us the order in which an atom will fill up its orbitals?

• Heisenberg uncertainty principle

• Aufbau principle

• Pauli exclusion principle

• Hund's rule

What is the electron configuration of a neutral chlorine atom?

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p6 3s2 3p5

• 1s2 2s2 2p6 3s2 3d5

• 1s2 2s2 2p6 3s2 3p4

Tags

NGSS.HS-PS1-1

What are atoms with unpaired electrons in their orbital diagrams called?

• Antiferromagnetic

• Ferromagnetic

• Paramagnetic

• Diamagnetic