States of Matter

solid, liquids and gases

particles tightly pact touching each other in an ordered arrangement and can only vibrate. they have the least energy as not much kinetic energy for vibration.

particles are close together with no distinct arrangement. they can flow around and touch eachother. liquids have a mid amount of energy as they can move with some kinetic energy.

particles are free-floating and can go anywhere with no distinct arrangement. they can collide and move with each other. gases have the most energy as they move around freely with lots of kinetic energy

changing state: melting, freezing, evaporation, condensation and sublimation

process of converting solid to liquid by adding heat as heat is added particles gain more kinetic energy causing them to vibrate more vigorously. they overcome the force of attraction holding them in a fixed arrangement to move freely like a liquid

the process of converting a liquid to a solid by removing heat energy. as you remove heat the particles lose energy and slow down. bringing them closer together. the attractive forces between the particles become stronger and they become in a fixed shape.

the process of converting a liquid to gas. adding heat energy to increase kinetic energy and move faster. eventually particles gain enough energy to overcome forces of attraction and escape to surroundings as a gas.

process of converting a gas to a liquid state. removing heat energy and losing kinetic energy so slow down. attractive forces between particles become stronger and form into liquid.

the process of converting solid directly to gas without touching liquid state. by adding heat energy to solid, particles gain enough energy to break intermolecular forces and become a gas straight.

By adding or removing heat energy the particles kinetic energy can change, further changing their state.

A substance (liquid) that a solute can dissolve in

A substance that can be dissolved in a solution by a solvent.

a homogeneous mixture of 2 or more substances

a solution in which no more solid can dissolve into the liquid at a given temperature

Adding a solvent into a coloured solution can decrease the concentration of the solute. as solution dilutes the particles of solute spread out. and the colour becomes lighter.

the interaction between the light and the particles of the solute. lower concentration = lower particles interacting with light = lighter colour & it goes vice versa

temperature, pressure and molecular mass. lighter gases diffuse more rapidly that heavier ones

maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature. often standardised as per 100g to compare across other solvents and temperatures.

temperature: x-axis solubility: y-axis

resulting curve provides information on the solubility of a substance and how it changes throughout different temperatures.

curves upwards: solubility increases with temperature curves downwards: solubility decreases with temperature

the point where the solubility curve passes a specific temperature is the maximum amount of solute that can dissolve in a solvent at that temperature if a point falls above the solubility curve means its supersaturated

more solute is dissolved in the substance that should be possible in that temperature. overdoing it/excess.