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chem 1.1.2
| Term | Definition |
|---|---|
| delocalised | free electrons that move throughout the whole lattice structureElectrostatic force of attraction |
| Lustre - metals | occurs due to the presence of delocalised electrons in the lattice which reflect light |
| Malleability and Ductility - metals | when beaten into sheets or drawn into wires, layers of cations are forced onto each other. The delocalised electrons move in order to maintain the electrostatic force of attraction by surrounding the moving cations. |
| Electrical conductivity- metals | when an electric field is applied to a metal, there is a fixed positive and negatively charged end. The delocalised electrons are attracted towards the positive end |
| Heat conductivity- metals | delocalised electrons gain kinetic energy when metals are heated, so they move faster. Electrons collide with other electrons and transfer kinetic energy between them, distributing heat evenly throughout a metal. |
| Hardness/Density- metals | metals have high density because the cations are closely packed together in metallic lattices |
| Melting point and hardness- metals | a large amount of energy is required to overcome the electrostatic force of attraction in metallic bonding. This means that a metal will need a high temperature for any kind of physical change to occur. |
| how to see which one of two metallic compounds is stronger | Higher # of negative charges results in greater electrostatic attraction |
| Oxidation reaction | when a substance loses electrons |
| reactivity of metals w water - general formula | Reactive Metal + H2O → metal hydroxide + h2 |
| reactivity of metals with acid - general formmula | Reactive Metal + acid → metal salt + h2 |
| pop test | Test for hydrogen presence. |
| reactivity of metals with oxygen general forumla | Reactive Metal + o2 → metal oxide |
| least 2 reactive metals | gold and silver |
| disposing metals in the waste leads to | a scarcity of materials and damage to the environment when extracting metals. |
| Metals are extracted from | metals ores mined from the Earth |
| advantages of mining for metals | provides employment (mining, production, transport and sales), exportation of metal ores contributes to economy |
| disadvantages of mining for metals | costly to obtain raw materals for mining, energy use is substantial, mine waste leads to environmental damage |
| Metal ores | rocks containing minerals from which a valuable metal can be removed. |
| why are reactive metals found in ores | they form compounds |
| Haematite | most common iron ore in Australia, (Fe2O3) |
| how is iron metal extracted from its ore | by a reduction reaction with carbon in a blast furnace |
| Electrolysis | uses an electric current to breakdown the ore and uses a huge amount of electricity. used for the most reactive metals. Heating the ore to 960degc and passing a large electric current through the molten substance |
| Typical impurities of metals | other metals, unreduced oxides of the metal, and non-metals such as carbon, silicon, phosphorus, and sulphur |
| advantages of recycling metals | Heating, melting and cooling do not destroy a metal’s basic structure |
| disadvantages of recycling metals | time consuming, e-waste only produces small amt of reusable metal, alloys are difficult, can be contaminated, can't be handles (too toxic or radioactive) |
| Urban mining | process of obtaining metals from e-waste and other materials in our cities - gold, silver, platinum, and palladium can be extracted from electronic devices. |
| general process of urban mining | collecion, sorting, processing, melting, refining, transportation, new products |
| Bioleaching | process of extracting valuable metals from ores or waste (tailings, e-waste or contaminated water) by using microorganisms such as specific bacteria or fungi. copper, nickel, cobalt, gold |
| advantages of bioleaching | less damage to environment as less SO2 emissions, produces less damaging material, less energy requires (cooler temps), fewer health problems for miners |
| Disadvantages of bioleaching | slower, acidic waste is produced, Technology needs further development before bioleaching can be effective at an industrial level |
| high melting temp ionic compounds | Very strong attraction between particles so more heat energy is needed to break the attractions/bonds |
| hard crystals - ionic | due to strong bonds |
| brittle crystals - ionic | When external force is applied, results in |
| like charges coming into contact with one another, causing the solid to shatter as the charges are repelled | |
| does not conduct electricity in the solid state - ionic | No sea of delocalised electrons, charged particles are in fixed positions in the lattice and not free to move around the solid, therefore cannot conduct electricity |
| conducts electricity in molted/dissolved | Ions become free to move and thus electric current can be conducted |
| Electrolyte | a solution or molten substance that conducts electricity by means of the movement of ions |
| Ionic compounds | are made by the chemical combination of metallic and non-metallic elements |
| Why are ionic crystals cubic in shape? | indicating the particles within have a regular arrangement, much like a metal lattice |
| ionic bonding | a strong electrostatic force of attraction between cations and anions |
| Uses of ionic compounds | Ions in the body, metals can be extracted, cooking (salt, bicarb, preservatives), cleaning products (ammonia), fertilisers |
| Electron diagrams show | the path that electrons take when they are removed from a metal and added to a non-metal during ionic bonding. |
| Empirical formula | A chemical formula for an ionic compound is called the empirical formula, the simplest ratio of ions in the lattice. |
| Hydrated salts | Hydrated ionic compounds contain water molecules bonded within the crystal. |
| Solute | the substance that is dissolved in a solution |
| Solvent | the liquid that the solute is dissolved into |
| Solution is formed when | the forces between solute particles AND solvent molecules have been overcome, creating new forces between solute particles and some solvent particles |
| When an ionic compound is dissolved | the ions become free to move and a solution forms. |
| Aqueous solution | When the solvent is water |
| An ionic compound dissolves into water when | the positive and negative sides of water form interactions with them anions and cations of the ionic compound. |
| How are some ionic compounds aqueous? | the ions in an ionic lattice are pulled apart by their attraction to the water molecules |
| Ion-dipole bonds | The positive ends of water are attracted to the anions, and the negative ends of water are attracted to the cations |
| Dissociation | process of separating the ions from the ionic lattice. NaCl (s) → Na+ (aq) + Cl- (aq) |
| the compound is insoluble | this means there is not enough energy released when the ion-dipole attractions are formed to provide the energy needed to break the bonds between ions |
| Precipitation reactions occur when | two aqueous solutions are mixed and a new compound with low solubility is formed |
| Precipitate | the solid formed when a cation from one solution combines with an anion from the other solution to form an insoluble compound |
| Spectator Ions | Ions that are still aqueous in solution |
Created by:
pg0612345
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