The type of bonding present in diamond C is covalent bonding. In a covalent bond, atoms share electrons with each other to form a stable electron configuration. In the case of diamond, each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement, with each carbon atom sharing one electron with each of its four neighboring carbon atoms.The reasoning behind this bonding type in diamond is based on the electronegativity of carbon and the nature of the element itself. Carbon has an electronegativity value of 2.55, which is intermediate between the values for metals and nonmetals. This means that carbon does not have a strong tendency to either lose or gain electrons, making ionic and metallic bonding unlikely.Ionic bonding occurs when there is a significant difference in electronegativity between two atoms, causing one atom to transfer its electrons to the other atom, resulting in the formation of positive and negative ions. This is not the case in diamond, as all the atoms involved are carbon atoms with the same electronegativity.Metallic bonding occurs in metals, where electrons are shared among a lattice of positively charged metal ions. This type of bonding results in the formation of a "sea" of delocalized electrons that can move freely throughout the metal lattice, giving metals their characteristic properties such as electrical conductivity and malleability. Since carbon is a nonmetal, it does not exhibit metallic bonding.In summary, the bonding present in diamond C is covalent bonding, as each carbon atom shares electrons with its neighboring carbon atoms in a tetrahedral arrangement. This type of bonding is consistent with the electronegativity of carbon and the fact that it is a nonmetal.