Oxidation, Reduction and Redox equations Flashcards
What is oxidation?
The loss of electrons
/Gain of Oxygen
/Loss of Hydrogen
What is reduction?
The gain of electrons
/Loss of Oxygen
/Gain of Hydrogen
What is an oxidising agent?
Species that gains electrons.
What is a reducing agent?
Species that lose electrons.
What are the half equations and the ionic equation for:
SnO + Zn → ZnO + Sn
Half Equations: Sn2+ + 2e- → Sn Zn → Zn2+ + 2e- Ionic Equation: Sn2+ + Zn → Sn + Zn2+
Define oxidation state.
A number which represents the number of electrons lost or gained by an atom of that element in the compound.
What is the oxidation
state of oxygen in OF2?
[O] = +2
What is the oxidation
state of hydrogen in KH ?
[H] = -1
What is the oxidation state of chlorine in NaClO ?
[Cl] = +1
Define the term disproportionation?
Where in a redox reaction, the oxidation states of atoms of the same element, increase for some atoms, whereas decrease
for some atoms.
What is the oxidation state of phosphorus in PCl5 ?
[P] = +5
What is the oxidation state of nitrogen in ammonia?
[N] = -3
What is the oxidation state of arsenic in AsO43- ?
[As] = +5
What is the oxidation state of iron in K4Fe(CN)6?
[Fe] = +2
Why is 1s22s22p5 a weaker reducing agent than 1s22s22p63s23p64s2 ?
The 2p electron is closer to the nucleus than the 4s electron. Hence the nuclear attraction is stronger so the 2p electron is lost less easily than the 4s electron.
What happens in a redox reaction.
Electrons are transferred from one species to another.
One element is oxidised whilst another is reduced.
Why is, 2CrO42- + 2H+ → Cr2O72- + H2O,
not a redox reaction?
Chromium is oxidised whereas hydrogen remains the same oxidation state (no element is reduced).
