9 (a) An aluminum atom has the atomic number 13 and the mass number 27. Which row shows the numbers of subatomic particles present in an aluminum ion, Al$^{3+}$? (b) Magnesium burns in excess oxygen to form magnesium oxide. The balanced equation for this reaction is $$2Mg + O_2 \rightarrow 2MgO$$ Starting with 1.35g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction. (relative atomic masses: Mg = 24.0; O = 16.0) You must show your working. (c) Chlorine reacts with hydrogen to form hydrogen chloride. Write the balanced equation for this reaction. (d) Sodium chloride is an ionic compound, containing sodium ions, Na$^+$, and chloride ions, Cl$^-$. Figure 15 shows the electronic configuration of sodium and chlorine. Explain how sodium and chlorine atoms form the ions in sodium chloride and how the ions are arranged in the solid sodium chloride. You may wish to use diagrams in your answer.

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9 (a) An aluminum atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry - Question 9 - 2019 - Paper 1

Question 9

9 (a) An aluminum atom has the atomic number 13 and the mass number 27. Which row shows the numbers of subatomic particles present in an aluminum ion, Al$^{3+}$? (b... show full transcript

Worked Solution & Example Answer:9 (a) An aluminum atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry - Question 9 - 2019 - Paper 1

Step 1

Which row shows the numbers of subatomic particles present in an aluminum ion, Al$^{3+}$?

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Answer

An aluminum atom has an atomic number of 13, which indicates it has 13 protons. The mass number is 27, which is the total of protons and neutrons. Therefore, the number of neutrons is 27 - 13 = 14. In an aluminum ion, Al $^{3+}$ , there are 10 electrons (13 protons - 3 for the positive charge). Thus, the subatomic particles are:

Protons: 13
Neutrons: 14
Electrons: 10

Step 2

Starting with 1.35g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction.

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Answer

Calculate the moles of magnesium:

$\text{Molar mass of Mg} = 24.0 \, g/mol$

$\text{Moles of Mg} = \frac{1.35 \, g}{24.0 \, g/mol} = 0.05625 \, mol$

According to the balanced equation, 1 mole of Mg reacts to produce 1 mole of MgO. Therefore, the moles of MgO produced are also 0.05625 mol.
Now, calculate the mass of MgO produced:

$\text{Molar mass of MgO} = 24.0 + 16.0 = 40.0 \, g/mol$

$\text{Mass of MgO} = 0.05625 \, mol \times 40.0 \, g/mol = 2.25 \, g$

Step 3

Write the balanced equation for this reaction.

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The balanced equation for the reaction of chlorine and hydrogen to form hydrogen chloride is:

$Cl_2 + H_2 \rightarrow 2HCl$

Step 4

Explain how sodium and chlorine atoms form the ions in sodium chloride and how the ions are arranged in the solid sodium chloride.

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Answer

Sodium (Na) has an electronic configuration of 2.8.1, meaning it has one electron in its outermost shell, which it can lose to achieve a full outer shell. When sodium loses this electron, it forms a sodium ion (Na $^+$ ). Chlorine (Cl) has an electronic configuration of 2.8.7, meaning it can gain one electron to complete its outer shell. When chlorine gains an electron, it forms a chloride ion (Cl $^-$ ).

In sodium chloride (NaCl), each Na $^+$ ion is surrounded by six Cl $^-$ ions, and each Cl $^-$ ion is surrounded by six Na $^+$ ions, forming a cubic lattice structure. This arrangement maximizes the attraction between oppositely charged ions, contributing to the stability and high melting points of ionic compounds.

9 (a) An aluminum atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry - Question 9 - 2019 - Paper 1

Worked Solution & Example Answer:9 (a) An aluminum atom has the atomic number 13 and the mass number 27 - Edexcel - GCSE Chemistry - Question 9 - 2019 - Paper 1

Which row shows the numbers of subatomic particles present in an aluminum ion, Al$^{3+}$?

Starting with 1.35g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction.

Write the balanced equation for this reaction.

Explain how sodium and chlorine atoms form the ions in sodium chloride and how the ions are arranged in the solid sodium chloride.

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