What kinds of bonds are present in graphite?
In graphite, the C-C bonds in the planes are very strong, but the force between the different planes is quite weak, and they can slip over one another. This explains the "soft" feel of graphite, and the fact that it is used as a lubricant, for example in motor oil.
Other "Big" Covalent Molecules
In solids like diamond and graphite, the different atoms all bond to one another to form one very large molecule. The atoms are bonded to each other in all directions in diamond, and in two directions (within the planes) in graphite, with no bonding in the other direction. Some important covalent molecules involve atoms bonding to each other repeatedly along just one direction, with no bonds in the others. These are called polymers.
chm.bris.ac.uk/pt/harvey/gcse/covalent.html
To follow that link above, just put w w w. ahead of that web link
no, i have options. select and tell me correct one.
hydrogen bond
hydrophobic bond
sigma sp
sigma sp2
sigma sp3
sigma sp4
sigma sp3d1
sigma sp3d2
pi bond
Pi bond
it is wrong
sigma sp2 AND pi bond
Graphite is a form of carbon that consists of covalently-bonded carbon atoms arranged in layers. It has a unique structure where carbon atoms are arranged in a hexagonal lattice, forming flat sheets of interconnected hexagons. In graphite, there are mainly two types of chemical bonds present:
1. Covalent Bonds: Within each layer of graphite, carbon atoms are bonded together through strong covalent bonds. Covalent bonds occur when atoms share electrons to achieve a stable electron configuration. In the case of graphite, each carbon atom forms three covalent bonds with three neighboring carbon atoms in a trigonal planar arrangement.
2. Van der Waals Forces: Between the layers of graphite, weak intermolecular forces, known as Van der Waals forces, exist. These forces occur due to temporary shifts in electron density, which induces a dipole moment in neighboring molecules. Van der Waals forces are relatively weak compared to covalent bonds but still contribute to the overall stability of the graphite structure.
To determine the types of bonds present in graphite, one can consider the molecular and atomic interactions within the material. Covalent bonds are formed through the sharing of electrons, while Van der Waals forces arise from temporary fluctuations in electron distributions. Experimental techniques such as X-ray diffraction and spectroscopy can also provide information about the atomic arrangement and bonding in graphite.