Final answer:
The oxidation state of Cl in HCl is -1, in Br2 it is 0, in ICl3 for iodine it is +3, and in HF for fluorine it is -1. These states reflect the most common oxidation numbers for halogens in compounds.
Step-by-step explanation:
In chemistry, specifically in the field of redox reactions, the oxidation state is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound. Understanding oxidation states is crucial in determining how atoms will interact in reactions. Let's examine the oxidation state of the halogen in each of the given compounds:
- Cl in HCl: In hydrochloric acid (HCl), hydrogen (H) has an oxidation state of +1, and since the compound is neutral overall, chlorine (Cl) must have an oxidation state of -1 to balance the charge.
- Br in Br₂: Elemental bromine (Br₂) is in its diatomic form, so the oxidation state of bromine is 0 because the atoms are in their elemental form.
- I in ICl₃: In iodine trichloride (ICl₃), the chlorine (Cl) atoms each have an oxidation state of -1. Since there are three Cl atoms, the total negative charge is -3. To balance this, iodine (I) must have an oxidation state of +3.
- F in HF: In hydrogen fluoride (HF), hydrogen has an oxidation state of +1, which means fluorine (F) has to be -1 to balance the hydrogen's positive charge.