Lacey_Che131_F2010_Lect-24-2p

Lacey_Che131_F2010_Lect-24-2p - Lec: 23-24: Electron...

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

View Full Document Right Arrow Icon
Lec: 23-24: Electron configurations & Periodic Trends Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 1 Electron Configurations Electrons enter and fill orbitals according to four rules: Pauli Exclusion Principle Orbitals can contain a maximum of two electrons which must be of opposite spin. Aufbau or Build-up Principle Electrons enter and fill lower energy orbitals before higher energy orbitals. Hund's Rule electrons will enter the orbitals one- at-a-time to maximize degeneracy Madelung's Rule Orbitals fill with electrons as n + l Electrons can not have the same four Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 2 quantum numbers
Background image of page 1

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

View Full DocumentRight Arrow Icon
Orbital filling Madelung's Rule Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 3 Orbital filling Electron configurations are reflected in the layout of the periodic table Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 4
Background image of page 2
Orbital Terms ` Orbitals that have the exact same energy level are degenerate. ` Core electrons are those in the filled, inner shells in an atom and are not involved in shells in an atom and are not involved in chemical reactions. ` Valence electrons are those in the outermost shell of an atom and have the most influence on the atom’s chemical behavior. Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 5 Orbital filling Electron configurations are reflected in the layout of the periodic table Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 6
Background image of page 3

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

View Full DocumentRight Arrow Icon
Electron Configurations 1s 2s 2p H: 1s 1 He: 1s 2 Li: 1s 2 2s 1 Be: 1s 2 2s 2 B: 1s 2 2s 2 2p 1 Roy A. Lacey, Stony Brook University; Che 131, Spring 2011 7 Electron Configurations 1s 2s 2p o C: 1s 2 2s 2 2p 2 or C: 1s 2 2s 2 2p 2 Hund’s Rule tells us which configuration is correc
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 02/21/2012 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

Page1 / 14

Lacey_Che131_F2010_Lect-24-2p - Lec: 23-24: Electron...

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