Exploring SPDF Orbitals and Quantum Numbers

This video tutorial covers the SPDF sublevels, their shapes, and how they relate to energy levels. It explains the four quantum numbers (n, l, ml, ms) and how to identify them for specific electrons. The video also demonstrates writing electron configurations and orbital diagrams, using phosphorus as an example. Key principles like the Aufbau principle and Hund's rule are discussed to help understand electron arrangements.

What shape does the 's' sublevel have?

• Unusual

• Spherical

• Clover leaf

• Dumbbell

How many sublevels are present when n=3?

• 1

• 2

• 3

• 4

Which block in the periodic table corresponds to the 's' sublevel?

• Group 1 and 2

• Group 13 to 18

• Transition metals

• Lanthanides

Tags

NGSS.HS-PS1-1

How many electrons can the 'd' sublevel hold?

• 2

• 6

• 14

• 10

What is the value of 'l' for the 'p' sublevel?

• 3

• 0

• 1

• 2

What does the quantum number 'ms' represent?

• Orbital orientation

• Orbital shape

• Electron spin

• Principal energy level

For the 3p5 electron, what is the value of 'ml'?

• -1

• 0

• 1

• 2

According to the Pauli Exclusion Principle, no two electrons can have the same set of which numbers?

• n, l, and ms

• n, l, ml, and ms

• l and ml

• n and l

What is the electron configuration for phosphorus?

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p6 3s2 3d3

• 1s2 2s2 2p6 3s2 3p3

• 1s2 2s2 2p6 3s2 3d5

Tags

NGSS.HS-PS1-1

According to Hund's rule, how should electrons be added to degenerate orbitals?

• All at once

• One at a time

• In pairs

• Randomly