Question 1

Why isn't a hydrogen bond a 'real' covalent bond?

Accepted Answer

A hydrogen bond is an intermolecular force, an attraction *between* molecules. It's about 5-10% of the strength of a typical covalent bond. A covalent bond is an intramolecular force, involving the sharing of electrons *within* a molecule, and is much stronger.

Question 2

Do polar molecules also have van der Waals forces?

Accepted Answer

Yes, absolutely. Van der Waals forces exist between *all* molecules because all molecules have electrons that are in constant motion. Polar molecules have both van der Waals forces and permanent dipole-dipole forces (and sometimes hydrogen bonds). The total intermolecular attraction is the sum of all these forces.

Question 3

How can I quickly determine if a molecule is polar or non-polar?

Accepted Answer

First, check for polar bonds by looking for atoms with different electronegativities. Second, consider the molecule's shape (from VSEPR theory). If the molecule is symmetrical and the polar bonds are arranged in a way that their dipoles cancel out (e.g., linear $CO_2$, tetrahedral $CCl_4$), the molecule is non-polar. If the shape is asymmetrical (e.g., bent $H_2O$, trigonal pyramidal $NH_3$), the dipoles won't cancel, and the molecule will be polar.

Intermolecular forces, electronegativity and bond properties

What you need to know

Molecular Stickiness