Advertisements
Advertisements
प्रश्न
Highest oxidation state of manganese in fluoride is \[\ce{+4 (MnF4)}\] but highest oxidation state in oxides is \[\ce{+7 (Mn2O7)}\] because ______.
पर्याय
fluorine is more electronegative than oxygen.
fluorine does not possess d-orbitals.
fluorine stabilises lower oxidation state.
in covalent compounds fluorine can form single bond only while oxygen forms double bond.
Advertisements
उत्तर
Highest oxidation state of manganese in fluoride is \[\ce{+4 (MnF4)}\] but highest oxidation state in oxides is \[\ce{+7 (Mn2O7)}\] because in covalent compounds fluorine can form single bond only while oxygen forms double bond.
Explanation:
Oxygen has the capacity to form multiple bonds which enables it to form a variety of covalent compounds.
In \[\ce{(Mn2O7)}\] also, 6 oxygen are doubly bonded to two manganese atoms and one oxygen is forming bridge between two.
While in \[\ce{(MnF4)}\], four fluorine atoms are singly bonded to manganese atom giving it a +4 oxidation state.
Therefore, due to capability of oxygen to have multiple bonds in covalent compounds, manganese is having higher oxidation state of +7 in \[\ce{(Mn2O7)}\].
APPEARS IN
संबंधित प्रश्न
Account for the following:
Mn shows the highest oxidation state of +7 with oxygen but with fluorine, it shows oxidation state of +4.
Account for the following:
Cu+2 salts are coloured, while Zn2+ salts are white.
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Which element is a strong oxidising agent in +3 oxidation state and why?
Which of the 3d series of the transition metals exhibits the largest number of oxidation states and why?
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
What is meant by ‘disproportionation’?
NF3 is possible, but NF5 is not. Why?
Assertion: \[\ce{Cu^2+}\] iodide is not known.
Reason: \[\ce{Cu^2+}\] oxidises \[\ce{I^-}\] to iodine.
Assertion: The highest oxidation state of osmium is +8.
Reason: Osmium is a 5d-block element.
When an oxide of manganese (A) is fused with KOH in the presence of an oxidising agent and dissolved in water, it gives a dark green solution of compound (B). Compound (B) disproportionates in neutral or acidic solution to give purple compound (C). An alkaline solution of compound (C) oxidises potassium iodide solution to a compound (D) and compound (A) is also formed. Identify compounds A to D and also explain the reactions involved.
Why are fluorides of transition metals more stable in their higher oxidation state as compared to the lower oxidation state?
The product of oxidation of I– with \[\ce{MnO^{-}4}\] in alkaline medium is:-
Passing H2S gas into a mixture of Mn2+ and Ni2+, Cu2+, ions in an acidified aqueous solution precipitates.
Among the following pairs of ions, the lower oxidation state in aqueous solution is more stable than the other in:-
Which one of the following characters tie of the transition metal is associated with higher catalytic activity?
A complex in which dsp2 hybridisation takes place is ______.
Write the ionic equation for reaction of KI with acidified KMnO4.
A pair of coloured ions is ______.
