Transition elements have unpaired electrons. More the number of unpaired electrons more will be the enthalpy of atomization.
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Mn2+ has more stable configuration than Mn3+ while Fe3+ has more stable configuration than Fe2+ consequently , large third ionisation enthalpy is required to change Mn2+ to Mn3+.As E0 is the sum of enthalpy of atomisation, ionization enthalpy and hydration enthalpy therefore E0 for Mn3+/Mn2+ couple is more positive than Fe3+/Fe2+ or Cr3+/Cr2+.☺️
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because they have large Number of unpaired electrons
Enthalpy of atomization is the energy required to break the metal lattice into individual atoms
so due to large number of unpaired electrons large energy is required this energy is the enthalpy of atomization hence it is large
Enthalpy of atomization is the energy required to break the metal lattice into individual atoms
so due to large number of unpaired electrons large energy is required this energy is the enthalpy of atomization hence it is large
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Dear the student , the answer for your question is;
due to variable unpaired valence electrons present in the series the enthalpy of atomisation is high;
and Mg^2+ has the maximum enthalpy of atomization and Zn^2+ has the minimum enthalpy of atomization ;
hope this is useful
due to variable unpaired valence electrons present in the series the enthalpy of atomisation is high;
and Mg^2+ has the maximum enthalpy of atomization and Zn^2+ has the minimum enthalpy of atomization ;
hope this is useful
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Transition elements have high effective nuclear charge and a large number of valence electrons. Therefore, they form very strong metallic bonds. As a result, the enthalpy of atomization of transition metals is high.
OR Enthalpy of atomisation is directly proportional to lone pair of electrons in its valence shell.
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Transition elements have high effective nuclear charge and a large number of valence electrons. Therefore, they form metallic bonds. So enthalpy of atomization of transition metals is very high.
#. The enthalpies of atomisation of the elments in the first transition series are lower than those of the correspondingl elements in the seconde and third transion series.
#. The enthalpies of atomisation of the elments in the first transition series are lower than those of the correspondingl elements in the seconde and third transion series.
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it is because from left to right the nuclear charge increases and unpaired electron also increases from 1 to five therefore they will be having greater in the atomic interaction which causes grey metallic bonding therefore to break the strong metallic Bond we need hire in Alleppey of atomic station
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