Chemical Bonding and Quantitative Aspects

Comprehensive vocabulary flashcards covering chemical bonding, molecular geometry, intermolecular forces, and quantitative chemistry based on the lecture notes.

Chemiese binding

The mutual attraction between two atoms as a result of the simultaneous attraction between their nuclei and outer electrons.

Valence electrons

The electrons that occur in the outermost energy level of the atom.

Covalent bonding

The sharing of electrons between two atoms to form a molecule.

Molecule

A group of two or more atoms that are covalently bonded and function as a neutral unit.

Bonding pair

An electron pair that is shared between two atoms in a covalent bond.

Lone pair

An electron pair in the valence energy level of an atom that is not shared with another atom.

Unpaired electron

An electron that occurs alone in an orbital in the valence energy level. These are the electrons shared with another atom during covalent bonding.

Dative covalent bond

A bond formed when an atom with a lone pair in the valence energy level shares it with another atom that has an empty orbital in its valence energy level.

VSEPR model

An abbreviation for the Valence Shell Electron Pair Repulsion model.

Electronegativity

A measure of the tendency of an atom in a molecule to attract the bonding pair of electrons.

Non-polar covalent bond

A covalent bond in which both atoms attract the bonding electrons equally and thus contains no dipole moment.

Polar covalent bond

A covalent bond in which the bonding electrons lie closer to the atom with the higher electronegativity so that it contains a dipole moment.

Non-polar molecule

A molecule in which the charge is evenly distributed and thus contains no net dipole moment.

Polar molecule

A molecule in which the charge is unevenly distributed and thus contains a net dipole moment.

Bond length

The average distance between the nuclei of two atoms in a molecule.

Bond energy

The energy required to break $1$ mole of a compound's molecules in the gas state into atoms.

Bond order

The number of bonds (single, double, or triple) that exist between two atoms.

London forces

Intermolecular forces between non-polar molecules, also known as induced dipole or dispersion forces.

Dipole-dipole forces

Intermolecular forces between two polar molecules.

Dipole-induced dipole forces

Intermolecular forces between polar and non-polar molecules.

Hydrogen bonds

Intermolecular forces between molecules in which hydrogen is covalently bonded with nitrogen, oxygen, or fluorine (NOF).

Ion-dipole forces

Forces existing between ions and polar molecules.

Boiling point

The temperature at which the vapor pressure of a substance is equal to atmospheric pressure.

Melting point

The temperature at which the solid and liquid phases of a substance are in equilibrium.

Vapor pressure

The pressure exerted by a vapor in equilibrium with its liquid in a closed system.

Solubility

The property of a solid, liquid, or gaseous chemical substance (solute) to dissolve in a solvent to form a homogeneous solution.

Mole

The SI unit for the amount of substance.

One mole

The amount of substance that contains as many particles (atoms, molecules, formula units) as there are atoms in $12\,g$ of carbon-12.

Avogadro's number ($N_A$)

The number of particles present in one mole, equal to $6.02 \times 10^{23}\,mol^{-1}$.

Molar mass ($M$)

The mass of one mole of a substance's particles measured in $g\,mol^{-1}$.

Avogadro's law

States that one mole of any gas occupies the same volume at the same temperature and pressure.

Molar gas volume ($V_m$)

At Standard Temperature and Pressure (STP), $1$ mole of any gas occupies a volume of $22.4\,dm^3$.

Standard Temperature and Pressure (STP)

A set of standard conditions defined as a temperature of $0\,^{\circ}C$ ($273\,K$) and a pressure of $1$ atmosphere ($101.3\,kPa$).

Concentration ($c$)

The number of moles of solute per $1\,dm^3$ of solution, measured in $mol\,dm^{-3}$.

Standard solution

A solution whose concentration is exactly known.

Empirical Formula

The simplest whole-number ratio of atoms in a compound.

Molecular Formula

An expression indicating the actual number of atoms of each element in a compound.

Theoretical yield

The maximum amount of products that can be calculated from a chemical reaction.

Actual yield

The amount of product obtained in practice in a laboratory or chemical plant, which is typically less than the theoretical yield.

Limiting reactant

The reactant that is used up first during a reaction and determines the amount of product formed.

Excess reactant

The reactant that remains at the end of a chemical reaction.