Question:
Graphite is soft while diamond is hard because:
Graphite is soft while diamond is hard because:
Updated On: Jun 7, 2022
- Graphite is in powder form
- diamond has $s p^{2}$ hybridisation but graphite has $s p^{3}$ hybridisation
- Graphite is in planar form while diamond is in tetrahedral form
- Graphite is covalent and diamond is ionic.
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The Correct Option is C
Solution and Explanation
In diamond each carbon atom is $s p^{3}$ hybridised and is joined to each other by strong covalent bond to form a tetrahedral structure. While in graphite carbon atoms form planar, hexagonal rings to give it a sheet like structure. Each sheet is joined to each other by weak van der Waal force. Hence diamond is harder than graphite.
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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