Final answer:
The P-Cl bonds in PCl3 are polar covalent since the electronegativity difference between phosphorus and chlorine falls within the range of 0.5 to 2.0, indicating an unequal sharing of electrons.
Step-by-step explanation:
Using electronegativity values, the P-Cl bonds in PCl3 are polar covalent bonds. The electronegativity difference (Δχ) between phosphorus (XP = 2.19) and chlorine (XCl = 3.16) is about 0.97, which falls within the range of 0.5 to 2.0, indicative of polar covalent bonding.
This means that within the P-Cl bonds, electrons are shared unequally, with a greater electron density surrounding the more electronegative chlorine atoms, leading to a partial negative charge on the chlorine and a partial positive charge on the phosphorus.
The greater electronegativity of chlorine results in a higher electron density around the chlorine atom, giving it a partial negative charge, while the phosphorus atom has a partial positive charge.
Therefore, the P-Cl bonds in PCl3 are polar covalent bonds.