Why does diamond have a much higher hardness compared to graphite?
Diamond has a three-dimensional network with strong bonds
In diamond each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement, forming a rigid three-dimensional network.
Breaking this network needs breaking many strong C–C bonds, so diamond is the hardest natural substance.
In graphite each carbon bonds to three others in flat hexagonal layers held together by weak van der Waals forces; the layers slide over each other, so graphite is soft — it has no metallic bonding or flexible chains.
Hence, diamond is harder because diamond has a three-dimensional network with strong bonds.
Which molecule contains a triple covalent bond?
Which of the following best describes the type of bond formed when a metal reacts with a non-metal?
If a molecule contains a central atom bonded to four other atoms and all bonds are single covalent, what is the most likely shape of this molecule?
Which of the following best describes an ionic bond?
Which property is most commonly associated with ionic compounds?
Which process results in the formation of a molecule of a compound?
Why does magnesium form an Mg2+ ion rather than Mg+ during ionic bond formation?
Ozone is:
Which of the following has sp 3d hybridization?
How many geometrical isomers are possible for the complex $ [Pt(NH_3)_2Cl_2] $?
Sulphur exhibit variable Valency due to
The compound 1, 2-butadiene has: