Fundamental Inorganic Chemistry Quiz

The study of the chemical properties and reactions of all elements except carbon, as well as carbon-based molecules that are less reduced than carbon dioxide.

A compound formed by the electrostatic attraction between two oppositely charged ions, typically resulting in a crystalline solid.

An atom that carries a net electrical charge due to the gain or loss of electrons.

A positively charged ion formed by the loss of electrons from an atom.

A negatively charged ion formed by the gain of electrons to an atom.

The process of an acid losing a hydrogen ion (H+).

An acid that can donate more than one proton (H+).

The salt formed when an organic acid reacts with a base.

The pH value at which 50% of a solution is in the acidic form (HA) and 50% is in the conjugate base form (A-)

The reaction of an acid with water to form a hydronium ion (H3O+) and the conjugate base of the acid.

The species that remains after an acid has donated a proton. It is the deprotonated form of the acid.

The reaction of a base with water to form a hydroxide ion (OH-) and the conjugate acid of the base.

The species that is formed when a base accepts a proton. It has one more proton than the base.

A chemical species that can donate a proton (H+).

A chemical species that can accept a proton (H+).

A model of acid-base interactions that describes acids as electron-pair acceptors and bases as electron-pair donors.

A measure of the concentration of hydronium ions (H3O+) in a solution, represented by the formula pH = -log10[H+], where [H+] represents the molar concentration of hydrogen ions.

A solution's pH does not change significantly even if there are changes in the concentration of hydronium ions (H3O+). This is achieved by the presence of a weak acid and its conjugate base, which act as a buffer system to resist pH changes.

The strength of an acid is determined by its pKa, which reflects how readily it releases a proton (H+). Strong acids have a pKa below 0, easily dissociating in solution. Weak acids have a pKa above 0, dissociating less readily.

The equilibrium reaction of water, where water molecules donate and accept protons, resulting in the formation of hydronium ions (H3O+) and hydroxide ions (OH-).

Aqueous solutions (water-based) cannot have a pH above 14, but can reach negative pH values. This is because the pH scale is logarithmic, so there are no values beyond the limits.