Unit1_Chap12_SUM08Zumdhal-4

Unit1_Chap12_SUM08Zumdhal-4 - The Aufbau Principle and the...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
The Aufbau Principle and the Periodic Table We can have n 2 atomic orbitals/principal energy level. Since two electrons can occupy one orbital, we can have a maximum of 2n 2 electrons/principal energy level. 1- Aufbau Principle: When writing electron configuration, electrons are added to the lowest energy level. n = 5 s p d f n = 4 s p d f n = 3 s p d n = 2 s p n = 1 s 2- Hund’s Rule: Electrons occupy all orbitals in a sublevel of energy before pairing begins. These unpaired electrons must have parallel spins. 3- Pauli Exclusion Principle: No two electrons in an atom can have the same four quantum numbers (2 electrons occupying the same orbital must have opposite spin). Paramagnetism and Diamagnetism Paramagnetism: Weak attraction toward a magnetic field. It is due to the presence of unpaired electrons. Diamagnetism: Weak repulsion by a magnetic field. It occurs when all the electrons are paired.
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
POLYELECTRONIC ATOMS How can the quantum mechanical model of the hydrogen atom be extrapolated to account for polyelectronic atoms? Let’s consider a He atom.
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 12/04/2010 for the course BIO 311 C taught by Professor Mcclelland during the Spring '09 term at University of Texas.

Page1 / 3

Unit1_Chap12_SUM08Zumdhal-4 - The Aufbau Principle and the...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online