Question:
In graphite, electrons are
In graphite, electrons are
Updated On: Apr 17, 2024
- localised on each C-atom
- localised on every third C-atom
- spread out between the structure
- Both (b) and (c)
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The Correct Option is D
Solution and Explanation
Structure of graphite consist of a two dimensional sheet like network joined together in hexagonal rings. These layers are held together by weak van der Waals' forces. In graphite each carbon atom is bonded to three others, forming $sp^2$ hybrid bonds. The fourth electron forms a $\pi$-bond. Graphite is a conductor of electricity which is due to the fact that all the carbon bonds being not satisfied. Thus, some of the electrons are free to move through the crystal.
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Concepts Used:
P-Block Elements
- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
- P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
P block elements consist of:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family