General Chemistry: Chemical Nomenclature, Chemical Bonding, and Intermolecular Forces

Comprehensive vocabulary flashcards covering chemical nomenclature, types of chemical bonds, electronegativity thresholds, polar and nonpolar molecules, intermolecular forces, and key historical figures from the lecture.

Chemical nomenclature

The system used to name chemical compounds based on their elements and chemical composition.

Ionic compounds

Compounds formed between metals and nonmetals or ions.

Covalent compounds

Compounds formed between two or more nonmetals.

Acids

Compounds that produce hydrogen ions ($\text{H}^+$) in water.

Binary acids

Acids consisting of hydrogen and one nonmetal, named using the pattern hydro- + nonmetal root + -ic acid (e.g., $\text{HCl}$ as hydrochloric acid, $\text{HBr}$ as hydrobromic acid).

Oxyacids

Acids containing hydrogen, oxygen, and another element, named by changing the anion ending -ate to -ic acid and -ite to -ous acid.

Intermolecular forces

Forces of attraction or repulsion between molecules that hold them together and affect the physical states and properties of substances.

Inter-ionic forces

Forces of attraction between charged particles called ions (e.g., the attraction between $\text{Na}^+$ and $\text{Cl}^-$).

Electronegativity

The ability of an atom to attract shared electrons toward itself.

Nonpolar covalent bond

A bond characterized by an electronegativity difference between $0$ and $0.4$.

Polar covalent bond

A bond characterized by an electronegativity difference between $0.4$ and $1.8$.

Ionic bond

A chemical bond characterized by an electronegativity difference above $1.8$.

Polar molecules

Molecules that have unequal sharing of electrons, partial positive and partial negative ends, and a net overall molecular dipole moment (e.g., $\text{HCl}$, $\text{NH}_3$, $\text{H}_2\text{O}$, $\text{PCl}_3$).

Nonpolar molecules

Molecules that have no overall molecular dipole because their bond dipoles cancel out or their bonds are nonpolar (e.g., $\text{CH}_4$, $\text{CO}_2$, $\text{BF}_3$, $\text{O}_2$).

Dipole-dipole forces

Attractive intermolecular forces between polar molecules, occurring when the partial positive end of one molecule attracts the partial negative end of another.

Ion-dipole forces

Attractive forces between a charged particle (ion) and a polar molecule, commonly observed when ionic compounds dissolve in water during hydration.

Dispersion forces (London forces)

The weakest intermolecular attractive force, caused by temporary dipoles induced by the movement of electrons; also known as induced-dipole–induced-dipole attraction.

Hydrogen bond

A special type of dipole-dipole attraction occurring between a hydrogen atom bonded to a highly electronegative atom and an $\text{N}$, $\text{O}$, or $\text{F}$ atom of another molecule.

Hydration

The interaction of water molecules with dissolved ions.

Temporary dipole

A brief separation of electrical charges caused by the spontaneous movement of electrons.

Dipole

The separation of positive and negative electrical charges.

Ion

A charged atom or group of atoms.

Johannes Diderik van der Waals

A scientist born on November 23, 1837, in Leiden, Netherlands, who presented the non-ideality of real gases in 1873 and contributed significantly to the study of intermolecular attraction.

Van der Waals forces

A category of intermolecular forces comprising dipole-dipole forces, ion-dipole forces, and dispersion forces.