Chemistry 1 Revision Support Booklet

Next Mock for Chemistry paper 1 is November 2019

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Define a compound Compounds contain two or more elements chemically combined

Define a mixture A mixture consists of two or more elements or compounds notchemically combined together

State the approximate radius of an atom 1x10-10 metres

Describe the current model of the atom A positively charged nucleus composed of both protons and neutrons surrounded by negatively charged electrons

What does the atomic number of an atom represent?

The number of protons

What does the mass number of an atom represent?

The number of protons and neutrons

Describe the plum pudding model of the atom

The plum pudding model of the atom is a ball of positive charge with negative electrons embedded in it

State the conclusions of the alpha scattering experiment

Most of the atom is empty space and there is a positive nucleus in the centre

How did Niels Bohr adapt the model of the atom?

He suggested that electrons orbit at specific distances

What did James Chadwick do to change the model of the atom?

His experiments provided evidence for the existence of the neutrons

State the electricalcharges of eachsubatomic particle

State the relativemass of eachsubatomic particle

Key Facts Memory Task: Chemistry - Atomic Structure

1. Define a compound

2. Define a mixture

3. State the approximate radius of an atom

4. Describe the current model of the atom

5. What does the atomic number of an atom represent?

6. What does the mass number of an atom represent?

7. Describe the plum pudding model of the atom

8. State the conclusions of the alpha scattering experiment

9. How did Niels Bohr adapt the model of the atom?

10. What did James Chadwick do to change the model of the atom?

11. State the electrical charges of each subatomic particle

12. State the relative mass of each subatomic particle

Key Facts Memory Task: Atomic Structure

How are elements arranged in the periodic table?

In order of atomic (proton) number and so that elements with similar properties are incolumns

What does the group number tell you about the atoms in that group?

The group number is the number of electrons in the outer shelle.g. all elements in group 2 have 2 electrons in their outer shell

How was the periodic table originally organised?

In order of atomic weight

How did Mendeleev improve the periodic table?

He left gaps so elements were in the same group as elements with the same properties

How did the discovery of isotopes affect the periodic table?

Knowledge of isotopes helped explain why placing elements in the order of atomic weight was not always correct

What is the difference between a metal and a non-metal?

Elements that react to form positive ions are metals.Elements that do not form positive ions are non-metals.

State the name of group 0, group 1 and group 7

Group 0 = The noble gases Group 1 = The alkali metals Group 7 = The halogens

Describe the properties of the elements in group 0

They are unreactive and do not easily form molecules

Explain why group 0 elements have the properties they do.

Their atoms have stable arrangements of electrons meaning they have a full outer shell

How does the reactivity change in group 1?

In Group 1, the reactivity of the elements increases as you go down the group.

Describe how the properties of group 7 elements changes as you go down the group

As you go down group 7 reactivity decreases, boiling point increases and melting point increases

Key Facts Memory Task: Periodic Table

1. How are elements arranged in the periodic table?

2. What does the group number tell you about the atoms in that group?

3. How was the periodic table originally organised?

4. How did Mendeleev improve the periodic table?

5. How did the discovery of isotopes affect the periodic table?

6. What is the difference between a metal and a non-metal?

7. State the name of group 0, group 1 and group 7

8. Describe the properties of the elements in group 0

9. Explain why group 0 elements have the properties they do.

10. How does the reactivity change in group 1?

11. Describe how the properties of group 7 elements changes as you go down the group

Key Facts Memory Task: Periodic Table

Describe ionic bonding Metal atoms lose electrons to become positively charged ions. Non-metal atoms gain electrons to become negatively charged ions. Opposites attract so they bond together.

Explain why ionic compounds have high melting and boiling points

There are strong electrostatic forces of attraction in all directions between oppositely charged ions

Explain why ionic compounds can conduct electricity when melted or dissolved in water

Ionic compounds conduct electricity because the ions are free to move and so charge canflow.

What form do ionic compounds take?

Giant lattice structure

Draw a diagram of the ionic bonding of sodium and chlorine

Draw a diagram of the metallic bonding

Describe metallic bonding A giant structure of positive metal ions is held together by the electrostatic attraction with the free electrons that can move throughout the structure.

Why are pure metals soft? In pure metals, atoms are arranged in layers which can slide over each other.

Why are alloys harder than pure metals?

Alloys are a mixture of metals and the different sized ions distort the layers so they can’t slide over each other

Why are metals good conductors? The delocalised electrons in the metal carry electrical charge through the metal

Key Facts Memory Task: Ionic and Metallic Bonding

1. Describe ionic bonding

2. Explain why ionic compounds have high melting and boiling points

3. Explain why ionic compounds can conduct electricity when melted or dissolved in water

4. What form do ionic compounds take?

5. Draw a diagram of the ionic bonding of sodium and chlorine

6. Draw a diagram of the metallic bonding

7. Describe metallic bonding

8. Why are pure metals soft?

9. Why are alloys harder than pure metals?

10. Why are metals good conductors?

Key Facts Memory Task: Ionic and Metallic Bonding

Describe covalent bonding Non-metal atoms share electrons to gain a full outer shell

Draw a diagram of a covalently bonded molecule

Ammonia NH3 Water H2O Oxygen O2

Why do small molecules have low melting and boiling points?

