Do now: Brainstorm how you would draw the Lewis diagram for: H 2 O CO 2
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1 Do now: Brainstorm how you would draw the Lewis diagram for: 2 O CO 2
2 Shapes of molecules C 4 N 3 2 O C 2 O CO 2
3 Shapes of molecules Shapes of molecules are determined by the number of bonding and non-bonding pairs around the central atom of the molecule. Determine the number of bonding and non-bonding regions around the central atom in the following molecules: 4 0 bonding regions non-bonding regions 3 1 bonding regions non-bonding regions C N 2 0 bonding regions non-bonding regions 2 2 bonding regions non-bonding regions O C O O
4 Determining shapes 1. Draw the Lewis diagram 2. Determine the number of bonding regions and non-bonding regions around the central atom 3. Use this information to determine the shape 4 regions of charge each electron pair will be at 109 to be as far away from each other as possible tetrahedral shape 3 regions of charge each electron pair will be at 120 to be as far away from each other as possible trigonal planar shape 2 regions of charge each electron pair will be at 180 to be as far away from each other as possible linear shape
5 Determining shapes 4 regions of charge each electron pair will be at 109 to be as far away from each other as possible tetrahedral shape Electron pair arrangement: tetrahedral Shape: tetrahedral Electron pair arrangement: tetrahedral Shape: trigonal pyramid Electron pair arrangement: tetrahedral Shape: bent C N O
6 4 regions around the central atom Bonding regions Nonbonding regions Shape Bond angle Example 4 0 tetrahedral 109 C 4 (methane) 3 1 trigonal pyramid 109 N 3 (ammonia) 2 2 bent O (water)
7 Determining shapes 3 regions of charge each electron pair will be at 120 to be as far away from each other as possible trigonal planar shape 2 regions of charge each electron pair will be at 180 to be as far away from each other as possible linear shape Electron pair arrangement: trigonal planar Shape: trigonal planar Electron pair arrangement: trigonal planar Shape: bent Electron pair arrangement: trigonal planar Shape: linear O C O S O O C O
8 2 and 3 regions around the central atom Bonding regions Nonbonding regions Shape 3 0 trigonal planar Bond angle Example 120 C 2 O (methanal) 2 1 bent 120 SO 2 (sulphur dioxide) 2 0 linear 180 CO 2 (carbon dioxide)
9 Determine the shape of the following PCl 3 C 3 Cl Cl Cl P Cl C Cl Bonding regions = 3 Non-bonding regions = 1 Trigonal pyramid CS 2 S 2 Bonding regions = 4 Non-bonding regions = 0 Tetrahedral S C S S Bonding regions = 2 Non-bonding regions = 0 Linear Bonding regions = 2 Non-bonding regions = 2 Bent
10 Tips and Tricks Examiners can try and trick you with Lewis diagrams. There are three common things to think about: If there is more than one lone pair they are drawn next to each other S NOT S Dots between atoms should be redrawn as lines, but lone pairs are always drawn S B only has 6 electrons around it to make a full shell Be only has 4 electrons around it to make a full shell
11 Answering exam questions In an exam you will always be asked to explain the shape and bond angles of the central atom of a molecule. Usually: A is stating the shape and bond angle M is explaining the shape OR bond angle using the arrangement of electrons around the central atom E is explaining the shape AND bond angle using the arrangement of electrons around the central atom We need to be able to do this to get good marks in the exam
12 Do now: Determine the shape of the following compounds C 4 O 2 N 3 C O N Bonding regions = 4 Non-bonding regions = 0 Tetrahedral Bonding regions = 2 Non-bonding regions = 2 Bent Bonding regions = 3 Non-bonding regions = 1 Trigonal pyramid
13 2013 exam Q 1 (b)
14 Answering Exam Questions Using a writing frame can help with your answer. State the total number of negative regions Explain that the negative regions want to repel each other to get the maximum separation State the bond angle State the number of bonding and non-bonding regions State the shape and link to number of bonding regions If asked compare two shapes or bond angles
15 2013 exam Q 1 (b) Make sure you read and check that you have covered all bullet points, it is surprising how many students don t cover all bullet points.
16 2013 exam Q 1 (b) What grade would you give this answer? Why? Achieved
17 Excellence response 2013 exam Q 1 (b)
18 2013 exam Q 1 (b)
19 2012 exam Q 1 (b)
Structures, Shapes and Polarity. of Molecules. Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity
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