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Step 1:I'll solve this problem step by step, focusing on determining the oxidation state of bromine (Br).
Step 2:: Understand the Concept of Oxidation State
The oxidation state (or oxidation number) is a measure of the degree of oxidation of an atom in a chemical compound. It represents the number of electrons an atom has gained or lost when forming a chemical bond.
Step 3:: Recall the Rules for Determining Oxidation State
Key rules include: - The sum of oxidation states in a neutral molecule must equal zero - In their elemental state, atoms have an oxidation state of 0 - For monatomic ions, the oxidation state equals the charge of the ion - Certain elements have consistent oxidation states in most compounds
Step 4:: Analyze Possible Oxidation States of Bromine
- $$+7$$ (in perbromate, $$\text{BrO}_{4}^{-}$$)
Bromine can have multiple oxidation states, ranging from - 1 to + 7. The most common oxidation states are:
Final Answer
Bromine can have oxidation states ranging from - 1 to + 7, with the most common being 0, - 1, + 1, + 3, + 5, and + 7, depending on the specific compound.
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