Final answer:
By comparing electronegativity values, we can predict bond types and the more electronegative atom for each pair given. The resulting bonds range from slightly polar covalent to ionic, with the element having higher electronegativity being more likely to attract electrons within the bond.
Step-by-step explanation:
To determine the electronegativity difference, the probable bond type, and the more-electronegative atom in each bond for the provided pairs of atoms, we use the concept that the difference in electronegativity (EN) values can indicate the bond type, ranging from nonpolar covalent to ionic.
For each pair:
- H and I: Iodine is more electronegative than hydrogen. The EN difference suggests the bond will be polar covalent.
- S and O: Oxygen is more electronegative. The EN difference implies a polar covalent bond.
- K and Br: Bromine is more electronegative. Due to the significant EN difference, the bond is likely ionic.
- Si and Cl: Chlorine is more electronegative, leading to a polar covalent bond.
- K and Cl: Chlorine is more electronegative, and the large EN difference indicates an ionic bond.
- Se and S: Selenium is slightly more electronegative, but the bond is still expected to be nonpolar covalent due to the small EN difference.
- C and H: Carbon is more electronegative. The difference is small, so the bond is slightly polar covalent.
This analysis helps predict the type of chemical bond and indicates which atom will have a partial negative charge in a polar covalent bond.