Advertisements
Advertisements
प्रश्न
Why are Mn2+ compounds more stable than Fe2+ towards oxidation to their +3 state?
Advertisements
उत्तर
- The electronic configuration of Mn2+ is [Ar]18 3d5 while that of Fe2+ is [Ar] 3d6.
- Since Mn2+ has a half-filled orbit (3d5), which is more stable than the 3d6 orbit of Fe2+, Mn2+ compounds are not easily oxidised to Mn3+ because of the very high second ionization enthalpy.
- In contrast, Fe2+ compounds are easily oxidised to Fe3+ due to a lower second ionization enthalpy.
- This is the reason that Mn2+ compounds are more stable than Fe2+ towards oxidation to their +3 state.
APPEARS IN
संबंधित प्रश्न
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Write the element which shows maximum number of oxidation states. Give reason.
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Electronic configurations
NF3 is possible, but NF5 is not. Why?
Following are the transition metal ions of 3d series:
Ti4+, V2+, Mn3+, Cr3+
(Atomic numbers: Ti = 22, V = 23, Mn = 25, Cr = 24)
Answer the following:
1) Which ion is most stable in an aqueous solution and why?
2) Which ion is a strong oxidising agent and why?
3) Which ion is colourless and why?
Complete and balance the following chemical equations
`Fe^(2+) + MnO_4^(-) + H^+ ->`
Why does the density of transition elements increase from Titanium to Copper? (at. no. Ti = 22, Cu = 29)
Which among the following transition metal has the lowest melting point?
Electronic configuration of Mn2+ is ____________.
When \[\ce{KMnO4}\] solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because ______.
Mention the type of compounds formed when small atoms like H, C and N get trapped inside the crystal lattice of transition metals. Also give physical and chemical characteristics of these compounds.
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?
Which of the following is non-metallic?
On strong heating AgNO3, the gases evolved are:-
The product of oxidation of I– with \[\ce{MnO^{-}4}\] in alkaline medium is:-
On adding NaOH, solution to the aqueous solution of K2CrO7 the colour of the solution changes from
A transition element X has an electronic configuration [Ar]4s23d3. Predict its likely oxidation states.
Consider the following standard electrode potential values:
\[\ce{Sn^{2+}_{ (aq)} + 2e^- -> Sn_{(s)}}\]; E0 = −0.14 V
\[\ce{Fe^{3+}_{ (aq)} + e^- -> Fe^{2+}_{ (aq)}}\]; E0 = +0.77 V
What is the cell reaction and potential for the spontaneous reaction that occurs?
Why are interstitial compounds well known for transition metals?
Decide which of the following atomic numbers are the atomic numbers of the inner transition elements:
29, 59, 74, 95, 102, 104
