Advertisements
Advertisements
Question
What are the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
H2S4O6
Solution
H2S4O6
| +1 | x | -2 |
| H2 | SO4 | O6 |
Now 2(+1) + 4(x) + 6(-2) = 0
⇒ 2 + 4x - 12 = 0
⇒ 4x = 10
⇒ `x = +2 1/2`
However, O.N. cannot be fractional. Hence, S must be present in different oxidation states in the molecule.
\[\begin{array}{cc}
\ce{O}\phantom{..........}\ce{O}\\
||\phantom{...........}||\\
\ce{H - O - S - S - S - S - O - H}\\
||\phantom{...........}||\\
\ce{O}\phantom{..........}\ce{O}
\end{array}\]
The O.N. of two of the four S atoms is +5 and the O.N. of the other two S atoms is 0.
APPEARS IN
RELATED QUESTIONS
Assign oxidation numbers to the underlined element in the following species:
NaH2PO4
Assign oxidation numbers to the underlined element in the following species:
H4P2O7
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 is the oxidation numbers of the underlined elements in the following and how do you rationalise your results?
Fe3O4
What is the oxidation numbers 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.
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?
\[\ce{PbO}\] 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 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) \[\ce{Cr2O^{2-}7}\] | (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 ______.
Oxidation number of potassium in K2O, K2O2 and KO2, respectively, 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 ______.
