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Step 1:I'll solve this problem step by step:
Step 2:: Understand Bromine's Position on the Periodic Table
- Bromine (Br) is located in Group 17 (Halogen group) on the periodic table - Halogens typically form negative ions by gaining electrons
Step 3:: Determine Electron Configuration
- Bromine's electron configuration is $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{5}
- It needs one more electron to complete its outer shell
Step 4:: Calculate Ion Charge
- This results in a charge of $$-1
- To achieve a stable electron configuration, bromine typically gains one electron
Step 5:: Verify Common Ion Formation
- Bromide ion has the formula $$Br^{-}
- The most common ion for bromine is the bromide ion - This represents a single negative charge
Final Answer
The most common ion charge for bromine is - 1, forming the bromide (Br^{-}) ion.
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