Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit

Principles of Chemistry

991 practice questions

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Topics covered

Practice questions

161–170 of 423 · Normal

Question 161
2 marks · Normal
State one exception to the general rule that metals are solid at room temperature, and one exception to the rule that non-metals do not conduct electricity.
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Question 162
4 marks · Normal
(a)
State the general rule for the acid–base character of oxides of metals and of non-metals.
[2 marks]
(b)
Give a specific example of (i) a basic oxide and (ii) an acidic oxide. Write a balanced chemical equation for the reaction of the acidic oxide with sodium hydroxide.
[2 marks]
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Question 163
6 marks · Normal
This question is about electronic configurations, the periodic table, and how elements are classified as metals or non-metals.
(a)
Element J has the electronic configuration 2,8,7.
State:
(i)
The group number and period number of element J.
[2 marks]
(ii)
Whether element J is a metal or a non-metal.
[1 mark]
(b)
Element K is in Group 1 and Period 3 of the periodic table.
State:
(i)
The electronic configuration of element K.
[2 marks]
(ii)
Whether the oxide of element K is likely to be acidic or basic.
[1 mark]
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Question 164
6 marks · Normal
This question is about the relationship between electronic configuration, position in the Periodic Table, and chemical behaviour.
(a)
State why all the elements in Group 2 have similar chemical reactions.
[2 marks]
(b)
Helium and argon are both found in Group 0 (noble gases) of the Periodic Table.
(i)
State the electronic configuration of argon.
[1 mark]
(ii)
Explain why the elements in Group 0 are so unreactive.
[2 marks]
(c)
Iron (Fe) and sulfur (S) are both in Period 4. Based on their position in the Periodic Table, state which is the metal and which is the non-metal.
[1 mark]
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Question 165
6 marks · Normal
This question is about explaining group trends and the inertness of Group 0 elements using the idea of electronic configuration.
(a)
State how the electronic configuration of chlorine is related to its position in the Periodic Table.
[2 marks]
(b)
Explain why all the elements in Group 1 react similarly when placed in water.
[2 marks]
(c)
Group 0 (the noble gases) are found at the far right of the Periodic Table.
Explain why the noble gases are so unreactive.
[2 marks]
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Question 166
2 marks · Normal
Write the balanced chemical equation, including state symbols, for the reaction between sodium hydroxide solution and hydrochloric acid when they form sodium chloride solution and water.
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Question 167
4 marks · Normal
Answer the questions about the compound sodium sulfate, Na2SO4.
(a)
State the relative atomic masses (Ar) of sodium (Na), sulfur (S), and oxygen (O).
[1 mark]
(b)
Calculate the relative formula mass (Mr) of sodium sulfate, Na2SO4.
[2 marks]
(c)
State the Mr of Na2SO4 to 1 decimal place.
[1 mark]
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Question 168
3 marks · Normal
A student has 21 g of magnesium chloride (MgCl2). Calculate the number of moles of MgCl2 present.
(Ar: Mg = 24, Cl = 35.5)
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Question 169
3 marks · Normal
The equation for a reaction is:
A student reacts 27.0 g of aluminium (Al) with 85.0 g of chlorine (Cl2). Using the information in the equation, explain how you would determine which reactant is in excess and calculate the maximum mass of aluminium chloride (AlCl3) that could be formed.
(Ar: Al = 27, Cl = 35.5)
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Question 170
4 marks · Normal
A compound contains 9.45 g potassium, 5.25 g phosphorus, and 12.80 g oxygen.
(Ar: K = 39, P = 31, O = 16)
(a)
Calculate the number of moles of each element present in the sample.
[2 marks]
(b)
Determine the empirical formula of the compound.
[2 marks]
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