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23:[["$","$L32",null,{"feature":"flashcards"}],"$L33",["$","$L34",null,{"href":"/gcse/chemistry/ocr/types-of-chemical-reactions/flashcards","label":"Types of chemical reactions","subjectCode":"gcse_chemistry__ocr","surface":"flashcards"}],["$","$L35",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L36",null,{"decks":[{"id":"9e910b45-1c91-4f8c-b46d-eba46f7b9a25","title":"Types of chemical reactions Flashcards","topicId":"6e392280-0e89-5b37-ab2a-ee73e047e67c","topicSlug":"types-of-chemical-reactions","cards":[{"id":"1b09d43e-b48d-42c0-a2cf-313ee969524c","cardType":"basic","points":2,"front":"What are oxidation and reduction in terms of oxygen transfer?","back":"

Oxidation: gain of oxygen
Reduction: loss of oxygen

","mcqOptions":[{"text":"

Oxidation: gain of oxygen
Reduction: loss of oxygen

","correct":true,"explanation":"Oxidation involves a substance gaining oxygen, while reduction involves a substance losing oxygen. Both processes occur together in an oxygen-transfer redox reaction."},{"text":"

Oxidation: loss of oxygen
Reduction: gain of oxygen

","correct":false,"explanation":"This reverses both definitions. In terms of oxygen transfer, oxidation is the gain of oxygen and reduction is the loss of oxygen."},{"text":"

Oxidation: gain of oxygen
Reduction: gain of oxygen

","correct":false,"explanation":"Reduction has been confused with oxidation. Oxidation is the gain of oxygen, but reduction is specifically the loss of oxygen."},{"text":"

