Chemical Bonding - HL.

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Presentation transcript:

Chemical Bonding - HL

14.1.1 Predict the shape and bond angles for species with five and six negative charge centers using VSEPR theory. Expanded valence shell Promote s electron to d shell Form bond to small, electronegative elements such as F, O, Cl

PF5 5 Charge centers trigonal bipyramidal

SF4 5 charge centers Saw-horse

ICl3 5 charge centers T-shaped

XeF2 5 charge centers Linear

SF6 6 charge centers Octahedral

BrF 6 charge centers square pyramid 5

XeF4 6 charge centers square planar

14.2.1 Describe sigma and pi bonds A sigma bond is a bond where the electron density is concentrated along the intranuclear axis A pi bond is a bond where the electron density is concentrated on either side of an imaginary line joining the 2 nuclei (the intranuclear axis)

14.2.2 Explain hybridization in terms of the mixing of atomic orbitals to form new orbitals for bonding. 14.2.3 identify and explain the relationships between Lewis structures, molecular shapes and types of hybridization (sp; sp2; sp3)

SP3 hybridization

SP2 hybridization

Hybridization in NH3? Hybridization in BF3?

Hybridization Summary Number of regions of electron density Hybridization of central atom Shape Examples 1 Unhybridized Linear H-H H-Cl 2 sp HCCH O=C=O 3 sp2 Triangular planar H2C=CH2 BF3 4 sp3 tetrahedral CH4 NH3 H2O

Resonance structures

Delocalized electrons