difference between the 1st,2nd and 3rd transition series?? pls answ
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In the 1st, 2nd and 3rd transition series, the 3d, 4d and 5dorbitals are respectively filled.
We know that elements in the same vertical column generally have similar electronic configurations.
In the first transition series, two elements show unusual electronic configurations:
Cr(24) = 3d5 4s1
Cu(29) = 3d10 4s1
Similarly, there are exceptions in the second transition series. These are:
Mo(42) = 4d5 5s1
Tc(43) = 4d6 5s1
Ru(44) = 4d7 5s1
Rh(45) = 4d8 5s1
Pd(46) = 4d10 5s0
Ag(47) = 4d10 5s1
There are some exceptions in the third transition series as well. These are:
W(74) = 5d4 6s2
Pt(78) = 5d9 6s1
Au(79) = 5d10 6s1
As a result of these exceptions, it happens many times that the electronic configurations of the elements present in the same group are dissimilar.
(ii) In each of the three transition series the number of oxidation states shown by the elements is the maximum in the middle and the minimum at the extreme ends.
However, +2 and +3 oxidation states are quite stable for all elements present in the first transition series. All metals present in the first transition series form stable compounds in the +2 and +3 oxidation states. The stability of the +2 and +3 oxidation states decreases in the second and the third transition series, wherein higher oxidation states are more important.
For example 1st translition elements form stable complexes, but no such complexes are known for the second and third transition series such as Mo, W, Rh, In. They form complexes in which their oxidation states are high. For example: WCl6, ReF7, RuO4, etc.
(iii) In each of the three transition series, the first ionisation enthalpy increases from left to right. However, there are some exceptions. The first ionisation enthalpies of the third transition series are higher than those of the first and second transition series. This occurs due to the poor shielding effect of 4felectrons in the third transition series.
Certain elements in the second transition series have higher first ionisation enthalpies than elements corresponding to the same vertical column in the first transition series. There are also elements in the 2nd transition series whose first ionisation enthalpies are lower than those of the elements corresponding to the same vertical column in the 1st transition series.
(iv) Atomic size generally decreases from left to right across a period. Now, among the three transition series, atomic sizes of the elements in the second transition series are greater than those of the elements corresponding to the same vertical column in the first transition series. However, the atomic sizes of the elements in the third transition series are virtually the same as those of the corresponding members in the second transition series. This is due to lanthanoid contraction.
We know that elements in the same vertical column generally have similar electronic configurations.
In the first transition series, two elements show unusual electronic configurations:
Cr(24) = 3d5 4s1
Cu(29) = 3d10 4s1
Similarly, there are exceptions in the second transition series. These are:
Mo(42) = 4d5 5s1
Tc(43) = 4d6 5s1
Ru(44) = 4d7 5s1
Rh(45) = 4d8 5s1
Pd(46) = 4d10 5s0
Ag(47) = 4d10 5s1
There are some exceptions in the third transition series as well. These are:
W(74) = 5d4 6s2
Pt(78) = 5d9 6s1
Au(79) = 5d10 6s1
As a result of these exceptions, it happens many times that the electronic configurations of the elements present in the same group are dissimilar.
(ii) In each of the three transition series the number of oxidation states shown by the elements is the maximum in the middle and the minimum at the extreme ends.
However, +2 and +3 oxidation states are quite stable for all elements present in the first transition series. All metals present in the first transition series form stable compounds in the +2 and +3 oxidation states. The stability of the +2 and +3 oxidation states decreases in the second and the third transition series, wherein higher oxidation states are more important.
For example 1st translition elements form stable complexes, but no such complexes are known for the second and third transition series such as Mo, W, Rh, In. They form complexes in which their oxidation states are high. For example: WCl6, ReF7, RuO4, etc.
(iii) In each of the three transition series, the first ionisation enthalpy increases from left to right. However, there are some exceptions. The first ionisation enthalpies of the third transition series are higher than those of the first and second transition series. This occurs due to the poor shielding effect of 4felectrons in the third transition series.
Certain elements in the second transition series have higher first ionisation enthalpies than elements corresponding to the same vertical column in the first transition series. There are also elements in the 2nd transition series whose first ionisation enthalpies are lower than those of the elements corresponding to the same vertical column in the 1st transition series.
(iv) Atomic size generally decreases from left to right across a period. Now, among the three transition series, atomic sizes of the elements in the second transition series are greater than those of the elements corresponding to the same vertical column in the first transition series. However, the atomic sizes of the elements in the third transition series are virtually the same as those of the corresponding members in the second transition series. This is due to lanthanoid contraction.
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Answered by
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Their reactivity increase from 1st to 3rd transition series. The is no much difference between the 2nd and 3rd due to the lanthanoid contractions
Oxidation state : the 1st series shows maximum of +6 oxidation state while the 2nd and 3rd shows +8 oxidation state.
Stability complex : the frist series make stable complex with Cr and Cu while the second series make stable complex with Fe and Ag etc while the third series make stable complex with Pt and Au.
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