This document discusses electron configuration and the principles that govern how electrons are arranged in atoms. It explains that electrons exhibit wave-like properties and occupy regions of space called atomic orbitals. The distribution of electrons in atoms, known as electron configuration, follows three main principles: the Pauli Exclusion Principle limits orbitals to two electrons of opposite spin; the Aufbau Principle states that orbitals are filled from lowest to highest energy; and Hund's Rule specifies that orbitals are singly occupied with parallel electron spins before double occupation occurs.

1. Electron configuration
Reported by Marvin B. Gonzaga

2. Atomic orbitals
• Since an electron moves so fast, it shows
wavelike properties.
• The electron is most likely to be found
where its wave intensity was greatest and
least likely to be found where its wave
intensity was smallest.

3. Orbitals
Specifies a volume
of space where
the electron is
most likely to be
found
Atomic orbitals

4. Electron Configuration
• How electrons are
distributed in an atom.
• Designation of the most
probable distribution of
electrons.

5. 3 Principles in Electron Configuration
• Pauli Exclusion Principle
• Aufbau Principle
• Hund’s Rule

6. Pauli Exclusion Principle
• A maximum of 2
electrons may
occupy an
orbital, and
these 2
electrons must
have opposite
spins

7. Aufbau Principle
• German for
“build up”
• Electrons fill
orbitals starting
at the lowest
available energy
state before
filling higher
states.

8. Electron Distribution Mnemonics

9. Hund’s Rule
• Every orbital in a
sublevel is singly
occupied before any
orbital is doubly
occupied.
• All of the electrons in
singly occupied
orbitals have the
same spin (to
maximize total spin).

10. Example

11. Thank You