Final answer:
The electronegativity difference between atoms helps determine the bond type, and the atom with the higher electronegativity in each pair is the more-electronegative one. Bond types range from nonpolar covalent, with very small differences, to ionic, with larger differences. Examples include H and I forming a nonpolar covalent bond, S and O forming a polar covalent bond, and K and Br forming an ionic bond.
Step-by-step explanation:
To determine the electronegativity difference, probable bond type, and the more-electronegative atom with respect to the bonds formed between the following pairs of atoms, we apply our understanding of electronegativity values:
- H & I: H (2.1) & I (2.5), Difference = 0.4, Bond type: Nonpolar Covalent, More-electronegative: I
- S & O: S (2.5) & O (3.5), Difference = 1.0, Bond type: Polar Covalent, More-electronegative: O
- K & Br: K (0.8) & Br (2.8), Difference = 2.0, Bond type: Ionic, More-electronegative: Br
- Si & Cl: Si (1.8) & Cl (3.0), Difference = 1.2, Bond type: Polar Covalent, More-electronegative: Cl
- H & F: H (2.1) & F (4.0), Difference = 1.9, Bond type: Polar Covalent, More-electronegative: F
- Se & S: Se (2.4) & S (2.5), Difference = 0.1, Bond type: Nonpolar Covalent, More-electronegative: S
- C & H: C (2.5) & H (2.1), Difference = 0.4, Bond type: Nonpolar Covalent, More-electronegative: C