Oxidation number of Mo in Ammonophosphomolybdate
Oxidation number of Mo in Ammonophosphomolybdate
Correct Answer: 6
Solution and Explanation
Calculation of Oxidation Number of Mo in \((NH_4)_3PMo_{12}O_{40}\)
Given Compound:
\((NH_4)_3PMo_{12}O_{40}\), which can also be written as \((NH_4)_3PO_4.12MoO_3\).
Step-by-Step Calculation:
- Let the oxidation number of Mo be \( x \).
- The oxidation numbers of the other components are:
- \( NH_4^+ \): \( +1 \) (3 ammonium ions contribute \( 3 \times +1 = +3 \)).
- \( P \): \( +5 \) (phosphorus in the phosphate group).
- \( O \): \( -2 \) (oxygen).
- Write the total oxidation number equation for the compound: \[ 3(+1) + (+5) + 12x + 40(-2) = 0 \]
- Simplify the equation: \[ 3 + 5 + 12x - 80 = 0 \]
- Combine terms: \[ 12x = 80 - 8 \]
- Simplify further: \[ 12x = 72 \]
- Divide by 12: \[ x = 6 \]
Conclusion:
The oxidation number of molybdenum (\( Mo \)) in \((NH_4)_3PMo_{12}O_{40}\) is +6.
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Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.