Which of the following elements has the lowest melting point ?

The melting point order of IV A group elements is $C > Si > Ge > Pb > Sn$

Which of the following elements has the lowest mel

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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

	List -I (Complex)		List II (Spin only Magnetic Moment)
A)	[CoF₆]^3-	I)	0
B)	[Co(C₂O₄)₃]^3-	II)	√24
C)	[FeF₆]³⁺	III)	√8
D)	[Mn(CN)₆]^3-	IV)	√35
		V)	√15