Oxidation: loss of oxygen
Reduction: loss of oxygen

","correct":false,"explanation":"Oxidation has been confused with reduction. Reduction is the loss of oxygen, whereas oxidation is specifically the gain of oxygen."}]},{"id":"61aa2cc3-fe0c-485a-b9ee-6f9e6da30761","cardType":"basic","points":2,"front":"How does an oxidising agent behave in a reaction?","back":"It donates oxygen to another substance and is reduced itself.","mcqOptions":[{"text":"It donates oxygen to another substance and is reduced itself.","correct":true,"explanation":"An oxidising agent supplies oxygen to another substance, causing that substance to be oxidised. By losing oxygen during the process, the agent is itself reduced."},{"text":"It accepts oxygen from another substance and is oxidised itself.","correct":false,"explanation":"Accepting oxygen describes the behaviour of the substance being oxidised, not the oxidising agent. An oxidising agent donates oxygen and is reduced itself."},{"text":"It donates oxygen to another substance and is oxidised itself.","correct":false,"explanation":"The first part is correct, but donating oxygen means the agent loses oxygen and is therefore reduced, not oxidised. It oxidises the other substance."},{"text":"It removes oxygen from another substance and is oxidised itself.","correct":false,"explanation":"Removing oxygen is the role of a reducing agent. An oxidising agent instead donates oxygen to another substance and is reduced itself."}]},{"id":"9928a797-2081-45ca-8fe3-1608b24462aa","cardType":"basic","points":2,"front":"How does a reducing agent behave in a reaction?","back":"It removes oxygen from another substance and is oxidised itself.","mcqOptions":[{"text":"It removes oxygen from another substance and is oxidised itself.","correct":true,"explanation":"A reducing agent causes reduction by taking oxygen away from another substance. Because the reducing agent gains this oxygen, it is itself oxidised."},{"text":"It donates oxygen to another substance and is reduced itself.","correct":false,"explanation":"Donating oxygen is the behaviour of an oxidising agent, not a reducing agent. A reducing agent removes oxygen from another substance and is oxidised itself."},{"text":"It removes oxygen from another substance and is reduced itself.","correct":false,"explanation":"Removing oxygen does reduce the other substance, but the reducing agent gains that oxygen and is consequently oxidised rather than reduced."},{"text":"It accepts oxygen from another substance and is oxidised itself.","correct":false,"explanation":"Accepting oxygen correctly implies oxidation, but a reducing agent specifically removes that oxygen from another substance rather than donating oxygen to it."}]},{"id":"c8d32a77-04c8-46e1-ad5d-49a976175ace","cardType":"cloze","points":null,"front":"In redox reactions, oxidation is the [ ] of electrons and reduction is the gain of electrons.","back":"In redox reactions, oxidation is the loss of electrons and reduction is the gain of electrons.","mcqOptions":[{"text":"loss","correct":true,"explanation":"Oxidation is the loss of electrons. The mnemonic OIL RIG summarises this relationship: Oxidation Is Loss, while Reduction Is Gain."},{"text":"gain","correct":false,"explanation":"Gain is the electron-transfer definition of reduction, not oxidation. Oxidation is the loss of electrons, as summarised by the mnemonic OIL RIG."},{"text":"sharing","correct":false,"explanation":"Sharing electrons describes covalent bonding rather than oxidation. In a redox reaction, oxidation is specifically the loss of electrons from a species."},{"text":"transfer","correct":false,"explanation":"Transfer is too general because electrons are transferred in both oxidation and reduction. Oxidation specifically involves the loss of electrons."}]},{"id":"4df52f30-5f91-4314-98b5-302d868c9712","cardType":"cloze","points":null,"front":"In redox reactions, oxidation is the loss of electrons and reduction is the [ ] of electrons.","back":"In redox reactions, oxidation is the loss of electrons and reduction is the gain of electrons.","mcqOptions":[{"text":"gain","correct":true,"explanation":"Reduction is the gain of electrons. The mnemonic OIL RIG summarises this relationship: Oxidation Is Loss, while Reduction Is Gain."},{"text":"loss","correct":false,"explanation":"Loss is the electron-transfer definition of oxidation, not reduction. Reduction is the gain of electrons, as summarised by the mnemonic OIL RIG."},{"text":"sharing","correct":false,"explanation":"Sharing electrons describes covalent bonding rather than reduction. In a redox reaction, reduction is specifically the gain of electrons by a species."},{"text":"transfer","correct":false,"explanation":"Transfer is too general because electrons are transferred during both oxidation and reduction. Reduction specifically involves the gain of electrons."}]},{"id":"ee4e4ec9-fbeb-4395-99e6-563c2e962f32","cardType":"basic","points":1,"front":"In terms of electron transfer, what is a reducing agent?","back":"A substance that loses/donates electrons to reduce another species.","mcqOptions":[{"text":"A substance that loses/donates electrons to reduce another species.","correct":true,"explanation":"A reducing agent donates electrons to another species, causing that species to gain electrons and be reduced. The reducing agent loses electrons and is oxidised."