Final answer:
The bond described has a δen value of 1.5, indicating a polar covalent bond. The correct descriptions of the bond are: a) The dipole moment of the bond is not zero. b) The two bonded atoms are not necessarily the same. c) The bond is a covalent bond. d) None of the bonded atoms are necessarily metal.
Step-by-step explanation:
To determine whether the descriptions of the bond are correct, we need to analyze the given information. The δen represents the electronegativity difference between the two bonded atoms. A δen of 1.5 indicates a polar covalent bond, where one atom has a partial positive charge and the other has a partial negative charge. Therefore, the correct descriptions of the bond are:
- a) The dipole moment of the bond is not zero, as it is a polar covalent bond.
- b) The two bonded atoms are not necessarily the same, as polar covalent bonds can form between different atoms with differing electronegativities.
- c) The bond is a covalent bond, specifically a polar covalent bond.
- d) None of the bonded atoms are necessarily metal, as polar covalent bonds can form between non-metal atoms.