They have only weak forces between the molecules (intermolecular forces). It is these intermolecular forces that are overcome, not the covalent bonds

If the size of a small covalent molecule increases, what effect does this have on the boiling points?

As the size of the molecule increases, the intermolecular forces increase, which increases the boiling point

How many covalent bonds are their between atoms in diamond and graphite?

Diamond – 4 covalent bonds between atomsGraphite – 3 covalent bonds between atoms

Why is diamond hard and has very high melting and boiling points?

The covalent bonds are very strong

Why is graphite brittle? Graphite is structure in layers with only weak intermolecular forces between each layer

What is graphene? A single layer of graphite

What is a fullerene? Molecules of carbon atoms with hollow shapes made mostly of hexagonal rings of carbon atoms

Give 2 examples of fullerenes Buckminsterfullerene (a sphere of carbon atoms)Carbon nanotubes (a tube of carbon atoms)

Key Facts Memory Task: Covalent Bonding

1. Describe covalent bonding

2. Draw a diagram of a covalently bonded molecule

3. Why do small molecules have low melting and boiling points?

4. If the size of a small covalent molecule increases, what effect does this have on the boiling points

5. How many covalent bonds are their between atoms in diamond and graphite

6. Why is diamond hard and has very high melting and boiling points?

7. Why is graphite brittle?

8. What is graphene?

9. What is a fullerene?

10. Give 2 examples of fullerenes

Key Facts Memory Task: Covalent Bonding

State the law of conservation of mass No atoms are lost or made during a chemical reaction so the mass of the productsequals the mass of the reactants

Define relative formula mass (Mr) The sum of the relative atomic masses of the atoms in the numbers shown in the formulae.g. H2O = 1 + 1 + 16 = 18

If mass appears to be loss or gained in a reaction, what is the most likely cause?

If mass is lost, one of the products was probably a gasIf mass is gained, one of the reactants is probably a gas

How do you calculate the uncertainty of a group of repeat readings?

Half the range of the repeat readingse.g. If the repeat readings are 3, 5, 4, 7,2 then the range is 7-2 = 5 so the uncertainty = 2.5

HT ONLY – What is a mole? A specific number atoms, molecules, ions, etc

HT ONLY – What is the Avogadro constant?

The number of atoms, molecules, etc in a mole 6.02 x 1023

HT ONLY – How is the mass number linked to the number of moles?

The mass number of an element is the mass in grams of 1 mole of that elemente.g. The mass number of oxygen is 16 so 1 mole of oxygen is 16g

How is the concentration of a solution usually expressed?

Mass per given volume e.g. grams per dm3 (g/dm3)

Key Facts Memory Task: Quantitative Chemistry

1. State the law of conservation of mass

2. Define relative formula mass (Mr)

3. If mass appears to be loss or gained in a reaction, what is the most likely cause?

4. How do you calculate the uncertainty of a group of repeat readings?

5. HT ONLY – What is a mole?

6. HT ONLY – What is the Avogadro constant?

7. HT ONLY – How is the mass number linked to the number of moles?

8. How is the concentration of a solution usually expressed?

Key Facts Memory Task: Quantitative

What is produced when metals react with oxygen? Give an example

Metal oxides are produced when metals react with oxygene.g. Iron + Oxygen Iron oxide Magnesium + Oxygen Magnesium oxide

What happens to a metal when it reacts with different substances?

It forms positive ions

How are unreactive metals found? In the Earth as the metal itself (e.g. gold)

How are metals less reactive than carbon extracted?

They are reduced with carbon

How are metals more reactive than carbon extracted?

Electrolysis

What are oxidation and reduction reactions?

Oxidation is when oxygen is gained and the loss of electronsReduction is when oxygen is lost and the gain of electrons

Describe electrolysis Passing an electric current through electrolytes causes the ions to move to the electrodes separating them

Which ion moves to which electrode in electrolysis?

Positively charged ions move to the negative electrode (the cathode), and negatively charged ions move to the positive electrode (the anode)

Draw an labelled diagram of the set up needed for simple electrolysis

Key Facts Memory Task: Metal Reactions and Electrolysis

1. What is produced when metals react with oxygen? Give an example

2. What happens to a metal when it reacts with different substances?

3. How are unreactive metals found?4. How are metals less reactive than carbon extracted?5. How are metals more reactive than carbon extracted?6. What are oxidation and reduction reactions?7. Describe electrolysis8. Which ion moves to which electrode in electrolysis?9. Draw an labelled diagram of the set up needed for

simple electrolysis

Key Facts Memory Task: Metal Reactions and Electrolysis

What is produced when a metal reacts with an acid?

