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WARM UP FEB 19th 2013 Draw the Lewis structures for the following… CO₂

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Presentation on theme: "WARM UP FEB 19th 2013 Draw the Lewis structures for the following… CO₂"— Presentation transcript:

1 WARM UP FEB 19th 2013 Draw the Lewis structures for the following… CO₂ IO₄⁻ HF H₂O

2 The SHAPES of molecules
Molecular Geometry The SHAPES of molecules

3 Why the shape of a molecule is important
The shape of a molecule may determine its properties and uses Properties such as smell, taste, and proper targeting (of drugs) are all possible because of the shapes of molecules

4 Prostaglandin which causes inflammation (swelling) is produced by the
Aspirin works because of its shape! Prostaglandin which causes inflammation (swelling) is produced by the COX-1 and COX-2 enzymes Aspirin can block the substrate from bonding to the COX-1 or COX-2 enzyme thus preventing the production of prostaglandin

5 Determining the Shape of a molecule
Lewis structures don’t give us a 3-dimensional view of how the atoms are bonded together The Lewis structure implies a cross shape with 90o angles Would you have predicted this arrangement of atoms from just seeing it’s Lewis structure?

6 So how do we find the shape of a molecule?
By using the VSEPR Theory (pronounced Vess Purr)

7 Valence Shell Electron Pair Repulsion Theory
VSEPR Theory Valence Shell Electron Pair Repulsion Theory Main Premise: Molecules will adopt a shape that is lowest in energy by minimizing the valence shell electron pair repulsion (VSEPR) between adjacent atoms

8 Huh??? Atoms in a molecule try to spread out from one another as much as possible to reduce the “like charge repulsion” between their outer electrons

9 methane, CH4 You might think this is the farthest that the hydrogens can get away from each other 109.5° 90° But if you think in 3 dimensions, the hydrogens can actually get farther away from each other and minimize adjacent electron cloud repulsions

10 The 5 Main VSEPR Shapes These shapes minimize the like charge repulsion between adjacent electron clouds

11 From Lewis to VSEPR Shape
From Lewis to VSEPR Shape 1. Draw a Lewis structure 2. Count the number of “electron domains” around the central atom -Each single, double and triple bond counts as ONE domain -Each lone pair counts as ONE domain 3. Use VSEPR Chart to determine the shape based on how many bonding and nonbonding domains are around the central atom

12 This Lewis structure shows
Electron domains Regions in a molecule where there are high concentrations of electrons Lone pairs= (non-bonding domains) This Lewis structure shows 2 bonding domains and 2 non bonding domains Bonds = (bonding domains)

13 How many “domains” around the central atom?
3 around nitrogen 4 around carbon Remember: single, double and triple bonds count as ONE domain 2 around each atom

14 Remember the BIG PICTURE?
Electron “domains” are all negatively charged so they want to spread out from each other as much as possible to minimize like-charge-repulsion within a molecule Doing this allows the molecule to be more stable (low energy)

15 You need to memorize this
The vsepr chart You need to memorize this

16 Let’s look at some Examples

17 VSEPR Example 1 How many bonding and non-bonding electron domains are there around the central atom? 2 bonding 0 non-bonding

18 VSEPR Example 1 Use the VSEPR chart…
VSEPR Example 1 2 bonding, 0 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “linear” Molecular geometry (how the atoms bonded to the central atom are arranged) is “linear” also

19 VSEPR Example 2 How many bonding and non-bonding electron domains are there around the central atom? 3 bonding 0 non-bonding

20 VSEPR Example 2 Use the VSEPR chart…
VSEPR Example 2 3 bonding, 0 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “trigonal planar” Molecular geometry (how the atoms bonded to the central atom are arranged) is “trigonal planar” also

21 VSEPR Example 3 How many bonding and non-bonding electron domains are there around the central atom? 2 bonding 1 non-bonding

22 VSEPR Example 3 Use the VSEPR chart…
VSEPR Example 3 2 bonding, 1 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “trigonal planar” Molecular geometry (how the atoms bonded to the central atom are arranged) is “bent”

23 VSEPR Example 4 How many bonding and non-bonding electron domains are there around the central atom? 4 bonding 0 non-bonding

24 VSEPR Example 4 Use the VSEPR chart…
VSEPR Example 4 4 bonding, 0 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “tetrahedral” Molecular geometry (how the atoms bonded to the central atom are arranged) is “tetrahedral”

25 VSEPR Example 5 How many bonding and non-bonding electron domains are there around the central atom? 3 bonding 1 non-bonding

26 VSEPR Example 5 Use the VSEPR chart…
VSEPR Example 5 3 bonding, 1 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “tetrahedral” Molecular geometry (how the atoms bonded to the central atom are arranged) is “trigonal pyramidal”

27 VSEPR Example 6 How many bonding and non-bonding electron domains are there around the central atom? 2 bonding 2 non-bonding

28 VSEPR Example 6 Use the VSEPR chart…
VSEPR Example 6 2 bonding, 2 nonbonding Use the VSEPR chart… Electron geometry (how the electron domains are arranged around the central atom) is “tetrahedral” Molecular geometry (how the atoms bonded to the central atom are arranged) is “bent”

29 Lone pairs (non-bonding domains) create a larger region of negative charge than bonding domains and thus push the adjacently bonded atoms even farther away from each other than normal

30 Lone pairs decrease the
expected bond angle .. .. 109.5° 104.5° 107°

31 For tetrahedral Shapes
For tetrahedral Shapes Number of lone pairs around central atom 1 2 Approximate bond angle 109.5 107 104.5

32 VSEPR Notation Also known as “AXE” notation It is just a shorthand way to communicate VSEPR information

33 Examples of using axe notation
Examples of using axe notation AX3E1 This subscript tells how many atoms are bonded to the central atom This subscript tells how many lone pairs are on the central atom AX3E1 is always trigonal pyramidal

34 Examples of using axe notation
Examples of using axe notation AX2E2 This subscript tells how many atoms are bonded to the central atom This subscript tells how many lone pairs are on the central atom AX2E2 is always bent

35 Examples of using axe notation
Examples of using axe notation AX4 This subscript tells how many atoms are bonded to the central atom Don’t put the “E” if there aren’t any lone pairs AX4 is always tetrahedral

36 Fisher Projections A way to make your Lewis structures indicate their three dimensional VSEPR shape on paper

37 .. ..

38

39 Fisher Projections Bonds in the plane of the paper are shown as lines Bonds projecting in front of the plane of the paper are shown as triangles Bonds projecting behind the plane of the paper are shown as stacked lines

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