},{"text":"A substance that gains/accepts electrons to reduce another species.","correct":false,"explanation":"A species that accepts electrons is reduced itself rather than acting as the reducing agent. A reducing agent donates electrons to reduce another species."},{"text":"A substance that loses/donates electrons to oxidise another species.","correct":false,"explanation":"Donating electrons causes the receiving species to be reduced, not oxidised. A reducing agent loses or donates electrons to reduce another species."},{"text":"A substance that gains/accepts electrons to oxidise another species.","correct":false,"explanation":"Accepting electrons from another species describes an oxidising agent, which causes the donor to be oxidised. A reducing agent instead donates electrons."}]},{"id":"bdd099f1-5666-43c6-94ba-adcb404c06fe","cardType":"basic","points":1,"front":"What ion is released by all acids in aqueous solution?","back":"Hydrogen ions ($H^+$)","mcqOptions":[{"text":"Hydrogen ions ($H^+$)","correct":true,"explanation":"All acids in aqueous solution release hydrogen ions, $H^+$. The concentration of these ions is responsible for the solution’s acidic properties."},{"text":"Hydroxide ions ($OH^-$)","correct":false,"explanation":"Hydroxide ions are released by alkalis in aqueous solution, not acids. All acids release hydrogen ions, $H^+$, when dissolved in water."},{"text":"Chloride ions ($Cl^-$)","correct":false,"explanation":"Chloride ions are released by hydrochloric acid but not by every acid. The ion common to all aqueous acids is the hydrogen ion, $H^+$."},{"text":"Sulfate ions ($SO_4^{2-}$)","correct":false,"explanation":"Sulfate ions occur in sulfuric acid and sulfate salts but are not released by every acid. All aqueous acids release hydrogen ions, $H^+$."}]},{"id":"f94f64d7-1fa5-48af-86c1-7f665161891f","cardType":"basic","points":1,"front":"What ion is released by all alkalis in aqueous solution?","back":"Hydroxide ions ($OH^-$)","mcqOptions":[{"text":"Hydroxide ions ($OH^-$)","correct":true,"explanation":"All alkalis release hydroxide ions, $OH^-$, in aqueous solution. These ions give alkaline solutions their characteristic chemical properties and high pH."},{"text":"Hydrogen ions ($H^+$)","correct":false,"explanation":"Hydrogen ions are released by acids in aqueous solution, not alkalis. All alkalis release hydroxide ions, $OH^-$, when dissolved in water."},{"text":"Sodium ions ($Na^+$)","correct":false,"explanation":"Sodium ions are present in sodium hydroxide but not in every alkali. The ion released by all aqueous alkalis is the hydroxide ion, $OH^-$."},{"text":"Oxide ions ($O^{2-}$)","correct":false,"explanation":"Oxide ions do not remain free in aqueous solution because they react with water. Alkalis release hydroxide ions, $OH^-$, in aqueous solution."}]},{"id":"111299ee-6852-4321-881e-084f3dee97ed","cardType":"basic","points":1,"front":"What is the difference between a base and an alkali?","back":"An alkali is a soluble base.","mcqOptions":[{"text":"An alkali is a soluble base.","correct":true,"explanation":"A base neutralises acids, but only a base that dissolves in water is called an alkali. Insoluble bases can still neutralise acids without being alkalis."},{"text":"An alkali is an insoluble base.","correct":false,"explanation":"Insolubility is the opposite of the defining property of an alkali. An alkali is a base that dissolves in water, while an insoluble base is not an alkali."},{"text":"A base is a soluble alkali.","correct":false,"explanation":"This reverses the relationship between the terms. All alkalis are soluble bases, but not all bases are soluble, so a base is not defined as a soluble alkali."},{"text":"An alkali is a neutral base.","correct":false,"explanation":"Being neutral does not define an alkali. Alkalis are soluble bases that produce hydroxide ions in water, whereas neutral substances have a pH of 7."}]},{"id":"e35060c8-dc9a-466c-b4d1-8312425d29df","cardType":"cloze","points":null,"front":"The ionic equation for neutralisation is: $\\text{[...]}$","back":"The ionic equation for neutralisation is: $\\boxed{H^+(aq) + OH^-(aq) \\to H_2O(l)}$","mcqOptions":[{"text":"$$H^+(aq) + OH^-(aq) \\to H_2O(l)$","correct":true,"explanation":"Neutralisation is the reaction between hydrogen ions from an acid and hydroxide ions from an alkali, producing liquid water in the net ionic equation."},{"text":"$$H^+(aq) + OH^-(aq) \\rightleftharpoons H_2O(l)$","correct":false,"explanation":"The reversible arrow incorrectly suggests that neutralisation readily reverses. The net ionic equation uses a one-way arrow because hydrogen and hydroxide ions form water."},{"text":"$$H^+(aq) + O^{2-}(aq) \\to H_2O(l)$","correct":false,"explanation":"The reacting negative ion is hydroxide, OH⁻, not oxide, O²⁻. Hydroxide contains one oxygen and one hydrogen and combines with H⁺ to make water."},{"text":"HCl(aq) + NaOH(aq) \\to NaCl(aq) + H_2O(l)","correct":false,"explanation":"This is a complete molecular equation for one particular neutralisation, not the net ionic equation. The ionic equation removes spectator ions such as Na⁺ and Cl⁻."}]},{"id":"f2c014f3-303c-4214-83c3-53796cf6fe43","cardType":"basic","points":2,"front":"What are the products of a reaction between an acid and a metal?","back":"

