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WorksheetsChemistry Notes 8B Edexcel_2
Total questions: 106
Worksheet time: 2hrs 42mins
Group 1 and 2 oxides react with acids in (a) reactions to form salts and water.
The solubility of Group 2 sulfates (a) down the group.
The ionic equation for the reaction of sulfate ions with barium ions is: Ba²⁺ (aq) + SO₄²⁻ (aq) → BaSO₄(s).
(a)
Limewater neutralizes excess (a) in the soil to improve crop yield.
All Group 2 sulfates are soluble in water.
True
False
Barium sulfate is used to detect sulfate ions because it forms a white precipitate.
True
False
Barium meals are poisonous because they contain barium ions.
True
False
Limewater reacts with carbon dioxide to form calcium carbonate.
True
False
What is the white precipitate formed when barium ions react with sulfate ions?
(a)
What acid is commonly added in the test for sulfate ions to prevent carbonate interference?
(a)
What is the general term for oxides that react with water to form metal hydroxides?
(a)
Which Group 2 sulfate is only slightly soluble in water?
Why is nitric acid added to the solution before testing for sulfate ions with barium chloride?
Why should limewater not be left exposed to air before using it for a test?
Explain why the solubility of Group 2 sulfates decreases down the group. Answer: The lattice energy of (a) decreases more slowly than the (b) energy of the larger (c) , making the sulfates less soluble as you move down the group.
Write balanced equations for the following reactions: a) Reaction of calcium oxide with nitric acid:
Write balanced equations for the following reactions:
b) Reaction of barium hydroxide with hydrochloric acid:
Write balanced equations for the following reactions:
c) Test for sulfate ions with barium chloride:
Ba(aq) + SO(aq) → BaSO(s).
Explain the role of barium sulfate in medical imaging.
What does thermal stability indicate about a compound?
Its ability to react with acids
Its stability when heated
Its solubility in water
Why do Group 2 nitrates decompose when heated, while Group 1 chlorides do not?
Group 2 cations are larger than Group 1 cations.
Group 2 cations have a smaller charge than Group 1 cations.
Group 2 cations have a higher charge and smaller ionic radius.
Group 2 nitrates have weaker bonds than Group 1 chlorides.
Which gas is released when nitrates decompose?
Carbon dioxide
Nitrogen dioxide
Hydrogen
Chlorine
Which cation exerts the greatest influence on an anion?
Caesium (Cs⁺)
Rubidium (Rb⁺)
Beryllium (Be²⁺)
Sodium (Na⁺)
The charge on a Group 2 cation is (a) that of a Group 1 cation.
The (a) ion is more complex than the chloride ion, influencing its thermal decomposition.
When nitrates decompose, they release oxygen gas and/or (a) .
Group 1 and Group 2 nitrates are typically (a) solids.
The thermal stability of nitrates decreases as the charge and size of the cation increase.
True
False
Nitrogen dioxide is observed as brown fumes during the decomposition of nitrates.
True
False
Group 2 carbonates decompose into oxides and carbon dioxide gas.
True
False
Caesium has the least influence on an anion due to its large size and low charge.
True
False
What gas is released along with oxygen during the decomposition of nitrates?
(a)
Which cation exerts the greatest influence on nitrate ions?
(a)
What ion is formed during the decomposition of carbonates?
(a)
Which group of compounds is more stable thermally, Group 1 or Group 2 nitrates?
(a)
Explain why Group 2 carbonates decompose more readily than Group 1 carbonates.
What is observed when nitrates containing water of crystallization are heated?
Why does beryllium exert the greatest influence on an anion compared to caesium?
Write balanced equations for the decomposition of: a) Sodium nitrate
Write balanced equations for the decomposition of: Calcium nitrate:
Describe the role of cation size and charge in determining the thermal stability of nitrates and carbonates.
What does the absence of brown fumes during nitrate decomposition indicate?
Complete decomposition
Greater decomposition
Lesser decomposition
No decomposition
Which Group 1 nitrate undergoes greater decomposition?
Sodium nitrate
Potassium nitrate
Lithium nitrate
Cesium nitrate
What are the decomposition products of lithium nitrate?
Metal oxide, nitrogen dioxide, and oxygen
Metal nitrite and oxygen
Metal hydroxide and water
Which property makes Group 2 nitrates decompose more readily than Group 1 nitrates?
Larger cation size
Higher cation charge
Presence of water of crystallization
Lower electronegativity of the cations
The decomposition of nitrates without brown fumes can be represented by the equation: Metal nitrate → metal (a) + oxygen
Greater decomposition of nitrates releases nitrogen dioxide gas, represented by the equation: Metal nitrate → metal (a) + nitrogen dioxide + oxygen
The only Group 1 nitrate that undergoes greater decomposition is (a) .
