Question

An sp hybridized central carbon atom with no lone pairs of electrons has what type of bonding?

A) 1 pi and 2 sigma bonds D) 3 pi and 2 sigma bonds
B) 1 pi and 3 sigma bonds E) 0 pi and 4 sigma bonds
C) 2 pi and 2 sigma bonds

Answer 1

A central carbon atom that is sp hybridized and has no lone pairs of electrons would have 2 pi bonds and 2 sigma bonds.

Step-by-step explanation:

A central carbon atom that is sp hybridized and has no lone pairs of electrons would have a linear geometry. In terms of bonding, this type of carbon atom would have 2 pi bonds and 2 sigma bonds.

The 2 pi bonds are formed by the overlap of unhybridized p orbitals, and the 2 sigma bonds result from the overlap of hybridized sp orbitals with other atoms.

Overall, the sp hybridized central carbon atom with no lone pairs of electrons would have 2 pi bonds and 2 sigma bonds.