IMF's & Polarity

Front

What are intermolecular forces (IMFs)?

Back

Intermolecular forces (IMFs) are forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). They play a crucial role in determining the physical properties of substances.

Front

What is polarity in molecules?

Back

Polarity refers to the distribution of electrical charge over the atoms joined by the bond. A polar molecule has a partial positive charge on one end and a partial negative charge on the other, due to differences in electronegativity.

Front

Which type of intermolecular force is present in polar molecules?

Back

Dipole-dipole forces are present in polar molecules, where the positive end of one polar molecule is attracted to the negative end of another.

Front

What is the strongest type of intermolecular force?

Back

Hydrogen bonding is the strongest type of intermolecular force, occurring when hydrogen is bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine.

Front

How many valence electrons does an atom need to be stable?

Back

Most atoms need 8 valence electrons to be stable, following the octet rule, except for hydrogen, which needs 2.

Front

What is the octet rule?

Back

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of 8 electrons, leading to greater stability.

Front

What is the molecular geometry of ammonia (NH3)?

Back

Ammonia (NH3) has a trigonal pyramidal molecular geometry due to the presence of a lone pair of electrons on the nitrogen atom.

Front

What are valence electrons?

Back

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms.

Front

How do you determine the polarity of a molecule?

Back

To determine the polarity of a molecule, assess the electronegativity differences between atoms and the molecular geometry. If the molecule has a net dipole moment, it is polar.

Front

What is a nonpolar molecule?

Back

A nonpolar molecule is one where the electrons are shared equally, resulting in no overall dipole moment. Examples include diatomic molecules like O2 and N2.