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Questions and Answers
What type of compound is produced when metals react with hydrochloric acid?
What type of compound is produced when metals react with hydrochloric acid?
Which of the following metals reacts with water to form a metal hydroxide and hydrogen gas?
Which of the following metals reacts with water to form a metal hydroxide and hydrogen gas?
Which one of the following is an example of an amphoteric oxide?
Which one of the following is an example of an amphoteric oxide?
What is produced when copper (II) oxide reacts with hydrochloric acid?
What is produced when copper (II) oxide reacts with hydrochloric acid?
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Which reaction demonstrates a non-metal reacting with an acid?
Which reaction demonstrates a non-metal reacting with an acid?
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What is the outcome when magnesium reacts with steam?
What is the outcome when magnesium reacts with steam?
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Which of the following reactions involves a base forming a salt and water?
Which of the following reactions involves a base forming a salt and water?
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What type of oxide do sodium and potassium oxide form when dissolved in water?
What type of oxide do sodium and potassium oxide form when dissolved in water?
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Which type of reaction involves a compound being broken down into simpler substances?
Which type of reaction involves a compound being broken down into simpler substances?
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What occurs during a displacement reaction?
What occurs during a displacement reaction?
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Which reaction is characterized by the release of heat during product formation?
Which reaction is characterized by the release of heat during product formation?
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Which of the following reactions is an example of thermal decomposition?
Which of the following reactions is an example of thermal decomposition?
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What is a characteristic of endothermic reactions?
What is a characteristic of endothermic reactions?
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Which reaction is classified as a double displacement reaction?
Which reaction is classified as a double displacement reaction?
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Which of the following describes a combination reaction?
Which of the following describes a combination reaction?
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Which of the following scenarios illustrates the preparation of a salt?
Which of the following scenarios illustrates the preparation of a salt?
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What is produced when an acid reacts with a metal carbonate?
What is produced when an acid reacts with a metal carbonate?
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What happens when an acid is dissolved in water?
What happens when an acid is dissolved in water?
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Which of the following correctly describes the reaction of sodium hydroxide with hydrochloric acid?
Which of the following correctly describes the reaction of sodium hydroxide with hydrochloric acid?
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How can hydrogen gas be tested for its presence?
How can hydrogen gas be tested for its presence?
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What is expected when a metal oxide reacts with an acid?
What is expected when a metal oxide reacts with an acid?
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What is the result of passing excess carbon dioxide through lime water?
What is the result of passing excess carbon dioxide through lime water?
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Which of the following correctly depicts the reaction of acids with metals?
Which of the following correctly depicts the reaction of acids with metals?
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What happens to the bromothymol blue indicator when exposed to carbon dioxide?
What happens to the bromothymol blue indicator when exposed to carbon dioxide?
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Study Notes
Chemical Reactions and Equations
- Word Equations: Show reactants (starting materials) and products (resulting materials)
- Balanced Equations: Represent chemical reactions accurately; the number of atoms of each element is equal on both sides
- Reaction Conditions: Indicate temperature, pressure, catalyst needed, use symbols (e.g., 340 atm, sunlight, Heat)
-
Combination Reaction: Two or more reactants combine to form one product
- Examples:
- Burning of coal: C(s) + O₂(g) → CO₂(g)
- Formation of water: 2H₂(g) + O₂(g) → 2H₂O(l)
- Formation of calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH)₂(aq) + Heat
- Examples:
Exothermic Reactions
- Release heat with product formation
- Examples:
- Burning of natural gas: CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) + Heat
- Respiration: C₆H₁₂O₆(aq) + 6O₂(g) → 6CO₂(aq) + 6H₂O(l) + energy
Decomposition Reactions
- A compound splits into two or more simpler substances
-
Thermal decomposition:
- Uses heat as energy for reaction
- Examples:
- 2FeSO₄(s) → Fe₂O₃(s) + SO₂(g) + SO₃(g)
- CaCO₃(s) → CaO(s) + CO₂(g)
- 2Pb(NO₃)₂(s) → 2PbO(s) + 4NO₂(g) + O₂(g)
-
Electrolytic decomposition:
- Uses electricity as energy source
- Example: 2H₂O(l) → 2H₂(g) + O₂(g)
-
Photolytic decomposition:
- Requires sunlight as the energy source
- Examples:
- 2AgCl(s) → 2Ag(s) + Cl₂(g)
- 2AgBr(s) → 2Ag(s) + Br₂(g)
-
Thermal decomposition:
Endothermic Reactions
- Require energy (heat, light, electricity) to break reactants
Displacement Reactions
- More reactive elements replace less reactive elements in a compound
- Examples:
- Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)
- Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)
- Pb(s) + CuCl₂(aq) → PbCl₂(aq) + Cu(s)
Double Displacement Reactions
- New compounds form by exchanging ions between two compounds
- Forms a precipitate or an insoluble substance
- Example: Na₂SO₄(aq) + BaCl₂(aq) → BaSO₄(s) + 2NaCl(aq)
Oxidation
- Gaining oxygen during a reaction
- Example: 2Cu + O₂ → 2CuO
Reduction
- Gaining electrons or a decrease in oxidation state
Redox Reactions
- Combination of oxidation and reduction; one reactant gets oxidized while the other gets reduced
Acids, Bases and Salts
- Reaction of Metals with Acids: Acid + Metal → Salt + Hydrogen gas
- Reaction of Metal Carbonates/Metal Hydrogen Carbonates with Acids: Acid + Metal Carbonate/Metal Hydrogen Carbonate → Salt + CO₂ + H₂O
- Reaction of Acids and Bases With Each Other: Acid + Base → Salt + Water
Preparation of Sodium Hydroxide
- 2NaCl(aq) + 2H₂O(l) -> 2NaOH(aq) + Cl₂(g) + H₂(g)
Other Preparations
- Bleaching powder: Ca(OH)₂(aq) + Cl₂(g) → CaOCl₂(aq) + H₂O(I)
- Baking soda: NaCl + H₂O + CO₂ + NH₃ → NH₄Cl
- Washing soda: Na₂CO₃ + 10H₂O → Na₂CO₃.10H₂O
- Plaster of Paris: CaSO₄.2H₂O → CaSO₄.1/2H₂O + 3/2H₂O
Metals and Non-metals
- Reaction of Metals with Air: Metal + O₂ → Metal Oxide (e.g., 2Cu + O₂ → 2CuO)
-
Reaction of Metals with Water: Metal + Water → Metal Hydroxide + Hydrogen
- Some metals react violently with cold water, others are slower and need steam
- Amphoteric Oxides: React with both acids and bases (e.g., Al₂O₃)
- Electrolytic Reduction : Used to extract metals from their ores
- Extraction by Roasting: Heat metal ore with oxygen to produce metal oxide
- Extraction by Calcination: Heat metal carbonate to form metal oxide
Reaction of Metals with Acids:
- Metal + Acid → Salt + Hydrogen
Extracting Metals Low in the Activity Series:
- Heating ores (e.g., cinnabar = HgS) with oxygen to produce mercury(Hg)
Extracting Metals in the Middle of the Activity Series
- Roasting: heating ZnS + 02 → ZnO + SO₂
- Calcination: heating ZnCO3 → ZnO + CO₂
Extracting Metals Towards the Top of the Activity Series
- Electrolytic Reduction (e.g., Na, Mg, Ca are obtained this way)
- Uses electricity to reduce metal ions to their elemental state
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Description
This quiz covers the fundamentals of chemical reactions and equations, including word equations, balanced equations, and various types of reactions such as combination, exothermic, and decomposition reactions. Test your knowledge on the conditions and representations involved in chemical processes.
