halogens decrease in reactivity down the group, because their ability to gain electrons decreases because:
the atomic radi increases
the electron shielding increases
...
how excactly do these two factors affect its oxidising ability? is it because the electrostatic attraction between the electrons they may gain has decreased because of these two factors, or something completely different?
3 comments:
Good thinking so far, Lewis...
What is a halogen actually doing if it is behaving as an oxidising agent? Why do the halogens get less able to do this as you go from F to I? (HINT: Your thinking re: reactivity is spot on, just adapt it to fit oxidising ability!)
it is oxidising other elements/compounds and so taking their electrons . . . so its attracting them to itself? and the ability to attract decreases because of the increased atomic radius and shielding?
Excellent! Do you feel confident about explaining that now?
Why do you think the halide ions (i.e. F-, Cl-, Br-) become better reducing agents as you go down Group 7?
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