Unit 2: Electrochemistry

Question 1

what does a redox reaction involve?

Answer 1

A transfer of electrons

Question 2

What reactions are never redox

Answer 2

double replacement

Question 2

OER REL

Answer 2

-Oxidation (electrons on right)
-Reduction (electrons on left)

Question 3

-The oxidizing agent is ________
-The reducing agent _________

Answer 3

-Reduced
-Oxidized

Question 4

When constructing a redox table, the element with the electrons is always the

Answer 4

OA

Question 5

Redox spontaneity rule (RSR)

Answer 5

A redox reaction occurs spontaneously when the OA is above the RA (When the RA is above the OA, no reaction occurs)

Question 6

Steps to calculate titration

Answer 6

1. Use SOA/SRA to determine the ratio of coefficients
2. Calculate “n” for known sample
3. Multiply by the ratio of coefficients determined in step 1 d.o.g (desired over given)
4. C=n/V

Question 7

When the O# increases the element has been ______

Answer 7

oxidized (RA)

Question 8

When the O# decreases the element has been _________

Answer 8

reduced (OA)

Question 9

What is a disproportionation reaction? Provide an example

Answer 9

-A reaction where the same element is oxidized and reduced

Examples: 2H2O2 –> 2H20 + O2
^ reaction of hydrogen peroxide
- Chlorine gas in water
- Reaction of copper ions in solution

Question 10

A cell consists of two different metals called _______

Answer 10

electrodes

Question 11

Electrodes are in contact with a conductive solution called:

Answer 11

an electrolyte

Question 12

Inert Electrodes

Answer 12

Conductors that are not OAs or RAs

Question 13

The cathode is connected to the ______ terminal of the voltmeter

Answer 13

red

Question 14

When (H) is connected to red the other half cell

Answer 14

has a negative reduction potential