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As we know that Cl, Br and I are highly electronegative elements, the receive electrons and become Cl-, Br- and I-. But my question is in which situation, they start donating electrons and become Cl+, Br+, and I+?
What is the chemical term for losing electrons?HCverma said:But my question is in which situation, they start donating electrons and become Cl+, Br+, and I+?
CationsTeethWhitener said:What is the chemical term for losing electrons?
No, cations are positively charged species. But Cl- can lose an electron to become neutral chlorine, for example:HCverma said:Cations
The term is called oxidation.TeethWhitener said:No, cations are positively charged species. But Cl- can lose an electron to become neutral chlorine, for example:
$$\textrm{2Cl}^- \longrightarrow \textrm{Cl}_2 + \textrm{2e}^-$$
What is the term for the process above, when a chemical undergoes a reaction which specifically causes a loss of electrons?
HCverma said:But here 2Cl^- forms Cl2 by sharing two electrons through the .covalent bond. So how do Cl^- lose electron rather than sharing a pair of electrons? Could you explain it, please?
This was the point I was trying to make. You'd need to oxidize the halogen to get a halonium.HCverma said:The term is called oxidation.
No, simply sharing the electrons would give you Cl22-. To get rid of the electrons requires an oxidizer (something that accepts electrons).HCverma said:But here 2Cl^- forms Cl2 by sharing two electrons through the .covalent bond.
I'm assuming that the OP was talking about formal halonium. Free H+ can't be made in solution either (apart from briefly upon exposure to something like high energy radiation), but it's useful to talk about acid-base chemistry as if free protons did exist in solution.snorkack said:Turns out that free Cl+ and even I+ cannot quite be made.
Could you name the oxidizer please and could you mention the reaction where we can get neutral Cl2?TeethWhitener said:This was the point I was trying to make. You'd need to oxidize the halogen to get a halonium.
No, simply sharing the electrons would give you Cl22-. To get rid of the electrons requires an oxidizer (something that accepts electrons).
I'm assuming that the OP was talking about formal halonium. Free H+ can't be made in solution either (apart from briefly upon exposure to something like high energy radiation), but it's useful to talk about acid-base chemistry as if free protons did exist in solution.
I'm a bit confused by your question. Do you want to know how to oxidize chloride (Cl-) to chlorine (Cl2)? The easiest way to do that is electrochemically (electrolyze an aqueous solution of NaCl, for example, and adjust the pH so that free Cl2 is released). You can also oxidize HCl with potassium permanganate, for example.HCverma said:Could you name the oxidizer please and could you mention the reaction where we can get neutral Cl2?
TeethWhitener said:I'm assuming that the OP was talking about formal halonium. Free H+ can't be made in solution either (apart from briefly upon exposure to something like high energy radiation), but it's useful to talk about acid-base chemistry as if free protons did exist in solution.