S1.1.1-2: Introduction to the particulate nature of matter

plasma

An ionised gas mainly found in outer space.

Density

the ratio of its mass to its volume

kinetic molecular theory (KMT)

All matter is made up of small particles.

These particles all have kinetic energy (the energy of motion) which causes the particles to constantly move.

The amount of kinetic energy is proportional to the temperature of the substance; therefore, the particles have greater motion at higher temperatures (straight line motion) and lesser motion at lower temperatures (vibrational motion).

Collisions between particles are elastic, which means no loss in kinetic energy.

Sublimation

change of state directly from a solid to a gas with no liquid phase

Deposition

the direct change from a gas to solid with no liquid phase

Evaporation

change of state from liquid to gas and takes place only at the surface of the liquid. It can occur at temperatures below the boiling point of the liquid

Boiling

change of state from liquid to gas throughout the liquid. When the vapour pressure is equal to the external pressure (1 atm) the liquid boils

atom

The smallest particle of an element that retains the properties of said element.

matter

A substance that has both mass and volume; typically classified as solid, liquid or gas.

pure substance

Consist of only one type of substance: either an element or a compound. Fixed composition

mixtures

Composed of more than one element or compound not in a fixed ratio, which are not chemically bonded.

allotropes

Alternative forms of an elemental substance in the same physical state

Compounds

Compounds are pure substances composed of two or more different elements chemically combined in fixed ratios.

homogeneous

A type of mixture that a uniform composition and no visible phases or boundaries.

heterogeneous

A type of mixture with a non-uniform composition with visible phases or boundaries.

Filtration

Separates insoluble solid from liquid or solution

Evaporation

Separates mixture with solute dissolved in solvent

Solvation

Separates heterogeneous mixture of solids based on solubility

Distillation

Separates liquid mixture by boiling point differences

Paper Chromatography

Separates a mixture of solutes in a solvent.
Mixture is dissolved in a solvent (mobile phase) and placed on chromatography paper (stationary phase).
Chromatography is a separation technique based on the different affinities of substances for a mobile phase vs a stationary phase.
Substances that interact more strongly with the stationary phase move slower.
Substances that interact more strongly with the mobile phase move faster.

Recrystallisation

Removes impurities from a solid using solubility differences

Absolute Zero

Lowest possible temperature, 0 K or -273°C

Freezing Point of Water

Temperature at which water freezes, 0°C or 273 K

Temperature During Melting

Remains constant to overcome intermolecular forces

Maxwell-Boltzmann distribution

moving particles in a gas or liquid do not all travel with the same velocity — The distribution of kinetic energies is shown by a Maxwell-Boltzmann curve
since number of particles will stay the same the area under the graph does not change

plasma

An ionised gas mainly found in outer space.

Density

the ratio of its mass to its volume

kinetic molecular theory (KMT)

All matter is made up of small particles.

These particles all have kinetic energy (the energy of motion) which causes the particles to constantly move.

The amount of kinetic energy is proportional to the temperature of the substance; therefore, the particles have greater motion at higher temperatures (straight line motion) and lesser motion at lower temperatures (vibrational motion).

Collisions between particles are elastic, which means no loss in kinetic energy.

Sublimation

change of state directly from a solid to a gas with no liquid phase

Deposition

the direct change from a gas to solid with no liquid phase

Evaporation

change of state from liquid to gas and takes place only at the surface of the liquid. It can occur at temperatures below the boiling point of the liquid

Boiling

change of state from liquid to gas throughout the liquid. When the vapour pressure is equal to the

external pressure (1 atm) the liquid boils

immiscible

not forming a homogeneous mixture when mixed

physical properties of the components that affect seperation method

boiling point, solubility, polarity, particle size, magnetism