Mediaspace scheduled maintenance: Aug 25, 2026 07:00 - 12:00 AM. During this time, videos will be temporarily unavailable. Check status updates.

Lecture

Chemical Equilibria and Reactivity

Description

This lecture covers the concepts of precipitation reactions, solubility rules for ionic compounds, acids and bases definitions, strong and weak acids, bases, and examples of acid-base reactions. It also discusses oxidation-reduction reactions, oxidation number changes, and properties of gases.

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Topics in inorganic chemistry

Chemical reactions: Chemical substances

Related concepts (32)

Acid–base reaction

An acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH via titration. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory. Their importance becomes apparent in analyzing acid–base reactions for gaseous or liquid species, or when acid or base character may be somewhat less apparent.

Ionic bonding

Ionic bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions, or between two atoms with sharply different electronegativities, and is the primary interaction occurring in ionic compounds. It is one of the main types of bonding, along with covalent bonding and metallic bonding. Ions are atoms (or groups of atoms) with an electrostatic charge. Atoms that gain electrons make negatively charged ions (called anions). Atoms that lose electrons make positively charged ions (called cations).

Acid

An acid is a molecule or ion capable of either donating a proton (i.e. hydrogen ion, H+), known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid. The first category of acids are the proton donors, or Brønsted–Lowry acids. In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents.

Lewis acids and bases

A Lewis acid (named for the American physical chemist Gilbert N. Lewis) is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct. For example, NH3 is a Lewis base, because it can donate its lone pair of electrons.

Salt (chemistry)

In chemistry, a salt is a chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions, which results in a compound with no net electric charge. A common example is table salt, with positively charged sodium ions and negatively charged chloride ions. The component ions in a salt compound can be either inorganic, such as chloride (Cl−), or organic, such as acetate (CH3COO−). Each ion can be either monatomic, such as fluoride (F−), or polyatomic, such as sulfate (SO42−).

Related lectures (50)

Acids and Bases: Definitions and Equilibrium

Explains acid-base definitions, equilibrium constants, pH scale, conjugate pairs, and buffers.

Chemical Equilibria and Reactivity

Explores electrolytes, precipitation, acids, bases, oxidation-reduction, and gas properties in chemical reactions.

Acid-Base Equilibria

Explores acid-base equilibria, including pH calculations for weak acids and bases, diacids, strong/weak bases, and salt solutions.

Acids and Bases: Equilibrium and Redox Reactions

Explores acids, bases, pH calculations, buffer solutions, and redox reactions.

Chemical Equilibria and Reactivity

Explores chemical equilibria, weak acids, buffers, titration curves, and indicators in acid-base reactions.

Related concepts (32)

Acid–base reaction

Ionic bonding

Acid

Lewis acids and bases

Salt (chemistry)