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Chapter 9 – Molecular Geometry and Bonding Theories
Homework:11, 13, 15, 19, 20, 21, 25, 26, 31, 34, 35, 36, 39, 41, 42, 43, 44, 47,
49, 51, 54, 56, 96, 100
9.2 – The VSEPR Model Two balloons
Linear arrangement Three balloons
Trigonal-planar arrangement Four balloons
Tetrahedral arrangement
Electrons in molecules behave like balloons
A single covalent bond forms between atoms when a pair of electrons is between the atoms A bonding pair of electrons defines a
region in which the electrons are most likely to be found between two atoms
This area we find electrons is called an electron domain
A nonbinding pair (or lone pair) defines an electron domain located around one atom
Example
• Four electron domains here
•In general, each nonbinding pair, single bond or multiple bond produces an electron domain around the central atom
Because electron domains are negatively charged, they repel each other.
The best arrangement of a given number of electron domains is the one that minimizes the repulsions between them. This is the basic idea behind the
VSEPR model.
Similar to Balloons? You bet! Two domains makes linear
arrangement Three domains makes trigonal-
planar arrangement Four domains makes tetrahedral
arrangement
pg. 349
The arrangement of electron domains about the central atom is called its electron–domain geometry.
In contrast, the molecular geometry is the arrangement of only the atoms in a molecule or ion So any non-bonding pairs are not a part
of the molecular geometry
The VSEPR model predicts electron-domain geometry From this and knowing how many domains
are due to nonbinding pairs, we can predict the molecular geometry
When all the electron domains in a molecule come from bonds, the molecular geometry is the same as the electron-domain geometry But if one or more domains comes from lone
pairs, we must ignore those domains for molecular shape
pg. 351
Example NH3
Already done this. 4 electron domains around central atom
So electron-domain geometry is tetrahedral We know 1 of those domains comes
from lone pairs So the molecular geometry of NH3 is trigonal
pyramidal Tetrahedral with one less end, see pg. 347
Steps using VSEPR model to predict shape of molecules
1. Draw Lewis structure Count number of electron domains around
central atom
2. Determine electron-domain geometry Use table 9.1, 9.2 or 9.3
3. Use the arrangement of the bonded atoms to determine the molecular geometry
Use table 9.2 or 9.3
Example CO2
1. Draw Lewis Structure
How many electron domains around the central atom are there?
2. What is the electron-domain geometry for this?
Linear
3. What molecular geometry is possible? Linear
Effect of Nonbonding Electrons and Multiple Bonds on Bond Angles
We refine the VSEPR model to predict and explain slight variances from the ideal bond angles Methane (CH4), ammonia (NH3) and
water (H2O) all have tetrahedral electron-domain geometries
But their bond angles are a little different CH4 = 109.5º, NH3= 107º and H2O = 104.5º Differences based around which type of
electron pairs make up the electron domains
Bond angles decrease as the # of nonbonding electron pairs increase. Bonding pair of electrons attracted by
both nuclei of the bonded atoms Lone pair of electrons attracted
primarily by one nucleus
Because lone pair has less nuclear attraction, it’s domain becomes more spread out So electron domain for lone pairs exert
more repulsive force on adjacent electron domains
This compresses (lessens) the bond angles Since H2O had the most lone pairs, it
gets the shortest bond angles
Multiple Bonds an Bond Angles Multiple bonds have a higher
electron-charge density than single bonds Also creates larger electron domains So electron domains for multiple
bonds exert a greater repulsive force on adjacent electron domains than single bonds do
So multiple bonds (double or triple) will decrease the bond angles too
Phosgene (Cl2CO)
Central atom has three electron domains 3 single bonds Trigonal planar geometry
Double bond acts like a lone pair, reducing the Cl-C-Cl bond angle
How Do These all Compare?
In terms of volume occupied by electron pairs In other words, who compresses the
most? Lone pair > triple bonds > double bonds
> single bonds
Molecules with Expanded Valence Shells So far we have assumed the
molecules have no more than an octet of electrons But the most common exception to
the octet rule is a central atom having greater than 8 valence electrons
So we need to deal with molecules with 5 or 6 electron domains
pg. 354
Example Use the VSEPR model to predict the
electron and molecular geometry of ClF3
Step 1: Lewis structure
How many electron domains around central atom? 5
5 electron domains Gives us an electron geometry of trigonal
bipyramidal How many bonding domains?
3 How many non-binding domains?
2 So its molecular geometry is
T-shaped
Shapes of Larger Molecules The VSEPR model can be extended
to more complex molecules than we’ve been dealing with.
Consider acetic acid CH3COOH
Acetic acid has 3 interior atoms Carbon, and each oxygen
We can use VSEPR to look at each central atom individually
9.3 – Molecular Shape and Molecular Polarity Remember that bond polarity
measures how equally the electrons in a bond are shared between the two atoms Higher bond polarity = less equal
sharing Higher electronegativity difference =
higher bond polarity
The dipole moment depends on both the polarities of the bonds and the geometry of the molecule Last chapter we focused just on the
polarity effect on the dipole moment For every bond in the molecule, we
can look at the bond dipole The dipole moment that is due ONLY
to the two atoms in the bond
Example CO2
O=C=O Each C=O bond is polar (O is more
electronegative than C) Since we have two O=C bonds, the
bonds are identical We end up with high electron density
around the O, and low electron density in the middle
Bond dipoles and dipole moments are vectors The overall dipole moment is the sum of the bond
dipoles that make it up But, must consider both the amount of the
dipole, and the direction of the dipole We have two identical C=O bonds, so the
amount of the dipoles are the same But the DIRECTION of the dipoles are opposite This causes the individual bond dipoles to cancel
each other out So the geometry of CO2 indicates that it is a NONPOLAR
molecule, even though it contains polar bonds.
Bond Dipole Activity Bond Dipole Activity
Steps to Determine Molecular Polarity
1. Draw Lewis structure2. Determine molecular geometry3. Look at effects of
electronegativity differences
9.4 – Covalent Bonding and Orbital Overlap The VSEPR gives as a method to predict
the shape of molecules Does not explain WHY the bonds exist
between atoms A mixture of Lewis’ notion of electron-
pair bonds and atomic orbitals leads to a model of chemical bonding This mixture of views is called the valence-
bond theory
In Lewis theory, covalent bonding occurs when atoms share electrons The sharing concentrates electron density
between the two nuclei involved In valence-bond theory, the build-up of
electron density between the nuclei is thought of as occurring when a valence atomic orbital of one atom merges
with a valence atomic orbital of another atom
This merger of orbitals Means that they share a region of
space Called overlap
The overlap of orbitals allows two electrons of opposite spin to share the common space between the nuclei
Forming an atomic bond
See figure 9.14 on pg. 360
Distance There is always an optimum
distance between the two bonded nuclei in a covalent bond Too close = too much repulsion
between the nuclei Too far = not much overlap, not a
strong bond
9.5 – Hybrid Orbitals