SHAPE OF BeCl₂ IN THE LIGHT OF E.P.R.T:
In BeCl₂, Be is the central atom.
Be has two bonding pair with chlorine.
It has no lone pair.
Structure of BeCl₂ is linear.
SHAPE OF BeCl₂ IN THE LIGHT OF H.O.M:
Be uses its Sp-hybrid orbital in bond making.
These orbital overlap with the orbital of two chlorine atoms to form sigma bonds.
All these atoms are arranged linearly at an angle of 180^o.

Explain the geometry of H₂O in the light of electron pair repulsion theory
and hybrid orbital model.

SHAPE OF H₂O IN THE LIGHT OF E.P.R.T:
In H₂O, oxygen is the central atom.
Oxygen has two bond pairs.
It has two lone pairs.
The repulsion of the lone pairs and the bonded pairs reduce the angle from 109^o to 104.5^o.
It has tetrahedral structure.
SHAPE OF H₂O IN THE LIGHT OF H.O.M:
In terms of hybrid orbital model, oxygen utilizes two of its Sp³ orbitals to form sigma bonds.
Due to reduced angle in H₂O, angular or bent structure is formed.

SHAPE OF NH₃ IN THE LIGHT OF E.P.R.T:
In NH₃, N is the central atom.
Nitrogen has three bond pairs.
It has only one lone pair which repels the bonding pairs with the result that angle is reduced from 109^o to 107^o.
SHAPE OF NH₃ IN THE LIGHT OF H.O.M:
In term of H.O.M, nitrogen utilizes three of the four Sp³ orbital to form sigma bonds with three hydrogen atoms.
Its structure is pyramidal with bond angles of 107^o.

SHAPE OF BF₃ IN THE LIGHT OF E.P.R.T:
In BF₃, boron is the central atom.
It has three electron pairs, geometry of molecules will be trigonal.
The angle between them is 120^o.
SHAPE OF BF₃ IN THE LIGHT OF H.O.M:
Boron atom undergoes Sp²-hybridization producing three Sp²-orbital.
These orbital are arranged trigonally in one plane