Advertisements
Advertisements
प्रश्न
Calculate the oxidation number of sulphur atom in the following compounds:
\[\ce{Na2SO4}\]
Advertisements
उत्तर
Let x = oxidation number of sulphur, and +1 is oxidation number of \[\ce{Na}\], –2 is oxidation number of \[\ce{O}\], also we can assume total charge on compound = 0 then solving we get.
+2 + x – 8 = 0
x = +6.
APPEARS IN
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
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
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 that exhibits both positive and negative oxidation states.
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
Calculate the oxidation number of phosphorus in the following species.
\[\ce{HPO^{2-}3}\]
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) | 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 P in Mg2P207 is ____________.
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]
In which of the following species oxidation number of the element(s) is equal to + 4?
In which of the following species, the oxidation number of the atom of the underlined elements is/are equal to +1?
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 ______.
Oxidation state of sulphur in anions `"SO"_3^(2-)`, `"S"_2"O"_4^(2-)` and `"S"_2"O"_6^(2-)` increases in the orders:
