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SHAPES OF MOLECULES Before you start it would be helpful to…

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1 SHAPES OF MOLECULES Before you start it would be helpful to…
know the definition of a covalent bond know what a lone pair is know that like charges repel SHAPES OF MOLECULES

2 ELECTRON PAIR REPULSION THEORY
“THE SHAPE ADOPTED BY A SIMPLE MOLECULE OR ION IS THAT WHICH KEEPS REPULSIVE FORCES TO A MINIMUM” Bonds are closer together so repulsive forces are greater Molecules contain covalent bonds. As covalent bonds consist of a pair of electrons, each bond will repel other bonds. Al Bonds are further apart so repulsive forces are less Bonds will therefore push each other as far apart as possible to reduce the repulsive forces. Because the repulsions are equal, the bonds will also be equally spaced All bonds are equally spaced out as far apart as possible Al

3 REGULAR SHAPES Molecules, or ions, possessing ONLY BOND PAIRS of electrons fit into a set of standard shapes. All the bond pair-bond pair repulsions are equal. All you need to do is to count up the number of bond pairs and chose one of the following examples... C A covalent bond will repel another covalent bond BOND BOND PAIRS SHAPE ANGLE(S) EXAMPLE 2 LINEAR º BeCl2 3 TRIGONAL PLANAR 120º AlCl3 4 TETRAHEDRAL º CH4

4 BERYLLIUM CHLORIDE Cl Be Cl Be
Beryllium - has two electrons to pair up Chlorine - needs 1 electron for ‘octet’ Two covalent bonds are formed Beryllium still has an incomplete shell

5 ADDING ANOTHER ATOM – ANIMATION
Wait……..

6 ALUMINIUM CHLORIDE Al Cl Cl Al
Aluminium - has three electrons to pair up Chlorine - needs 1 electron to complete ‘octet’ Three covalent bonds are formed; aluminium still has an incomplete outer shell.

7 120° TRIGONAL PLANAR ALUMINIUM CHLORIDE Al Cl Cl Al BOND PAIRS 3
Aluminium - has three electrons to pair up Chlorine - needs 1 electron to complete ‘octet’ Three covalent bonds are formed; aluminium still has an incomplete outer shell. BOND PAIRS 3 LONE PAIRS 0 Cl 120° Cl Al BOND ANGLE... SHAPE... 120° TRIGONAL PLANAR Cl

8 120° TRIGONAL PLANAR ALUMINIUM CHLORIDE Al Cl Cl Al BOND PAIRS 3
Aluminium - has three electrons to pair up Chlorine - needs 1 electron to complete ‘octet’ Three covalent bonds are formed; aluminium still has an incomplete outer shell. BOND PAIRS 3 LONE PAIRS 0 Cl 120° Cl Al BOND ANGLE... SHAPE... 120° TRIGONAL PLANAR Cl

9 ADDING ANOTHER ATOM – ANIMATION
Wait…..

10 METHANE H C H C Carbon - has four electrons to pair up
Hydrogen - 1 electron to complete shell Four covalent bonds are formed C and H now have complete shells

11 109.5° TETRAHEDRAL METHANE H C H C BOND PAIRS 4 LONE PAIRS 0 C H
Carbon - has four electrons to pair up Hydrogen - 1 electron to complete shell Four covalent bonds are formed C and H now have complete shells BOND PAIRS 4 LONE PAIRS 0 109.5° H C BOND ANGLE... SHAPE... 109.5° TETRAHEDRAL

12 109.5° TETRAHEDRAL METHANE H C H C BOND PAIRS 4 LONE PAIRS 0
Carbon - has four electrons to pair up Hydrogen - 1 electron to complete shell Four covalent bonds are formed C and H now have complete shells BOND PAIRS 4 LONE PAIRS 0 BOND ANGLE... SHAPE... 109.5° TETRAHEDRAL

13 IRREGULAR SHAPES If a molecule, or ion, has lone pairs on the central atom, the shapes are slightly distorted away from the regular shapes. This is because of the extra repulsion caused by the lone pairs. BOND PAIR - BOND PAIR < LONE PAIR - BOND PAIR < LONE PAIR - LONE PAIR O O O As a result of the extra repulsion, bond angles tend to be slightly less as the bonds are squeezed together. Note the order …… looks unusual but is the same as in class and book ….. lp:lp is strongest repulsion.

14 AMMONIA N H N H Nitrogen has five electrons in its outer shell
BOND PAIRS 3 LONE PAIRS 1 TOTAL PAIRS 4 H Nitrogen has five electrons in its outer shell It cannot pair up all five - it is restricted to eight electrons in its outer shell It pairs up only three of its five electrons 3 covalent bonds are formed and a pair of non-bonded electrons is left As the total number of electron pairs is 4, the shape is BASED on a tetrahedron

15 AMMONIA N H N BOND PAIRS 3 LONE PAIRS 1 TOTAL PAIRS 4 H The shape is based on a tetrahedron but not all the repulsions are the same LP-BP REPULSIONS > BP-BP REPULSIONS The N-H bonds are pushed closer together Lone pairs are not included in the shape 107° H N H N N H ANGLE ° SHAPE... PYRAMIDAL H H

16 AMMONIA N H N BOND PAIRS 3 LONE PAIRS 1 TOTAL PAIRS 4 H

17 WATER O H O H Oxygen has six electrons in its outer shell
BOND PAIRS 2 LONE PAIRS 2 TOTAL PAIRS 4 H Oxygen has six electrons in its outer shell It cannot pair up all six - it is restricted to eight electrons in its outer shell It pairs up only two of its six electrons 2 covalent bonds are formed and 2 pairs of non-bonded electrons are left As the total number of electron pairs is 4, the shape is BASED on a tetrahedron

18 WATER O H O BOND PAIRS 2 LONE PAIRS 2 TOTAL PAIRS 4 H The shape is based on a tetrahedron but not all the repulsions are the same LP-LP REPULSIONS > LP-BP REPULSIONS > BP-BP REPULSIONS The O-H bonds are pushed even closer together Lone pairs are not included in the shape O 104.5° H O O H H ANGLE ° SHAPE... V H H H

19 What is the shape of each of the following molecules?
(Name and then Bond Angle) H2O V shaped 104.5 o NH3 Pyrimidal 107 o BF3 Trigonal Planar 120 o AlF3 120 o approx. H2S 104.5 o approx. f) SiH4 Tetrahedral 109.5

20 REVISION CHECK What should you be able to do? CAN YOU DO ALL OF THESE?
Recall the theory of Electron Pair Repulsion Understand why repulsion between electron pairs affects the shape Recall and explain the shapes and bond angles of molecules with 2,3,4 bond pairs Recall the relative strengths of bond pair and lone pair repulsions Recall and explain the shapes and bond angles of water ammonia methane etc Apply the above concepts to other molecules CAN YOU DO ALL OF THESE?

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