Revision for Elements from the Sea module
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| What is the ionic equation for the reaction below? NaOH(aq) + HCl(aq) --> NaCl(aq) + H2O(l) | H+(aq) + OH-(aq) --> H2O(l)
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| What is the ionic equation for the reaction below? Fe(NO3)3(aq) + 3KOH(aq) --> Fe(OH)3(s) + 3KNO3(aq) | Fe3+(aq) + 3OH-(aq) --> Fe(OH)3(s)
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| Ionic solids have high melting points because | there is a large number of electrostatic interactions between the positive and negative ions that require lots of energy to break
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| Ionic liquids and solutions conduct electricity because | the free ions act as charge carriers
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| The sodium chloride lattice is | alternating Na+ and Cl- ions in layers Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+
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| State and explain the general trend in ionisation energy from Na to Ar | Increasing due to increasing nuclear charge and all outer electrons are in the same energy level
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| Explain why there is a decrease in ionisation energy between Mg and Al | The outermost electron in Al is in the 3p subshell, which is further from the nucleus and shielded by the 3s subshell
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| Explain why there is a decrease in ionisation energy between P and S | Increase in repulsion due to the outermost electron in sulphur being in a filled p-orbital when the outermost electron in phosphorus is not
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| The first ionisation enthalpy of magnesium is | Mg(g) --> Mg+(g) + e-
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| The second ionisation enthalpy of phosphorus is | P+(g) -->P^2+(g) + e-
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| The electronic configuration of calcium is | 1s2, 2s2, 2p6, 3s2, 3p6, 4s2
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| The electronic configuration of iron is | 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d6
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| The electronic configuration of copper is | 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10
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| For solutions, the equation for moles is | Moles = concentration * volume in dm3
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| 250cm3 of 0.5mol dm3 HCl contains how many moles of HCl? | Moles = 0.5 * 0.25 = 0.125 moles
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| The oxidising power of halogens | increases as you go down the group
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| The reaction of chlorine with bromide ions is shown as | 1/2Cl2 + Br- --> 1/2Br2 + Cl-
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| When iodine is added to a solution containing chloride ions, what happens? | Nothing, because iodine is less oxidising than chlorine
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| When chlorine is added to a solution containing iodide ions what happens? | The solution turns red/brown due to iodine
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| The melting point of halides increase down the group because | the number of electrons increases, which increases the strength of van-der-waals forces
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| Chlorine can be manufactured by electrolysing what raw material? | Sea water (or brine)
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| Bromine is manufactured by treating sea water with chlorine gas. Why? | The chlorine displaces bromide ions in the sea water
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| The hazards of manufacturing chlorine gas include | It is toxic and a gas, so difficult to transport
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| What colour precipitate is formed when chloride ions are mixed with silver nitrate | White precipitate
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| How can the cream precipitate of silver bromide and the yellow precipitate of silver iodide be distinguished? | Add concentrated ammonia, which dissolves silver bromide but not silver iodide
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| Industrial uses of chlorine include | Bleach, water treatment and plastics (PVC)
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| Industrial uses of bromine include | Medicines, pesticides and flame retardents
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| Halogenoalkanes are | alkanes with one or more hydrogens replaced with a halogen atom
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| Are halogenoalkanes polar or non-polar? | Non-polar
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| Name the mechanism for the reaction between chlorobutane and sodium hydroxide | nucleophilic substitution
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| What is represented by a curly arrow in a reaction mechanism? | The movement of a pair of electrons
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| What type of bond fission is involved in the leaving of the halogen atom? | Heterolytic fission
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| From what homologous series is the product of the reaction between bromobutane and ammonia? | Amines
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| State the trend in rate of hydrolysis for fluoro-, chloro-, bromo- and iodoalkanes | The rate increases as you descend the group
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| What is a nucleophile? | A species that can donate a lone pair of electrons
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