The loss of electrons. Also, when there is an increase in the oxidation number of the element.
What is oxidation?
100
Fe2O3+3CO->2Fe+3CO2
Identify the one being oxidized.
What is 3CO->3CO2
100
Atoms in this state have an oxidation number of 0.
What is elemental state?
100
Used to determine if a particular redox reaction will be feasible between a metal and the ions of another metal.
What is reactivity series?
100
Removing the charge of an ion.
What is discharging?
200
The gain of electrons. Also, when there is a decrease in the oxidation number.
What is reduction?
200
Write the half equations: 2Mg(s)+O2(g)->2MgO(s)
What are
2Mg(s)->2Mg2+(s)+4e-
O2(g)+4e- ->2O2-(g)
200
When naming compounds, this refers to the oxidation number of the elements.
What is Roman Numerals?
200
This metal is least reactive.
What is Platinum?
200
These have a tendency to lose electrons.
What are metals?
300
Compounds that have different oxidation numbers.
What is oxidation states?
300
These reactions always occur together and are dependent upon one another.
What are oxidation and reduction?
300
The oxidation numbers of all atoms in a polyatomic ion must add up to this.
What is the charge of the ion?
300
React by gaining electrons and forming negative ions, acting as oxidizing agents, and removing electrons from another substance.
What are halogens?
300
H2O and H+ ions are used for this.
What is balance half equations?
400
The product when you separate half reactions that allow the electrons to flow between them only through an external circuit.
What is half cell?
400
Balance the equation:
I-+ClO- ->I2+Cl-+H2O
What is 2H+ +ClO-+2I- ->Cl-+H2O+I2?
400
These elements have fixed oxidation numbers.
What are Group 1, Group 2, Al, H, F, Cl, and O?
400
More reactive non-metals are this.
What are stronger oxidizing agents?
400
This does the reverse of a voltaic cell.
What is an electrolytic cell?
500
A series of chemical elements arranged in order of their strength as reducing agents.
What is reactivity series?
500
These are the rules for balancing redox reactions.
What are:
1. Write half equations
2. Balance atoms other than H and O
3. Balance O by adding H2O
4. Balance H by adding H+
5. Balance net charge by adding e-
6. Make e- gains equal e- losses then add half equations
7. Cancel anything on both sides