Praxis Chemistry: Redox

Front 1

Electrochemistry:

Back 1

The study of the interchange of chemical and electrical energy.

Front 2

Oxidation:

Back 2

The loss of electrons. Since electrons are negative, this will appear as an increase in the charge (e.g., Zn loses two electrons; its charge goes from 0 to +2). Metals are oxidized.

Front 3

Oxidizing agent (OA):

Back 3

The species that is reduced and thus causes oxidation.

Front 4

Reduction:

Back 4

The gain of electrons. When an element gains electrons, the charge on the element appears to decrease, so we say it has a reduction of charge (e.g., Cl gains one electron and goes from an oxidation number of 0 to -1). Nonmetals are reduced.

Front 5

Reducing agent (RA):

Back 5

The species that is oxidized and thus causes reduction.

Front 6

Oxidation number:

Back 6

The assigned charge on an atom. You’ve been using these numbers to balance formulas.

Front 7

Half-reaction:

Back 7

An equation that shows either oxidation or reduction alone.

Front 8

Batteries

Back 8

are cells that are connected in series; the potentials add to give a total voltage.

Front 9

In a galvanic cell, oxidation

Back 9

occurs at the anode.

an ox!

Front 10

In a galvanic cell, reduction

Back 10

occurs at the cathode

red cat!