Properties of ionic compounds

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?

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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?

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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 ?

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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?

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Table 8 shows diagrams which represent the structures of two substances.

Compare the structure and bonding of sodium chloride and oxygen.

This question is about structure and properties.

Which pair of substances both contain atoms in hexagonal rings? Tick (✓) one box.

Explain why the structure of copper allows the conduction of thermal energy.

Explain why copper oxide (CuO) has a high melting point.

Explain why water (H₂O) has a low melting point.

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.

This question is about elements and compounds.

Figure 8 shows a reactivity series.

Figure 8

Give the method and conditions used to extract metal Y from a compound of metal Y

Sodium reacts with titanium chloride (TiCl₄) to produce titanium.

Complete the equation. You should balance the equation.

The reaction between sodium and titanium chloride is a redox reaction. Write a half-equation to show that sodium is oxidised in this reaction.

108 g of aluminum reacts with 1.21 kg of copper chloride to produce copper. The equation for the reaction is:

Calculate the maximum mass of copper produced in grams (g). You should determine the limiting reactant. Relative atomic masses (A_r): Al = 27 Cu = 63.5 Relative formula masses (M_r): CuCl₂ = 134.5 AlCl₃ = 133.5

Limiting reactant is Mass of copper = g

Sodium metal and sodium chloride are both able to conduct electricity.

Describe how sodium metal conducts electricity.

Explain how sodium chloride can conduct electricity.

This question is about structure and bonding.

Figure 5 shows part of the structure and bonding in diamond.

Explain why diamond has a high melting point.

Figure 6 shows part of the structure and bonding in sodium chloride (NaCl).

Explain the conditions needed for sodium chloride to conduct electricity.

Figure 7 shows the structure of sodium.

Describe how sodium conducts thermal energy.