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प्रश्न
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?
पर्याय
The oxidation number of hydrogen is always +1.
The algebraic sum of all the oxidation numbers in a compound is zero.
An element in the free or the uncombined state bears oxidation number zero.
In all its compounds, the oxidation number of fluorine is – 1.
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उत्तर
The oxidation number of hydrogen is always +1.
Explanation:
Oxidation number of hydrogen is – 1 in metal hydrides like \[\ce{NaH}\].
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संबंधित प्रश्न
Assign oxidation numbers to the underlined element in the following species:
H4P2O7
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:
NaBH4
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
Consider the elements: Cs, Ne, I and F
Identify the element that exhibits only negative oxidation state.
Consider the elements: Cs, Ne, I and F
Identify the element that exhibits both positive and negative 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
Nitric acid is an oxidising agent and reacts with \[\ce{PbO}\] but it does not react with \[\ce{PbO2}\]. Explain why?
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:
\[\ce{Na2S2O3}\]
Match Column I with Column II for the oxidation states of the central atoms.
| Column I | Column II |
| (i) \[\ce{Cr2O^{2-}7}\] | (a) + 3 |
| (ii) \[\ce{MnO^{-}4}\] | (b) + 4 |
| (iii) \[\ce{VO^{-}3}\] | (c) + 5 |
| (iv) \[\ce{FeF^{3-}6}\] | (d) + 6 |
| (e) + 7 |
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:
