Question

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. \(\mathrm{N}-\mathrm{Cl}\) b. \(\mathrm{N}-\mathrm{P}\) c. \(\mathrm{N}-\mathrm{S}\) d. \(\mathrm{N}-\mathrm{C}\)

Short answer

The bond dipoles for the given bonds are: a. N-Cl: arrow pointing from N (δ+) to Cl (δ-) b. N-P: arrow pointing from P (δ+) to N (δ-) c. N-S: arrow pointing from S (δ+) to N (δ-) d. N-C: arrow pointing from C (δ+) to N (δ-)

Step-by-step solution

Electronegativities Values

Using the electronegativity values from the Pauling scale, consider the following information: Electronegativity values: - N (Nitrogen): 3.04 - Cl (Chlorine): 3.16 - P (Phosphorus): 2.19 - S (Sulfur): 2.58 - C (Carbon): 2.55 Now, let's find the bond dipoles for each of the given bonds.

a. N-Cl bond

In this bond, Nitrogen has an electronegativity value of 3.04 and Chlorine has a value of 3.16. Since Chlorine is more electronegative, it will have a partial negative charge (δ-) and will be the negative end of the bond. Nitrogen, being less electronegative, will have a partial positive charge (δ+) and will be the positive end of the bond. The bond dipole will point from Nitrogen towards Chlorine.

b. N-P bond

In the N-P bond, Nitrogen has an electronegativity value of 3.04 and Phosphorus has a value of 2.19. Since Nitrogen is more electronegative, it will have a partial negative charge (δ-) and will be the negative end of the bond. Phosphorus, being less electronegative, will have a partial positive charge (δ+) and will be the positive end of the bond. The bond dipole will point from Phosphorus towards Nitrogen.

c. N-S bond

In the N-S bond, Nitrogen has an electronegativity value of 3.04 and Sulfur has a value of 2.58. Since Nitrogen is more electronegative than Sulfur, it will have a partial negative charge (δ-) and will be the negative end of the bond. Sulfur, being less electronegative, will have a partial positive charge (δ+) and will be the positive end of the bond. The bond dipole will point from Sulfur towards Nitrogen.

d. N-C bond

In the N-C bond, Nitrogen has an electronegativity value of 3.04 and Carbon has a value of 2.55. Since Nitrogen is more electronegative than Carbon, it will have a partial negative charge (δ-) and will be the negative end of the bond. Carbon, being less electronegative, will have a partial positive charge (δ+) and will be the positive end of the bond. The bond dipole will point from Carbon towards Nitrogen. In summary, the bond dipoles for each of the given bonds are as follows: a. N-Cl: arrow pointing from N (positively charged, δ+) to Cl (negatively charged, δ-) b. N-P: arrow pointing from P (positively charged, δ+) to N (negatively charged, δ-) c. N-S: arrow pointing from S (positively charged, δ+) to N (negatively charged, δ-) d. N-C: arrow pointing from C (positively charged, δ+) to N (negatively charged, δ-)