Answer
See the explanation
Work Step by Step
a. $C-H, Si-H, Sn-H$
The polarity of a bond is determined by the electronegativity difference between the two atoms involved. The more electronegative the atom, the more it will attract the shared electrons in the bond, making the bond more polar.
In the group $C-H, Si-H, Sn-H$, the electronegativity values are:
- Carbon (C): 2.55
- Silicon (Si): 1.90
- Tin (Sn): 1.96
The electronegativity difference between C and H is larger than the electronegativity difference between Si or Sn and H. Therefore, the $C-H$ bond will be the most polar in this group.
b. $Al-Br, Ga-Br, In-Br, Tl-Br$
The electronegativity values for the elements in this group are:
- Aluminum (Al): 1.61
- Gallium (Ga): 1.81
- Indium (In): 1.78
- Thallium (Tl): 1.62
- Bromine (Br): 2.96
The electronegativity difference between the group 13 elements (Al, Ga, In, Tl) and Bromine (Br) decreases as you go down the group. Therefore, the $Al-Br$ bond will be the most polar in this group.
c. $C-O$ or $Si-O$
The electronegativity values for the elements in this group are:
- Carbon (C): 2.55
- Silicon (Si): 1.90
- Oxygen (O): 3.44
The electronegativity difference between C and O is larger than the electronegativity difference between Si and O. Therefore, the $C-O$ bond will be the most polar in this group.
d. $O-F$ or $O-Cl$
The electronegativity values for the elements in this group are:
- Oxygen (O): 3.44
- Fluorine (F): 3.98
- Chlorine (Cl): 3.16
The electronegativity difference between O and F is larger than the electronegativity difference between O and Cl. Therefore, the $O-F$ bond will be the most polar in this group.
