Final answer:
The electronegativity difference in H-Cl is 0.96, indicating a polar covalent bond. Cl-Cl has a difference of 0.00, resulting in a nonpolar covalent bond. For Be-O, assuming an approximate electronegativity for Be, the difference is about 2.0, indicating an ionic bond.
Step-by-step explanation:
To determine the difference in electronegativity for the compounds Hydrochloric acid (H-Cl), Diatomic chlorine (Cl2), and Beryllium oxide (Be-O), we refer to the electronegativity values for each element: XH = 2.20, XCl = 3.16, and XBe is approximately 1.5 (reference needed for precise value), XO = 3.5.
1. For Hydrochloric acid (H-Cl), the difference in electronegativity is XCl - XH = 3.16 - 2.20 = 0.96, indicating a polar covalent bond.
2. For Diatomic chlorine (Cl2), since both atoms are chlorine, the difference in electronegativity is XCl - XCl = 0.00, indicating a nonpolar covalent bond.
3. Although we do not have the exact electronegativity value for beryllium (Be) listed, we can follow the trend that as the electronegativity difference increases between two atoms, the bond becomes more ionic. For Beryllium oxide (Be-O), assuming XBe is approximately 1.5, the difference in electronegativity would be XO - XBe = 3.5 - 1.5 = 2.0, which is quite high and typical of an ionic bond.