Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]
(a) C―C
(b) C―O
(c) C―H
(d) C―F
(e) C―Cl
(f) C―S

For the molecules shown, indicate the direction of the dipole moment.

(a)

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(a)

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(b)

Carbon dioxide (CO₂) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO₂) does have a dipole moment (μ = 1.6 D) Explain this observation.

Rank the following elements from least electronegative to most electronegative.

Na, Si, F, Mg, C, O, N

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?

(b) N vs. O

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?

(d) B vs. Si

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?

(c) O vs. S