I am having difficulty understanding why Br2 acts as an electrophile, because as I understand it, an electrophile is: "an atom (or group of atoms) that is attracted to an electron-rich centre or atom that accepts a pair of electrons to form a new covalent bond." and is usually either a positively charged (or electron deficient) ion or a molecule with a δ+ atom.
But Br2 (Br–Br) to me doesn't seem to have a δ+ atom, seeing as it is a linear molecule. I have read that both Br atoms in the molecule have a δ+ partial charge, but wouldn't the electronegativites cancel each other out?
But Br2 (Br–Br) to me doesn't seem to have a δ+ atom, seeing as it is a linear molecule. I have read that both Br atoms in the molecule have a δ+ partial charge, but wouldn't the electronegativites cancel each other out?
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When the Br2 molecule approaches an area of high electron density, e.g. a double bond from an ethene molecule, what will happen is, it causes one bromine to be more electronegative than the other. so causing bromine to be polar. (originally non-polar)