Why do transition metals have strong metallic bonding?
Correct answer: D. Both s and d electrons take part in bonding
- A. Because of high melting point
- B. Because d-electrons of outer shell take part in bonding
- C. Because s-electrons of the outer shell take part in bonding
- D. Both s and d electrons take part in bonding
Explanation
Metallic bonding is a type of chemical bonding that arises from electrostatic attractive forces between conduction electrons in the form of an electron cloud of delocalized electrons. The reason for metallic bonding in transition metals is that they can involve the 3d electrons in the delocalization as well as the 4s. The more electrons you can involve, the stronger the attractions tend to be.
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About Electronic Structure of d-Block Elements
The electronic structure of d-block elements covers the filling of the (n-1)d and ns orbitals, general electronic configurations, and the exceptions shown by chromium and copper. It explains how partially filled d orbitals produce variable oxidation states, coloured ions, magnetic behaviour and complex formation, while distinguishing transition elements from elements with completely filled d subshells.
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