Calcium carbide ($$CaC_2$$) is an ionic compound consisting of $${Ca^{2+}}$$ and carbide ions $${C_2^{2-}}$$. In this compound, the two carbon atoms are bonded together in the carbide ion $${C_2^{2-}}$$. The bonding in the carbide ion involves one sigma ($$\sigma$$) bond and two pi ($$\pi$$) bonds, which forms a triple bond between the two carbon atoms.

The reasoning is as follows:

Each carbon atom in the $${C_2^{2-}}$$ ion is sp hybridized, having one sigma ($$\sigma$$) bond from the overlap of sp hybrid orbitals and two pi ($$\pi$$) bonds from the lateral overlap of p orbitals. Therefore, the carbide ion $${C_2^{2-}}$$ has a carbon-carbon triple bond.

Thus, the correct option is:

Option B: one sigma ($$\sigma$$) and two pi ($$\pi$$) bonds