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Within each transition series, the oxida...

Within each transition series, the oxidation states

A

first increase till the middle of the period and then decrease

B

decrease regularly in moving form left to right

C

first increase till the middle of period and then increase

D

increase regularly in moving from left to right

Text Solution

Verified by Experts

The correct Answer is:
A
There exists a general trend of lesser number of oxidation states at each end of the series and a higher number in the middle. The lesser number of oxidation states in the beginning of the series is due to the presence of too few (n - 1) d electrons to lose or share, towards the end of the series it can be ascribed to the presence of too many (n - 1) d electrons and thus fewer unpaired electrons as well as empty orbitals to share electrons with the ligands.
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The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In 3d series, the maximum oxidation state is shown by

The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In which of the following pairs , the first species is more stable than second one

The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . Identify the correct statement

An element of 3d-transition series shows two oxidation states x and y, differing by two units. Then:

In which complex is the transition metal in zero oxidation state:

R SHARMA-THE D AND F BLOCK ELEMENTS-Question Bank (Building the Knowledge)
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