Question

How do transition elements differ from the typical elements?

Answer 1

Hint: Transition elements are d-block elements. Transition elements are present in groups 3-12. These elements are present between s-block and p-block elements.

Complete answer:
- The transition elements are those which either as elements or ions have partially filled (n-1) d orbitals. Since these differentiating electrons enter the (n-1)d orbitals, these are also called d-block elements.
- The word transition is used because these elements are placed in between the electropositive metals (s-block element) and electronegative non-metal (p-block elements).
- Transition elements are less reactive than the alkali and alkaline earth metals. The low reactivity of transition elements is due to high ionization energy.
- As valence electrons of transition elements present in ns and (n-1)d orbitals, all transition elements except the last member of each series exhibit variable oxidation state.
- Most of the transition metals are colour in the solid or solution states.
- Transition metals have a higher melting point than the representative elements.
- Transition elements have a higher density than the representative elements.
- Most of the transition elements are paramagnetic and form colour complexes.
- Transition elements are less electropositive than the s-block elements.
- Transition elements form covalent bonds while s-block elements form an ionic bond.

Note: Elements that lie in between s-block metals and p-block non-metals are known as transition metals. Though they are metals their few properties are different than the s-block metals. In the case of representative elements valence electrons are present in the outermost shell while in the case of transition elements valence electrons are present in ns and (n-1)d orbitals.