single covalent bond between each carbon.
Diamond and Graphite both have single covalent bonds whereas Buckminsterfullerene has double covalent bonds.
Graphite is a pure carbon compound with layers. The carbon bonds used are single covalent bonds.
Van der Waals interactions
covalent
Graphite is a giant molecule bonded with covalent bonds.Some of the bonds involve delocalised electrons.
Diamond and Graphite both have single covalent bonds whereas Buckminsterfullerene has double covalent bonds.
Graphite is a pure carbon compound with layers. The carbon bonds used are single covalent bonds.
They are most similar to delocalised bonds such as in graphite. Sometimes described as lattice of metal ions in a cloud of electrons they have little in common with covalent bonds or ionic bonds.
Covalent bonds are formed by sharing of electrons between the atoms. They are usually weaker than the ionic bonds but there are exceptions such as diamond and graphite.
Van der Waals interactions
covalent
covalent
In almost all cases, ionic bonds are stronger than covalent bonds. Although there are exceptions such as diamond and graphite.
Graphite is a giant molecule bonded with covalent bonds.Some of the bonds involve delocalised electrons.
covalent bonds
Ionic compounds are said to be the compounds that form relatively stronger bonds. But there are exceptions such as diamond, graphite and carborundum which are covalent compounds.
covalent bonds