Secondary School Chemistry Flashcards

Comprehensive vocabulary flashcards covering the kinetic particle theory, states of matter, atomic structure, bonding, physical properties, separation techniques, and mole concepts from lecture notes.

Kinetic Particle Theory of Matter

A theory stating that particles of matter are discrete and too small to be seen directly, there are spaces between particles that vary across solids, liquids, and gases, and particles are in constant random motion at different speeds.

Solid State (Particle Arrangement and Movement)

Particles are packed closely in an orderly arrangement, vibrating and rotating about fixed positions.

Liquid State (Particle Arrangement and Movement)

Particles are packed closely in a disorderly arrangement, sliding past each other freely throughout the liquid.

Gaseous State (Particle Arrangement and Movement)

Particles are very far apart in a disorderly arrangement, moving fast and freely in all directions.

Sublimation

The phase transition process directly from a solid to a gas.

Vapour Deposition

The phase transition process directly from a gas to a solid.

Heating Curve (Change of State Behavior)

During a change of state on a heating curve, temperature remains constant because absorbed heat energy is taken in by particles to overcome the forces of attraction between them.

Cooling Curve (Change of State Behavior)

During a change of state on a cooling curve, temperature remains constant because heat energy is released as the forces of attraction between particles increase.

Ionic Compounds

Compounds consisting of a giant ionic lattice structure held by strong electrostatic forces of attraction, having high melting/boiling points, low volatility, solubility in water, and electrical conductivity in molten and aqueous states due to free-moving ions.

Covalent Molecules

Structures consisting of small covalent molecules held by weak intermolecular forces, having low melting/boiling points, high volatility, solubility in organic solvents, and no electrical conductivity in any state due to the absence of free-moving ions or mobile electrons.

Element

A pure substance that cannot be broken down into two or more simpler substances by chemical methods.

Compound

A pure substance containing two or more elements that are chemically combined in a fixed ratio.

Mixture

A system containing two or more elements and/or compounds that are not chemically combined, having a variable ratio of constituents and boiling/melting over a range of temperatures.

Alloy

A mixture of a metal and another element that is stronger and harder than pure metals because atoms of different sizes disrupt the orderly layers of pure metal atoms, making it difficult for layers to slide over one another.

Isotopes

Atoms of the same element that have the same proton number but a different nucleon number due to a different number of neutrons.

Ion

A charged particle formed when an atom or group of atoms gains or loses electrons while the number of protons and neutrons remains unchanged.

Proton Number

The total number of protons in the nucleus of an atom.

Nucleon Number

The total number of protons and neutrons in the nucleus of an atom.

Atom

The smallest particle that can still have the chemical characteristics of an element.

Electron

An extremely tiny sub-atomic particle located in the electron shell, carrying a relative charge of $-1$ and a relative mass of $\frac{1}{1840}$.

Avogadro's Constant

The constant value $6.02 \times 10^{23}$, representing the number of particles present in one mole of any substance.

Solvent

A liquid that dissolves solids.

Solute

A solid that dissolves in a solvent.

Saturated Solution

A solution in which no more solute can be dissolved at a given temperature.

Miscible Liquids

Liquids that mix together completely to form a uniform solution.

Immiscible Liquids

Liquids that do not form a uniform solution when mixed, separating into distinct layers.

Simple Distillation

A separation method used to separate a pure solvent from a solution at its fixed boiling point.

Fractional Distillation

A separation method used to separate a mixture of miscible liquids with different boiling points using a fractionating column.

Paper Chromatography

A technique used to separate a mixture of substances based on their differing solubilities in a given solvent.

Filtration

A method used to separate an insoluble solid from a liquid or solid-liquid mixture.

Evaporation to Dryness

A process used to separate a dissolved solid solute from its solvent by heating the mixture until all solvent vaporises.

Crystallisation

A process used to obtain a pure solid sample from its saturated solution.

Mass Concentration

The mass of solute dissolved per unit volume of solvent, measured in $g\,dm^{-3}$ and calculated as $\text{mass concentration} = \frac{\text{mass of solute (g)}}{\text{volume of solvent } (dm^3)}$.

Molar Concentration

The moles of solute dissolved per unit volume of solvent, measured in $mol\,dm^{-3}$ and calculated as $\text{molar concentration} = \frac{\text{mole of solute (mol)}}{\text{volume of solvent } (dm^3)}$.

Molar Volume

The volume occupied by $1\,mol$ of any gas, which is $24\,dm^3$ at room temperature and pressure.

Molar Mass

The mass of one mole of a substance expressed in $g\,mol^{-1}$, equal in value to relative atomic mass ($A_r$) or relative molecular/formula mass ($M_r$).