Lecture Notes: Behavior of Electrons and Atoms

Key Properties of Electron Waves

1. Energy and Size of Electron Waves

   • More loops in the electron wave = higher energy and larger size
   • Represented by n (Principal Quantum Number)

2. Shape of Electron Waves

   • Depends on the number of nodal planes
   • Represented by l (Azimuthal Quantum Number)

Understanding Single Electron Species

• For single electron species, focusing on n and l suffices, but multi-electron atoms require additional considerations.

Principles Governing Electron Behavior

1. Ground State

   • Electrons occupy the lowest possible energy wave available unless acted upon.
   • The lowest energy state of an atom is its ground state.
   • Example: Hydrogen's electron is a 1s electron unless excited.

2. Aufbau Principle

   • Electrons will always be in the lowest possible energy state available.

3. Pauli Exclusion Principle

   • No two electrons can have identical quantum numbers.
   • Allows for multiple electrons (e.g., 1s or 2p electrons) in an atom without violating this principle.

Upcoming Topics

• Further discussion on additional quantum numbers is needed for complete understanding of electron behavior in multi-electron atoms.
• These will be covered in the next few videos.