Oxidation/Reduction and Periodicity

Question 1

oxidation state/number

Answer 1

the hypothetical charge of an atom if all of its bonds were ionic

Question 2

what does it mean for something to be oxidized?

Answer 2

When it loses its electrons to a more electronegative element

Question 3

What does it mean for something to be reduced?

Answer 3

the charge of an element by another element

Question 4

oxidation vs. reduction

Answer 4

losing electrons is oxidation and gaining electrons is reduction

Question 5

what are alkaline metals usually? (Hint: what oxidation state would they be?)

Answer 5

oxidized, 1+

Question 6

what are alkaline earth metals usually? (Hint: what oxidation state would they be?)

Answer 6

oxidized, 2+

Question 7

what are halogens usually? (Hint: what oxidation state would they be?)

Answer 7

reduced, 1-

Question 8

what are oxygen group usually? (Hint: what oxidation state would they be?)

Answer 8

reduced, 2-

Question 9

H2O2 oxidation

Answer 9

H: +, O: -

Question 10

OF2 oxidation

Answer 10

F: -, O: 2+

Question 11

oxidation state of free element

Answer 11

0

Question 12

oxidation state of monoatomic ion

Answer 12

the atom’s charge is its charge

Question 13

reducing and oxidizing agent

Answer 13

reducing agent is the one that is oxidized while the oxidizing agent is the one that is reduced.

Question 14

how can we tell if a reaction is a redox reaction

Answer 14

see if there is a change in oxidation states for each element

Question 15

recall the half-reaction method for balancing redox reactions

Answer 15

1. split the reaction into 2 half-reactions (1 representing oxidation and 1 representing reduction).
2. Balance the half-reactions for mass, charge, and # of electrons transferred
3. Add the half-reactions together

Question 16

When we do not have a simple redox reaction, what may we do in order to fully balance the equation?

Answer 16

Add H2O, OH- (Basic solution), or H+. (Acidic solution)