Salt
Hydrogen gas

","mcqOptions":[{"text":"

Salt
Hydrogen gas

","correct":true,"explanation":"Acids react with sufficiently reactive metals to form a salt and hydrogen gas. The particular salt depends on the acid and the metal used."},{"text":"

Salt
Oxygen gas

","correct":false,"explanation":"Oxygen is not the gas produced in the usual acid-metal reaction. Metals displace hydrogen from acids, so the products are a salt and hydrogen gas."},{"text":"

Salt
Carbon dioxide gas

","correct":false,"explanation":"Carbon dioxide is produced when an acid reacts with a carbonate, not with an ordinary metal. An acid reacting with a metal releases hydrogen gas instead."},{"text":"

Water
Hydrogen gas

","correct":false,"explanation":"Water is formed during acid reactions with bases or carbonates, but not normally in the acid-metal pattern. That reaction produces a salt and hydrogen gas."}]},{"id":"b36eaf8b-838a-4283-8b7d-0fda2067a4d3","cardType":"basic","points":3,"front":"What are the three products of a reaction between an acid and a metal carbonate?","back":"

Salt
Water
Carbon dioxide

","mcqOptions":[{"text":"

Salt
Water
Carbon dioxide

","correct":true,"explanation":"An acid reacting with a metal carbonate follows the pattern acid + carbonate → salt + water + carbon dioxide. All three products must be included."},{"text":"

Salt
Hydrogen gas
Carbon dioxide

","correct":false,"explanation":"Hydrogen is associated with acid-metal reactions. Carbonates instead produce water and carbon dioxide alongside the salt, so hydrogen should not be included."},{"text":"

Salt
Water
Oxygen

","correct":false,"explanation":"Oxygen is not released when an acid reacts with a metal carbonate. The carbonate produces carbon dioxide, giving the products salt, water and carbon dioxide."},{"text":"

Salt
Carbon dioxide
Hydrogen gas

","correct":false,"explanation":"This omits water and adds hydrogen, confusing carbonate reactions with acid-metal reactions. A metal carbonate always gives salt, water and carbon dioxide with an acid."}]},{"id":"5cbb5ad8-604d-4c26-a712-8246bbc77e5e","cardType":"cloze","points":null,"front":"A strong acid [ ] in water, whereas a weak acid only partially ionises.","back":"A strong acid fully ionises in water, whereas a weak acid only partially ionises.","mcqOptions":[{"text":"fully ionises","correct":true,"explanation":"A strong acid ionises completely in water, so virtually every acid molecule forms ions. This contrasts with a weak acid, which only partially ionises."},{"text":"partially ionises","correct":false,"explanation":"Partial ionisation describes a weak acid, not a strong acid. A strong acid ionises completely in water, producing a higher proportion of ions at the same concentration."},{"text":"does not ionise","correct":false,"explanation":"An acid must ionise to produce hydrogen ions in aqueous solution. Strong acids ionise completely, whereas weak acids ionise only partially."},{"text":"reacts slowly","correct":false,"explanation":"Acid strength refers to the extent of ionisation, not the speed of reaction. A strong acid fully ionises in water, regardless of how quickly another reaction occurs."}]},{"id":"04e14718-f4f0-463b-85e4-a6533a64a5ec","cardType":"cloze","points":null,"front":"A strong acid fully ionises in water, whereas a weak acid only [ ].","back":"A strong acid fully ionises in water, whereas a weak acid only partially ionises.","mcqOptions":[{"text":"partially ionises","correct":true,"explanation":"A weak acid ionises only to a limited extent in water, leaving many molecules unchanged. Therefore, it partially ionises rather than fully ionising."},{"text":"fully ionises","correct":false,"explanation":"Complete ionisation is the defining behaviour of a strong acid. A weak acid establishes an equilibrium in which only some acid molecules form ions."},{"text":"does not ionise","correct":false,"explanation":"Weak acids still ionise and produce hydrogen ions, although only partly. Saying they do not ionise would incorrectly describe a non-acidic substance."},{"text":"dilutes completely","correct":false,"explanation":"Dilution changes concentration, not the definition of acid strength. A weak acid partially ionises in water; it does not become completely diluted as part of ionisation."}]},{"id":"c6637f70-4915-4c6a-b8b5-9d58f2d81ad7","cardType":"basic","points":1,"front":"In a chemical equation, what symbol indicates that an acid is weak?","back":"A reversible arrow ($\\rightleftharpoons$)","mcqOptions":[{"text":"A reversible arrow ($\\rightleftharpoons$)","correct":true,"explanation":"The reversible arrow shows that ionisation occurs in both directions and reaches an equilibrium. This is characteristic of a weak acid, which only partially ionises."},{"text":"A one-way arrow ($\\to$)","correct":false,"explanation":"A one-way arrow represents essentially complete reaction in this context, as used for strong acid ionisation. Weak acids are shown with a reversible arrow."},{"text":"A left-pointing arrow ($\\leftarrow$)","correct":false,"explanation":"A left-pointing arrow alone does not show the forward and reverse processes of weak acid ionisation. The correct symbol is a reversible arrow with points in both directions."},{"text":"A double equals sign ($=$)","correct":false,"explanation":"An equals sign is not the reaction symbol for partial ionisation. Weak acid equations use a reversible arrow to indicate an equilibrium between molecules and ions."}]},{"id":"a818a3aa-2ece-4bff-b0aa-47c7644006ed","cardType":"basic","points":2,"front":"What is the difference between acid strength and concentration?","back":"

