The sliping is between the covalently bonded layers in graphite - conventionally the bonding is assumed to be inter -molecular between the layers, principally London dispersion forces..
The bonds are ionic or covalent.
Covalent bonds are formed when atoms share electrons
In almost all cases, ionic bonds are stronger than covalent bonds. Although there are exceptions such as diamond and graphite.
They are bonded by nonpolar covalent bonds. Each of the atoms is sp2 hybridized. It is sometimes depicted as having alternating single and double bonds, but this is not quite accurate. The bonds are subject to what is called resonance so that the bonds are neither single nor double but sort of in between.
Covalent.
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.
Covalent crystals are atoms held together in an extensive three-dimensional network entirely by covalent bonds. Two examples are diamond and graphite (pencil lead)
Diamond and Graphite both have single covalent bonds whereas Buckminsterfullerene has double covalent bonds.
The covalent bonds are their role in combining atoms Is In Your Facee ;D
When atoms are bonded together with covalent bonds, the result is a molecule.
single covalent bond between each carbon.
Graphite is a pure carbon compound with layers. The carbon bonds used are single covalent bonds.
Covalent bonds hold atoms together. Ionic bonds hold ions together
Graphite is made from carbon atoms. The carbon atoms are joined together by things called "covalent bonds". Carbon atoms in graphite form flat sheets, and the atoms are joined together by alternating double and single bonds. A single covalent bond contains two electrons and a double covalent bond contains 4 electrons. These alternating bonds swap positions many times every second, and as a result, electrons can move from one end of the graphite to the other. This is a "Year 9" answer to the question. University physics students would need to discuss virtual particles and a bunch of other quantum mechanical concepts to answer this question properly.
Carbon can atoms can form four covalent bonds with many, many different elements.
Giant covalent, lattice structures contain a lot of non-metal atoms, each joined to adjacent atoms by covalent bonds. The atoms are usually arranged into giant regular lattices. The structure requires an element with very strong bonds between the atoms to create various materials. A couple of examples are (carbon) Diamond and Buckminster Fullerine. Graphite is also one but has weak bonds as well. Silica and molybdenum can also make covalent lattice structures.
covalent bonds.