14.1 Shapes of molecules and ions (HL). 14.1.1 State and predict the shape and bond angles using the VSEPR theory for 5 and 6 negative charge centers. . Molecules with more than 4 electron pairs. Molecules with more than 8 valence electrons [expanded valence shell]
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14.1.1 State and predict the shape and bond angles using the VSEPR theory for 5 and 6 negative charge centers.
SF6 is octahedral
XeF4 is square planar
14.2.1 Describe σ (sigma) and π (pi) bonds
14.2.2 State and explain the meaning of the term hybridization
14.2.3 Discuss the relationships between Lewis structures, molecular shapes and types of hybridization (sp, sp2, sp3).
Overlap four s-orbitals from four hydrogens (blue) with four sp3 hybrids on carbon leads to formation of bonds, each containing one electron from the carbon and one from the hydrogen
14.3.1 Describe the delocalization of (pi) π- electrons and explain how this can account for the structure of some species