Strength: the degree of ionisation in water
Concentration: the amount of acid dissolved in a specific volume

","mcqOptions":[{"text":"

Strength: the degree of ionisation in water
Concentration: the amount of acid dissolved in a specific volume

","correct":true,"explanation":"Strength describes how completely an acid ionises in water, while concentration describes how much acid is present per given volume. They are different properties."},{"text":"

Strength: the amount of acid dissolved in a specific volume
Concentration: the degree of ionisation in water

","correct":false,"explanation":"These definitions have been swapped. Concentration is the amount dissolved per volume, whereas strength is determined by the degree of ionisation in water."},{"text":"

Strength: the speed of reaction with a metal
Concentration: the amount of acid dissolved in a specific volume

","correct":false,"explanation":"Concentration is correctly described, but strength is not the speed of reaction with a metal. Strength means the degree to which acid particles ionise in water."},{"text":"

Strength: the degree of ionisation in water
Concentration: the number of ions produced by each acid molecule

","correct":false,"explanation":"The first definition is correct, but the second describes ionisation rather than concentration. Concentration is the amount of acid dissolved in a specific volume."}]},{"id":"941d8f82-31b5-4478-aeaa-cbb4786756e8","cardType":"basic","points":2,"front":"Why is a pH meter better than Universal Indicator for measuring pH?","back":"It is more precise (digital value) and objective (no human error in colour matching).","mcqOptions":[{"text":"It is more precise (digital value) and objective (no human error in colour matching).","correct":true,"explanation":"A pH meter gives a numerical reading with greater precision, while Universal Indicator depends on visually matching a colour to a chart, introducing subjective human judgement."},{"text":"It is less precise (digital value) and more subjective (human error in colour matching).","correct":false,"explanation":"Universal Indicator relies on judging colours, so it is less objective than a pH meter. The correct comparison is that a pH meter is more precise and objective."},{"text":"It is more precise (colour value) and more subjective (human error in digital matching).","correct":false,"explanation":"A pH meter does not use colour matching, so it reduces subjective judgement rather than increasing it. It is more precise and objective than Universal Indicator."},{"text":"It is less precise (approximate value) and more objective (no human error in colour matching).","correct":false,"explanation":"Universal Indicator gives an approximate colour-based pH, whereas a pH meter gives a precise digital value. Therefore, the meter is more precise and objective, not less."}]},{"id":"0976c75e-01d6-45e7-9533-e8db734c6d09","cardType":"cloze","points":null,"front":"If the concentration of $H^+$ ions increases by a factor of 10, the pH value [ ] by 1 unit.","back":"If the concentration of $H^+$ ions increases by a factor of 10, the pH value decreases by 1 unit.","mcqOptions":[{"text":"decreases","correct":true,"explanation":"pH is related to hydrogen-ion concentration by a logarithmic scale. Increasing the concentration by a factor of 10 makes the pH decrease by exactly 1 unit."},{"text":"increases","correct":false,"explanation":"A tenfold increase in hydrogen-ion concentration makes the solution more acidic, so pH decreases rather than increases. The change is exactly 1 unit because the scale is logarithmic."},{"text":"stays constant","correct":false,"explanation":"The logarithmic pH scale means a tenfold concentration change causes a one-unit change, not no change. Increasing $H^+$ concentration lowers the pH."},{"text":"decreases by 2","correct":false,"explanation":"A factor of 10 changes the pH by one unit, not two. Because greater hydrogen-ion concentration means greater acidity, the pH decreases by 1."}]},{"id":"ef4cdec8-c01f-4055-8831-cf8c2deb2ff9","cardType":"cloze","points":null,"front":"If the concentration of $H^+$ ions increases by a factor of 10, the pH value decreases by [ ] unit.","back":"If the concentration of $H^+$ ions increases by a factor of 10, the pH value decreases by 1 unit.","mcqOptions":[{"text":"1","correct":true,"explanation":"The pH scale is logarithmic: a tenfold increase in $H^+$ concentration corresponds to a decrease of exactly 1 pH unit."