The decomposition of beryllium nitrate releases oxygen and (a) fumes.
The decomposition of Group 2 nitrates produces nitrogen dioxide gas.
True
False
Sodium nitrate undergoes greater decomposition than lithium nitrate.
True
False
Brown fumes observed during nitrate decomposition indicate lesser decomposition.
True
False
All Group 1 nitrates decompose to metal nitrites and oxygen.
True
False
What gas relights a glowing splint during nitrate decomposition?
(a)
What color fumes indicate nitrogen dioxide is released during decomposition?
(a)
Which Group 2 nitrate undergoes greater decomposition?
(a)
What is the smallest Group 1 cation that undergoes greater decomposition?
(a)
Why does lithium nitrate undergo greater decomposition compared to other Group 1 nitrates?
Explain why Group 2 nitrates decompose more readily than Group 1 nitrates.
How can you differentiate between nitrate(V) and nitrate(III) during decomposition?
Explain the redox nature of nitrate decomposition reactions.
Predict what would happen if a Group 1 nitrate like potassium nitrate is heated in the absence of oxygen.
What gas is released during the decomposition of carbonates?
Oxygen
Carbon dioxide
Which gas is released when Group 2 carbonates decompose?
Nitrogen dioxide
Sulfur dioxide
Carbon dioxide
Which Group 1 carbonate decomposes at relatively low temperatures?
Sodium carbonate
Potassium carbonate
Lithium carbonate
Cesium carbonate
What is the general observation when Group 2 carbonates decompose?
Brown fumes
Release of oxygen gas
Formation of solid oxides and release of carbon dioxide
Formation of water and oxygen gas
Why does lithium carbonate decompose differently from other Group 1 carbonates?
It has a larger ionic radius.
It has a smaller ionic radius and greater charge density.
It contains water of crystallization.
It does not react with heat.
The decomposition of carbonates releases (a) gas.
The decomposition of lithium carbonate occurs at (a) temperatures compared to other Group 1 carbonates.
A typical equation for the decomposition of calcium carbonate is: CaCO₃ → CaO + CO₂
(a)
The (a) charge and smaller ionic radius of Group 2 cations make their carbonates decompose more readily.
All Group 1 carbonates decompose when heated under normal conditions.
True
False
Group 2 carbonates decompose into metal oxides and carbon dioxide.
True
False
Lithium carbonate behaves similarly to Group 2 carbonates when heated.
True
False
Barium carbonate decomposes less readily than calcium carbonate.
True
False
Which Group 1 carbonate decomposes readily at lower temperatures?
(a)
What solid is formed when calcium carbonate decomposes?
(a)
What gas is released during the decomposition of Group 2 carbonates?
(a)
What is the term for the extent to which a compound decomposes when heated?
(a)
Why does lithium carbonate decompose more readily than other Group 1 carbonates?
Explain why Group 2 carbonates decompose more readily than Group 1 carbonates.
Describe the changes observed when calcium carbonate is strongly heated in a Bunsen flame.
Write balanced equations for the decomposition of: - a) Lithium carbonate
Write balanced equations for the decomposition of: b) Calcium carbonate:
Why is it incorrect to assume that all Group 1 carbonates decompose easily when heated?
Explain the role of cation charge and radius in determining the thermal stability of carbonates.
What is the main purpose of a flame test?
To identify anions
To identify cations
To measure thermal stability
To detect impurities
Why is hydrochloric acid used in flame tests?
To neutralize the compound
To convert metal compounds to chlorides
To provide a colored flame
To dissolve the compound fully
What color does sodium produce in a flame test?
Lilac
Brick red
Yellow/orange
Blue/green
Which metal cation produces no color in a flame test?
Calcium
Magnesium
Strontium
Potassium
A flame test is used to identify the presence of (a) in a compound.
Sodium produces a (a) /orange flame during the test.
The (a) of some metals, like magnesium, do not produce any flame color.
Electron (a) are responsible for the colors observed in flame tests.
Flame tests are reliable for detecting all metal cations in Group 1 and 2.
True
False
Sodium contamination can obscure the flame colors of other metals.
True
False
Chlorides are preferred in flame tests because they are less volatile.
True
False
Describing flame test colors is subjective and may vary among observers.
True
False
What is the flame color for lithium?
(a)
What metal cation produces a lilac color in the flame test?
(a)
What is the flame color for barium?
(a)
What is responsible for the flame colors in the test?
(a)
Why is it important to use clean platinum or nichrome wire in a flame test?
Explain why the flame test may not always give accurate results for mixtures.
Impurities such as sodium can produce an intense yellow flame, which can mask the colors of other cations.
Why are flame test colors considered subjective?
Observers may interpret colors differently based on their perception, and terms like "brick red" or "lilac" can vary regionally or personally.
Describe the steps involved in carrying out a flame test for a compound.
