Choose the 4 statements below that are TRUE of the reaction.
a
The oxidation number of Chlorine (Cl) decreases.
b
The oxidation number of Chlorine (Cl) increases.
c
The oxidation number of Phosphorous (P) increases.
d
The oxidation number of Phosphorous (P) decreases.
e
Chlorine (Cl) undergoes oxidation.
f
Chlorine (Cl) undergoes reduction.
g
Phosphorous (P) undergoes reduction.
h
Phosphorous (P) undergoes oxidation.
To properly evaluate these statements, I would need to see the chemical reaction in question. However, I can still explain the terms and guide you on how to assess each statement once you have the reaction.
When analyzing a chemical reaction to determine changes in oxidation states and identify redox processes, you should do the following:
1. Assign oxidation numbers to each element in both the reactants and products.
2. Compare the oxidation numbers of each element in the reactants versus the products.
3. Identify any elements that have changed oxidation numbers; these are involved in redox processes.
Here are definitions to help with the evaluation process:
- Oxidation is the process wherein an element's oxidation number increases as it loses electrons.
- Reduction is the process wherein an element's oxidation number decreases as it gains electrons.
- The element that undergoes oxidation (its oxidation number increases) is said to be oxidized.
- The element that undergoes reduction (its oxidation number decreases) is said to be reduced.
Unfortunately, without the specific reaction provided, I cannot conclusively tell you which of the statements a through h are true.
Please provide the chemical equation or further information about the changes in the oxidation states of chlorine and phosphorous in the reaction for me to help you select the four true statements.