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प्रश्न
Consider the elements: Cs, Ne, I and F
Identify the element that exhibits both positive and negative oxidation states.
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उत्तर
I exhibits both positive and negative oxidation states. It exhibits oxidation states of – 1, + 1, + 3, + 5, and + 7.
संबंधित प्रश्न
Assign oxidation numbers to the underlined elements in the following species:
K2MnO4
Assign oxidation numbers to the underlined elements in the following species:
CaO2
Assign oxidation numbers to the underlined elements in the following species:
H2S2O7
What are the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
KI3
What is the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
Fe3O4
What are the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
CH3CH2OH
The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is not correct in this respect?
In which of the following compounds, an element exhibits two different oxidation states.
The largest oxidation number exhibited by an element depends on its outer electronic configuration. With which of the following outer electronic configurations the element will exhibit largest oxidation number?
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
\[\ce{PbO}\] 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.
\[\ce{PO^{3-}4}\]
Calculate the oxidation number of sulphur atom in the following compounds:
\[\ce{Na2S4O6}\]
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 and covalency of sulphur in sulphur molecules (Sg) are:
The oxidation states of iron atoms in compounds (A), (B) and (C), respectively are x, y, z. The sum of x, y, z is ______.
(A) Na4[Fe(CN)5(NOS)]
(B) Na4[FeO4]
(C) [Fe2(CO)9]
Oxidation number of potassium in K2O, K2O2 and KO2, respectively, is ______.
