Chemistry - Classifying Compounds, Gas Laws, Acids, and Bases

Flashcards reviewing key vocabulary and concepts from a Chemistry lecture on classifying compounds, gas laws, acids, and bases.

Ionic Compound

A pure substance formed from a metal and a nonmetal.

Molecular Compound

A pure substance formed from two or more different nonmetals.

Electrical Conductivity

The ability of a material to allow electricity to flow through it.

Electrolyte

A substance that forms a solution that conducts electricity.

Atmospheric pressure

Force per unit area exerted by air on all objects.

Boyle’s Law

As the pressure on a gas increases, the volume of the gas decreases proportionally, provided that the temperature and amount of gas remain constant; the volume and pressure of a gas are inversely proportional.

Absolute Zero

Believed to be the lowest possible temperature.

Kelvin Temperature Scale

A temperature scale with zero kelvin (0 K) at absolute zero and the same size divisions as the Celsius temperature scale.

Charles’s Law

The volume of a gas varies directly with its temperature in kelvin, if the pressure and amount of gas are constant.

Pressure and Temperature Law

The pressure exerted by a gas varies directly with the absolute temperature if the volume and amount of gas remain constant.

Combined Gas Law

The product of the pressure and volume of a gas sample is proportional to its absolute temperature in kelvin; pv = kT.

Titration

A laboratory procedure involving the carefully measured and controlled addition of a solution from a buret into a measured volume of a sample solution.

Titrant

The solution in the buret during a titration.

Endpoint

The point in a titration at which a sharp change in a property occurs (e.g., a colour change).

Standard Solution

A solution of precisely and accurately known concentration.

Strong Base (Arrhenius Theory)

An ionic hydroxide that dissociates 100% in water to produce hydroxide ions.

Weak Base (Reaction-with-Water Theory)

A chemical that reacts less than 50% with water to produce hydroxide ions.

Acid (Brønsted-Lowry Concept)

A proton donor.

Base (Brønsted-Lowry Concept)

A proton acceptor.

Amphiprotic

A substance capable of acting as an acid or a base in different chemical reactions; an entity that can gain or lose a proton (sometimes called amphoteric).

Conjugate Base

The base formed by removing a proton (H+) from an acid.

Conjugate Acid

The acid formed by adding a proton (H+) to a base.

Conjugate Acid-Base Pair

An acid-base pair that differs by one proton (H+).

pH

A measure of the acidity of a solution; the negative logarithm, to the base ten, of the hydrogen ion molar concentration.

Neutralization

A reaction between an acid and a base that results in a pH closer to 7.

Saturated Solution

A solution containing the maximum quantity of a solute at specific temperature and pressure conditions.

Solubility

A property of a solute; the concentration of a saturated solution of a solute in a solvent at a specific temperature and pressure.

Immiscible

Two liquids that form separate layers instead of dissolving

Miscible

Liquids that mix in all proportions and have no maximum concentration

Kinetic Molecular Theory

The idea that all substances contain particles that are in constant, random motion

Boyle's Law

As the pressure on a gas increases, the volume of the gas decreases.

Thermal Energy

The total energy of the particles in a material.

Avogadro's Law

Volume is directly proportional to the # of moles.

Dalton's Law of Partial Pressures

For a mixture of gases in a container, PTOTAL = P1 + P2 + P3 + …

Chemical Bond

The forces of attraction holding atoms or ions together

Formula Unit

The simplest whole-number ratio of atoms or ions of the elements in an ionic compound