States of Matter

Question 1

What are the 3 states of matter?

Answer 1

solid, liquids and gases

Question 2

Describe the arrangement and movement and energy of a solid

Answer 2

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.

Question 3

Describe the arrangement and movement and energy of a liquid

Answer 3

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.

Question 4

Describe the arrangement , movement and energy of gases

Answer 4

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

Question 5

What are interconversions?

Answer 5

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

Question 6

Describe melting

Answer 6

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

Question 7

Describe freezing

Answer 7

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.

Question 8

Describe Evaporation

Answer 8

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.

Question 9

Describe Condesation

Answer 9

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.

Question 10

Describe Sublimation

Answer 10

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.

Question 11

How do interconversions happen?

Answer 11

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

Question 12

Define Solvent

Answer 12

A substance (liquid) that a solute can dissolve in

Question 13

Define Solute

Answer 13

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

Question 14

Define solution

Answer 14

a homogeneous mixture of 2 or more substances

Question 15

Define saturated solution

Answer 15

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

Question 16

What dilutes a solution?

Answer 16

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.

Question 17

What determines the colour of a solution?

Answer 17

the interaction between the light and the particles of the solute.

lower concentration = lower particles interacting with light = lighter colour
& it goes vice versa

Question 18

What are the factors of diffusion in gases?

Answer 18

temperature, pressure and molecular mass.

lighter gases diffuse more rapidly that heavier ones

Question 19

What is solubiltity?

Answer 19

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.

Question 20

On which axis of a solubility curve are temperature and solubility (per 100g) on?

Answer 20

temperature: x-axis
solubility: y-axis

Question 21

What does the resulting curve on a solubility curve represent?

Answer 21

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

Question 22

Interpret a solubility curve

Answer 22

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

Question 23

What is the saturation point?

Answer 23

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

Question 24

What is supersaturation?

Answer 24

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

Question 25

How do you determine the solubility of a solid in water at a specific temperature? PRACTICAL

Answer 25

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.