1. Chapter 9 – Molecular Geometry and Bonding Theories
Lewis Dot Diagrams shows the type of covalent bonds and number of nonbonding electrons in a molecule. But it doesn’t show us how the atoms are arranged in the molecule. The Valence Shell Electron Pair Repulsion (VSEPR) Theory allows us to determine the spatial arrangement of the atoms in a molecule. This is important because the molecular geometry determines the physical properties of a substance.

2. Covalent Compounds VSEPR Theory Valence Shell Electron Pair Repulsions
Bonding electrons and lone pairs of electrons will repel themselves so that they will separate by the maximum distance possible.

3. Covalent Compounds VSEPR Theory Valence Shell Electron Pair Repulsions
The shape of a molecule is determined by these repulsive forces.

4. Covalent Compounds Molecular Shapes
The geometry of most molecules can be explained using 9 geometric shapes
Linear
Trigonal Planar
Tetrahedral
Trigonal Bipyrimidal
See-Saw
T-Shaped
Square Planar
Square Pyramidal
Octahedral

5. Covalent Compounds Molecular Shapes Bonding versus Nonbonding Domains
A bonding domain refers to the number of bonding pairs of electrons.
A nonbonding domain refers to the number of nonbonding (lone pairs) of electrons on a central atom.
Ammonia has 4 domains – 3 bonding domains and 1 nonbonding domain.
Water has 4 domains – 2 bonding domains and 2 nonbonding domains.

6. Covalent Compounds Molecular Shapes Bonding Domains
How many domains does CO2 have?
How many domains does SO3 have?

7. Covalent Compounds Molecular Shapes Electron Domain Geometry
Predicts the shapes of molecules based on the geometric arrangement of electrons.
This method allows us to predict the shapes of many molecules.

8. Molecular Geometry Linear
A molecule consisting of just 2 electron domains will be linear.

9. Molecular Geometry Trigonal Planar
Will have a total of 3 bonding domains
3 bonding and
0 nonbonding domains bonding and 1 nonbonding domain
Trigonal Planar Bent

10. Molecular Geometry Tetrahedral Will have A total of 4 bonding domains
4 bonding domains 3 bonding and 1 nonbonding domain
Trigonal Pyramidal

11. Molecular Geometry Tetrahedral Will have a total of 4 bonding domains
2 bonding and 2 nonbonding domain
Bent

12. Molecular Geometry Trigonal Bipyramidal
Will have a total of 5 bonding domains
5 bonding and bonding and
0 nonbonding domains nonbonding domain
Trigonal Bipyramidal Seesaw

13. Molecular Geometry Trigonal Bipyramidal
Will have a total of 5 bonding domains
3 bonding and bonding and
2 nonbonding domains nonbonding domain
T-shaped Linear

14. Molecular Geometry Octahedral Will have a total of 6 bonding domains
6 bonding and bonding and
0 nonbonding domains nonbonding domain
Octahedral Square Pyramidal

15. Molecular Geometry Octahedral Will have a total of 6 bonding domains
4 bonding and
2 nonbonding domains
Square Planar

16. Molecular Geometry Molecular Polarity
Polarity means to have two electrically ‘opposite ends’.
Molecular shape and electronegativity of atoms determines the overall polarity of a molecule.

17. Molecular Geometry Molecular Polarity
Polarity means to have two electrically ‘opposite ends’.
Molecular shape and electronegativity of atoms determines the overall polarity of a molecule.
Nonpolar Polar

18. Molecular Geometry Molecular Polarity
Identify the following substances as either polar or nonpolar;
SO2
SF6
NF3
BCl3

19. Molecular Geometry Covalent Bonding and Molecular Overlap
Orbital overlapping occurs when two atoms form a covalent bond.
A molecule of hydrogen consists of two hydrogen atoms with overlapping s-orbitals.

20. Molecular Geometry Covalent Bonding and Molecular Overlap
Hydrogen chloride consists of a covalent bond formed form the overlapping of the hydrogen s-orbital with the chlorine p-orbital.

21. Molecular Geometry Covalent Bonding and Molecular Overlap
When atomic orbitals overlap, they can form a hybridized orbital.
A hydridized orbital has properties of both atomic orbitals that have combined to form a covalent bond.

22. Molecular Geometry Hybrid Orbitals
sp hybrid orbitals – forms when an s-orbital combines with one of the p-orbitals.
The resulting sp hybrid orbital has a two lobed shape with one the lobes being larger than the other.

23. Molecular Geometry Hybrid Orbitals
sp2 hybrid orbitals – forms when an s-orbital combines with two of the p-orbitals.
The resulting sp2 hybrid orbital has a three lobed shape.

24. What does this all mean? Molecular Geometry Hybrid Orbitals
sp3d hybrid orbitals – forms when an s-orbital combines with three of the p-orbitals and one d-orbital.
sp3d2 hybrid orbitals – forms when an s-orbital combines with three p-orbitals, and two d-orbitals.
What does this all mean?

25. Molecular Geometry Hybrid Orbitals
The hybridization of orbitals explains how an atom can form a covalent bond with other atoms and have a specific geometric shape.
If a central atom forms covalent bonds with 4 other atoms, then it must have hybridized its orbitals to accommodate 4 bonding spaces. Therefore one s and three p-orbitals must have hybridized to form an sp3.

26. Number of Electron Domains Electron Domain Geometry
Molecular Geometry
Hybrid Orbitals
Atomic Orbitals
Hybridized Orbitals
Number of Electron Domains
Electron Domain Geometry
s,p
2 - sp 2
linear
s,p,p
3 – sp2 3
Trigonal planar
s,p,p,p
4 – sp3 4
tetrahedral
s,p,p,p,d
5 – sp3d 5
Trigonal bipyramidal
s,p,p,p,d,d
6 – sp3d2 6
Octahedral
s,p,p,p,d,d,d
7 – sp3d3 7 ?

27. Molecular Geometry Sigma and Pi Bonds
Sigma Bond - A covalent bond where the overlapping bonding electrons are between the two nuclei of the bonding atoms.

28. Molecular Geometry Sigma (σ) and Pi (π) Bonds
Pi Bond - A covalent bond where the overlapping bonding electrons are perpendicular the two nuclei of the bonding atoms.

29. Molecular Geometry Sigma (σ) and Pi (π) Bonds
Single covalent bonds consist of 1 sigma bond.
Double covalent bonds consists of 1 sigma bond and 1 pi bond.
Triple covalent bonds consist of 1 sigma bond and 2 pi bonds.
CHCH