Polarity and Bonding in N2

The video tutorial explains how to determine if N2 is polar or nonpolar by examining its Lewis structure and molecular geometry. It describes the distribution of valence electrons and the presence of a triple bond in N2, highlighting its linear geometry. The video further discusses the electrostatic potential, showing that N2 is symmetrical with no net dipole, leading to the conclusion that N2 is a non-polar molecule.

What is the first step in determining the polarity of a molecule like N2?

• Analyzing the molecular weight

• Examining the Lewis structure

• Measuring the boiling point

• Checking the color of the molecule

What type of bond is present between the nitrogen atoms in N2?

• Double bond

• Single bond

• Quadruple bond

• Triple bond

How many lone pairs are present in the Lewis structure of N2?

• One lone pair

• Three lone pairs

• Four lone pairs

• Two lone pairs

What is the molecular geometry of N2?

• Trigonal planar

• Bent

• Linear

• Tetrahedral

What does the uniform electrostatic potential of N2 indicate?

• Uniform charge distribution

• Presence of ionic bonds

• Non-uniform charge distribution

• Presence of a net dipole

Why is N2 considered a nonpolar molecule?

• Due to its symmetrical shape and equal sharing of electrons

• Due to its colorless nature

• Because it has a high boiling point

• Because it contains ionic bonds

What is the significance of equal electronegativity in N2?

• It ensures equal sharing of electrons

• It causes a net dipole moment

• It results in a polar molecule

• It leads to unequal sharing of electrons