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प्रश्न
What is the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
Fe3O4
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उत्तर
On taking the O.N. of O as - 2, the O.N. of Fe is found to be `+2 2/3`. However, O.N. cannot be fractional.
Here, one of the three Fe atoms exhibits the O.N. of +2 and the other two Fe atoms exhibit the O.N. of +3
| +2 | +3 |
| FeO, | Fe2O3 |
संबंधित प्रश्न
Assign oxidation numbers to the underlined element in the following species:
NaHSO4
Assign oxidation numbers to the underlined elements in the following species:
CaO2
Assign oxidation numbers to the underlined elements in the following species:
NaBH4
Assign oxidation numbers to the underlined elements in the following species:
KAl(SO4)2.12 H2O
What are the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
H2S4O6
In which of the following compounds, an element exhibits two different oxidation states.
The exhibition of various oxidation states by an element is also related to the outer orbital electronic configuration of its atom. Atom(s) having which of the following outermost electronic configurations will exhibit more than one oxidation state in its compounds.
(i) 3s1
(ii) 3d14s2
(iii) 3d24s2
(iv) 3s23p3
The reaction \[\ce{Cl2 (g) + 2OH- (aq) -> ClO- (aq) + Cl- (aq) + H2O (l)}\] represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action.
\[\ce{PbO}\] and \[\ce{PbO2}\] react with \[\ce{HCl}] according to following chemical equations:
\[\ce{2PbO + 4HCl -> 2PbCl2 + 2H2O}\]
\[\ce{PbO2 + 4HCl -> PbCl2 + Cl2 + 2H2O}\]
Why do these compounds differ in their reactivity?
Calculate the oxidation number of phosphorus in the following species.
\[\ce{HPO^{2-}3}\]
Calculate the oxidation number of sulphur atom in the following compounds:
\[\ce{Na2S2O3}\]
Calculate the oxidation number of sulphur atom in the following compounds:
\[\ce{Na2S4O6}\]
Calculate the oxidation number of sulphur atom in the following compounds:
\[\ce{Na2SO4}\]
Match Column I with Column II for the oxidation states of the central atoms.
| Column I | Column II | |
| (i) | Ions having positive charge | (a) +7 |
| (ii) | The sum of oxidation number of all atoms in a neutral molecule |
(b) –1 |
| (iii) | Oxidation number of hydrogen ion \[\ce{(H+)}\] | (c) +1 |
| (iv) | Oxidation number of fluorine in \[\ce{NaF}\] | (d) 0 |
| (v) | Ions having negative charge | (e) Cation |
| (f) Anion |
The oxidation number of U in \[\ce{UO2(NO3)2}\] is ______.
The oxidation number and covalency of sulphur in sulphur molecules (Sg) are:
In which of the following species oxidation number of the element(s) is equal to + 4?
In order to oxidise a mixture of one mole of each of \[\ce{FeC2O4, Fe2(C2O4)3, FeSO4 and Fe2(SO4)3}\] in acidic medium, the number of moles of KMnO4 required is ______.
On reaction with a stronger oxidizing agent like KIO4, hydrogen peroxide with the evolution of O2. The oxidation number of I in KIO4 changes to ______.
