Chapter 9 Pptrevised

Chapter 9 Notes Part I Covalent Bonding

Obj. 1…Octet Rule ,[object Object],[object Object],[object Object],- (+) cations - (-) anions ,[object Object],- happy already! *** atoms need other atoms in order to lose/gain e-. - electronegativity differences determine bond. - metals = low / non-metals = high electroneg.

Obj. 2…Ionic Bonds ,[object Object],- compounds created are neutral - 10% of all bonds - strongest bond - forms crystalline solids - highest melting/boiling pts. - can conduct electricity in molten states.

Obj. 3…Pure Covalent Bonds ,[object Object],- compounds created are neutral - 2% of all bonds - weakest bond - typically form gases - lowest melting/boiling pts. - do NOT conduct electricity!

Obj. 4…Polar Covalent Bonds ,[object Object],- compounds created are neutral - 88% of all bonds - intermediate bond strength - typically form soft solids and liquids - intermediate melting/boiling pts. - some conduct electricity in molten states.

Obj. 6…Metallic Bonds ,[object Object],mobile e-…(‘ delocalized e- ’). ,[object Object],- cushion b/n cations cations.

Obj. 6 cont… ,[object Object],- as e- enter one end, an = # of e- leave the other ,[object Object],- can be drawn into a wire ,[object Object],[object Object],- can be hammered

Obj. 7…Bonding Vocabulary ,[object Object],atom w/ a charge. - has lost or gained e- ,[object Object],all e- in outer ‘s’ and ‘p’ orbitals. ,[object Object],molecule w/ one slightly (-) end and one slightly (+) end. - occurs in polar covalent bonds ,[object Object],a group of atoms (covalently bonded), that act as a single atom - NH 4 +1 , SO 4 -2 , ClO 3 -1 ,[object Object],atoms covalently bonded together.

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

It ends up being a “tug of war” of electrons Where the electrons end up somewhere in the middle.

Single Bonds ,[object Object],[object Object]

Double and Triple Bonds ,[object Object],[object Object]

Sigma and Pi Bonds ,[object Object],[object Object]

Sigma and Pi Bonds ,[object Object]

Sigma and Pi Bonds ,[object Object],[object Object],[object Object]

Sigma and Pi Bonds ,[object Object],NH 3 CH 2 O SiO 2

Strength of Covalent Bonds ,[object Object],[object Object],[object Object]

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

Naming Molecules 9.2 ,[object Object],[object Object],[object Object],[object Object]

Prefixes in Covalent Compounds ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Naming Acids binary acids ,[object Object],[object Object],[object Object]

Naming Oxyacids ,[object Object],[object Object],[object Object]

Writing Formulas from Names ,[object Object],[object Object]

Coordinate Covalent Bonding ,[object Object]

Resonance, cont. ,[object Object],[object Object]

An Addendum to Lewis Structures ,[object Object]

Drawing Dot Diagrams ,[object Object],[object Object],[object Object],X 1 2 8 5 7 4 6 3

The reason for this order, is the first two spots for electrons represent the one orbital in the s sublevel, the last three spots represent the three orbitals of the p sublevel.

Your book’s way to Draw Lewis Dot Structures ,[object Object],[object Object],[object Object],[object Object]

Exceptions to the Octet Rule ,[object Object],[object Object],[object Object]

Covalent Bonding and Polyatomic Ions ,[object Object],[object Object]

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

Chapter 16 Notes Part II VSEPR Theory

The VSEPR Theory ,[object Object],[object Object]

Shapes not involving unshared pairs: ,[object Object]

Shapes not involving unshared pairs: ,[object Object],[object Object],[object Object],[object Object]

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

Trigonal Planar ,[object Object],[object Object],[object Object]

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

Trigonal Bipyramidal ,[object Object],[object Object],[object Object]

Shapes that involve an unshared pair: ,[object Object],[object Object],[object Object]

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

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

Obj. 8… Intra molecular Bonds vs. Inter molecular Attraction ,[object Object],- bonds w/in a molecule - i.e. holds H and O together in water (H 2 O) - ionic, covalent, polar covalent and metallic ,[object Object],- attraction b/n two or more different molecules. - i.e. holds H 2 O molecules together in a pond. ** always weaker than intramolecular bonds. - strength indicates solid, liquid or gas.

Obj. 9-10…Intermolecular Attractions ,[object Object],- dispersion forces - dipole interactions - Hydrogen bonds van der Waals forces ( weakest ) (strongest) ,[object Object],- seen in Halogen diatomic molecules (Z 2 ) - strength of force as # of e- in molecules - F and Cl have few e- = weak DF (gases) - Br has more e- = stronger DF (liquid) - I has most e- = strongest DF (solid)

Obj. 9-10 cont… ,[object Object],- slightly (-) pole attracted to (+) pole of another molecule. - similar to but much weaker than ionic bonds

Obj. 9-10 cont… ,[object Object],- strong attraction b/n H on one polar molecule and the e- of an electronegative atom (N,O, or F) from a different molecule. - H atom is forced to share its only e- - H is therefore very attracted to pair of e- in neighboring molecule.

Obj. 9-10 cont… ,[object Object],dispersion forces dipole interactions Hydrogen bonds Covalent bonds Metallic bonds Ionic bonds van der Waals inter molecular intra molecular WEAKEST STRONGEST (Pure and Polar)

Chapter 16 Notes, part III Bond Polarity and Molecular Polarity

Types of Bonds ,[object Object],[object Object]

Nonpolar Covalent ,[object Object],[object Object],[object Object],[object Object]

Polar Covalent ,[object Object],[object Object],[object Object]

[object Object],[object Object],Polar Covalent H—Cl H—Cl  +  - OR

Ionic Bonds ,[object Object],[object Object]

How can you tell what kind of bond there is? ,[object Object],[object Object],[object Object]

Ionic Bonds - highest electronegativity diff. (ED  1.67) Ex… NaCl: Na + = 0.9 Cl - = 3.0 3.0 – 0.9 = KBr: K + = 0.8 Br - = 2.8 2.8 – 0.8 = 2.1 2.0

Polar Covalent Bonds - lowest electronegativity diff. (ED  0.4) Ex… H 2 : H + = 2.1 H + = 2.1 2.1 – 2.1 = 0 CH 4 : C = 2.5 H + = 2.1 2.5 – 2.1 = 0.4

Nonpolar Covalent Bonds - int. electronegativity diff. (ED 0.41 - 1.66) Ex… H 2 O: H = 2.1 O = 3.5 3.5 – 2.1 = 1.4 CO 2 : C = 2.5 O = 3.5 3.5 – 2.5 = 1.0

Nonpolar Bonds: EN Diff ≤ 0.4 Polar Bonds: 0.4 < EN Diff ≤ 1.7 Ionic Bonds: EN Diff > 1.7

Practice ,[object Object],HBr KCl CO 2 2.8 – 2.1 = 0.7 PC 3.0 – 0.8 = 2.2 I 3.5 – 2.5 = 1.0 PC Li 2 O 3.5 – 1.0 = 2.5 I Br 2 2.8 – 2.8 = 0 ,[object Object],1 2 3 4 5 C

What type of bond is between: ,[object Object],[object Object],[object Object],[object Object]

What type of bond is between: ,[object Object],[object Object],[object Object]

Polar Molecules ,[object Object]

Polar Molecules ,[object Object],[object Object]

Chapter 9 Pptrevised

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