S1.1: Introduction to the Particulate Nature of Matter

Question 1

Define the term matter: (1)

Answer 1

• The material that makes up the world around us. (1)
• That has mass and takes up space. (1)

Question 2

Define the term atom: (1)

Answer 2

• The smallest unit of matter that contains specific properties. (1)

Question 3

Define the term element: (2)

Answer 3

• A pure substance that cannot be broken down any further. (1)
• And still retain its unique properties. (1)

Question 4

Define the term compound: (1)

Answer 4

When atoms of different elements can chemically bond together in a fixed ratio. (1)

Question 5

State what happens if the ratio of atoms in a compound changes: (1)

Answer 5

Its properties also change. (1)

Question 6

State why compounds and elements are classified as a pure substance: (1)

Answer 6

• Because they have a uniform composition. (1)

Question 7

Define the term mixture: (2)

Answer 7

• When there is more than one element or compound in no fixed ratio. (1)
• Which are not chemically bonded. (1)

Question 8

Explain why it is easy to separate mixtures such as sugar water:

Answer 8

• Water and mixture both have different properties. (1)
• When you put them together, they create a mixture and spread out next to each other. (1)
• Neither of them change at the chemical level so it can be easily separated. (1)

Question 9

Define the following terms:

• Homogeneous mixture: (2)
• Heterogeneous mixture:

Answer 9

• Homogeneous mixture: A mixture that has a uniform composition. (1)
• Meaning everything is spread out evenly so it has uniform properties. (1)

Question 10

State how filtering can separate mixtures:

Answer 10

• Used for mixtures that don’t fully dissolve. (1)

Question 11

Describe how magnets can separate mixtures: (2)

Answer 11

• Used for separating a magnetic substance from a non-magnetic substance. (1)
• Using a magnet. (1)

Question 12

State how distillation/evaporation can separate mixtures: (1)

Answer 12

• Separates liquids with different boiling points. (1)

Question 13

Define the term kinetic molecular theory: (1)

Answer 13

A model to explain physical properties and behaviour of matter. (1)

Question 14

State the process where:

• A solid turns into a liquid: (1)
• A liquid turns into a gas: (1)
• A gas turns into a liquid: (1)
• A liquid turns into a solid: (1)
• A solid turns into a gas: (1)
• A gas turns into a solid: (1)

Answer 14

• Melting (1)
• Evaporation (1)
• Condensation (1)
• Freezing (1)
• Sublimation (1)
• Deposition (1)

Question 15

Define the term kinetic: (1)

Answer 15

The energy an object has due to its motion. (1)

Question 16

Explain what happens when you apply heat to ice:

Answer 16

• The molecules will vibrate and move faster(1)
• Until some of them start to break off and are able to move around in a liquid state. (1)
• Heat can continue to be applied until they move so much until they can break off into a gaseous state. (1)

Question 17

Define the following terms:

• Endothermic: (2)
• Exothermic: (1)

Answer 17

• The change of state from more compact to less compact. (1)
• Because energy is taken up for the physical change to take place. (1)
• When energy is released from the substance to cause the state change. (1)

Question 18

Explain why deposition and sublimation skip the liquid phase: (2)

Answer 18

• They have a larger exothermic or endothermic swing and energy. (1)
• compared to condensing or melting. (1)

Question 19

Define the term temperature: (1)

Answer 19

• A measure of average kinetic energy of particles. (1)

Question 20

State what does ‘absolute zero’ mean in Kelvins: (1)

Answer 20

• There is no kinetic energy between the particles being measured. (1)

Question 21

State how to convert:

• From degrees celcious to kelvin: (1)

Answer 21

• Add 273.15