},{"text":"2","correct":false,"explanation":"A tenfold change in hydrogen-ion concentration changes pH by one unit, not two. The logarithmic relationship gives a decrease of 1 unit."},{"text":"10","correct":false,"explanation":"The concentration factor is 10, but pH changes by the logarithm of 10, which is 1. It therefore decreases by 1 unit."},{"text":"0","correct":false,"explanation":"The pH does change when hydrogen-ion concentration increases tenfold. The change is one unit, so zero would incorrectly treat the pH as unchanged."}]},{"id":"6369204a-2e47-4d96-87a1-6ae72693268a","cardType":"basic","points":2,"front":"An acid has a pH of 4. If the $H^+$ concentration is decreased by a factor of 100, what is the new pH?","back":"pH 6 (a $10^2$ decrease in concentration adds 2 to the pH).","mcqOptions":[{"text":"pH 6 (a $10^2$ decrease in concentration adds 2 to the pH).","correct":true,"explanation":"pH decreases by 1 for each tenfold increase in hydrogen-ion concentration, so a hundredfold decrease, $10^2$, increases the pH by 2: pH 4 becomes pH 6."},{"text":"pH 2 (a $10^2$ decrease in concentration subtracts 2 from the pH).","correct":false,"explanation":"Decreasing hydrogen-ion concentration makes the solution less acidic and raises pH. A factor of 100 adds 2 units, so pH 4 becomes pH 6, not pH 2."},{"text":"pH 5 (a $10^2$ decrease in concentration adds 1 to the pH).","correct":false,"explanation":"A hundredfold concentration change corresponds to 2 pH units, not 1. Since the concentration decreases, those 2 units must be added to pH 4, giving pH 6."},{"text":"pH 7 (a $10^2$ decrease in concentration adds 3 to the pH).","correct":false,"explanation":"A factor of 100 is $10^2$, so it changes pH by 2 units rather than 3. The decrease in $H^+$ concentration raises pH from 4 to 6."}]},{"id":"e0017ef2-b944-4078-8378-81165c8e198c","cardType":"basic","points":2,"front":"Write the half-equation for the oxidation of magnesium ($Mg$) to magnesium ions ($Mg^{2+}$).","back":"$$Mg \\to Mg^{2+} + 2e^-$","mcqOptions":[{"text":"$$Mg \\to Mg^{2+} + 2e^-$","correct":true,"explanation":"Oxidation is loss of electrons. A neutral magnesium atom loses two electrons to form a magnesium ion with a 2+ charge, giving this balanced half-equation."},{"text":"$$Mg + 2e^- \\to Mg^{2+}$","correct":false,"explanation":"This equation shows magnesium gaining electrons, which would produce a negatively charged ion. Oxidation requires magnesium to lose two electrons: $Mg \\to Mg^{2+} + 2e^-$."},{"text":"$$Mg \\to Mg^{2+} + e^-$","correct":false,"explanation":"Magnesium forms $Mg^{2+}$ by losing two electrons, not one. Losing only one electron would give $Mg^+$ and would not balance the stated ion charge."},{"text":"$$Mg \\to Mg^{2+} + 4e^-$","correct":false,"explanation":"The charge and atom balance require two electrons on the product side. Producing four electrons would represent a 4+ ion, not magnesium ions with a 2+ charge."}]},{"id":"d3cb7027-564f-4adf-be21-d7687cda14a0","cardType":"basic","points":2,"front":"Write the half-equation for the reduction of copper(II) ions ($Cu^{2+}$) to copper atoms ($Cu$).","back":"$$Cu^{2+} + 2e^- \\to Cu$","mcqOptions":[{"text":"$$Cu^{2+} + 2e^- \\to Cu$","correct":true,"explanation":"Reduction is gain of electrons. A copper(II) ion gains two electrons to balance its 2+ charge and becomes a neutral copper atom."},{"text":"$$Cu^{2+} \\to Cu + 2e^-$","correct":false,"explanation":"Putting electrons on the product side represents oxidation, not reduction. Copper(II) must gain two electrons on the reactant side to form neutral copper."},{"text":"$$Cu^{2+} + e^- \\to Cu$","correct":false,"explanation":"One electron would reduce the 2+ ion only to $Cu^+$, not to a neutral copper atom. Two electrons are needed to cancel the full 2+ charge."},{"text":"$$Cu^{2+} + 4e^- \\to Cu$","correct":false,"explanation":"Adding four electrons gives an excess negative charge and does not balance the conversion of $Cu^{2+}$ into neutral copper. Exactly two electrons are required."}]},{"id":"c4464866-a106-47ff-b222-8910b8d903c3","cardType":"basic","points":3,"front":"How do you obtain pure, dry crystals of a soluble salt from an acid and an insoluble base?","back":"

