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 aluminium ion, Al³⁺? (b) Magnesium burns in excess oxygen to form magnesium oxide. The balanced equation for this reaction is 2Mg + O₂ → 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 aluminium ion, Al³⁺? (b) M... 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

(a) Which row shows the numbers of subatomic particles present in an aluminium ion, Al³⁺?

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Answer

An aluminum atom has 13 protons and 14 neutrons, as it has an atomic number of 13 and a mass number of 27. In the ion Al³⁺, it loses 3 electrons, resulting in 10 electrons. Thus, the correct configuration of subatomic particles in Al³⁺ is:

Protons: 13
Neutrons: 14
Electrons: 10.

Therefore, the answer is option B.

Step 2

(b) 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

To calculate the maximum mass of magnesium oxide (MgO) formed, we first need to find out how many moles of magnesium we have:

The molar mass of Mg is 24.0 g/mol.
The moles of magnesium can be calculated as follows:

$ext{Moles of Mg} = \frac{\text{mass}}{\text{molar mass}} = \frac{1.35 g}{24.0 g/mol} = 0.05625 mol$
From the balanced equation, 2 moles of Mg produce 2 moles of MgO. Therefore, the moles of MgO formed will be equal to the moles of magnesium used:

$\text{Moles of MgO} = 0.05625 mol$
The molar mass of MgO (Mg = 24.0 g/mol, O = 16.0 g/mol) is:

$\text{Molar mass of MgO} = 24.0 + 16.0 = 40.0 g/mol$
Finally, to find the mass of MgO formed:

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

Thus, the maximum mass of magnesium oxide that could be formed is 2.25 g.

Step 3

(c) Write the balanced equation for this reaction.

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Answer

The balanced equation for the reaction between chlorine (Cl₂) and hydrogen (H₂) to form hydrogen chloride (HCl) is:

$Cl_2 + H_2 \rightarrow 2HCl$

Step 4

(d) 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 chloride (NaCl) is formed when sodium (Na) and chlorine (Cl) combine. The electronic configuration of sodium is 2.8.1, and that of chlorine is 2.8.7.

Ion Formation: Sodium has one electron in its outer shell and readily loses that electron to achieve a full outer shell (2.8). This loss results in the formation of a sodium ion (Na⁺), which has a positive charge:

$Na \rightarrow Na^+ + e^-$

Chlorine has seven electrons in its outer shell and needs one more to complete it. It gains the electron from sodium, forming a chloride ion (Cl⁻) with a negative charge:

$Cl + e^- \rightarrow Cl^-$

Ionic Bonding: The oppositely charged ions (Na⁺ and Cl⁻) attract each other, forming an ionic bond.
Arrangement in Solid State: In solid sodium chloride, these ions are arranged in a crystal lattice structure, where each sodium ion is surrounded by six chloride ions and vice versa. This regular arrangement maximizes the electrostatic attraction between the oppositely charged ions.

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

(a) Which row shows the numbers of subatomic particles present in an aluminium ion, Al³⁺?

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

(c) Write the balanced equation for this reaction.

(d) 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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