Relative formula mass

Lithium, carbon, nitrogen, fluorine and neon are elements in the same row of the periodic table.

What is the chemical symbol of lithium?

Use the periodic table.

Lithium has metallic bonding.

Which electrons are involved in metallic bonding?

Tick () one box.

Lithium reacts with fluorine to produce lithium fluoride.

Draw one line from each substance to the particle diagram that represents the substance.

Table 2 shows the electrical conductivity of three substances.

Lithium fluoride is an ionic compound.

Which substance is lithium fluoride?

Tick () one box.

Carbon can exist in different forms.

Figure 4 represents one form of carbon.

What is the name of the form of carbon in Figure 4 ?

Tick () one box.

Carbon and fluorine form a compound with the formula CF₄

Calculate the relative formula mass (M_r) of CF₄

Relative atomic masses (A_r): C = 12 F = 19

Figure 5 represents a molecule of nitrogen.

What is the total number of shared electrons in the covalent bond shown in Figure 5 ?

Lithium and nitrogen form a compound with the formula Li₃N

Complete the sentence.

Choose the answer from the box.

Neon does not react with other elements to form compounds.

Why is neon unreactive?

Tick () one box.

A student investigated an exothermic reaction.

The student reacted solid calcium oxide with water to produce calcium hydroxide.

What is meant by an ‘exothermic’ reaction?

The formula of calcium hydroxide is Ca(OH)₂

Calculate the percentage by mass of oxygen in calcium hydroxide.

Relative atomic mass (A_r): O = 16

Relative formula mass (M_r): Ca(OH)₂ = 74

When solid calcium oxide is added to water, the temperature of the reaction mixture changes.

Plan a method to investigate how changing the mass of calcium oxide affects the temperature change of the reaction mixture.

A student investigated an exothermic reaction.

The student reacted solid calcium oxide with water to produce calcium hydroxide.

What is meant by an ‘exothermic’ reaction?

The formula of calcium hydroxide is Ca(OH)₂

Calculate the percentage by mass of oxygen in calcium hydroxide.

Relative atomic mass (A_r): O = 16

Relative formula mass (M_r): Ca(OH)₂ = 74

When solid calcium oxide is added to water, the temperature of the reaction mixture changes.

Plan a method to investigate how changing the mass of calcium oxide affects the temperature change of the reaction mixture.

Copper is a useful metal.

Figure 11 shows the mass of copper produced between 1900 and 2010.

Give two conclusions that can be made from Figure 11.

Mixtures of copper and zinc are heated to produce alloys.

Figure 12 represents the structures of pure copper and of an alloy of copper and zinc.

Explain why the alloy of copper and zinc is harder than pure copper.

Use Figure 12.

A 5.25 g sample of an alloy of copper and zinc contains 13.5% zinc by mass.

Calculate the mass of copper in the 5.25 g sample.

Give your answer to 3 significant figures.

Copper is a useful metal.

Figure 1 shows the mass of copper produced between 1900 and 2010.

Give two conclusions that can be made from Figure 1.

Mixtures of copper and zinc are heated to produce alloys.

Figure 2 represents the structures of pure copper and of an alloy of copper and zinc.

Explain why the alloy of copper and zinc is harder than pure copper.

Use Figure 2.

A 5.25 g sample of an alloy of copper and zinc contains 13.5% zinc by mass.

Calculate the mass of copper in the 5.25 g sample.

Give your answer to 3 significant figures.

Lithium hydroxide reacts with sulfuric acid to produce lithium sulfate. The equation for the reaction is:

What type of reaction is this?

Relative atomic masses (A_r): H = 1 O = 16 S = 32

Relative atomic mass (A_r): O = 16

Give your answer to 2 significant figures.

A solution of lithium sulfate contains 0.30 g of lithium sulfate in 25 cm³. Calculate the concentration of lithium sulfate in g/dm³.

Lithium hydroxide reacts with sulfuric acid to produce lithium sulfate. The equation for the reaction is:

What type of reaction is this?

Relative atomic masses (A_r): H = 1 O = 16 S = 32

Relative atomic mass (A_r): O = 16

Give your answer to 2 significant figures.

A solution of lithium sulfate contains 0.30 g of lithium sulfate in 25 cm³. Calculate the concentration of lithium sulfate in g/dm³.

This question is about structure and bonding. Figure 6 represents part of the structure of silicon dioxide.

What type of structure is silicon dioxide? Tick (✓) one box.

Each oxygen atom forms two bonds. What is the number of bonds formed by each silicon atom? Use Figure 6.

Figure 7 represents part of a fullerene.

Complete the sentence. Choose the answer from the box.

Complete the sentence. Choose the answer from the box.

