molecular geometries and isomers. topics å vsepr å the different geometries å electronic and...

Molecular Geometries and Molecular Geometries and IsomersIsomers

Topics

VSEPRThe Different GeometriesElectronic and MolecularBond AnglesIsomers

VSEPR

The Valence Shell Electron Pair Repulsion Theory states that electron pairs will take up postions in space, as far apart from one another as possible.This is because like charges repel each other.

Nonbonded pairs will take up more space around the central atom than bonded pairs.

This will affect the bond angles and the shape of the molecule.

Nonbonded vs. Bonded Pairs

Bond Angles are the angles formed between the atoms bonded around the central atom.

Ex. In a linear molecule such as CO2, the bond angles are 180o

O = C = O180o

Names of Molecular GeometriesNames of Molecular Geometries

Linear has 180o bond angles

Angular (Bent)~ 105o or ~120o

Triangular Planar ~ 120o

Pyramidal ~ 107o

Tetrahedral ~ 109o

There are exceptions to the octet rule. The names of these Geometries are...

Square Planar

Triangular Bipyramidal

Octahedral

Irregular Tetrahedral or see-saw

Square Pyramidal

T - Shaped

Don’t be disappointed but...

We will not be covering the exceptions to the octet rule.

Two Types of GeometriesTwo Types of Geometries

1. The electronic The electronic geometry is the shape of geometry is the shape of the particle, due to the particle, due to electron pairs electron pairs around the around the central atom.central atom.

Types of Geometries...Types of Geometries...

2. TheThe Molecular Molecular geometry is the shape of geometry is the shape of the particle, made by the the particle, made by the atoms bonded to atoms bonded to the the central atom.central atom.

How To Determine The Shape Of a Particle.

1. Draw the Lewis Dot Structure.

2. Count up how many positions are occupied around the central atom, (Atoms and / or electron pairs).

Use the following guide lines to draw a starting shape:

Two positions occupied = Linear.

Three positions occupied = Triangular Planar.

Four Positions occupied = Tetrahedral.

This is only how to start the drawing. There is more to come !

Ex. Consider H2O

The dot structure of water will show that there are 4 positions occupied around the O atom. Two positions are Hydrogens and two positions are nonbonding pairs of electrons.

The dot structure of water...

H O H:

..

..:1

23

4

So we start by drawing a tetrahedral shape.

Tetrahedral Shape

O

Two lines are on the same plane, the third is pointing back and the fourth points forward.

Now put the bonded atoms on the shape.

OH

H

Bond angles between bonding atoms are ~105o

105o

What this diagram shows is...

A structure that has 4 positions around it has an electronic geometry of TETRAHEDRAL.

If only Two of the Four positions are bonded, then the molecular geometry is ANGULAR.

Ex. 2 Four Positions Occupied

Consider NH3

The dot structure of NH3 has 4 positions around the Nitrogen.

Notice that there are only 3 bonds.

Draw the structure for 4 positions.

N

add the bonded atoms

HH

H

Bond angles between bonding atoms are ~ 107o

107o

What this diagram shows is...

Since there are 4 positions occupied, the electronic geometry is still tetrahedral.

Only 3 of the 4 positions are bonded atoms, so the molecular geometry is PYRAMIDAL.

Ex. 3 Four positions occupied and all four are bonded.

CH4 H

H C H

H

:.... :

Four positions occupied and Four positions occupied and all four all four bondedbonded make a tetrahedral electronic make a tetrahedral electronic andand molecular geometry. molecular geometry.

Some models of molecules with 4 occupied positions...

Tetrahedral electronic and molecular geometries

~109o

angles

Pyramidal - 4 positions, 3 bonded (Molecular geometry)

Ex. NH3

Angular Molecular Geometry - 4 positions, 2 are bonded

Ex. H2O

Structures with 3 occupied positions - Electronic geometry = triangular Planar

Ex. SO2 The dot structure shows that only 2 of the positions are bonded.

O S O:.. ....

