Lecture on Reactivity of Elements and Acids/Bases

Flashcards relating to the reactivity of elements, acids and bases, redox reactions, and relevant chemical concepts.

Reactivity

The tendency of an element to engage in chemical reactions.

Platinum

A metal known for its very low reactivity; does not react with sulfuric or hydrochloric acid.

Lithium

An alkali metal that reacts vigorously with water, potentially igniting.

Aluminum

A highly reactive metal that forms a protective layer of aluminum oxide when exposed to air.

Acids

Substances that produce H+ ions in solution and can disassociate completely in water.

Bases

Substances that produce OH- ions in solution; they can be strong or weak depending on their ability to disassociate.

Strong Acid

An acid that completely disassociates in solution, leaving no intact molecules.

Weak Acid

An acid that only partially disassociates in solution, leaving most of the molecules intact.

Dynamic Equilibrium

A condition in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction.

Neutralization Reaction

A chemical reaction in which an acid and a base react to form water and a salt.

Oxidation States

The hypothetical charge an atom would have if all bonds to atoms of different elements were ionic.

Redox Reaction

A chemical reaction that involves the transfer of electrons between two species.

OILRIG

An acronym for Oxidation Is Loss of electrons and Reduction Is Gain of electrons.

Hydrochloric Acid (HCl)

A strong acid that disassociates completely in water to produce H+ and Cl- ions.

Sulfuric Acid

The most produced chemical compound, commonly used in various industrial applications.

Ammonia

A basic compound that reacts with water to generate OH- but does not contain OH- in its molecular form.

Polyatomic Ions

Ions composed of two or more atoms that are covalently bonded, with a net charge.

Sodium Hydroxide

A common strong base that dissociates completely into sodium ions and hydroxide ions in solution.