Chapter 8 - Electronic Configuration Filling up of...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

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

View Full DocumentRight Arrow Icon
Electronic Configuration Filling up of electrons in atoms. 1. The Aufbau principle: Electrons are filled in such a way that the energy of atom is minimum. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, ……… 2. Pauli’s exclusion principle: No two electrons have all the four same quantum numbers same. 1. When orbitals of identical energy are available, electrons initially occupy these orbitals singly. Hund’s rule: An atom tends to have as many unpaired electrons as possible. Representations: 1. spdf notation (condensed). 2. spdf notation (expanded). 3. orbital diagram. http://www.chem.queensu.ca/people/faculty/Mombourquette/FirstYrChem/atomic/image145.gif The Aufbau Principle
Background image of page 2
Classification according to electronic configuration s-block p-block d-block f-block What is the electronic configuration of Ca, Mg, Li, K, F, Cl, Al, Sc and Zn? http://www.tabulka.cz/english/images/periodic_table.gif
Background image of page 3

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

View Full DocumentRight Arrow Icon
Noble gases He 2 1s 2 Ne 10 2s 2 2p 6 Ar 18 3s 2 3p 6 Kr 36 Xe 54 Rn 86 Special features: 1. Filled sub-shells.
Background image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 04/01/2011 for the course CHEMISTRY 1212 taught by Professor Staff during the Spring '11 term at Georgia State.

Page1 / 12

Chapter 8 - Electronic Configuration Filling up of...

This preview shows document pages 1 - 5. Sign up to view the full document.

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