VSEPR theory-definition-postulates-shape and limitations
VSEPR theory and shape of covalent molecules
The geometry of covalent molecules depends upon the
number and arrangement of electron pairs [which present in the valence shell of
the central atom], due to electrostatic
repulsion between bond
pair and lone pair of electrons.
To explain the geometry or
shape of covalent molecules, Gillespie and Nyholn put
forward a new theory which is known
as valence shell electron pair repulsion theory or in a nutshell VSEPR theory.
VSEPR theory postulates for covalent molecules
There are five main postulates of this theory, which may be summarized as follows .
Postulate: I The shape of a covalent molecule is determined
by the repulsion among all the electron pairs [ bond pair(b.p ) of electrons and lone pair( l.p ) of electrons ] present in the valence shell of the
central atom .
If only
bonding electron pairs are present on the central atom, the covalent molecule
will have a regular geometry .
Thus for AB 2 type of molecule
with two bond pair [such as BeCl2, CO2 etc ], the geometry is linear.
Similarly,
molecules with three bond pair, four bond pair, five bond pair and six bond
pair, the geometry of the concern molecules are trigonal , tetrahedral ,
trigonal bipyramidal and octahedral respectively .
For examples, BCl3 ( trigonal ) , CH4
( tetrahedral ), PCl5 ( trigonal bipyramid ) and SF6 (
octahedral ) etc.
Postulate: II When both the bond pair( b.p ) and lone pair ( l.p ) are present on the central
metal atom, the molecules will have a
distorted geometry.
Because, the
lone pair takes up more space on the central atom than a bond pair and the lone
pair is attracted by one nucleus while the bond pair is attracted by two nuclei .
Hence, the l.p–l.p repulsion is greater than l.p – b.p repulsion and l.p – b.p repulsion is greater than b.p –b.p repulsion .
That is , l.p–l.p repulsion > l.p – b.p repulsion
> b.p –b.p repulsion.
For examples, ammonia molecule contain one lone pair and three bond pair of electrons . The
geometry of ammonia molecule is distorted tetrahedral with sp3 hybridization .
That is, it has pyramidal structure .The H –N –H bond angle is 107o28’
instead of 109o28’ .
Similarly, H2O molecule contain two bond pair and two lone pair of electrons .Hence ,the geometry of water molecule is distorted tetrahedral or V–shaped geometry with sp3 hybridization.
The H –O –H bond angle in water molecule is 104o27’
instead of 109o28’ .
Postulate: III The magnitude of repulsion between bond pairs
depend on the electronegativity difference between central atom (A ) and
other bonded atom ( B ).
That is ,
the B – A – B bond angle decreases with increasing in
electronegativity of ‘B’ as the electronegativity of ‘B’ increases.
The bond
pair move away from the central atom and repulsion between bond pair decreases.
So the bond angle decrease .
For examples, the order of
bond angle of PI3 , PBr3
and PCl3 is PI3 > PBr3 > PCl3.
Postulate: IV Triple bond take more space than double bond . Similarly , double bond take more space than single bond.
So double
bond causes more repulsion than single bond and triple bond causes more
repulsion than double bond .
That is, t.b –t.b repulsion > d.b–d.b repulsion
> d.b–s.b repulsion > s.b –s.b repulsion . [ t.b = triple bond, d.b =
double bond and s.b = single bond ].
For example , F –
C – F and F – C – O bond angle of carbonic difluoride ( COF2 ) .
Postulate: V The bond angle contraction of incomplete
valence shell is greater than complete valence shell due to the l.p–l.p or l.p – b.p repulsion.
For
examples, in case of ammonia the H –N –H
bond angle is 107o28’ instead of 109o28’ . But in case of phosphine , the H – P –H bond angle becomes 94o
instead of 109o28’.
Limitations of VSEPR Theory.
Like other theory, VSEPR Theory also some draw back. The main two limitation of VSEPR Theory are discussed below .
( I ) VSEPR
Theory fails to explain isoelectronic species. Isoelectronic species are elements, ions and molecules that share the
same number of electrons.
According to VSEPR theory, shape of the molecule depends on
number of bond pair and lone pair of electrons of the central atom.
But, isoelectronic species can differ in geometry , despite the fact that they have
the same numbers of valence electrons.
( II ) VSEPR
Theory does not explain the geometry of transition metal compounds. This
theory is also unable to guess the
structure of certain compounds.
This is because of that it does not take associated sizes of
the substituent’s and inactive lone pairs into account.
- VSEPR theory postulates for covalent molecules
- Limitations of VSEPR Theory.
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