The fullerene molecule shown in Figure 7 is made from

What is the fullerene molecule shown in Figure 7 used for? Tick (✓) one box.

Figure 8 represents part of the structure of a polymer.

What holds the atoms together in a polymer chain? Tick (✓) one box.

Complete the sentence. Choose the answer from the box.

In Figure 8 the polymer chains are held together by

Figure 9 represents part of the structures of:

• magnesium metal

• a magnesium alloy.

Calculate the percentage of copper atoms in the alloy. Number of magnesium atoms in the alloy = Number of copper atoms in the alloy = Total number of atoms in the alloy =

Explain why the magnesium alloy is harder than magnesium metal. Use Figure 9.

This question is about elements and compounds.

Magnesium and oxygen react to produce magnesium oxide. Balance the equation for the reaction.

Suggest one safety precaution that should be taken when heating magnesium and oxygen.

Calculate the relative formula mass (M_r) of magnesium fluoride (MgF₂). Relative atomic masses (A_r): F = 19 Mg = 24

Argon is a noble gas. Explain why no product is formed when magnesium and argon are heated together.

Figure 10 shows a reactivity series.

Figure 10

Draw one line from each metal to the method used to extract that metal. Use Figure 10.

Metal Method used to extract that metal

A substance conducts electricity when it has charged particles that are free to move.

Figure 11 represents the structure of sodium chloride.

Explain why sodium chloride conducts electricity when molten but not when solid.

Figure 12 represents the structure of sodium metal.

Explain why sodium metal conducts electricity when solid.

Magnesium is in Group 2 of the periodic table. 1.0 g of magnesium reacted with chlorine to produce magnesium chloride.

Which types of element react when magnesium reacted with chlorine? Tick (✓) one box.

Write the word equation for the reaction when magnesium reacts with chlorine.

What apparatus was used to measure the mass of 1.0 g of magnesium? Tick (✓) one box.

What mass of magnesium chloride was produced? Tick (✓) one box.

Magnesium reacts with oxygen to produce magnesium oxide. Calculate the percentage mass of magnesium in magnesium oxide (MgO). Relative atomic mass (A_r): Mg = 24 Relative formula mass (M_r): MgO = 40

Magnesium carbonate decomposes to produce magnesium oxide and carbon dioxide.

The word equation for the reaction is: magnesium carbonate → magnesium oxide + carbon dioxide Four students heated 2.00 g of magnesium carbonate for 10 minutes. Table 1 shows the results.

What is the most likely reason for Student 3 ’s anomalous result? Tick (✓) one box.

Calculate value X in Table 1. Do not use the anomalous result. Give your answer to 2 significant figures.

Sodium and potassium are Group 1 elements.

What is the name of Group 1 elements? Tick (✓) one box.

Figure 5 represents the melting points of Group 1 elements.

What is the melting point of sodium?

Sodium reacts with water to produce sodium hydroxide and hydrogen. Balance the equation for the reaction.

Calculate the relative formula mass (M_r) of sodium hydroxide (NaOH). Relative atomic masses (A_r): H = 1 O = 16 Na = 23

Sodium and potassium both react with water. Figure 6 shows sodium reacting with water.

Compare what is seen when sodium reacts with water and when potassium reacts with water.

This question is about gold and compounds of gold. In the alpha particle scattering experiment alpha particles are fired at gold foil. Alpha particles are positively charged. Figure 4 shows the results.

Some alpha particles are deflected. Complete the sentence. Choose the answer from the box.

Some alpha particles are deflected because the nucleus of the atom is.

Why are most alpha particles not deflected? Tick (✓) one box.

What was one conclusion from the alpha particle scattering experiment? Tick (✓) one box.

Gold reacts with the elements in Group 7 of the periodic table.

What are Group 7 elements known as? Tick (✓) one box.

Fluorine, chlorine and bromine react with gold. Which element will be the most reactive with gold?

Tick (✓) one box.

3.94 g of gold reacts with chlorine to produce 6.07 g of gold chloride. The word equation for the reaction is: gold + chlorine → gold chloride Calculate the mass of chlorine that reacts with 3.94 g of gold.

Calculate the relative formula mass (M_r) of gold chloride (AuCl₃). Relative atomic masses (A_r): Cl = 35.5 Au = 197

This question is about oxygen and compounds of oxygen.

What is the state symbol of oxygen at room temperature?

Figure 4 shows the percentage by mass of the elements calcium, carbon and oxygen in calcium carbonate.

What is the percentage by mass of calcium in calcium carbonate?

At high temperature, sodium nitrate decomposes into sodium nitrite and oxygen. A student heats three samples of sodium nitrate. The mass of each sample was 4.50 g The mass of solid after heating was recorded. Table 2 shows the mass of solid after heating in each experiment.

