Question

1. arrange the bonds in order of least to greatest polar character (1 point) *

c-o
ge-o
si-f
c-br
c-cl

1. what type of bond exist between a hydrogen and an oxygen atom? (1 point) *

polar covalent
nonpolar covalent
ionic

Explanation:

Question 26

Step1: Recall Electronegativity Difference

The polarity of a bond is determined by the electronegativity difference (\(\Delta \chi\)) between the two atoms. A larger \(\Delta \chi\) means a more polar bond. Electronegativity values (approximate, Pauling scale): \(C = 2.5\), \(O = 3.5\), \(Ge = 2.0\), \(Si = 1.8\), \(F = 4.0\), \(Br = 2.8\), \(Cl = 3.0\).

Step2: Calculate \(\Delta \chi\) for Each Bond

• \(C - O\): \(\Delta \chi = |3.5 - 2.5| = 1.0\)
• \(Ge - O\): \(\Delta \chi = |3.5 - 2.0| = 1.5\)
• \(Si - F\): \(\Delta \chi = |4.0 - 1.8| = 2.2\)
• \(C - Br\): \(\Delta \chi = |2.8 - 2.5| = 0.3\)
• \(C - Cl\): \(\Delta \chi = |3.0 - 2.5| = 0.5\)

Step3: Order by \(\Delta \chi\) (Least to Greatest)

Sort the bonds by their electronegativity differences (smallest to largest): \(C - Br\) (\(0.3\)) < \(C - Cl\) (\(0.5\)) < \(C - O\) (\(1.0\)) < \(Ge - O\) (\(1.5\)) < \(Si - F\) (\(2.2\)).

Hydrogen (\(\chi = 2.1\)) and oxygen (\(\chi = 3.5\)) have an electronegativity difference (\(\Delta \chi = 1.4\)), which is between 0.4 and 1.7 (range for polar covalent bonds). They share electrons unequally, so the bond is polar covalent. Nonpolar covalent has \(\Delta \chi < 0.4\), ionic has \(\Delta \chi \geq 1.7\), so neither applies here.

Answer:

\(C - Br\), \(C - Cl\), \(C - O\), \(Ge - O\), \(Si - F\)

Question 27