Reactive Chemistry Vocabulary

Flashcards covering key vocabulary terms from the Reactive Chemistry lecture notes.

Intermolecular Forces

Forces between molecules, weaker than intramolecular forces.

Intramolecular Forces

Forces within molecules, such as covalent, ionic, and metallic bonds.

Synthesis Reaction

A reaction where two or more substances combine to form a new substance; also known as a combination reaction.

Decomposition Reaction

A reaction where a compound breaks down into two or more substances.

Combustion Reaction

A type of synthesis reaction where a fuel is burned in oxygen to form the oxide of the fuel, releasing heat.

Incomplete Combustion

Combustion with insufficient oxygen, forming water and carbon monoxide and releasing less energy.

Single Displacement Reaction

Reaction when a metal displaces the ion of a less reactive metal from a solution.

Precipitation Reaction

Reactions where two clear solutions mix and form a solid precipitate; also called double displacement reaction.

Spectator Ions

Ions that do not participate in a precipitation reaction and remain dissolved in the solution.

Full Ionic Equation

Equation showing all ions in a reaction as separate ions.

Net Ionic Equation

An ionic equation that excludes spectator ions, showing only the reacting species.

Acids

Substances that can donate protons (H+).

Bases

Substances that can accept protons (H+).

Neutralisation

Reaction between an acid and a base, often producing water and salt.

Acidic Oxides

Non-metallic oxides that react with water to form an acid.

Basic Oxides

Metallic oxides that act as a base, producing water and salt when reacted with an acid.

Limewater Test

A test for carbon dioxide gas where limewater turns cloudy due to formation of calcium carbonate.

Ionisation Energy

The energy required to remove electrons from an atom; linked to metal reactivity.

Electronegativity

Measure of the ability of an atom to attract electrons; inversely proportional to metal reactivity.

Atomic Radius

The distance between the valence electron and the nucleus.

Activity Series of Metals

A list showing the reactivity of metals, following the trend on the periodic table.

Oxidant (Oxidizing Agent)

The substance that causes oxidation and is itself reduced.

Reductant (Reducing Agent)

The substance that causes reduction and is itself oxidized.

Oxidation State

A number representing the charge of an element in a substance, used to determine if a redox reaction has occurred.

Oxidation

The process of losing electrons.

Reduction

The process of gaining electrons.

Galvanic Cell

Scientific name for a battery; derives electrical energy from chemicals inside.

Anode

The electrode where oxidation occurs in a galvanic cell.

Cathode

The electrode where reduction occurs in a galvanic cell.

Standard Electrode Potential

The voltage measured when a substance is placed in a galvanic cell against a hydrogen half-cell under standard conditions.

Voltage

Measure of the electromotive force in a conductor Voltage pushes the electrons through the circuit.

Spontaneity of a Cell

The ability of a cell to produce electricity without needing a outside source of energy.

Electrolyte

A solution containing dissolved ionic substances, allowing for easy electrical conduction.

Salt Bridge

A component used to equalize charges in a galvanic cell by moving ions between half-cells.

Galvanic Cell Notation

Notation used to represent galvanic cells.

Activation Energy

Energy required to break chemical bonds and start a reaction.

Rate of Reaction

Speed at which chemical reactions occur; rate of change of concentration with time.

Catalyst

Substance that increases the rate of reaction without being used up.

Heterogeneous Catalyst

Catalyst in a different phase from the reactants, providing a surface for the reaction.