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 ______.
विकल्प
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.
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Which element has the highest m.p?
Why do the transition elements have higher enthalpies of atomisation?
How would you account for the following : Transition metals form coloured compounds
Account for the following:
Zn is not considered as a transition element.
In the series Sc (Z = 21) to Zn (Z = 30), the enthalpy of atomization of zinc is the lowest, i.e., 126 kJ mol−1. Why?
Why are Mn2+ compounds more stable than Fe2+ towards oxidation to their +3 state?
Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.
When acidified \[\ce{K2Cr2O7}\] solution is added to \[\ce{Sn^{2+}}\] salts then \[\ce{Sn^{2+}}\] changes to ______.
Identify A to E and also explain the reactions involved.
When a chromite ore (A) is fused with sodium carbonate in free excess of air and the product is dissolved in water, a yellow solution of compound (B) is obtained. After treatment of this yellow solution with sulphuric acid, compound (C) can be crystallised from the solution. When compound (C) is treated with KCl, orange crystals of compound (D) crystallise out. Identify A to D and also explain the reactions.
Why are fluorides of transition metals more stable in their higher oxidation state as compared to the lower oxidation state?
It has been observed that first ionization energy of 5 d series of transition elements are higher than that of 3d and 4d series, explain why?
The element with atomic number 46 belongs to
The product of oxidation of I– with \[\ce{MnO^{-}4}\] in alkaline medium is:-
Give reason for the following statement:
Physical and chemical properties of the 4d and 5d series of the transition elements are quite similar to expected.
Account for the following:
Sc3+ is colourless whereas Ti3+ is coloured in an aqueous solution.
Consider the following standard electrode potential values:
\[\ce{Fe^{3+}_{ (aq)} + e^- -> Fe^{2+}_{ (aq)}}\], E0 = +0.77 V
\[\ce{MnO^{-4}_{ (aq)} + 8H^+ + 5e^- -> Mn^{2+}_{ (aq)} + 4H2O_{(l)}}\], E0 = +1.51 V
What is the cell potential for the redox reaction?
The second ionization enthalpies of chromium and manganese are 1592 and 1509 kJ/mol respectively. Explain the lower value of Mn.
