To compare how fluorine (F) and bromine (Br) form bonds, we can look at their electron configurations, electronegativities, and typical bonding behavior.
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Fluorine (F): Fluorine has 7 valence electrons and needs to gain 1 electron to achieve a stable octet configuration. When it gains one electron, it becomes a negatively charged ion (F⁻), which is very stable.
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Bromine (Br): Like fluorine, bromine also has 7 valence electrons. It can also gain 1 electron to achieve a stable octet configuration, becoming a negatively charged ion (Br⁻) that is stable as well.
Given this, the following statements can be evaluated:
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Both a fluorine atom and a bromine atom lose one electron, and both atoms become stable: This statement is incorrect as both F and Br typically gain electrons rather than lose them to achieve stability.
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A fluorine atom becomes stable by losing one electron, but a bromine atom cannot become stable by losing only one electron: This statement is also incorrect. Fluorine gains electrons to become stable, and bromine can gain one electron as well.
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Both a fluorine atom and a bromine atom gain one electron, and both atoms become stable: This statement is correct. Both elements achieve stability through the gain of one electron.
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A fluorine atom becomes stable by gaining one electron, but a bromine atom cannot become stable by gaining only one electron: This statement is incorrect. Both fluorine and bromine can gain one electron to become stable.
Thus, the most accurate statement is: Both a fluorine atom and a bromine atom gain one electron, and both atoms become stable.
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