Redox Reactions - Chemistry

How to complete a redox reaction

1) Assign oxidation numbers. Use this to figure out what is oxidized and what is reduced.

2) Split the equation into two half equations

3) Balance equations in terms of mass

4) Balance equations in terms of charge/electrons

• Find the charge and add electrons to one side to neutralize this charge (for both half reactions)

5) Make both half reactions have the same number of electrons (added to one side) by multiplying and finding least common multiple.

6) Electrons now cancel (one on products side, one on reactants side) so half equations can be added with their new coefficents

Spectator

Ion or particle that does not lose/gain e- from reactants or products in a reaction

All pure/solo elements have an oxidation state of…

0

All monoatomic (single) ions have an oxidation state of…

0

All group 1 metals in a compound have an oxidation state of…

+1

All group 2 metals in a compound have an oxidation state of…

+2

Hydrogen in a compound bonded with a metal has an oxidation state of..

-1

Hydrogen in a compound bonded with a nonmetal has an oxidation state of..

+1

Halogens are most of the time _______ when it is the most

________

• Also: what group number is Halogens

Halogens (group 17) are usually -1 when it is the most electronegative atom (MOST OF THE TIME)

Oxygen in a compound has an oxidation state of _____

• what is the exception/ratio

Oygen in a compound has an oxidation state of… -2

Peroxide is an exception 2:2 ratio, typically a nonmetal

In a neutral molecule or polyatomic ion that sum of oxidation states is..

the oxidation state equals the overall charge

What is oxidation state (in terms of electrons)

Oxidation state, also known as oxidation number, describes the hypothetical charge an atom would have if all its bonds were fully ionic. In simpler terms, it represents the degree of oxidation, or the number of electrons an atom has effectively lost or gained in forming a chemical bond. A positive oxidation state indicates a loss of electrons (oxidation), while a negative oxidation state indicates a gain of electrons (reduction). 

What is a redox reaction and what does it stand for

A redox reaction, short for oxidation-reduction reaction, is a chemical reaction that involves the transfer of electrons between two species. It is characterized by one species being oxidized (losing electrons) and another being reduced (gaining electrons). The term "redox" is a portmanteau of "reduction" and "oxidation". 

What process involves the transfer of electrons?

The process that involves the transfer of electrons is called an oxidation-reduction reaction (also known as a redox reaction). In these reactions, one substance loses electrons (oxidation) while another substance gains electrons (reduction

When an element/compound is gaining electrons it is being ______ and oxidation state/number _______

When an element/compound is losing electrons it is being _______

and oxidation state/number _______

When an element or compound gains electrons, it is being reduced and oxidation number DECREASES

When an element or compound loses electrons, it is undergoing oxidation and oxidation number INCREASES

The substance that is being oxidized is also the _________

The substance that is being reduced is also the ________

The substance that is being oxidized is also the reducing agent

The substance that is being reduced is also the oxidation agent

The oxidation number of a reducing agent ________

The oxidation number of an oxidation agent __________

The oxidation number of a reducing agent is what is being oxidized so oxidation number INCREASES (more positive)

The oxidation number of an oxidation agent is what is being reduced so the oxidation number DECREASES (more negative)

Redox versus oxidation-reduction

THEYRE THE SAME (redox is a abbreviated reduction-oxidation)

Oxidized =

When a substance is oxidized, it loses electrons and its oxidation number increases

Reduced:

When a substance is oxidized, it gains electrons and its oxidation number decreases