Question

1. describe the bond polarity and molecular polarity for both ccl4 and ch2cl2. can the lewis structure of ch2cl2 be drawn differently so that its molecular polarity is different? ch2cl2 is polar ccl4 is nonpolar 3. sketch the possible overlap of pi bonds and sigma bond described below: a. when two s - orbitals form a sigma bond b. when two p - orbitals form a pi bond c. when two p - orbitals form a sigma bond chm 210 - lab 4 63

Explanation:

2.

Bond polarity depends on electronegativity difference between atoms. In \(C - Cl\) bond, \(Cl\) is more electronegative than \(C\), creating a polar bond. In \(CCl_4\), the symmetrical tetrahedral shape causes bond - dipoles to cancel out, making the molecule non - polar. In \(CH_2Cl_2\), the non - symmetrical structure means bond - dipoles don't cancel, so it is polar.

a. Sigma bonds from s - orbitals form by head - on overlap. b. Pi bonds from p - orbitals form by side - on overlap. c. Sigma bonds from p - orbitals form by head - on overlap.

Answer:

The bond polarity in \(C - Cl\) is due to the electronegativity difference with \(Cl\) being more electronegative. \(CCl_4\) is non - polar because of its symmetrical tetrahedral geometry which cancels out bond dipoles. \(CH_2Cl_2\) is polar as its structure is non - symmetrical and bond dipoles don't cancel.

3.