Monday and Tuesday March 26 and 27. Lewis Dot Structures.

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Presentation transcript:

Monday and Tuesday March 26 and 27

Lewis Dot Structures

Review? 1.What is a valence electron? 2.What is the lewis dot structure of: a)Lithium b)Bromine Do your best to answer on your own.

Valence Electrons The valence electrons are the electrons in the last shell or energy level of an atom. Why are they important? -BONDING!

Valence Electrons How many for each element?

Lewis Dot Structures What is the lewis dot structure of: a)Lithium b) Bromine

Lewis Dot Structures Draw the lewis dot structure for lithium bromide: Draw the lewis dot structure of calcium chloride: Draw the lewis dot structure of methane (CH 4 ): Identify the lone pairs and bonding pairs! **NO LONELY ELECTRONS!! Draw the lewis dot structure of oxygen gas:

Chemical Bonding Types of Bonds, Polarity, and Dipoles

What is electronegativity? The ability of an element to steal an electron from another element

What are BONDS? The attraction between atoms Causes shape and structure of chemicals

Types of Bonds Non-polar (Covalent) 0.0 Polar (Covalent) 0.1 to 1.9 Ionic 2.0 or higher

Nonpolar Covalent Bond Electronegativity Difference of 0.0 Electrons are shared equally

Polar Covalent Bond Electronegativity Difference of 0.1 – 1.6 Electrons are shared, however, they favor one side of the molecule.

Copyright © 2006 by the Regents of the University of California.

Two types of Covalent Bonds NONPOLAR POLAR

Ionic Bond Electronegativity Difference of 1.7 or higher Electrons are transferred to the other element.

Types of Bonds Non-polar (Covalent) 0.0 Polar (Covalent) 0.1 to 1.9 Ionic 2.0 or higher

Practice Draw the lewis dot structure for the formulas below and identify the bond type: Potassium Bromide Carbon Disulfide Nitrogen Trifluoride

Wednesday 3/28 and Thursday 3/29

Modeling Lab

Friday 3/30

How are molecular shapes determined? VSEPR

Lewis Structures & VSEPR Valence Shell Electron Pair Repulsion electron pairs spread apart as far as possible

Electron Pair Geometry: Linear Molecular Geometry: Linear Number of Lone Pairs: 0 Number of Bonds: 2 Angle: 180 ̊

Electron Pair Geometry: Trigonal Planar Molecular Geometry: Trigonal Planar Number of Lone Pairs: 0 Number of Bonds: 3 Angle: 120 ̊

Electron Pair Geometry: Trigonal Planar Molecular Geometry: Bent Number of Lone Pairs: 1 Number of Bonds: 2 Angle: 117 ̊

Electron Pair Geometry: Tetrahedral Molecular Geometry: Tetrahedral Number of Lone Pairs: 0 Number of Bonds: 4 Angle: ̊

Number of Lone Pairs: 1 Number of Bonds: 3 Electron Pair Geometry: Tetrahedral Molecular Geometry: Trigonal Pyramidal Angle: ~107 ̊

Electron Pair Geometry: Tetrahedral Molecular Geometry: Bent Number of Lone Pairs: 2 Number of Bonds: 2 Angle: ̊

Questions on shape?

Dipoles Contains a positive end and a negative end.

Copyright © 2006 by the Regents of the University of California.

Practice CO 2 NH 3 BF 3 Li 2 O