IBDP HL bonding
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Transcript of IBDP HL bonding
Draw the VESPR structures for 14.1.1
Include bond angles, names of shapes
Bonding AHL
• Describe sigma and pi bonds
• Explain hybridization in terms of sp sp2 sp3
• Explain relationship between Lewis structure, shape and hybridisation
Sigma Bonds
• Sigma bonds are all single bonds, and result from axial overlap of orbitals.
π Bonds
• Result from sideways overlap of parallel p orbitals
Basics
• A single bond is a SIGMA bond
• A double bond is ONE SIGMA ONE PI
• A triple bond is ONE SIGMA TWO PI
Hybridisation – sp3
Hybridisation – sp2
Hybridisation - sp
Homework Task
• Using the following molecules create a student help sheet to explain the bonding, the shape, the hybridisation, and number of sigma and pi bonds.
• In Carbon Dioxide, Methane and Propene.
Geometry and Hybridisation
• All you have to do is count the negative centres, and don’t forget lone pairs
• Inorganic :• 4 negative centres is sp3, e.g. NF3 ( 3bp 1nbp in this case )
• 3 negative centres is sp2, e.g. BF3 ( 3bp in this case )
• 2 negative centres if sp
• Organic : • sp3 is Td 109.5, e.g. Alkanes• sp2 is Trig Pl 120, e.g. Alkenes, Carbonyl groups• sp is lin 180, e.g. Alkynes
Starter
• Explain how sp2 hybridization arises
• Use electrons in boxes notation to explain your answer.
When electron pairs are not confined to two adjacent bonding atoms but extend over 3 or more atoms
Benzene Facts
• Planar regular hexagon
• All bond angles 120 degrees
• Bond lengths intermediate between single and double bonds
• Reluctant to undergo addition reactions.
Nitrate Ion
Nitrite Ion Resonance Structures ?
Carbonate Anion
Ozone
Ethanoate
Learning Check
• N01/420/H(2) part (a) ONLY