Question

Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to each end of the bond. C-O, O-CL, O-F, C-N, C-L, S-H, S-CL

Answer 1

Answer:

C→O, O→Cl, O→F, C→N, C←Li, S ←H, S→Cl

Explanation:

The general convention for indicating polarity in molecules is that of showing the direction of polarity from the positive to the negative part of the bond. This is indicated in the answer by arrows that show the direction of the dipole.

The negative end of the dipole must be the more electronegative element while the positive end of the dipole is the less electronegative element, hence the answer shown above.

Answer 2

The delta notation, indicating the polarity of for the presented covalent bonds are:

• δ+   C-O   δ-
• δ-   O-Cl   δ+
• δ+   O-F   δ-
• δ+   C-N   δ-
• δ+   C-Cl   δ-
• δ-   S-H   δ+
• δ+   S-Cl   δ-

Polar bonds are those in which atoms have different electronegativities.

The delta notation is used to indicate the direction of the polarity.

The atom with the greater electronegativity acquires a partial negative charge (goes with the symbol δ-), while the atom with the lesser electronegativity acquires a partial positive charge (goes with the symbol δ+).

Let's consider the following elements with their electronegativities.

• C (2.5)
• O (3.5)
• Cl (3.0)
• F (4.0)
• N (3.0)
• S (2.5)
• H (2.1)

The delta notation for the presented bonds are:

• δ+   C-O   δ-
• δ-   O-Cl   δ+
• δ+   O-F   δ-
• δ+   C-N   δ-
• δ+   C-Cl   δ-
• δ-   S-H   δ+
• δ+   S-Cl   δ-

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