Chemical Bonding and Molecular Structure Test - 4

CO₂, due to sp hybridisation bond angle is 180 º.

BCl₃, BeCl₂ and CCl₄ has zero dipole moment due to symmetric strucuture where as shape pf NCl₃ is pyramidal due to presence of lone pair.

The bond angle in PH₃ would be expected to be close to 90 ° as there is a lone pair repelling 3 bond pairs in the pyramidal structure (the actual bond angle H-P-H in PH₃ is 93 °which indicates that P atom is almost unhybridised)

If the angle between a lone pair, the central atom and a bond pair is increased, it follows that the actual bond angle between the atoms must be decreased.

Option 1: With 3 bond pairs and two lone pairs, ClF₃ has trigonal pyramidal geometry. Due to repulsion between the lone pairs ClF₃moelcule is a T-shaped moelcule.

Option 2: CO₂ has a linear shape due to presence of two bond pairs.

Option 3: H₂O has 2 bond pairs and 2 lone pairs. It has tetrahedral geometry and bent shape.

Option 4: In O(CH₃)₂ the central carbon atom has one double-bonded oxygen and two single-bonded methyl groups. It has no lone pair of electrons, so this compound will have a trigonal planar geometry.