Practice Problem: Electron Configuration and Quantum Numbers

Professor Dave explains a practice problem involving quantum numbers and electron configurations for a neutral atom of arsenic. He details the ground state electron configuration and assigns quantum numbers to electrons in the highest energy subshell. The tutorial covers the electron configuration of arsenic, using the periodic table, and explains the assignment of quantum numbers, including principal quantum number, orbital type, and spin.

What is the ground state electron configuration for a neutral atom of arsenic?

How do the quantum numbers for the electrons in the highest energy subshell differ from those in lower energy subshells?

What is the role of Hund's Rule in filling the P orbitals for arsenic?

Explain the significance of the principal quantum number (N) in electron configurations.

What does the L value represent in quantum numbers, and how is it determined for P orbitals?

Describe how the M sub L values are assigned to electrons in the 4P subshell.

What is the significance of the spin quantum number (M sub S) in electron configurations?