17822548
Description
Flashcards by Oliver Faragher, updated more than 1 year ago
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Created by Oliver Faragher
over 5 years ago
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| Question | Answer |
| What does iron ore look like and where are some of its biggest mines? | It is a red-brown, often dirty rock The largest mines are in Australia and Brazil The most common ore is haematite |
| What is an oxidation reaction? | A reaction where something gains oxygen e.g Iron + Oxygen -> Iron oxide |
| What is reduction? | A reaction where something loses oxygen |
| Describe aluminium in a world context | It is the most common metal on earth and the third most abundant element One common aluminium ore is Bauxite (aluminium oxide) |
| What dictates if something can be reduced or if it needs electrolysis to separate it? | If it is less reactive than carbon then it can be removed by reduction If it is more reactive it must be removed by electrolysis |
| What is a soluble base? | An alkali which dissolves to make an alkaline solution |
| How does magnesium and calcium react with water? | Magnesium = Only with steam Calcium = less vigorously than lithium |
| What metals form positive ions? | Potassium, sodium, lithium, calcium, magnesium, zinc, iron, copper |
| How does displacement work? | A more reactive metal can replace a less reactive metal in a compound |
| When magnesium displaces iron what happens? | The iron coats the magnesium when it is displaced |
| Which metals need to be extracted by electrolysis and why? | Potassium, sodium, calcium, magnesium and aluminium need to undergo electrolysis because they are more reactive than carbon |
| What are some metals that can be reduced by carbon? | Zinc, iron and lead |
| How is iron extracted? | Carbon is heated for form carbon monoxide Carbon monoxide reduces the oxygen from iron and forms carbon dioxide and pure iron |
| What happens when something is displaced? | The electrons are forced onto the ions of less reactive metals |
| How would you make a crystallized salt? | Add excess of the metal in use Filter the solution into a crystallizing dish Evaporate the solution to condense |
| What are the charges of key metals? | Mg 2+ Fe 2+ Zn 2+ Na + K + Ca 2+ |
| What are the ions that make up sulfuric and hydrochloric acids? | Sulfuric (H2So4) = 2H +, So4 2- Hydrochloric = H +, Cl - |
| What is a redox reaction? | A reaction where at least one thing is oxidized and at least one thing is reduced |
| What is the difference between an Alkali and a Base? | A base is anything with a PH of over 7 An Alkali is a base which can be dissolved in water |
| What is the word equation for a neutralization reaction? (give an example too) | Acid + Base -> Salt + Water ZnO + H2So4 -> ZnSO4 + H20 |
| What happens when a metal carbonate does this? | It does the same but forms carbon dioxide too |
| What are the four ways of making a metal salt? | Metal + acid -> metal salt + hydrogen Metal oxide + acid -> metal salt + water Metal hydroxide + acid -> metal salt + water Metal carbonate + acid -> metal salt + hydrogen + carbon dioxide |
| List all of the key ion charges | Single: Cl- , NO3 - , OH- , Na+ , K+ , H+ Double: So4 2- , Ca 2+ , Mg 2+ , Zn 2+ , Fe 2+, Cu 2+ |
| How does universal indicator work / what is the pH scale based on? | The number of H+ ions (the higher the number of H+ the lower the pH) |
| What type of ion does an alkali contain? | OH- (hydroxide) |
| In a burette what is the volume measured in and where is it measured from? | cm cubed The bottom of the meniscus |
| List some strong and weak acids | Strong: Hydrochloric Nitric Sulfuric Weak: Ethanoic Citric Carbonic |
| What is the difference between strength and concentration? | The stronger the acid the more ionized the liquid is The more concentrated an acid is the more of it is found in a mixture or substance (mmol/dm cubed or g/dm cubed) |
| What is electrolysis? | The process of passing direct current through a solution or melted ionic compound to move the ions apart and so break the compound down and discharge some of the elements at the electrodes |
| What is an electrolyte? | A liquid where ions are free to move about and carry electricity |
| What are the two rods inserted into the electrolyte? | Electrodes: Cathode = negative Anode = positive |
| How / why do electrons move during electrolysis? | Electric current is passed through causing the ions to move to the electrodes Positive to cathode (negative), called cations Negative to anode (positive), called anions |
| What happens when the ions reach their electrodes? | Negative ions at the anode lose electrons to the current Positive ions at the cathode gain electrons from the current |
| How is aluminium ore extracted? | Bauxite (aluminium ore) is mixed with cryolite to lower its melting point This solution is placed in a steel electrolysis cell and then electrolysed with carbon electrodes The oxygen is drawn to the anode where oxygen ions ate discharged and then the carbon reacts with the oxygen to form carbon dioxide The liquid aluminium pools and is collected at the bottom |
| What happens in the electrolysis of an aqueous solution? | There is PREFERENTIAL DISCHARGE The least reactive ions are preferentially discharged as elements |
| During the electrolysis of an aqueous solution what happens at the electrodes? |
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