....:::

Draw the structure with 3 occupied positions...

and add the bonded atoms.

S

O O The molecular geometry is ANGULAR

resonance

Three occupied positions with all three positions bonded...

Ex. NO31-

The dot structure shows that the electronic and molecular geometries are triangular planar.

Some molecular diagrams with three occupied positions...

Ex. SO2

3 Occupied Positions...

Ex. NO3

~120o

bond angles

Two Occupied Positions Are Always Linear Electronic and Molecular

Ex. CO2

The dot structure shows that there are two positions occupied and both positions are bonded.

Two Positions ...

:: :: : :..

.. Note that the CENTRAL ATOM has no nonbonded electrons. If it did, they would cause the molecule to bend.

O C O

Two positions occupied with one postion bonded...

Ex. CN- C N:::: :

When ever there are only TWO Atoms, both the electronic and molecular geometries are Linear.

Molecular Diagrams With Two Occupied Positions...

Ex.

CN-

Two Positions...

Two resonance structures of CO2 - LINEAR

180o bond angles

IsomersIsomers are two or more compounds with the same molecular formula but different bonding arrangements. Some of them have different physical and chemical properties while others only have reactive differences.

Constitutional or Structural Isomers

These isomers have their atoms bonded in a different order.

The order of bonding may change the functional group.

It may involve branching in the carbon chain.

The double bonds may be in different locations.

Ex. C3H8O

Structural Isomers

H H H

H C C C O H

H H H

: : : : :.. .. ..

.. .. .. ....

H H H

H C O C C H

H H H..

..

Propanol-->

<--Methoxy ethane

Example; Branching

C 4 H10 H H H H

H C C C C H

H H H H

..:

.. .. ..

.. .. .. ..:: : :

continued...

C 4 H10continued...

H H H

H C C C H

H H

H C H

H

Double bond locations differ...

C4H8

H H H H

C C C C H

H H H

H H H H

H C C C C H

H H

(a)

(b)

How do these structures differ?

The top structure (a) is called 1-butene and the bottom structure (b) is called 2-butene.

They have different physical and chemical properties; b.p., m.p. etc.

StereoisomersStereoisomers

Cis and Trans isomers

Optical isomers

Cis and Trans Isomers

The atoms are bonded in the same order but they are oriented differently in space.

H CH3

C C

CH3 H

Trans-2-butene

A trans isomer...

C 4 H 8

A cis isomer...

CH3 CH 3

C C

H H

cis-2-butene

C4H8

Optical Isomers

Optical isomers are substances that rotate plane polarized light.

An optical isomer contains a chiral carbon in its structure.

Rotation of plane polarized light...

Visible light travels in scattered waves. A polarizer concentrates the light so that it travels in only one direction. It is then polarized.

When polarized light is passed through an optical isomer and viewed through an instrument called a polarimeter, the angle of the light wave is rotated.

Rotation of plane polarized light continued...

A Chiral Carbon

A chiral carbon is an asymmetrical carbon, that is, one that has four different groups bonded to it.

Ex. of chiral carbons

CH2 OH This is NOT a chiral carbon because there are Two H’s bonded to it. It doesn’t have 4 different groups.

Chiral Carbons continued...

HCBrFOH

H

F C

Br OH

The carbon in this compound is chiral because it DOES contain 4 different groups.

Enantiomers

Entiomers are pairs of optical isomers that are non-superimposible mirror images.

EnantiomersMirror images are like your right and left hands. They are the same but opposite and no matter how hard you try, you cannot lie them flat on top of each other in the same direction.

Enantiomers

Non-superimposible means just that, you cannot lie them flat on top of each other in the same direction and have them fit.

Enantiomers

Many drugs (medications) are enantiomers (non-superimposible mirror images). One of the mirror images will be more active or beneficial than the other.

What To Know, What To Know

VSEPR

THE GEOMETRIES -draw and name them, give real examples

Types of isomers - draw examples of each. (The book has several examples).

Bond angles