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Oxidation Number - Practice Questions & MCQ
Edited By admin | Updated on Sep 18, 2023 18:35 AM | #JEE Main
Quick Facts
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Oxidation Number and Oxidation State is considered one of the most asked concept.
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67 Questions around this concept.
Solve by difficulty
In which compound does Vanadium have an oxidation number of +4?
When KMnO4 acts as an oxidising agent and ultimately forms then the number of electrons transferred in each case respectively is
Which of the following is a redox reaction?
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Which of the following chemical reactions depict the oxidising behaviour of ?
Oxidiation states of P in and
are respectively
Which of the following cannot function as an oxidising agent?
Reduction potential of ions are given below:
$\begin{array}{ccc}\mathrm{ClO}_4^{-} & \mathrm{IO}_4^{-} & \mathrm{BrO}_4^{-} \\ \mathrm{E}^{\circ}=1.19 \mathrm{~V} & \mathrm{E}^{\circ}=1.65 \mathrm{~V} & \mathrm{E}^{\circ}=1.74 \mathrm{~V}\end{array}$
The correct order of their oxidizing power is.
In acidic medium, $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ shows oxidizing action as represented in the half reaction. $\mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{XH}^{+}+\mathrm{Ye}^{-} \rightarrow 2 \mathrm{~A}+\mathrm{ZH}_2 \mathrm{O}$
$\mathrm{X}, \mathrm{Y}, \mathrm{Z}$ and $\mathrm{A}$ respectively are :
Concepts Covered - 1
Oxidation Number and Oxidation State
Oxidation
It is a process that involves the loss of electrons by the atoms or ions.
Reduction
It is a process that involves the gain of electrons by the atoms or ions.
Any reaction, in which the electrons are exchanged between atoms or ions, represents a simultaneous process of oxidation and reduction and is called as a Redox Reaction.
In a Redox Reaction, the species that loses electron (i.e., gets oxidised) is known as reducing agent or reductant, (since it causes reduction of other species), the species which accepts electrons from reductant (i.e., gets reduced) is known as oxidising agent or oxidant (as it causes oxidation of other species).
Oxidation State (O.S.): It refers to the hypothetical charge on atoms in a compound if all the bonds were assumed to be 100% ionic.
Oxidation state, many times, is also referred to as Oxidation Number.
This means oxidation number of an element in a compound is equal to the oxidation state of that element multiplied by total atoms of that element in a particular compound.
(i) In ionic compounds, it is simply the charge on corresponding cation and anion which is expressed as the oxidation state of that particular element. For example, the oxidation state of potassium and chlorine in potassium chloride (KCl) is simply +1 and –1 respectively as KCl is treated as K+Cl–.
Refer to the following examples where oxidation states are written above the atoms:
| +2-1 | +2-2 | +3-1 | +1+6-2 |
| MgCl2 | CaS | AlCl3 | K2SO4 |
NOTE: (a) In MgCl2 and AlCl3, -1 is the oxidation state of Cl.
(b) In each of the cases, the sum of oxidation number of all atoms of all kinds is equal to zero since the compound is neutral.
(ii) In Covalent Compounds, it is not so easy to assign oxidation state of an atom. In order to simplify the concept, we are going to define a set of rules which would enable us to assign oxidation state to every element in any compound.
Rules for Assigning Oxidation State (O.S.) and Oxidation Number (O.N.):
- Any element in free state is assigned an oxidation state of zero. For example: O.S. of H, P, S, O in H2, P4, S8, O2 respectively is zero.
- The oxidation state of any cation or anion (of form A+ or B-) is equal to the magnitude of its charge. For example: O.S of Ca in Ca2+ = +2 and O.S of Al in Al3+ = +3.
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The algebraic sum of the oxidation number of all atoms in a neutral compound is equal to 0. The algebraic sum of the oxidation numbers of all atoms in an ion (like PO43-) is equal to charge on the ion.
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The oxidation states of Alkali Metals (Group IA) is +1 in all of their compounds and that of Alkaline Earth elements (Group IIA) is +2 in all of their compounds.
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Hydrogen in almost all of its compounds is assigned an oxidation state of +1. The exception occurs when hydrogen forms compounds with strong metals like KH, NaH, MgH2, CaH2, etc. In all of these, the oxidation state of hydrogen is -1.
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Oxygen in almost all of its compounds is assigned an oxidation state of -2. But in certain compounds like Peroxides(H2O2), the oxidation state of oxygen is -1. Another exception is OF2, where O.S. is +2. O2F2, where O.S. is +1 and KO2 in which O.S. is -1/2.
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Fluorine is most electronegative element and is assigned an O.S. of -1, in all its compounds. For other halogens, O.S. is generally -1 except when they are bonded to a more electronegative halogen or oxygen. O.S. of iodine in IF7 is +7, O.S. of chlorine in KClO3 is +5.
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Generally, an element with greater electronegativity is assigned -1 by hypothetical breaking of one covalent bond.
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