Section 5.3—Molecules in 3D

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Presentation transcript:

Section 5.3—Molecules in 3D

Bonds repel each other Bonds are electrons. Electrons are negatively charged Negative charges repel other negative charges Bonds repel each other Molecules arrange themselves in 3-D so that the bonds are as far apart as possible

Valence Shell Electron Pair Repulsion Theory (VSEPR Theory) This theory (that bonds repel each other because they have like charges) attempts to explain why molecules form the shapes they form. Lewis Dot’s only allow us to see in 2-D! VSEPR allows us to visualize in 3-D!

What shapes do molecules form? http://intro.chem.okstate.edu/1314f00/lecture/chapter10/vsepr.html Linear 2 bonds, no lone pairs Indicates a bond going away from you Trigonal planar 3 bonds, no lone pairs Indicates a bond coming out at you

What shapes do molecules form? Tetrahedron 4 bonds, no lone pairs

Lone Pairs Lone pairs are electrons, too…they must be taken into account when determining molecule shape since they repel the other bonds as well. But only take into account lone pairs around the CENTRAL atom, not the outside atoms!

What shapes do molecules form? Bent 2 bonds, 1 lone pair

What shapes do molecules form? Bent 2 bonds, 2 lone pairs

What shapes do molecules form? Trigonal pyramidal 3 bonds, 1 lone pair

Ionic Compound structures Ionic compounds are made of positive and negative ions. They pack together so that the like-charge repulsions are minimized while the opposite-charge attractions are enhanced. Na+1 Cl-1