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 main focus of the problem discussed in the video?

• Understanding quantum numbers and electron configurations

• Calculating atomic mass

• Identifying isotopes

• Balancing chemical equations

Which element's electron configuration is being analyzed in the video?

• Oxygen

• Arsenic

• Carbon

• Helium

What is the abbreviated electron configuration for arsenic?

• [Ne] 3s2 3p6

• [Ar] 4s2 3d10 4p3

• [He] 2s2 2p6

• [Kr] 5s2 4d10

According to Hund's Rule, how are electrons distributed in orbitals?

• All electrons pair up in the first orbital

• Electrons fill each orbital singly before pairing

• Electrons fill the highest energy orbital first

• Electrons are randomly distributed

What is the principal quantum number (n) for the highest energy subshell in arsenic?

• 2

• 3

• 4

• 5

What is the azimuthal quantum number (l) for a p orbital?

• 0

• 1

• 2

• 3

What is the spin quantum number (m_s) for electrons in the highest energy subshell of arsenic?

• 0

• -1/2

• +1/2

• +3/2