Redox Flashcards
OILRIG
OXIDATION is loss of electrons, REDUCTION is gain of electrons
displacement reaction
more reactive metal takes the place of the metal ion and it is converted to a solid.
what is included in an ionic equation
charges for any acids/ionic substances
electrochemical cells
- metal higher up in ECS will lose electrons
- electrons flow through wire and other metal gains electrons.
electrolyte
ionic solution
ways of extracting metals
- heat alone
- heat with carbon
- electrolysis
ore
rock with metal inside
reducing agent
brings about reduction (a gain of electrons) by losing and donating electrons itself i.e. it is oxidised.
write equation backwards to show oxidation
oxidising agent
brings about oxidation (a loss of electrons) by accepting and gaining electrons itself i.e. it is reduced.
what is H- known as
Hydride ion
where are strong reducing agents found
top right of ECS
where are strong oxidising agents found
bottom left of ECS
electronegativity and oxidising agents
elements with a high electronegativity are likely to act as oxidising agents as they tend to form ions by gaining electrons. These tend to be non-metals.
electronegativity and reducing agents
elements with a low electronegativity tend to form ions by losing electrons so act as reducing agents. These tend to be metals.
what group are the strongest reducing agents found in
group 1 (alkali metals)
what group are the strongest oxidising agents found in
group 7 (halogens)
how to use data booklet to find out what could be used to oxidise ions
to the left and further down than the ion
everyday uses of oxidising agents
- potassium permanganate used to treat fungal infections such as athlete’s foot and prevent disease in fish in ponds.
- hydrogen peroxide used to break down coloured compounds and used as ‘bleach’ for clothes and hair.
examples of compounds as oxidising agents
- Dichromate (Cr2O7^2-)
- Permanganate (MnO4^-)
- Hydrogen Peroxide (H2O2) not in db
examples of compounds as reducing agents
- carbon monoxide (CO)
blast furnace- reduced Iron (III) ions to Iron atoms
steps for complex ion-electron equations
- check the main element is balanced
- add in H2O to balance out oxygen
- add in H+ ions to balance out hydrogen
- add in electrons to same side as H+ to balance the charge.
electrodes
electrodes (one + and one -) dip into the electrolyte and from the connection of the electric wires. Any chemical reactions occur at their surfaces.
