U5 Molecular Geometry & IMF Practice Test

Front

What are polar molecules?

Back

Molecules that have a net dipole moment due to the presence of polar bonds, resulting in an uneven distribution of electron density.

Front

Give examples of polar molecules.

Back

Water (H2O), Ammonia (NH3), and Carbon Monoxide (CO) are examples of polar molecules.

Front

What is the shape of a trigonal pyramidal molecule?

Back

A molecular shape where a central atom is bonded to three other atoms and has one lone pair, resulting in a pyramid-like structure.

Front

What is the difference between polar and nonpolar molecules?

Back

Polar molecules have a partial positive and negative charge due to unequal sharing of electrons, while nonpolar molecules have an even distribution of charge.

Front

Are all molecules with polar covalent bonds polar?

Back

No, some molecules with polar covalent bonds can be nonpolar if their shape allows for symmetrical charge distribution.

Front

What types of compounds dissolve easily in water?

Back

Polar and ionic compounds dissolve easily in water due to their ability to interact with water molecules.

Front

What is the definition of intermolecular forces (IMF)?

Back

Forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions).

Front

Name the three main types of intermolecular forces.

Back

Dipole-dipole interactions, hydrogen bonding, and London dispersion forces.

Front

What is hydrogen bonding?

Back

A strong type of dipole-dipole interaction that occurs between molecules containing hydrogen bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine.

Front

What is the significance of molecular geometry in determining polarity?

Back

The shape of a molecule affects the distribution of charge, which in turn determines whether the molecule is polar or nonpolar.