Calculate the mean mass of solid after heating. Give your answer to 3 significant figures.

Table 3 shows the electronic structure of hydrogen and oxygen.

Figure 5 shows part of a dot and cross diagram of a molecule of water (H₂O). Complete the dot and cross diagram. You should show only the electrons in the outer energy levels.

Oxygen and sulfur are examples of simple molecules.

Complete the sentence. Choose the answer from the box.

Figure 6 shows the relative sizes of an oxygen molecule and a sulfur molecule.

How does the boiling point of sulfur compare with the boiling point of oxygen? Complete the sentences.

than the intermolecular forces in oxygen.

This question is about salts. Ammonium nitrate solution is produced when ammonia gas reacts with nitric acid.

Give the state symbol for ammonium nitrate solution.

What is the formula of nitric acid? Tick (✓) one box.

Ammonia gas dissolves in water to produce ammonia solution. Ammonia solution contains hydroxide ions, OH^– A student adds universal indicator to solutions of nitric acid and ammonia. What colour is observed in each solution?

Colour in nitric acid Colour in ammonia solution

The student gradually added nitric acid to ammonia solution. Which row, A, B, C or D, shows the change in pH as the nitric acid is

Calculate the percentage by mass of oxygen in ammonium nitrate (NH₄NO₃). Relative atomic masses (A_r): H = 1 N = 14 O = 16 Relative formula mass (M_r): NH₄NO₃ = 80

Describe a method to investigate how the temperature changes when different masses of ammonium nitrate are dissolved in water. You do not need to write about safety precautions.

This question is about salts. Ammonium nitrate solution is produced when ammonia gas reacts with nitric acid.

Give the state symbol for ammonium nitrate solution.

What is the formula of nitric acid? Tick (✓) one box.

Ammonia gas dissolves in water to produce ammonia solution. Ammonia solution contains hydroxide ions, OH^– A student adds universal indicator to solutions of nitric acid and ammonia. What colour is observed in each solution?

Colour in nitric acid Colour in ammonia solution

The student gradually added nitric acid to ammonia solution. Which row, A, B, C or D, shows the change in pH as the nitric acid is

Calculate the percentage by mass of oxygen in ammonium nitrate (NH₄NO₃). Relative atomic masses (A_r): H = 1 N = 14 O = 16 Relative formula mass (M_r): NH₄NO₃ = 80

Describe a method to investigate how the temperature changes when different masses of ammonium nitrate are dissolved in water. You do not need to write about safety precautions.

This question is about the elements in Group 2 of the periodic table.

Figure 9 shows the positions of four elements, A, B, C, and D, in the periodic table.

Which element is in Group 2? Tick one box.

Group 2 metal carbonates break down when heated to produce a metal oxide and a gas. metal carbonate metal oxide + gas

Name the two products when calcium carbonate (CaCO₃) is heated.

What type of reaction happens when a compound breaks down? Tick one box.

The metal carbonate takes in energy from the surroundings to break down. What type of reaction takes in energy from the surroundings? Tick one box.

Figure 10 shows the volume of gas produced when a Group 2 metal carbonate is heated.

The student collected 5.2 dm³ of gas. What mass of the Group 2 metal carbonate is heated?

Calculate the mass of the Group 2 carbonate needed to produce 24 dm³ of gas. Use your answer from question 04.5 to help you.

A student heated different masses of a Group 2 carbonate. The student measured the volume of gas produced. Figure 11 shows a graph of the student’s results. The student calculates the gradient of the line in Figure 11 The student makes two mistakes.

Identify the two mistakes the student makes. Calculate the correct gradient of the line.

A student repeated the experiment with a different Group 2 metal carbonate (XCO₃). The relative formula mass (M_r) of XCO₃ is 84 Relative atomic masses (A_r): C = 12 O = 16 Calculate the relative atomic mass (A_r) of X. Name metal X. Use the periodic table.

Group 2 metal carbonates thermally decompose to produce a metal oxide and a gas.

Give the formula of each product when calcium carbonate (CaCO₃) is heated.

The relative formula mass (M_r) of a Group 2 metal carbonate is 197 Relative atomic masses (A_r): C = 12 O = 16 Calculate the relative atomic mass (A_r) of the Group 2 metal in the metal carbonate. Name the Group 2 metal.

Figure 8 shows the volume of gas produced when a different Group 2 carbonate, W, is heated.

Calculate the gradient of the line in Figure 8 Give the unit.

24 dm³ of gas is produced when one mole of a Group 2 carbonate is heated. Determine the relative formula mass of the Group 2 carbonate W. Use Figure 8