NAT Chemistry MCQs

Four equivalent bonding directions correspond to sp3 hybridization.
The ideal geometry is tetrahedral.

Each carbon has three sigma-bonding regions.
The remaining p orbitals form the pi bond.

Lone pairs influence shape and reactivity.
They repel bonding pairs strongly in VSEPR theory.

Each carbon has two electron domains.
Sp hybridization gives linear geometry and leaves two p orbitals for pi bonds.

A single bond has order one, double bond two, and triple bond three.
Higher bond order generally means shorter, stronger bonds.

Triple bonds have higher bond order than single or double bonds.
They are usually shorter and stronger.

No single resonance structure fully represents the electron distribution.
The real structure is a resonance hybrid.

Formal charge helps compare possible Lewis structures.
Preferred structures often minimize charge separation.

Electron groups arrange to minimize repulsion.
Lone pairs and bonding regions determine molecular geometry.

Two electron groups arrange 180 degrees apart.
This minimizes repulsion.

Three electron groups arrange about 120 degrees apart.
They lie in one plane.

Four electron groups point toward tetrahedral corners.
The ideal bond angle is about 109.5 degrees.