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CC10H SC10H
Pearson GCSE Combined and Separate Chemistry Higher
| Question | Answer |
|---|---|
| What is produced during the electrolysis of molten lead bromide? | Molten lead and bromine gas |
| What name is given to a positively charged ion and the negatively charged ion? | Cation(Positive) Anion (Negative) |
| What type of substance tends to form cations and anions? | Cations - metals and hydrogen Anions - non-metals |
| What name is given to the positively charged electrode and the negatively charged electrode? | Anode(Positive) Cathode(Negative) |
| Which electrical supply is used in electrolysis? | Direct Current |
| What happens to compounds during electrolysis? | They decompose(break down) |
| What are oxidation and reduction? | Oxidation is loss of electrons Reduction is gain of electrons |
| Which electrode are positively charged ions and negatively charged ions attracted to? | Positive ions - Cathode Negative ions – Anode |
| What happens at the anode and the cathode? | They form neutral particles At the anode the anion loses electrons At the cathode the cation gains electrons |
| What is an electrolyte? | An ionic compound that is either molten or dissolved in water |
| Explain electrolysis in terms of electron movement | The anion loses electrons at the anode, these travel to the power source and then go to the cathode where they are gained by the cation |
| What is the half equation for the reduction of sodium ions | Na+ + e- → Na |
| What is the half equation for the oxidation of chloride ions | 2Cl- → Cl2 + 2e- |
| What is the difference between the electrolysis of a molten compound and that of a compound in aqueous solution? | When a molten compound is electrolysed only the ions from the compound itself are involved, When an aqueous compound is electrolysed the hydrogen and hydroxide ions from the water are also involved |
| What positive and negative ions are present in copper sulphate solution? | Cu2+, SO42-, OH-, H+ |
| Which ion is discharged the most and the least readily out of OH-, SO42- and Cl-? | Most readily - Cl- Least readily - SO42- |
| Which ion is discharged the most and the least readily out of Na+, H+ and Cu2+? | Most readily - Cu2+ Least readily - Na+ |
| What inert material are electrodes made from? | Graphite |
| What is produced during the electrolysis of copper chloride solution? | Copper, chlorine and water |
| What is produced during the electrolysis of copper sulphate solution? | Copper, oxygen and sulphuric acid |
| What is produced during the electrolysis of sodium sulphate solution? | Hydrogen, oxygen and sodium sulphate |
| What is produced during the electrolysis of sodium chloride solution? | Hydrogen, chlorine and sodium hydroxide |
| What is the relationship between the amount of hydrogen and oxygen produced in the electrolysis of water? | The amount of hydrogen is always double the amount of oxygen |
| What happens at the anode when copper electrodes are used in the electrolysis of copper sulphate solution? | Copper atoms lose electrons and turn into ions which go into the solution The anode gets smaller |
| What happens at the cathode when copper electrodes are used in the electrolysis of copper sulphate solution? | Copper ions gain electrons and turn into atoms The cathode gets bigger |
| Electrolysis is used to purify copper, What is the difference in the copper used at each electrode? | The anode is made of impure copper and the cathode is made of pure copper |
| Magnesium carbonate is insoluble What do you need to do before it will conduct electricity? | Melt it Sodium fluoride is soluble |
| Explain what the easiest way for it to conduct electricity is | Dissolve it in water because this does not require high temperatures |
| Which ions are in NaCl | Na⁺ and Cl⁻ |
| Which ions are in CuCl₂ | Cu²⁺ and two Cl⁻ |
| Which ions are in Na₂SO₄ | 2 ions of Na⁺ and one SO₄²⁻ |
| Is this process oxidation or reduction? Al → Al³⁺ + 3e⁻ | Oxidation |
| Is this process oxidation or reduction? Na⁺ + e⁻ → Na | Reduction |
| Is this process oxidation or reduction? F₂ + 2e⁻ → 2F⁻ | Reduction |
| Is this process oxidation or reduction? Fe²⁺ → Fe³⁺ + e⁻ | Oxidation |
| In this reaction, what has been oxidised and what has been reduced? Mg²⁺ + 2Na → 2Na⁺ + Mg | Na has been oxidised, Mg²⁺ has been reduced |
| In this reaction, what has been oxidised and what has been reduced? 2Al + 3Ca²⁺ → 2Al³⁺ + 3Ca | Al has been oxidised, Ca²⁺ has been reduced |
| In this reaction, what has been oxidised and what has been reduced? K + Na⁺ → K⁺ + Na | K has been oxidized, Na⁺ has been reduced |
| What is electrolysis? | Using a dc electric current to decompose (break down) a substance |
| What is an electrolyte? | An ionic compound in the molten state or dissolved in water |
| What happens to an ionic substance when it is melted or dissolved in water? | The ions become free to move around |
| What is the name for the positive electrode? | The anode |
| What is the name for the negative electrode? | The cathode |
| Do positive ions move to the anode or the cathode? | Cathode |
| Do negative ions move to the anode or the cathode? | Anode |
| Where does reduction occur? | Cathode |
| Where does oxidation occur? | Anode |
| At which electrode would Zn²+(aq) turn into Zn(s)? | Cathode (needs to gain electrons) |
| At which electrode would Cl⁻(aq) turn into Cl₂(g)? | Anode (needs to lose electrons |
| Balance the equation: Al³⁺ + e⁻ → Al | Al³⁺ + 3e⁻ → Al |
| Balance the equation: Cl⁻ → Cl₂ + e⁻ | 2Cl⁻ → Cl₂ + 2e⁻ |
| Balance the equation: O²⁻ → O₂ + e⁻ | 2O²⁻ → O₂ + 4e⁻ |
| What will be the products for the electrolysis of molten iron bromide? | Iron and bromine |
| What will be the products for the electrolysis of molten zinc oxide? | Zinc and oxygen |
| Define oxidation in terms of electrons | Oxidation is the loss of electrons |
| Define reduction in terms of electrons | Reduction is the gain of electrons |
| What will be the products for the electrolysis of sodium sulfate solution? | Hydrogen gas and Oxygen gas |
| What will be the products for the electrolysis of acidified water? | Hydrogen gas and Oxygen gas |
| What happens to the change in mass of the electrodes if you increase the current? | As current increases so does the change in mass |
| When copper sulphate solution is electrolysed using copper electrodes, What happens to the mass of the electrodes? | The cathode mass increases, The anode mass decreases |
| Why use propanone to dry the electrodes when reweighing them after the electrolysis | It evaporates drying the electrodes, no need to physically dry them |
| What will be the products for the electrolysis of copper chloride solution? | Copper and chlorine |
| What will be the products for the electrolysis of molten lead bromide? | lead and bromine |
| In the electrolysis of sodium chloride solution, what are the products? | Chlorine gas and hydrogen gas |
| Why is sodium not produced in the electrolysis of sodium chloride solution? | It is more reactive than hydrogen so hydrogen is produced instead |
| What is produced at the anode in electrolysis of solutions? | Either a halogen or oxygen (when there is no halogen present) |
| For the extraction of which metals is electrolysis needed? | Ones more reactive than carbon, eg aluminium |
Created by:
Davenant Foundation School
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