Question:
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
Updated On: Feb 25, 2024
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Solution and Explanation
The oxidation states displayed by the first half of the first row of transition metals are given in the table below
| Oxidation state | Sc | Ti | V | Cr | Mn |
| +2 | +2 | +2 | +2 | ||
| +3 | +3 | +3 | +3 | +3 | |
| +4 | +4 | +4 | +4 | ||
| +5 | +5 | +6 | |||
| +6 | +7 |
It can be easily observed that except Sc, all others metals display +2 oxidation state. Also, on moving from Sc to Mn, the atomic number increases from 21 to 25. This means the number of electrons in the 3d-orbital also increases from 1 to 5.
Sc (+2) = d1
Ti (+2) = d2
V (+2) = d3
Cr (+2) = d4
Mn (+2) = d5
+2 oxidation state is attained by the loss of the two 4selectrons by these metals. Since the number of delectrons in
(+2) state also increases from Ti(+2) to Mn(+ 2), the stability of +2 state increases (as d-orbital is becoming more and
more half-filled). Mn (+2) has d 5electrons (that is half-filled dshell, which is highly stable).
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Concepts Used:
Properties of D Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behavior and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high because of the presence of unpaired electrons and partially filled d orbitals. They form strong bonds and have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements