FIRST OF all use the following formula for finding out the hybridising
by H= S+(1/2)[E - V +/- C]
HERE H is the hybridisation
S is the no of surrounding atoms to the central atom
E is the no of outer shell es in the central atom
V is the no of valence electrones of the central atom
and C is the charge on the molecule
C= +ve for -ve charge and -ve for the + ve charge.
if H= 2,3,4,5,6,7 then the hybridization will be sp sp2 sp3 sp3d sp3d2 and sp3d3 respectively and if
sp the structure is linear
sp2 then trigonal planer
v shape for the one lone pair
sp3 then tetrahedral
pyramidal (1lone pair)
v shape (2lone pair)
and linear (3lone pair)
sp3d trigonal bipyramidal
distorted bipyramidal (1 lone pair)
t shape (2 lone pair)
linear (3 lone pair)
sp3d2 octahedral
square planer(1 lone pair)
planer (2 lone pair)
sp3d3 pentagonal bipyramidal
distorted pentagonal bipyramidal (1 lone pair)
thus after knowing the hybridization we can get the structure closer to some. now for knowing the no of lone pairs we follows following path
example we take NH3
HERE WE find first the hybridisation
by the above mentioned formula
here central atom is N and S= 3 atoms
and E= 5 (outer shell es) and C=0 and V= 3 thus
H= 3 + 1/2*[ 5-3+0]= 3+1=4 means sp3 hybridization.now
find out the no of lone pair
we know the no of outer es =5
use of es by H atom = 3 then remaining atoms= 5-3=2/2=1 lone pair
so the structure is pyramidal.
SOLVED BY
DEVENDRA KUMAR VERMA
(RESEARCH SCHOLAR),
DELHI TECHNOLOGICAL UNIVERSITY, DELHI.
Trigonal pyramidal
Bent, like water.
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
upon looking at it, this molecule is bentif you draw out the diagram for it, you can see that the central atom has 4 domains, 2 bonding and 2 nonbonding(lone pairs)pairs.when getting the molecular shape, we ignore the 2 lone pairs, and going from tetrahedral -->removing 2 domainswe are left with a bent shape molecule
Methane has a tetrahedral molecular geometry. It has 4 bonding pairs of electrons and no lone pairs.
No. There is no such thing as a diatomic atom. A diatomic molecule is a molecule that contains two atoms. The number of lone pairs depends on what atoms are bonded.
Yes, each oxygen atom in the molecule has two lone pairs.
A molecule with two bound atoms and one line electron pair
Yes it is tetrahedral in shape.It has no lone pairs
3
two
Yahoo it Google it
lone pairs
There are 2 non bonding pairs in a nitrogen molecule
It is a bent molecule because of Oxygen's lone pairs
The factors affecting the shape of the molecules are the bonded e and the lone pairs of electrons
There are four electrons, which is two pair.