redox Flashcards

1
Q

oxidation

A
  • gain of oxygen
  • loss of electrons
  • increase in oxidation number
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2
Q

reduction

A
  • loss of oxygen
  • gain of electrons
  • decrease in oxidation number
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3
Q

disproportionation

A
  • when a single species is simultaneously both oxidised and reduced
  • use OS to work this out
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4
Q

oxidising agents

A
  • give oxygen to another substance
  • remove electrons from another substance (so are reduced themselves)
  • strongest oxidising agents are found in group 7
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5
Q

reducing agents

A
  • remove oxygen from another substance
  • give electrons to another substance (so are oxidised themselves)
  • strongest reducing agents are found in group 1
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6
Q

oxidation states (OS)

A
  • oxidation/reduction in covalent compounds

- instead of true loss/gain of electrons, ‘degree of sharing’ of electrons changes

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7
Q

Rules for assigning OS

A
  • OS of an atom in its elemental state = 0
  • sum of the OS of all the atoms in a compound = 0
  • OS of an ion = the charge on the ion (Cl- = -1)
  • OS of a group ion = the charge on the ion
  • OS of an oxygen atom in a compound = −2, except in peroxides it = -1 / when with fluorine it = +2
  • OS of a hydrogen atom in a compound = +1, except in metal hydrides it = -1
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8
Q

using OS to spot oxidation/reduction

A
  • If the OS of an element increases, then it has been oxidised.
  • If the OS of an element decreases, then it has been reduced.
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9
Q

water OS

A
  • oxygen = -2

- hydrogen = +1

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