chm115_lecture15

chm115_lecture15 - 22-1Chemistry 115Lecture 15...

Info iconThis preview shows pages 1–6. Sign up to view the full content.

View Full Document Right Arrow Icon

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

View Full DocumentRight Arrow Icon

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

View Full DocumentRight Arrow Icon

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

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 22-1Chemistry 115Lecture 15 OutlineChapter 8Intro to BondingLewis Dot StructuresEXAM 2: Thursday, March 10, 8pmElliot Hall of MusicChapters 5, 6, 7, 8 (Lewis dots)Recitation:Chapter 8: Lewis dot structuresExam 2 preparation (review Chapters 5-8)15-2Chapter 8 – Chemical BondingChemical bonding is a key to understanding the microscopic aspects that determine materials properties.We’ll talk about three types of bonding1. Ionic Bonding -electrostatic forces that hold ions together2. Covalent Bonding – shared electrons between atoms3. Metallic Bonding – metal nuclei “floating” in a sea of electrons.A key to understanding bonding is to know what the Valence electrons are doing, i.e, those electrons in the outer orbital shell of the atoms.15-3The three models of chemical bondingLewis electron-dot structuresDepicts the valence electronsUse A groupnumber to place dots around the atomsPair up the dots until they are all usedFor metals, number of dots = number of electrons it losesFor non-metals, the number of unpaired electrons tells you the number of bonds it can form.....·F:Cu·Na·Question: What are the Lewis dot structures for sodium, fluorine and copper(I)?15-4Ionic BondsInvolves a transfer of electron(s) from metal to non-metal and the formation of a solid ionic compoundLi [He]2s1+ F [He]2s22p5Li+1s2(or [He]) + F-[He]2s22p6or [Ne]Can also show this with Lewis dots:........Li· + ·F: Li++ :F:-Note that the F- ion has an octet of electrons – very stable. Li+also has a closed shell ([He])....
View Full Document

This note was uploaded on 04/09/2011 for the course CHM 115 taught by Professor Towns during the Spring '08 term at Purdue.

Page1 / 21

chm115_lecture15 - 22-1Chemistry 115Lecture 15...

This preview shows document pages 1 - 6. Sign up to view the full document.

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