shapes Flashcards
1
Q
what does VSEPR stand for?
A
valence shell electron pair repulsion
2
Q
what is the VSEPR theory?
A
pairs of electrons that have a negative charge will repel each other to the maximum angle possible to minimise the total repulsion in the molecule
3
Q
where are lone pairs?
A
close to the nucleus => only attracted to the positive nucleus of an atom
4
Q
what are bonding pairs?
A
spread out between two bonded atoms => attracted to the nucleus of both atoms they join
5
Q
order of repulsion size?
A
LP-LP > LP-BP > BP-BP
6
Q
- Linear
A
> 2BP, 0LP
bond angle: 180º
examples: BeCl2, BeH2, CO2
7
Q
- Bent
A
> 2BP, 2LP
104.5º
examples: H2O, H2S
8
Q
- trigonal planar
A
> 3BP, 0LP
120º
examples: BF3, AlCl3, BCl3
9
Q
- tetrahedral
A
> 4BP, 0LP
109.5º
examples: CH4, SIH4, NH4+, SiF4, CCl4
10
Q
- pyramidal
A
> 3BP, 1LP
107º
examples: NH3, PH3, PCl3, H3O+
11
Q
- octahedral
A
> 6BP, 0LP
90º
examples: SF6
