Using the symbols \(\delta\) - and \(\delta+\), indicate the direction of polarity, if any, in each covalent bond. (a) \(\mathrm{C}-\mathrm{Cl}\) (b) \(\mathrm{S}-\mathrm{H}\) (c) \(\mathrm{C}-\mathrm{S}\) (d) \(\mathrm{P}-\mathrm{H}\)

You can find the electronegativity values of the elements in the periodic table or any chemistry reference material. Here are the approximate electronegativity values for the relevant elements: - Carbon (C): 2.5 - Chlorine (Cl): 3.0 - Sulfur (S): 2.5 - Hydrogen (H): 2.1 - Phosphorus (P): 2.1

Determine which atom in each bond has a higher electronegativity value. The atom with a higher value will have a partial negative charge (\(\delta-\)), while the atom with a lower value will have a partial positive charge (\(\delta+\)). (a) \(\mathrm{C}-\mathrm{Cl}\): Carbon (C) has an electronegativity value of 2.5, while Chlorine (Cl) has a value of 3.0. Since Cl has a higher electronegativity value, the bond will have a polarity as follows: $$\mathrm{C}\delta^+ - \mathrm{Cl}\delta^-$$ (b) \(\mathrm{S}-\mathrm{H}\): Sulfur (S) has an electronegativity value of 2.5, while Hydrogen (H) has a value of 2.1. Since S has a higher electronegativity value, the bond will have a polarity as follows: $$\mathrm{S}\delta^- - \mathrm{H}\delta^+$$ (c) \(\mathrm{C}-\mathrm{S}\): Carbon (C) and Sulfur (S) both have electronegativity values of 2.5. Since they have equal values, there is no polarity in this bond. The bond can be represented as: $$\mathrm{C} - \mathrm{S}$$ (d) \(\mathrm{P}-\mathrm{H}\): Phosphorus (P) has an electronegativity value of 2.1, while Hydrogen (H) has a value of 2.1 as well. Since they have equal values, there is no polarity in this bond. The bond can be represented as: $$\mathrm{P} - \mathrm{H}$$