Ionic BondingIonic Bonding

Table of ContentsLecture/Lab/Activity Date Pg#

22. The Periodic Table 9/24/10 4723. Periodic Def & Trends 9/27/10 4924. Electron config practice 10/4/10 5125. Ions and Oxidation Numbers 10/5/10 5326. Lewis Dot Diagram 10/6/10 5427. Intro to Chemical Bonding 10/7/10 5728. Covalent Bonding 10/12/10 6129. Ionic Bonding 10/14/10 61

Objective:The student will construct Lewis dot diagrams to illustrate ionic bonds and discuss their properties during lecture.

Agenda:Ionic Bonding– LectureCovalent & Ionic Bonding - Homework

Ionic bonds are characterized as:

- bonds between metals & non-metals

- bonds between cations & anions

- bonds involving a transfer of e- (from a metal to a nonmetal)

Ionic compounds form crystalline lattice structures which are very strong.

High Melting Point Ex. Melting point for NaCl is 800°C

Na Cl+ Na+ Cl -+

Remember!!!

[Ne]3s1 [Ne]3s23p5 [Ne] [Ne]3s23p6

Na Cl Na+ Cl-

Anions have larger atomic radii

Cations have smaller atomic radii

Starting Valence e- = 8 Final Valence e- = 8

End Total Charge = 0Starting Total Charge = 0

When ionic compounds dissolve into solution, their + and – ions separate (electrolyte).

H2O surrounds ions in solution to prevent cations & anions from recombining (solvation)

+ = Na+(aq)

- = Cl-(aq)

Good electrolytes, like many ionic compounds are good conductors of electricity.

Electrolysis

How do ionic compounds with subscripts form?

Ex. How does MgCl2 form?

Mg

Cl

ClMg

Cl-

Cl-

2+

Diagram the formation of the ionic compound AlF3!

Al

F F

-

AlF

F

3+ F

-

F-

Find the balanced ionic formula for Calcium & Bromine.

Ca oxidation # = Br oxidation # =

+2

-1We need a 2nd Br atom to balance the net charge!

CaBr2

Ca

Br

Br

Ca2+

Br

Br-

-