States of Matter Flashcards
What are the 3 states of matter?
solid, liquids and gases
Describe the arrangement and movement and energy of a solid
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.
Describe the arrangement and movement and energy of a liquid
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.
Describe the arrangement , movement and energy of gases
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
What are interconversions?
changing state:
melting, freezing, evaporation, condensation and sublimation
Describe melting
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
Describe freezing
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.
Describe Evaporation
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.
Describe Condesation
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.
Describe Sublimation
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.
How do interconversions happen?
By adding or removing heat energy the particles kinetic energy can change, further changing their state.
Define Solvent
A substance (liquid) that a solute can dissolve in
Define Solute
A substance that can be dissolved in a solution by a solvent.
Define solution
a homogeneous mixture of 2 or more substances
Define saturated solution
a solution in which no more solid can dissolve into the liquid at a given temperature
What dilutes a solution?
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.
What determines the colour of a solution?
the interaction between the light and the particles of the solute.
lower concentration = lower particles interacting with light = lighter colour
& it goes vice versa
What are the factors of diffusion in gases?
temperature, pressure and molecular mass.
lighter gases diffuse more rapidly that heavier ones
What is solubiltity?
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.
On which axis of a solubility curve are temperature and solubility (per 100g) on?
temperature: x-axis
solubility: y-axis
What does the resulting curve on a solubility curve represent?
resulting curve provides information on the solubility of a substance and how it changes throughout different temperatures.
Interpret a solubility curve
curves upwards: solubility increases with temperature
curves downwards: solubility decreases with temperature
What is the saturation point?
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
What is supersaturation?
more solute is dissolved in the substance that should be possible in that temperature. overdoing it/excess.
How do you determine the solubility of a solid in water at a specific temperature?
PRACTICAL
Prepare a known mass of the solid substance (solute) and a specified volume of water (solvent) at the desired temperature.
Add the solid substance to the water and stir the mixture until the solute is completely dissolved.
If the solute does not dissolve completely, you have reached the saturation point at that temperature.
If the solute completely dissolves, add more of the solid substance in small increments while stirring until no more solute dissolves. This step helps determine the maximum solubility at that temperature.
Measure the mass of the undissolved solid to determine the amount of solute that did not dissolve.
Calculate the solubility by dividing the mass of the dissolved solute by the mass of the solvent used (water) and multiplying by 100.
