Lewis Dot Structures and

Molecular GeometryChapter 8 in online textChapter 15 in desk text

Why STUDY?

Warm-Up

What is the electron configuration of carbon?

How many valence electrons does Carbon have?

1s22s22p2

4

To determine the Lewis dot structure for Carbon we look at the number of valence electrons carbon has.

Carbon has four valence electrons and we represent electrons as DOTS.

C

Lewis Dot Structures for the first 10 elements on the periodic table.

Chemists use Lewis Dot Structures to determine how elements are covalently bonded to each other in a molecule.

• Covalently Bonded means to share electrons between elements. Sharing of electrons occurs between a nonmetal and another nonmetal.

• Single Bond- 2 electrons are shared• Double Bond- 4 electrons are shared• Triple Bond- 6 electrons are shared

Draw the Lewis Dot structure for BeF2.

1.Count the number of valence electrons you have to work with.Be F

Total : valence electrons

2. Put the least electronegative element in the center (remember the trend of E.N)**One exception: we never put Hydrogen in the center, because it can only make one bond.

3.Use pairs of electrons to form bonds between all atoms. (2 electrons make one bond)4.Use the remaining electrons to complete the octet rule for each element. (Exception: Be disobeys the octet rule it only has two valence electrons)

5.If you run out of electrons, you must introduce multiple bonds to maintain the octet rule. (BeF2 does not have multiple bonds-we will do more examples of this)

Let’s try to draw a Lewis Dot Structure of CO2 using the Rules1.Count the number of valence electrons you have to work with.

C O

Total : valence electrons

2. Put the least electronegative element in the center (remember the trend of E.N!!!?)

3.Use pairs of electrons to form bonds between all atoms. (2 electrons make one bond)4.Use the remaining electrons to complete the octet rule for each element.

5.If you run out of electrons, you must introduce multiple bonds to maintain the octet rule.

C OO

Let’s try NH3

Try these with a partner….

CH4

H2O

HCN

C

H

H

HH

H C N

Valence Shell Electron Pair RepulsionVSEPR

Electron pairs surrounding an atom want to be as far apart from each other as possible.

This gives rise to different molecular shapes.

The simplest shape is a LINE

Alkali Metals and Halogens make a line because they can only bond once.

Groups 1 and 17 make a line

Let’s look at another simple molecular shape

The electron pairs are the farthest apart they can be.

This molecule is LINEAR The center atom bonds twice.

Elements in group 2 make linear structures.

How is the Be atom able to covalently bound to the fluorines?

Hybridization of the orbitals explains this.

Two or more of the orbitals of the central atom must mix to form new orbitals of equal energy so bonding can take place.

2s

2p

Hybrid mixing

s p

A linear molecule has sp hybridization

Fill in valence electrons

Trigonal Planar Shape

BH3

Draw Lewis Structure:

This arrangement lets all the electron pairs be the furthest apart from each other.

Group 13 makes a trigonal planar shape

Draw electron diagram for B

Hybrid mixing

2s

2p s p p

A trigonal planar molecule has a sp2 hybridization

TetrahedralCH4 Methane

Structure:

This arrangement lets all the electron pairs be the furthest away from each other.

Group 14 makes tetrahedral shapes.

What does the word ‘tetra’ mean?

Draw the electron diagram of Carbon

What do you think is the hybridization of tetrahedral molecules??

2s

2p

Trigonal Pyramidal

NH3

This arrangement lets all the electron pairs be the furthest apart from each other. With one lone pair.

This is similar to the tetrahedral arrangement ,but has one lone pair.

Group 16 makes Trigonal Pyramidal Shapes

2s

2p

What is the hybridization of NH3( trigonal pyramidal)

Fill in valence electrons for Nitrogen

Bent shape

H2O

This arrangement lets all the electron pairs be the furthest apart from each other. With two lone pairs.

What is the hybridization of the bent molecule? Do you think it will be similar to tetrahedral?

Group 15 makes bent shapes.

What is the hybridization of H20? (bent shape)

2s

2p

Fill in valence electrons for oxygen

VSEPR Theory Summary

Linear 2 sp CO2

Trigonal Planar

3 sp2 BH3

Tetrahedral 4 sp3 CH4

Trigonal Pyramidal

3 with one lone pair

sp3 NH3

Bent 2 with two lone pairs

sp3 H2O

Shape #of atoms Hybridization Examples

Group 2

Group 13

Group 14

Group 15

Group 16

In some covalent bonds electrons are not shared equally between the elements.

The more electronegative element ‘WINS’ the electrons.

The charge difference across the bond as well as the shape of the molecule results in a POLAR Molecule.

Polarity of MoleculesWe can determine if a molecule is polar or nonpolar by the

molecule’s shape.

Polarity of Water

Lets take water for example:

Polar molecules act as tiny dipoles because they have un even charges.

A dipole is created by equal but opposite charges that are separated by a short distance.

Direction of dipole is from positive end to more negative end (more electronegative element)

Because WATER is a BENT Molecule the polarities of each bond add together to make this molecule highly

POLAR

What about NH3 Trigonal PyramidalPOLAR OR NONPOLAR?

The dipoles of the three bonds are additive combining to form an overall net dipole

Because NH3 is trigonal pyramidal shape it is POLAR

CH4

CO2

The individual bond polarities extend equally and symmetrically in different

directions canceling out . OVERALL the molecules are NONPOLAR.

What about CH3Cl? NonPolar or Polar?

Try with a partner…

Cl

H

H

H

POLAR