Identify the oxidizing agent and the reducing agent for mg(s)+fe2+(aq)→mg2+(aq)+fe(s). express your answers as chemical formulas
separated by a comma.
2 answers:
The Mg element is the reducing agent and the Fe element is the oxidizing agent
<h3>Further explanation</h3>The oxidation-reduction reaction or abbreviated as Redox is a chemical reaction in which there is a change in oxidation number
3 basic theories explain this Redox concept:
- 1. Binding/release of oxygen
The oxidation reaction is the binding of a substance with oxygen. (O₂)
For example:
2SO₂ + O₂ ----> 2SO₃
The reduction reaction is the release of oxygen from a substance.
For example:
2CuO → 2Cu + O₂
- 2. Electron release / binding reaction
Oxidation is an electron release event
Example:
2F ---> 2Fe³⁺ + 6e⁻
The reduction is an electron capture event
Example:
3O₂ + 6e⁻ ---> 3O²⁻
- 3. The reaction of addition/reduction of oxidation number
Oxidation is an increase/increase in oxidation number, while reduction is a decrease in oxidation number.
In the redox reaction, it is also known
Reducing agents are substances that experience oxidation
The oxidizing agent is a substance that is reduced
The formula for determining Oxidation Numbers in general:
1. Single element atomic oxidation number = 0. Examples of Ar, Mg, Cu, Fe, N₂, O₂, etc. = 0
Group IA (Li, Na, K, Rb, Cs, and Fr): +1
Group IIA (Be, Mg, Ca, Sr and Ba): +2
H in compound = +1, except metal hydride compounds (Hydrogen which binds to IA or IIA groups) oxidation number H= -1, for example, LiH, MgH₂, etc.
2. Oxidation number O in compound = -2, except OF2 = + 2 and in peroxide (Na₂O₂, BaO₂) = -1 and superoxide, for example KO₂ = -1/2.
3 The oxidation number in an uncharged compound = 0,
Total oxidation number in ion = ion charge, Example NO₃⁻ = -1
Redox reactions are reactions that are accompanied by changes in oxidation numbers, so what must be examined is whether there are elements that experience changes in oxidation numbers in the reaction
Let's look at the reaction
Mg(s)+Fe²⁺(aq)→Mg²⁺(aq)+Fe(s)
Let see the change in the oxidation number of each element
Mg on the left = 0 (single element)
Fe²⁺ on the left = +2 ( ion charge)
Mg on the right = +2 ( ion charge)
Fe on the right = 0 (single element)
Means that the element Mg has increased oxidation number from 0 to +2 so that it experiences an oxidation reaction and acts as a reducing agent
While Fe has decreased the oxidation number from +2 to 0, so it has a reduction reaction and acts as an oxidizer
<h3>Learn more</h3>an oxidation-reduction reaction
a reducing agent
element is reduced
Keywords: oxidation-reduction, an oxidizing agent, a reducing agent
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.
Explanation :
The given balanced chemical reaction is,
From the given balanced reaction, we conclude that the 2 moles of silver iodide react with the 1 mole of sodium sulfide to give product as 1 mole of silver sulfide and 2 moles of sodium iodide.
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Therefore, in a chemical reaction the products are Silver sulfide and Sodium iodide.
<u>Answer:</u> The correct answer is Option D.
<u>Explanation:</u>
Reduction reaction is defined as the reaction in which a substance gains electrons. Here, the oxidation state of the substance decreases.
Oxidizing agents are the agents that helps in the oxidation of other substance and itself gets reduced. These agents undergoes reduction reactions.
Oxidation reaction is defined as the reaction in which a substance looses its electrons. Here, oxidation state of the substance increases.
Reducing agents are the agents that helps in the reduction of the other substance and itself gets oxidized. These agents undergoes reduction reactions.
Oxidation state is the number which is given to an atom when it looses or gains electron. It is written as a superscript. In a compound, the total charge is equal to the sum of the charges of all atoms in that compound. <u>For Example:</u> In , manganese has +7 oxidation number and oxygen has -2.
So, the charge on the compound =
Hence, the correct answer is Option D.