A salt and hydrogen ( Metal + Acid Salt + Hydrogen )

What is produced when a metal carbonatereacts with an acid?

A salt, water and carbon dioxide( Metal Carbonate + Acid Salt + Water + Carbon dioxide )

What is produced when an acid is neutralised by an alkali or base?

A salt and water ( Acid + Base Salt + Water )

What makes a chemical an acid? Acids produce hydrogen ions (H+) in aqueous solutions

What makes a chemical an alkali? Aqueous solutions of alkalis contain hydroxide ions (OH–).

How can the pH of a chemical be measured?

Universal indicator or a pH probe

Where are acids and alkalis on the pH scale?

0-6 = Acid 7 = Neutral 8-14 = Alkali

State the general equation for the reaction between an acid and an alkali

HT ONLY – What is the difference between a strong and a weak acid?

A strong acid is completely ionised in aqueous solution. A weak acid is only partially ionised in aqueous solution.

Why are solid bases often added ‘in excess’ when making a salt?

To make sure all the acid has been neutralised

Describe the steps to make a soluble salt

1. Add the base to the acid in excess2. Filter the solution to remove the excess

base3. Heat the solution to evaporate most of

the water4. Leave the solution to let the last of the

water evaporate and allow crystals toform

Key Facts Memory Task: Reactions of Acids

1. What is produced when a metal reacts with an acid?

2. What is produced when a metal carbonate reacts with an acid?

3. What is produced when an acid is neutralised by an alkali or base?

4. What makes a chemical an acid?

5. What makes a chemical an alkali?

6. How can the pH of a chemical be measured?

7. Where are acids and alkalis on the pH scale?

8. State the general equation for the reaction between an acid and an alkali

9. HT ONLY – What is the difference between a strong and a weak acid?

10. Why are solid bases often added ‘in excess’ when making a salt?

11. Describe the steps to make a soluble salt

Key Facts Memory Task: Reactions of Acids

What is an exothermic reaction? An exothermic reaction is one that transfers energy to the surroundings so the temperature of the surroundings increases

State examples and uses of exothermic reactions

Examples: Combustion, respiration, many oxidation reactionsUses: Hand warmers and self-heating cans

What is an endothermic reaction? An endothermic reaction is one that takes in energy from the surroundings so the temperature of the surroundings decreases

State examples and uses of endothermic reactions

Examples: thermal decompositions and the reaction of citric acid and sodium hydrogencarbonateUses: Cooling sports injury packs

Define activation energy The minimum amount of energy that particles must have to react

Draw and label the reaction profile for an exothermic reaction

Draw and label the reaction profile for an endothermic reaction

HT ONLY – Describe an exothermic reaction in terms of bond energies

The energy released from forming new bonds is greater than the energy needed to break existing bonds

HT ONLY – Describe an endothermic reaction in terms of bond energies

The energy needed to break existing bonds is greater than the energy released from forming new bonds

Key Facts Memory Task: Energy Changes

1. What is an exothermic reaction?

2. State examples and uses of exothermic reactions

3. What is an endothermic reaction?

4. State examples and uses of endothermic reactions

5. Define activation energy

6. Draw and label the reaction profile for an exothermic reaction

7. Draw and label the reaction profile for an endothermic reaction

8. HT ONLY – Describe an exothermic reaction in terms of bond energies

9. HT ONLY – Describe an endothermic reaction in terms of bond energies

Key Facts Memory Task: Energy Changes

Question Set Attempt 1 Attempt 2 Attempt 3 Attempt 4 Attempt 5

1 - Atomic Structure1 2 3 4 5 6 7 8 9 10 11 12 1 2 3 4 5 6 7 8 9 10 11 12 1 2 3 4 5 6 7 8 9 10 11 12 1 2 3 4 5 6 7 8 9 10 11 12 1 2 3 4 5 6 7 8 9 10 11 12

2 - Periodic Table1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11

3 - Ionic and Metallic Bonding1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10

4 - Covalent Bonding1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10 1 2 3 4 5 6 7 8 9 10

5 - Quantitative Chemistry1 2 3 4 5 6 7 8 1 2 3 4 5 6 7 8 1 2 3 4 5 6 7 8 1 2 3 4 5 6 7 8 1 2 3 4 5 6 7 8

6 - Metal Reactions and Electrolysis 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9

7 - Reactions of Acids1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11 1 2 3 4 5 6 7 8 9 10 11

8 - Energy Changes1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9 1 2 3 4 5 6 7 8 9

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