AQA GCSE Trilogy Chemistry Paper 1 Foundation November 2021 question paper 8464/C/1F

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.

This question is about electrolysis.

Complete the sentence. Choose the answer from the box.

Copper chloride can conduct electricity when in solution or

Figure 1 shows the apparatus used for the electrolysis of copper chloride solution.

There are four ions in copper chloride solution:

• Cu²⁺

• Cl^–

• H⁺

• OH^–

Why do Cl^– ions and OH^– ions move to the positive electrode?

Where do the H⁺ and OH^– ions come from in the electrolysis of copper chloride solution? Tick (✓) one box.

Which ion produces a metal? Tick (✓) one box.

Figure 2 shows the apparatus during the electrolysis of copper chloride solution.

Describe what is seen at each electrode during the electrolysis of copper chloride solution. Positive electrode

Negative electrode

500 cm³ of copper chloride solution contains 6.50 g of copper chloride. Calculate the mass of copper chloride in 40.0 cm³ of this copper chloride solution.

Carbon can exist in a number of different structures.

What is the approximate radius of a carbon atom? Tick (✓) one box.

Figure 3 shows an atom of carbon.

Describe the atomic structure of this carbon atom. You should include the number of electrons, neutrons and protons.

In graphite the carbon atoms are held together by bonds.

Figure 4 represents part of the structure of graphite.

How many bonds does each carbon atom have in graphite? Use Figure 4. Tick (✓) one box.

What type of bonds hold the carbon atoms together in graphite? Tick (✓) one box.

Lubricants allow objects to slide over each other easily. Suggest why graphite can be used as a lubricant. Use Figure 4.

The two structures represent different forms of carbon. Draw one line from each structure to the form of carbon.

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.

A student investigated the change in temperature when different masses of zinc were added to copper sulfate solution. This is the method used.

1. Measure the volume of copper sulfate solution using a measuring cylinder.

2. Pour the copper sulfate solution into a metal container.

3. Add 2 g of zinc.

4. Measure the temperature of the solution.

5. Repeat steps 1 to 4 with different masses of zinc.

Figure 7 shows the apparatus.

Give three improvements to the investigation to make the results more accurate.

Figure 8 shows part of the measuring cylinder.

What is the volume of copper sulfate solution in Figure 8 ?

When zinc was added to copper sulfate solution the temperature increased. Figure 9 shows the reaction profile.

What type of reaction is shown in Figure 9 ? Tick (✓) one box.

Figure 10 shows the results.

Determine the gradient of the line in Figure 10. Use the equation:

Suggest why the student should not use more than 10 g of zinc. Use Figure 10. You should extend the graph line.

This question is about the periodic table.

Figure 11 shows part of Mendeleev’s version of the periodic table.

Which group of elements had not been discovered when Mendeleev’s version of the periodic table was published?

Figure 12 represents different models of the atom.

Which model represents the plum pudding model? Tick (✓) one box.

Which model resulted from Chadwick’s experimental work? Tick (✓) one box.

Potassium has different isotopes.

What is meant by ‘isotopes’? You should refer to subatomic particles.

Table 2 shows the mass numbers and the percentage abundance of two isotopes of potassium.

Calculate the relative atomic mass (A_r) of potassium. Give your answer to 1 decimal place.

Acids react to produce salts. Universal indicator is added to water and then nitric acid is added to the mixture.

Give the colour change when nitric acid is added to the mixture of universal indicator and water. Tick (✓) one box.

What happens to the pH of water when nitric acid is added? Tick (✓) one box.

What is the state symbol for nitric acid?

Zinc carbonate reacts with nitric acid.

The word equation for the reaction is: zinc carbonate + nitric acid → zinc nitrate + water + carbon dioxide white solid colourless solution

Give two observations that would be made when zinc carbonate is added to nitric acid until the zinc carbonate is in excess.

The formula of the zinc ion is Zn²⁺ The formula of the nitrate ion is NO₃^– What is the formula for zinc nitrate? Tick (✓) one box.

Acids react with insoluble metal oxides to produce salts. Plan a method to produce a pure, dry sample of the soluble salt copper chloride from an acid and a metal oxide.