Chemistry Combo Sheet: Acids, Bases, Redox, and Electrochemistry

Vocabulary practice flashcards covering Bronsted-Lowry acid-base theory, pH, ocean acidification, redox rules, and electrochemical cells.

Acid (Bronsted-Lowry)

A proton ($H^+$) donor.

Base (Bronsted-Lowry)

A proton ($H^+$) acceptor.

Conjugate base

The species that remains after an acid has lost a proton ($H^+$).

Conjugate acid

The species formed after a base has gained a proton ($H^+$).

Dissociation

The process of substances splitting into ions in water.

Ion

Formed when an atom gives up an electron to another one.

pH Scale

A logarithmic measurement of $H$ concentration where a change of 1 pH equals a $10 \times$ change in $[H]$.

Ocean Acidification

The process where human activities release excess $CO_2$ which dissolves in seawater to form carbonic acid ($H_2CO_3$).

Neutralisation Reaction

A reaction in which $H^+\text{(aq)}$ and $OH^-\text{(aq)}$ form pure water, resulting in a pH of 7 and the general equation: $\text{acid} + \text{base} \rightarrow \text{salt} + \text{water}$.

Titration Volume Conversion

$1000\text{ cm}^3 = 1\text{ dm}^3$.

Oxidation

The loss of electrons.

Reduction

The gain of electrons.

Oxidising agent

The species being reduced that causes oxidation in the other species.

Reducing agent

The species being oxidised that causes reduction in the other species.

Free Element Oxidation Number

The oxidation number is 0 for elements like $O$, $Na$, $Mg$, $O_2$, or $S_8$.

Hydrogen Oxidation States

$+1$ when bonded to non-metals; $-1$ when bonded to metals or boron.

Oxygen Oxidation States

$-2$ generally, except in $OF_2$ where it is $+2$ or in hydrogen peroxide ($H_2O_2$) where it is $-1$.

Halogen Oxidation Number

Group 7 elements have an oxidation of $-1$ unless bonded to Oxygen or Fluorine.

Galvanic / Voltaic cell

A cell that converts chemical energy to electrical energy through a spontaneous reaction using two half-cells.

Electrolytic cell

A cell that converts electrical energy to chemical energy using a power supply for a non-spontaneous reaction.

Anode

The electrode where oxidation occurs; it is negatively charged in galvanic cells and positively charged in electrolytic cells.

Cathode

The electrode where reduction occurs; it is positively charged in galvanic cells and negatively charged in electrolytic cells.

Salt bridge

A component in a galvanic cell that allows the movement of ions to maintain electrical neutrality.