Next, the following chemical equations are presented, identify which ones belong to an oxidation-reduction reaction (redox). After identifying those equations that pertain to a redox reaction, indicate:
1. Oxidizing agent.
2. Reducing agent.
3. Element that rusts.
4. Element that is reduced.
To answer the previous indicators, you need to determine the number or oxidation state of each element present in the equation.
Chemical equations:
- Zn + HCl → ZnCl2 + H2
- HCl + NaOH → NaCl + H2O
- Zn + FeS → ZnS + Fe
- C2H6O + O2 → CO2 + H2O
Answers
Answer:
In both of these examples, the electrons are moving around, from one element to another, and since each electron has a charge of -1 the overall charge of an element changes during redox reactions.
Electron = -1 Charge
Oxidation = Loss of electron(s) = Loss of -1 for each electron, so... -(-1) = +1
During oxidation, the charge of the atom or ion INCREASES by the number of electrons lost
Reduction = Gain of electron(s) = Gain of -1 for each electron, so... +(-1) = -1
During reduction, the charge of the atom or ion DECREASES by the number of electrons gained
The following videos will help you understand exactly what is going on to an atom during oxidation and reduction.
Oxidation of Lithium
Reduction of Fluorine
When you look at a reaction of only oxidation, or only reduction, you are looking at what is called a half reaction.
The half reaction for the oxidation of lithium would be:
Lithium lost an electron to become the Li+ ion
The half reaction for the reduction of fluorine would be:
The fluorine gas gained two electrons to become two fluoride ions
Try a few examples of half reactions and see if you can determine whether the reaction taking place is an oxidation reaction, or a reduction reaction
Answer:
4 equation
I hope this help to u