Topic 2: Definitions Flashcards
Oxidation
Losing electrons
OIL - oxidation is losing
Reduction
Gaining electrons
RIG - reduction is gaining
Anode
Negative electrode where oxidation occurs
An Ox - Anode Oxidation
Cathode
Positive electrode where reduction occurs
Red Cat - Reduction Cathode
Acid-base reaction
Neutralisation double-replacement reaction
acid + base ⇌ water + salt
side notes:
Acid - hydrogen-containing substance capable of donating a proton or hydrogen ions
Base - donates electrons, accepts protons, or releases hydroxide (OH-) ions in aqueous solution
Reversible - ⇌
Water - H2O
Salt - ionic bond (M+NM)
Acid
Ions/compounds that donate protons (H+) and accepts electrons
hydrogen-containing substance capable of donating a proton or hydrogen ions (H+)
HCl, H2SO4, HNO3, H3PO4, HS3O3 (no need to memorise)
Base
Ions/compounds that accept protons (H+)
Donates electrons, accepts protons, or releases hydroxide (OH-) ions in aqueous solution
Strong acids and bases
Strong acids easily donate protons
Strong bases easily accept protons
Amphoteric
Is a molecule or ion that can react both as an acid or base
e.g. H20
Conjugate acids and bases
e.g. HCl + NH3 → NH4+ + Cl-
Conjugate acid - similar structure to the base but with an additional hydrogen (NH4+)
Conjugate base - similar structure to the acid but with a removed hydrogen (Cl-)
Ionisation
Electrically neutral atoms are converted to electrically charged atoms (ions).
acid + water reaction
Ionisation reaction
HX + H2O → H3O+ + X-
Monoprotic acids (didn’t learn but might be important to know)
Have one proton (hydrogen) available to donate in a chemical reaction.
e.g. HCl (only one hydrogen is available to donate)
Polyprotic acids (didn’t learn but might be important to know)
Have more than one proton available to donate in a chemical reaction.
Stoichiometry
Predicts the quantities of reactants consumed and produced in an acid-base reaction