part b: short answer and calculations (thinking and inquiry and application)
1. for the following reaction, write (and clearly label) the complete oxidation half - reaction and the complete reduction half - reaction (including the number of electrons transferred in each). also, indicate who the reducing agent is and who the oxidizing agent is.
\ce{mg_{(s)} + 2ag^{+}_{(aq)} - mg^{2+}_{(aq)} + 2ag_{(s)}}
| overall expectations: f2 and f3 | not yet | level 4++ 100% | level 4+ 95% | level 4 85% | level 3 75% | level 2 65% | level 1 55% |
| --- | --- | --- | --- | --- | --- | --- | --- |
| | | demonstrates the concept of redox reactions with a high degree of effectiveness and accuracy: - correct writing of half reactions - correct id of electrons - correct id of ra and oa - no errors in solutions | demonstrates the concept of redox reactions with a high degree of effectiveness and accuracy: - correct writing of half reactions - correct id of electrons - correct id of ra and oa - slight error in solutions | demonstrates the concept of redox reactions with a high degree of effectiveness and mostly correct writing of half reactions - mostly correct id of electrons - no id of ra and oa - minor errors in solutions | demonstrates the concept of redox reactions with considerable effectiveness and accuracy: - somewhat correct writing of half reactions - somewhat correct id of electrons - no id of ra and oa - multiple errors in solutions | demonstrates the concept of redox reactions with some effectiveness and accuracy: - some correct writing of half reactions - some correct id of electrons - no id of ra and oa - multiple errors in solutions | demonstrates the concept of redox reactions with limited effectiveness and accuracy: - limited use of half reactions and electron transfer - limited correct solutions - showed something conceptually related to the questions |

Question

part b: short answer and calculations (thinking and inquiry and application)
1. for the following reaction, write (and clearly label) the complete oxidation half - reaction and the complete reduction half - reaction (including the number of electrons transferred in each). also, indicate who the reducing agent is and who the oxidizing agent is.
\ce{mg_{(s)} + 2ag^{+}_{(aq)} -> mg^{2+}_{(aq)} + 2ag_{(s)}}
| overall expectations: f2 and f3 | not yet | level 4++ 100% | level 4+ 95% | level 4 85% | level 3 75% | level 2 65% | level 1 55% |
| --- | --- | --- | --- | --- | --- | --- | --- |
|  |  | demonstrates the concept of redox reactions with a high degree of effectiveness and accuracy: - correct writing of half reactions - correct id of electrons - correct id of ra and oa - no errors in solutions | demonstrates the concept of redox reactions with a high degree of effectiveness and accuracy: - correct writing of half reactions - correct id of electrons - correct id of ra and oa - slight error in solutions | demonstrates the concept of redox reactions with a high degree of effectiveness and mostly correct writing of half reactions - mostly correct id of electrons - no id of ra and oa - minor errors in solutions | demonstrates the concept of redox reactions with considerable effectiveness and accuracy: - somewhat correct writing of half reactions - somewhat correct id of electrons - no id of ra and oa - multiple errors in solutions | demonstrates the concept of redox reactions with some effectiveness and accuracy: - some correct writing of half reactions - some correct id of electrons - no id of ra and oa - multiple errors in solutions | demonstrates the concept of redox reactions with limited effectiveness and accuracy: - limited use of half reactions and electron transfer - limited correct solutions - showed something conceptually related to the questions |

Accepted Answer

# Explanation:
## Step1: Identify Oxidation Half - Reaction
Oxidation is the loss of electrons. In the reaction $Mg_{(s)}+2Ag^{+}_{(aq)}
ightarrow Mg^{2 + }_{(aq)}+2Ag_{(s)}$, magnesium ($Mg$) goes from an oxidation state of 0 (in $Mg_{(s)}$) to + 2 (in $Mg^{2+}_{(aq)}$). So the oxidation half - reaction is the process where $Mg$ loses electrons. The oxidation half - reaction is: $Mg_{(s)}
ightarrow Mg^{2+}_{(aq)} + 2e^-$. Here, $Mg$ loses 2 electrons.
## Step2: Identify Reduction Half - Reaction
Reduction is the gain of electrons. Silver ($Ag$) goes from an oxidation state of + 1 (in $Ag^{+}_{(aq)}$) to 0 (in $Ag_{(s)}$). For 2 moles of $Ag^{+}$, the reduction half - reaction is: $2Ag^{+}_{(aq)}+2e^-
ightarrow 2Ag_{(s)}$. Here, each $Ag^{+}$ gains 1 electron, and for 2 $Ag^{+}$ ions, a total of 2 electrons are gained.
## Step3: Identify Oxidizing and Reducing Agents
The reducing agent is the substance that is oxidized (loses electrons). Since $Mg$ is oxidized (loses electrons in the oxidation half - reaction), $Mg$ is the reducing agent. The oxidizing agent is the substance that is reduced (gains electrons). Since $Ag^{+}$ is reduced (gains electrons in the reduction half - reaction), $Ag^{+}$ (or the species containing $Ag^{+}$, in this case, the $Ag^{+}_{(aq)}$ from the reactants) is the oxidizing agent.

# Answer:
- Oxidation half - reaction: $Mg_{(s)}
ightarrow Mg^{2+}_{(aq)} + 2e^-$ (oxidation, 2 electrons lost)
- Reduction half - reaction: $2Ag^{+}_{(aq)}+2e^-
ightarrow 2Ag_{(s)}$ (reduction, 2 electrons gained)
- Reducing agent: $Mg_{(s)}$ (because it is oxidized, loses electrons)
- Oxidizing agent: $Ag^{+}_{(aq)}$ (because it is reduced, gains electrons)

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QUESTION IMAGE

Question

Explanation:

Step1: Identify Oxidation Half - Reaction

Step2: Identify Reduction Half - Reaction

Step3: Identify Oxidizing and Reducing Agents

Answer: