Bonding 2008

Bonding ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

I. Metallic Bonds ,[object Object],[object Object],[object Object],[object Object]

I. Metallic Bonds Cont’d ,[object Object],[object Object],[object Object],[object Object]

II. Ionic compounds ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object]

Reminder: Valence electrons ,[object Object],[object Object]

II. Ionic compounds 4. Salts such as NaCl form crystals a. Crystals = solids w/ repeating patterns (“crystal lattice”)held together by electrostatic attractions

III. CovalentCompounds ,[object Object],[object Object],[object Object],[object Object],[object Object]

E. Polarity ,[object Object],[object Object],[object Object],[object Object],[object Object]

I. Lewis Structures for Molecular Cmpds ,[object Object],[object Object],[object Object],[object Object]

I. Lewis Structures ,[object Object],[object Object],[object Object],[object Object]

[object Object],C. Compounds formed with covalent bonds are neutral and follow the OCTET rule ! 1. All atoms are most stable when they have the electron configuration of a noble gases (THIS MEANS HAVING EIGHT* VALENCE ELECTRONS) *Exceptions exist

II. Steps for drawing Lewis Structures ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

II. Steps for Drawing Lewis Structures D. Some General Guidelines 1. Often the central atom is the first one in the formula 2. Carbon likes to be in the middle with four bonds around it 3. Halogens like to be on ends with only one bond 4. Hydrogen MUST be on an end 5. Oxygen likes two bonds

Try these examples ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

III. Special Cases ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

III. Special Cases ,[object Object],[object Object],[object Object],[object Object]

III. B 1a. Electron deficient ,[object Object],[object Object],[object Object],[object Object]

III. B 1b Expanded Octets ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Periodic Table Trends ,[object Object],[object Object],[object Object],[object Object],[object Object]

I. Ionization Energy ,[object Object],[object Object],[object Object]

Ionization Energy & the Periodic Table Elements with the highest ionization energies occur in the upper right corner (most chemically active nonmetals) Elements with the lowest ionization energies are in the lower left corner of the table (most chemically active metals)

II. Electronegativity ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

III. Atomic size ,[object Object],[object Object]

III. Atomic Size & the P.T. Size is decreasing Size is decreasing

IV. Ionic size ,[object Object],[object Object]

Bonding 2008

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Bonding 2008