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25 Cards in this Set
- Front
- Back
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Exo or endo neutralisation reaction |
Exothermic |
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Bond dissociation enthalpy |
The enthalpy change required to break a covalent bond with all species in a gaseous state |
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Give 2 features of a reaction at equilibrium |
Concentrations remain the same Forward rate=backward rate |
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How to distinguish between AgBr and AgI |
Conc ammonia- AgBr precipitate redissolves,AgI no change |
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How to distinguish between HCl and HNO3 |
Silver nitrate- HCl white precipitate HNO3 no change |
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Group 2 sulphates |
Decrease in solubility down the group |
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Group 2 hydroxides |
Increase in solubility up the group X(OH)2 |
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How are haloalkanes made |
Free radical substitution (alkane) Electrophilic addition (alkene) |
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Reaction of chlorine with cold water |
Cl2+ H20→ HClO + HCl |
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Extraction of Titanium |
Ti02 is converted to TiCl4 by reacting with coke and chlorine Ti02 + 2C + 2Cl2→ TiCl4 + 2CO Then react with sodium TiCl4 + 4Na → Ti + 4NaCl |
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Extraction of tungsten |
WO3 + 3H2 → W + 3H2O |
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Extraction of aluminium |
Electrolysis Molten cryolite Na3AlF6 |
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The blast furnace |
At the base coke burns in a blast if hot air. This generates heat making the temp around 2000k CO2 is formed which reacts with more carbon to for carbon monoxide. This is the reducing agent Fe2O3 + 3CO → 2Fe + 3CO2 |
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Standard conditions |
100kPa and 298K |
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Neutralisation reactions |
Exothermic Acid+ alkali→ salt and water |
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Bond dissociation enthalpy |
The enthalpy change required to break a covalent bond with all species in the gaseous state |
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Transition state or activated complex |
When bonds are being made and broken at the same time |
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Catalytic converters |
Honeycomb made of ceramic material with platinum or rhodium metals. Polluting gases react with each other usually form nitrogen and co2 The gases form bonds with the metal (adsorption) they hold the gases in place then the gades react on the surface. The gases break away (desorption) |
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Sodium bromide and sulphuric acid |
Fumes of hydrogen bromide and brown fumes of bromine. Sulfur dioxide also formed. Acid base reaction also reduces to SO2 |
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Sodium Iodide and sulphuric acid |
Hydrogen iodide fumes. Black solid iodine. Hydrogen sulfide egg smell. Yellow solid sulfur. Reduces to SO2, S and H2S |
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Disproportionation |
Where the oxidation state of some atoms of the same element increase and others decrease. |
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Chlorine and water in the sun |
2Cl2 + 2h2O → 4HCl + O2 |
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Sodium chlorate |
NaClO+ H2O←→ Na+ + OH- + HClO |
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Chlorine and sodium hydroxide |
Cl2 + 2NaOH → NaClO + NaCl + H2O |
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Stereoisomers |
Same structural formula with atoms arranged differently in space |