React acid with excess base
Filter off the unreacted solid
Evaporate the water from the filtrate

","mcqOptions":[{"text":"

React acid with excess base
Filter off the unreacted solid
Evaporate the water from the filtrate

","correct":true,"explanation":"Using excess insoluble base ensures all acid reacts. Filtering removes the unreacted solid, and evaporating water from the filtrate leaves soluble salt crystals that can be dried."},{"text":"

React base with excess acid
Filter off the unreacted liquid
Evaporate the water from the solid

","correct":false,"explanation":"Using excess acid leaves acid in the solution, and filtering cannot remove dissolved acid. The correct method uses excess insoluble base, filters the solid, then evaporates the filtrate."},{"text":"

React acid with exactly enough base
Distil off the unreacted solid
Evaporate the water from the filtrate

","correct":false,"explanation":"An insoluble base must be filtered from the solution, not distilled away, and the water is evaporated from the filtrate. Excess base ensures no acid remains."},{"text":"

React acid with excess base
Evaporate the water from the mixture
Filter the crystals from the filtrate

","correct":false,"explanation":"The unreacted insoluble base must be removed before crystallisation; otherwise it contaminates the salt. The water is then evaporated from the filtered solution, not the original mixture."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"Types of chemical reactions","title":"Types of chemical reactions Flashcards","topbar":{"backHref":"/gcse/chemistry/ocr/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"6e392280-0e89-5b37-ab2a-ee73e047e67c","walled":"$L38"}],"$L39","$L3a"]