Advertisements
Advertisements
Question
In which of the following compounds, an element exhibits two different oxidation states.
Options
\[\ce{NH2OH}\]
\[\ce{NH4NO3}\]
\[\ce{N2H4}\]
\[\ce{N3H}\]
Solution
\[\ce{NH4NO3}\]
Explanation:
The oxidation states are given below:
In \[\ce{NH2OH}\] oxidation of N is – 1.
\[\ce{NH4NO3}\] exists as \[\ce{NH^{+}4 . NO^{-}3}\],
Thus, the oxidation state of N in \[\ce{NH^{+}4}\] is – 3 while in \[\ce{NO^{-}3}\] is + 5.
In \[\ce{N2H4}\] oxidation of N is – 2
In \[\ce{N2H}\] oxidation of N is `(-1)/3`.
APPEARS IN
RELATED QUESTIONS
Assign oxidation numbers to the underlined element in the following species:
NaH2PO4
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
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.
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?
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 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?
Oxidation number of potassium in K2O, K2O2 and KO2, respectively, is ______.
