Characterizing Oxidation and Reduction

Question 1

how does an ionic equation look?

Answer 1

a chemical equation in which soluble ionic substances are written in dissociated form

elements are written individually with their charges

Question 2

describe a net ionic equation

Answer 2

ionic equation where spectator ions are not included

Question 3

what are spectator ions?

Answer 3

a substance present in a solution but not in the chemical reaction

elements on the product side and on the reactant side that have the same states

Question 4

what is an oxidation reaction?

Answer 4

gaining of oxygen

loss of hydrogen

a reaction where there is a loss of electrons!

Numbers become more positive

LEO

Question 5

what is reduction reaction?

Answer 5

a reaction where there is a gaining of electrons, more specifically a loss of oxygen and a gaining of hydrogen

GER

Question 6

what is a redox reaction?

Answer 6

the transfer of electrons between two different chemicals

• oxidation is the loss of electrons
• reduction is the gaining of electrons
• also known as an oxidation and reduction reaction, because it’s a reaction when oxidation and reduction occur together

Question 7

electronegativity definition

Answer 7

the ability of the atom of an element to attract sharing electrons to itself in order to bond

Question 8

what is electron sharing

Answer 8

occurs when the electrons in the outermost electron shell of an atom can be used to complete the outermost electron without the electron being completely transferred

Question 9

what does oxidation number mean?

Answer 9

the number tells electrons lost, gained, or shared as a result of chemical bonding for a specific element

Question 10

what does a positive oxidation number mean?

Answer 10

number of electrons an element lost

Question 11

what does a negative oxidation number mean?

Answer 11

number of electrons an element gained

Question 12

what is the oxidation exception for hydrogen?

Answer 12

hydrogen can lose, gain, or share electrons

Question 13

oxidation rule for hydrogen

Answer 13

it is +1 for metals

it is -1 for nonmetals, not only when it’s beside a nonmetal but in the formula in general

Question 14

oxidation rule for oxygen

Answer 14

• 2

- 1 in peroxide (H2O2)

Question 15

oxidation rule for fluorine

Answer 15

always -1

Question 16

what does it mean when an element is in a standard state?

Answer 16

if an element is in its natural state or is s diatomic molecule HOFBrINCl, then the oxidation number is 0

Question 17

oxidation rule for sulfate

Answer 17

sulfate (SO4) always has an oxidation number of -2 that’s not always visible

Question 18

what is the goal of finding oxidation numbers

Answer 18

all the elements have to add up to the charge

if there’s no charge, then they have to add up to 0

Question 19

oxidation number vs charge

Answer 19

oxidation number is on top of the element and the sign is before the number

the charge is beside the top of the element and the sign is after the number

Question 20

how to balance an ionic equation for acidic conditions, then find the oxidizing agent and the reducing agent

Answer 20

1. Write the half-reactions (they don’t have to be balanced)
2. Make sure elements other than oxygen and hydrogen are balanced
3. Balance the equation with oxygen atoms by adding waters
4. Balance the equation with hydrogen atoms by adding hydrogen ions
5. Balance the charges by adding electrons to give the same net charge
6. Multiply one or both of the new half-reactions that will bring the number of electrons to the lowest common multiple (common denominator)
7. Combine the completely balanced half-reactions together.
8. Cancel out spectator ions
9. Lastly, identify the oxidizing agent and the reduction agent (the reducing agent is the atom being oxidized, the oxidizing agent is the atom being reduced, look at the initial equation)

Question 21

oxidation rule for halogens

Answer 21

usually -1, but it is positive 1 with oxygen