Molecular Shapes. VSEPR Valence Shell Electron Pair Repulsion The main idea is that electrons don’t like to hang around near each other because they repel.

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Presentation transcript:

Molecular Shapes

VSEPR Valence Shell Electron Pair Repulsion The main idea is that electrons don’t like to hang around near each other because they repel each other. As a result, the atoms in a molecule tend to separate as far as they can because their bonds repel each other.

Shapes Linear Lone pairs : 0 A Lone Pair is a pair of electrons that are not involved with bonding

Shapes Bent Lone pairs : 2

Shapes Trigonal Planar Lone pairs : 0 This shape is typically formed with Boron. Boron is an exception to the octet rule and can be happy with only 6 valence electrons.

Shapes Trigonal Pyrimidal Lone pairs : 1

Shapes Tetrahedral Lone pairs : 0

Recap Linear = 0 lone pairs Bent = 2 lone pairs Trigonal Planar = 0 lone pairs Trigonal Pyramidal = 1 lone pair Tetrahedral = 0 lone pairs

Polar covalent molecules: A type of bond that forms when electrons are not shared equally (nonsymmetrical) Non polar molecules: A type of bond that forms when electrons are shared equally (symmetrical)

Polarity Go back to page 6 and for each shape, include the following examples of when the shape is polar and non polar.

Shapes Linear Symmetrical Non-Polar Nonsymmetrical Polar Linear can be Non- Polar OR Polar depending on if the outside atoms are similar or different.

Shapes Bent Always Nonsymmetrical Polar This molecule is NOT symmetrical horizontally.

Shapes Trigonal Planar Symmetrical Non-Polar Nonsymmetrical Polar Trigonal Planar can be Non- Polar OR Polar depending on if the outside atoms are similar or different.

Shapes Trigonal Pyrimidal Lone pairs : 1 Always Nonsymmetrical Polar This molecule is NOT symmetrical horizontally.

Shapes Tetrahedral Symmetrical Non-Polar Nonsymmetrical Polar Tetrahedral can be Non-Polar OR Polar depending on if the outside atoms are similar or different.

Molecular Lab On the next page in the Unit 6 Packet. You will draw electron dot diagrams, and then build the molecules using the plastic models. All of the holes need to be filled. Use the longer “bendy” ones to make double bonds. Each kit should have the exact number of atoms in order to make all of the molecules without having to take any apart. We will fill in the last column next class together.

Substance (Formula) Dot Diagram Name of shape # Lone Pairs Drawing of modelMolecular PolaritySoluble in Water? hydrogen ( H 2 ) H-HLinear 0 NonpolarNo Water (H 2 O) Ammonia (NH 3 ) Methane (CH 4 ) Carbon Dioxide (CO 2 ) Hyrochloric Acid (HCl) Ethyne (C 2 H 2 ) CH 3 Cl Molecular Model Lab