molecular shape
DESCRIPTION
Molecular Shape. Things to remember. shape of molecule influenced by location of nuclei nuclei go to certain locations because of its electron pairs. Use the Lewis Structure. Lewis structure is 2-D, but can help figure out 3-D shape. Atom. Lewis Structure. # Unpaired Electrons. - PowerPoint PPT PresentationTRANSCRIPT
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Molecular Shape
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Things to remember
shape of molecule influenced by location of nuclei – nuclei go to certain locations because
of its electron pairs
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Use the Lewis Structure
• Lewis structure is 2-D, but can help figure out 3-D shape
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Bonding CapacityBonding Capacity
0000:Ne::Ne:Ne, Ar, KrNe, Ar, Kr
2222·O:·O:O, SO, S
3333·N··N·N, PN, P
4444·C··C·C, SiC, Si
1111·F:·F:F, Cl, Br, IF, Cl, Br, I
1111HHH H
Bonding Bonding CapacityCapacity
# Unpaired # Unpaired ElectronsElectrons
Lewis Lewis StructureStructure
AtomAtom
.
..
..
.
......···
··
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Molecular Shape
• Determined by overlap of orbitals
• Shape determined by two factors:
1.1. total # atoms total # atoms & &
2.2. # e# e-- pairs pairs in different locationsin different locations on on central atomcentral atom
classify eclassify e-- pairs as bonding or non-bonding pairs as bonding or non-bonding
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Molecular Shape & VSEPR
• electron pairs repel each other: –want to be as far apart from each other as can be
• non-bonding pairs take up a little more room than bonding pairs
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Orientation of Electron Pairs
tetrahedral: 3-D, 4 e- pairs 109 apart
4
planar Triangular: 3 electron pairs 120 apart
3
linear: 2 electron pairs 180 apart
1 or 2
OrientationTotal # of electron pairs
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2-Atom Molecules
• atoms located next to each other
• linear molecules!
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3-Atom Molecules
• linear or bentlinear or bent
LinearLinear
Bent Bent
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CO2
Lewis structure:Lewis structure: O :: C :: O O :: C :: O....
.... ....
....
4 bonding pairs4 bonding pairsbut onlybut only 2 regions2 regions of electron density: of electron density: 180180 apart so CO apart so CO22 is linear is linear
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Lewis Structure of HLewis Structure of H22O: O: H:O: H:O: HH
....
....H2O
•2 bonding pairs between each O and H2 bonding pairs between each O and H•2 nonbonding pairs on O2 nonbonding pairs on O•4 different regions of electron density4 different regions of electron density
Count up the electron pairs:Count up the electron pairs:
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H2O
• 4 electron pairs are 109 apart
• nonbonding pairs spread out a bit more
– squeeze bonding pairs together so
bent shape
H – O H
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3-Atom Molecules
• Triangular?
Yes, ozone (OYes, ozone (O33) is triangular ) is triangular
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4-Atom Molecules
• Two possibilities:–Trigonal Planar – in 1 plane
–Trigonal Pyramidal
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4-Atom Molecules: Trigonal Planar
Bond angles Bond angles =120=120
All 4 atoms lie in All 4 atoms lie in the same planethe same plane
arenaren’’t likely to see this because theset likely to see this because these molecules molecules dondon’’t obey octet rule!t obey octet rule!
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BF3: Trigonal Planar• B has 3 valence electrons
– very small atom e– each F has 7 valence electrons – total = 3 X 7 + 3 = 24 e-
: F : B : F : B ....
........FF
FF....
....
....
....
.... ........
These molecules These molecules dondon’’t obey octet rule t obey octet rule - so aren- so aren’’t likely to t likely to see themsee them - 3 regions- 3 regions - FBF = 120- FBF = 120
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4-Atom Molecules: AX3
shape most likely to seeshape most likely to see
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NH3
Lewis Structure:Lewis Structure: H : N : H H : N : H
HH
....
....
•3 bonding pairs3 bonding pairs•1 non-bonding pair1 non-bonding pair•4 regions 4 regions •little less than 109little less than 109 apart apart•shape: trigonal pyramidalshape: trigonal pyramidal
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5-Atom Molecules: AX4
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5 Atoms & Tetrahedrons
Tetrahedral means 4 Tetrahedral means 4 faces:faces:- 1 atom in center - 1 atom in center - 4 atoms at the points- 4 atoms at the points
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CH4 = a 5-atom molecule
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CH4
Lewis structure =Lewis structure = H : C : H H : C : HHH
HH........
•4 bonding pairs4 bonding pairs•4 regions of electron density4 regions of electron density•electron pairs are 109electron pairs are 109 apart apart
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CH4 = a 5-atom molecule
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Summary of Molecular Shapes
• start with Lewis Structure!
• look at # regions of e- density on central atom
• look at # atoms bonded to central atom
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Molecular Polarity
• Look at shape of molecule:–non-polar molecular is symmetricalnon-polar molecular is symmetrical
–polar molecular is asymmetricalpolar molecular is asymmetrical
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Molecular Polarity• molecule is symmetric if:
– electrical charge on 1 side is same as electrical charge at matching point on opposite side
–“pull” of one polar bond is offset by “pull” of another polar bond
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Symmetrical Symmetrical Molecules are Molecules are Non-polarNon-polar
NonpolarNonpolar
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AsymmetricAsymmetricMolecules areMolecules arePolarPolar