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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?
विकल्प
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:
NaH2PO4
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
What is the oxidation number of the underlined elements in the following and how do you rationalise your results?
CH3COOH
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 only postive oxidation state.
Consider the elements : Cs, Ne, I and F
Identify the element which exhibits neither the negative nor does the positive oxidation state.
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.
Calculate the oxidation number of phosphorus in the following species.
\[\ce{HPO^{2-}3}\]
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 |
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?
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 ______.
