Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to each end of the bond. the first bond is between c and o. the second bond is between o and c l. the third bond is between o and f. the fourth bond is between c and n. the fifth bond is between c l and c. the sixth bond is between s and h. the seventh bond is between s and c l.

(δ+) C → O (δ-)

(δ-) O ← Cl (δ+)

(δ+) O → F (δ-)

(δ+) C → N (δ-)

(δ-) Cl ← C (δ+)

(δ-) S ← H (δ+)

(δ+) S → Cl (δ-)

Explanation:

The polarity of a bond depends on the difference of electronegativity (EN) between the atoms that form it. The dipole moment (μ) points to the atom with the highest electronegativity, which is the one with a negative charge density (δ-), while the other atom has a positive charge density (δ+).

The first bond is between C and O.

EN(C) = 2.5; EN (O) = 3.5

(δ+) C → O (δ-)

The second bond is between O and Cl.

EN(O) = 3.5 ; EN(Cl) = 3.0

(δ-) O ← Cl (δ+)

The third bond is between O and F.

EN(O) = 3.5; EN(F) = 4.0

(δ+) O → F (δ-)

The fourth bond is between C and N.

EN(C) = 2.5; EN(N) = 3.0

(δ+) C → N (δ-)

The fifth bond is between Cl and C.

EN(Cl) = 3.0; EN(C) = 2.5

(δ-) Cl ← C (δ+)

The sixth bond is between S and H.

EN(S) = 2.5; EN(H) = 2.1

(δ-) S ← H (δ+)

The seventh bond is between S and Cl.

EN(S) = 2.5; EN(Cl) = 3.0

(δ+) S → Cl (δ-)