1- Determine the electronic geometry of each molecule.
http://en.wikipedia.org/wiki/VSEPR_theory
Allow me to detail the first molecule.
P is of group 15 and therefore has 5 e⁻s of valence. It uses three of these e⁻s to form the three P:F σ bonds.
The number of lone pairs:
#lp = ½[ (5 valence e⁻ of P)- 3(the three P:F σ bonds)] = 1 lp
The electronic structure involves the P sp^3 AO (you can call it hybridization), i.e. the tetrahedral coordinate. A site is occupied by lp which is ignored when naming, so PF3 is trigonal pyramidal.
The repulsions e⁻↔ and⁻ follow the order lp-lp>lp-bp>bp-bp so that the angle FPF is
Ch3br Molecular Geometry
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Determine electronic geometry, molecular geometry and idealized bond angles… HELP?
1- Determine the electronic geometry of each molecule.
2- Determine the molecular geometry of each molecule.
3- Determine the idealized bond angle for each molecule.
4- In which cases do you expect deviations from the idealized bond angle?
a) FP3
(b) SBr2
(c) CH3Br
(d) BCl3
I really…
Part A: = Molecules 1, 2 and 3 are tetrahedral. Molecule 4 is trigonal planar.
Part B = trigonal pyramid – molecule 1; folded – molecule 2; tetrahedral – molecule 3; trigonal plane – molecule 4
Part C = Molecule 1, 2 and 3 – 109.5 degrees; molecule 4 – 120 degrees
Part D = SBr2, CH3Br and PF3
Source(s): Mastering Chemistry – the POS program everyone loves to hate.
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1. They are all tetrahedral. 2. a is tetrahedral, b is bipyramidal trigonal, c and d are doubled 3. they are all at 109.5 degrees 4. all compounds except CF4 as it has no lone pair…