Ionic Bonding

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December 03, 2009

Ionic Bonding - the force of attraction between oppositely charged particles (+ - ) "magnetism" It is a very strong force of attraction. Therefore very strong IMFs!

Characteristics of Ionic compounds: Solids 1. do not conduct heat or electricity 2. brittle crystalline structure 3. very high melting point 4. typically soluble (dissolvable) in polar solvents such as water. Solution 5. Can conduct electricity in proportion to it's concentration (is an "electrolyte") Why? because of the body of mobile charge that now exists

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December 03, 2009

Ionic Bonding- the force of attraction between oppositely charged particles. Main Ideas1. Usually between a metal and a nonmetal 2. Typically the difference in electronegativity between atoms is greater than or equal to 1.7 3. Ionic bonds form compounds that are NEUTRAL, electrons lost(+) = electrons gained (-) Structures and Formulas always include: BRACKETS, DOTS and CHARGES Structure ex1) Na Cl

Na

Formula

[ Cl ]

NaCl

[ O]

K O 2

K ex2) K

O

K Al ex3) Al

[S]

S

Al

[S] [S]

Al2S3

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December 03, 2009

Shortcut to writing Formulas 1. If the charges balance it's a 1:1 ratio

2. If the charges are multiples, reduce then switch

3. If 1 or 2 above does not apply, switch charges

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December 03, 2009

Naming Rules for Ionic Compounds1. metal/nonmetal- name metal first, nonmetal second with "ide" ending ex: NaBr - sodium bromide K2O - potassium oxide Mg2N3 - magnesium nitride

2. transitional metal/nonmetal- same as #1 but specify the ox.# of metal with roman numerals ex: FeO - iron II oxide Fe2O3 - iron III oxide

MnO2 - manganese IV oxide

3. polyatomic ions- #1,2 still apply in addition simply read p.a.i. from Table E. ex. NH NO - ammonium nitrate 4 3 (NH4)3PO4 - ammonium phosphate Ti(C O ) - titanium IV oxalate 2 42