To determine the electronegativity difference, probable bond types, and the more electronegative atom between each pair of atoms, we will refer to the Pauling scale of electronegativity. The electronegativities of the relevant elements are as follows:
- Hydrogen (H): 2.20
- Iodine (I): 2.66
- Sulfur (S): 2.58
- Oxygen (O): 3.44
- Potassium (K): 0.82
- Bromine (Br): 2.96
- Silicon (Si): 1.90
- Chlorine (Cl): 3.16
- Fluorine (F): 3.98
- Selenium (Se): 2.55
- Carbon (C): 2.55
Now, let’s analyze each pair:
a. H – I
Electronegativity Difference: |2.20 – 2.66| = 0.46
Bond Type: Polar Covalent
More Electronegative Atom: Iodine
b. S – O
Electronegativity Difference: |2.58 – 3.44| = 0.86
Bond Type: Polar Covalent
More Electronegative Atom: Oxygen
c. K – Br
Electronegativity Difference: |0.82 – 2.96| = 2.14
Bond Type: Ionic
More Electronegative Atom: Bromine
d. Si – Cl
Electronegativity Difference: |1.90 – 3.16| = 1.26
Bond Type: Polar Covalent
More Electronegative Atom: Chlorine
e. H – F
Electronegativity Difference: |2.20 – 3.98| = 1.78
Bond Type: Polar Covalent
More Electronegative Atom: Fluorine
f. Se – S
Electronegativity Difference: |2.55 – 2.58| = 0.03
Bond Type: Nonpolar Covalent
More Electronegative Atom: Sulfur
g. C – H
Electronegativity Difference: |2.55 – 2.20| = 0.35
Bond Type: Polar Covalent
More Electronegative Atom: Carbon