The slippery nature of graphite is attributed to? a)covalent bonding b)preserve of sp2 hybridized carbon...

The slippery nature of graphite is attributed to? a)covalent bonding b)preserve of sp2 hybridized carbon c) Layer covalent bonding d)Network covalent bonding

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Answers (4)

isaaq
6 months ago
am sorry, the answer is C. layer covalent bonding not network covalent bonding it was a mistake.
Graphite is Carbon atoms arranged in layers of hexagons (imagine a carbon atom at each corner). These bonds are very strong (hence the potential uses of graphene), but the layers only have weak forces between them. Only a little energy is needed to overcome these forces, so the layers slide over each other. Plus, graphite uses only 3 of its 4 valence electrons in bonding, so has a spare electron which can delocalise and make it carry a current.
isaaq
6 months ago
answer is D.because of the network covalent bonding.
explanation.
Graphite is made of carbon hexagonal patterns that stack on top of each other. This is also known as Pi stacking when we consider the orbitals.
The reason it is slipper is because this stacking is not as rigid as something like NaCl. The stacks can move slightly past each other and when you put something like your finger on it, it "slides" stacks feeling smooth, and not rough. It is like if you stacked small CD's and applied pressure in a certain direction, it would slide on the CD below it and feel like a "smooth" slide.
EmX
6 months ago
Answer is C.
layer covalent bonding.
the carbon atoms in Graphite from flat layers, These layers are arranged in parallel, one above the other.

This is what makes it an excellent lubrixant..
Chinny
6 months ago
Answer is A.
The principal element of graphite is carbon. carbon has 4 valence electrons. In graphite, 3 of the valence electrons participate in covalent bonding with the surrounding carbons. One electron does not participate in bonding.
The carbon in graphite creates layers. And there is no colavent bonds between the layers. The layers though have a van der Waals attraction force between them, which is very weak and lets the layers slide over each other very easily. That's why graphite is slippery in nature.
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