REDOX

Question 1

oxidation

Answer 1

donate e-

positive

Question 2

reduction

Answer 2

accept e-

negative

Question 3

oxidising agent

Answer 3

oxidises other species

gets reduced

Question 4

reducing agent

Answer 4

reduced other species

gets oxidised

Question 5

half reaction - oxidation + reduction

Answer 5

all metal act as reducing agent - donate e- and oxidised

Question 6

measuring standard reduction potential

Answer 6

using electrochemical reduction potential

Question 7

electrochemical reduction potential

and example

Answer 7

2 half cell connect via salt bridge and electric current flow between them
e.g. zinc in zinc solution

Question 8

size of potential difference

Answer 8

is proportional to readiness of e- by reducing agent

Question 9

determining standard reduction potential

Answer 9

uses H electrode = 0.00V

used to compare reducing potential of all species

Question 10

standard H electrode

under standard conditions

Answer 10

H - bubbled in 1M H+ ions solution and metal is platinum - does not react and coat in Pt
increase SA and increase for H reaction therefore equilibrium set up faster

Question 11

forward reaction in standard H electrode

Answer 11

reduction

Question 12

standard redutcion

Answer 12

equilibrium position in half reaction

more -ve value = further left of half reaction at equilibrium

Question 13

example of standard reduction - Mg and Zn

Answer 13

more heavy weight - to left than Zn therefore Mg - stronger reducing agent than Zn - forward reaction - Mg
Mg loses 2e- and Zn gains 2e-

Question 14

strongest reducing agents

Answer 14

oxidised during REDOX