Final answer:
Dioxygen heptafluoride, if it existed, would likely have the formula O2F7 and be covalent, but it is not a known stable molecule. The correct formulas for phosphorus pentachloride, dinitrogen monoxide, iodine heptafluoride, and carbon tetrachloride are PCl5, N2O, IF7, and CCl4 respectively.
Step-by-step explanation:
The formula for dioxygen heptafluoride is not provided in the given options or information. However, we can infer from similar compounds that if it existed, its formula would likely be O2F7. This is based on the fact that dioxygen implies two oxygen atoms, and heptafluoride implies seven fluorine atoms.
As for whether it is covalent, assuming this compound could exist, it would involve the sharing of electrons between the oxygen and fluorine atoms, making it a covalent compound. Yet, we should note that in real chemistry, dioxygen heptafluoride is not a known stable molecule.
For the exercise 5.7.2, the chemical formulas for the listed compounds are as follows:
- Phosphorus pentachloride: PCl5
- Dinitrogen monoxide: N2O
- Iodine heptafluoride: IF7
- Carbon tetrachloride: CCl4
When it comes to the formation of covalent bonds and stable molecules, Period 2 elements do not typically form compounds with central atoms covalently bonded to five or more atoms.
This is because the energy required to form the necessary hybrid orbitals is not compensated by the energy released in bond formation.