chapter 9

Question 1

oxidization

Answer 1

losing e-
- gets more positive, e- go on the products side

Question 2

reduction

Answer 2

gaining e-
- gets more negative, e- go on the reactants side

Question 3

redox reaction

Answer 3

occurs when electrons are transferred from an atom that is oxidized to an atom that is reduced
- overall the # of e- lost in oxidation must be gained in reduction

Question 4

electro chem

Answer 4

study if relationships between electricity and chemical reactions. includes the study of both spontaneous and non-spontaneous reactions

Question 5

oxidation number

Answer 5

used to keep track of electrons in redox reaction (also known as oxidization state)

Question 6

how to assign oxidation #

Answer 6

atom=0
monatomic ion= same as ion charge
flourine= -1 in compounds
oxygen= -2 in compounds
hydrogen= +1 in compounds
compounds= must sum to 0
polyatomic ions= add to overall charge
compound+ element furthest to right gets most common oxidation #

Question 7

balancing equations

Answer 7

• divide equaition into oxidation and redution reactions
• balance other elemtns
• balance oxygen by adding H2O
• balancing H2O by adding H+
• check charges and add more e- where needed
• if basic add same # of OH- as you did H+ on both sides
• times the reactions by # of e- to make #e- equal
• add reactions together and cancel
• combine and check work

Question 8

standard reduction potentials to predict redox reactions

Answer 8

lower right to upper left- only way to be spontaneous

Question 9

left side in STP

Answer 9

e- takers, oxidizing agents and reduction reactants

Question 10

right side STP

Answer 10

e- givers, reducing agents, oxidization reactants

Question 11

the confusing rule

Answer 11

oxidization reaction–> reducing agent
reduction reaction–> oxidizing agent

• electors passed in clockwise positions