Electrochemistry1

Question 1

Oxidation

Answer 1

Loss of Electrons

Question 2

Reduction

Answer 2

Gain of Electrons

Question 3

ELECTRONS MOVE FROM

REACTANT WITH ….. TO REACTANTS WITH ….

Answer 3

LESS
ATTRACTION FOR ELECTRONS…
…TO REACTANT WITH MORE
ATTRACTION FOR ELECTRONS

Question 4

Electronegativity increases

Answer 4

upwards and to the right, with N, O, F being the most electronegative atoms in the periodic table

Question 5

Oxidizing Agent

Answer 5

causes oxidation in another species (is reduced)

Question 6

Reducing Agent

Answer 6

causes reduction in another species (is oxidized)

Question 7

How would you define the O.N.?

Answer 7

The O.N. is the charge that the atom would have IF the electrons
were transferred completely to/from bonded atoms

Question 8

O.N. number of an atom in its elemental form

Answer 8

An atom in its elemental form – oxidation number = 0 (e.g. Na or Cl2)

Question 9

O.N. of a monoatomic ion

Answer 9

Monoatomic ion: Oxidation number = ion charge

Question 10

O.N. of a molecule

Answer 10

The sum of oxidation numbers for all atoms in a molecule is equal to the charge on the molecule

Question 11

O.N. assigned to a group 1 atom

Answer 11

Grp1 (+1)

Question 12

O.N. assigned to a group 2 atom

Answer 12

Grp2 (+2

Question 13

O.N. assigned to a H atom

Answer 13

H (+1)

Question 14

O.N. assigned to a F atom

Answer 14

F (-1)

Question 15

O.N. assigned to an O atom (most cases)

Answer 15

O (-2)

Question 16

O.N. assigned to a group 17 atom

Answer 16

Grp17 (-1)

Question 17

What are groups in the periodic table?

Answer 17

they are the columns of the periodic table

Question 18

Oxidation

Answer 18

O.N. increases (becomes less electronegative)

Question 19

Reduction

Answer 19

O.N. decreases (becomes more electronegative)

Question 20

IN A BALANCED REDOX EQUATIONS:

Answer 20

# ELECTRONS LOST (OXIDATION)
= # ELECTRONS GAINED (REDUCTION)

Question 21

What is step 1 in balancing Redox Equations?

Answer 21

1. Break “skeleton” equation (no spectator ions) into two half-reactions

Question 22

What is step 2 in balancing Redox Equations?

Answer 22

2. Balance atoms, everything but O&H, then O (add H2O), then H (add H+)

Question 23

What is step 3 in balancing Redox Equations?

Answer 23

3. Balance charge, add electrons (e–) to more positive side

Question 24

What is step 4 in balancing Redox Equations?

Answer 24

4. Scale (multiply) both halves so # electrons are equal, add coefficients

Question 25

What is step 5 in balancing Redox Equations?

Answer 25

5. Add balanced half-reactions together, add spectator ions & states of matter
   (if basic solution, add one OH– to each side for every H+ at this stage)

Question 26

Redox in Organic Chemistry

Answer 26

OXIDATION: ADD OXYGEN OR REMOVE HYDROGEN
REDUCTION: REMOVE OXYGEN OR ADD HYDROGEN