Which of the following could be the identity of this compound?
Select all that are true.
- iodine trifluoride
- chlorine trifluoride
- bromine pentafluoride
- iodine pentafluoride
- chlorine pentafluoride
The correct answer and explanation is :
To determine which of the listed compounds could be the identity of the given compound, let’s examine each option closely in terms of its chemical composition, structure, and oxidation states.
The Oxidation States:
First, recall that halogens such as iodine (I), chlorine (Cl), bromine (Br), and fluorine (F) have specific tendencies regarding their oxidation states in compounds with fluorine. Fluorine is the most electronegative element and typically takes an oxidation state of -1.
For the halogen-based compounds with fluorine, the possible oxidation states of the halogens will depend on how many fluorine atoms are bonded to them.
Option Analysis:
- Iodine trifluoride (IF₃):
- The molecular formula is IF₃.
- Iodine (I) is the central atom and fluorine atoms surround it.
- Fluorine, as mentioned, has an oxidation state of -1, so the oxidation state of iodine must be +3 to balance the three fluorine atoms.
- This corresponds to iodine trifluoride, which is a well-known compound. Therefore, this is a correct identity.
- Chlorine trifluoride (ClF₃):
- The molecular formula is ClF₃.
- Chlorine (Cl) is the central atom, with fluorine atoms surrounding it.
- Since fluorine has an oxidation state of -1, chlorine must have an oxidation state of +3 to balance the three fluorine atoms.
- Chlorine trifluoride is a known compound with this composition. Therefore, this is a correct identity.
- Bromine pentafluoride (BrF₅):
- The molecular formula is BrF₅.
- Bromine (Br) is the central atom, surrounded by five fluorine atoms.
- Fluorine has an oxidation state of -1, so bromine must have an oxidation state of +5 to balance the five fluorine atoms.
- This compound is also known and stable, making this a correct identity.
- Iodine pentafluoride (IF₅):
- The molecular formula is IF₅.
- Iodine (I) is the central atom, with five fluorine atoms surrounding it.
- Fluorine has an oxidation state of -1, so iodine must have an oxidation state of +5 to balance the five fluorine atoms.
- This is a known compound, iodine pentafluoride, which is stable and commonly encountered. Therefore, this is a correct identity.
- Chlorine pentafluoride (ClF₅):
- The molecular formula is ClF₅.
- Chlorine (Cl) is the central atom, surrounded by five fluorine atoms.
- Chlorine must have an oxidation state of +5 to balance the five fluorine atoms, which corresponds to chlorine pentafluoride.
- This is a known compound, so this is also a correct identity.
Conclusion:
The correct identities for the compound in question are iodine trifluoride (IF₃), chlorine trifluoride (ClF₃), bromine pentafluoride (BrF₅), iodine pentafluoride (IF₅), and chlorine pentafluoride (ClF₅). All of these compounds are real and match the descriptions provided.