If anyone is unsure about why it's easy to go from cl2 > 2cl-. Chlorine is higher up the group, so it has fewer shells, shorter atomic radius so it has a higher/ stronger attraction with the nucleus. Now if there's a high attraction (think of magnets), it's easy for an electron to become attracted and so it's easier for chlorine to gain en electron due to being highly electronegative. Now if it's easy to gain an electron because of the strong attraction, then at the same time it's also hard to lose the outer electron and go from 2cl- > cl2. It's difficult to lose that electron because it's attracted so much to the chlorine. Now it's easier for iodide/bromide ions to lose their outer electron because they're further form the nucleus and so they're less electronegative. Their electron is attracted less (lower ionisation energy) and so it's easier to remove that outer electron
Is there a way to figure out the products of all those reactions without having to learn the equations by heart? I want to actually understand where everything's coming from
QUESTION...…...Can you make HBr acid from sulfuric acid and IRON bromide or TIN bromide????????????????/ Meaning can the halide salt be with a transition metal or does it have to be a group one metal like sodium bromide????????????
@@ChemistryTuition ……………..wow you actually responded. THANK YOU SO MUCH. I was trying to think of how I could recycle my sodium bromide after i make ntiro alkane from a victor meyer reaction. I think i figured it out. Take iron metal and mix with the silver bromide to precip the silver out and make iron bromide. THEN I CAN JUST ADD NaOH to the iron bromide solution and filter out the iron hydroxide formed and i would be left with NaBr in solution. That way i can make more alkyl bromide to do the victor meyer reaction again
DrOrchard………..Curious about the transition metals now. How would the transition metal cation in a salt be reduced to metal by sulfuric acid? I mean sulfuric acid is an oxidizer right? Or did you mean the H2SO4 will oxidize the transition metal bromide salt to bromine?
Since TM can have various oxidation states, if you started with Iron (II), it could be oxidised to Iron (III). They will just complicate the chemistry.
If anyone is unsure about why it's easy to go from cl2 > 2cl-. Chlorine is higher up the group, so it has fewer shells, shorter atomic radius so it has a higher/ stronger attraction with the nucleus. Now if there's a high attraction (think of magnets), it's easy for an electron to become attracted and so it's easier for chlorine to gain en electron due to being highly electronegative. Now if it's easy to gain an electron because of the strong attraction, then at the same time it's also hard to lose the outer electron and go from 2cl- > cl2. It's difficult to lose that electron because it's attracted so much to the chlorine. Now it's easier for iodide/bromide ions to lose their outer electron because they're further form the nucleus and so they're less electronegative. Their electron is attracted less (lower ionisation energy) and so it's easier to remove that outer electron
Please show the half equations.
Is there a way to figure out the products of all those reactions without having to learn the equations by heart? I want to actually understand where everything's coming from
You really need to learn the equations but also understand the difference in terms of oxidation ability down group 7.
DrOrchard thank you ! I revised this topic just yesterday and your video was very helpful! Thanks !
Wish you were my teacher 🙄
thanks
so much
QUESTION...…...Can you make HBr acid from sulfuric acid and IRON bromide or TIN bromide????????????????/ Meaning can the halide salt be with a transition metal or does it have to be a group one metal like sodium bromide????????????
Group 1 metals are best as they will not be reduced to the metal. If you use TM they are likely to get involved in any redox reaction.
@@ChemistryTuition ……………..wow you actually responded. THANK YOU SO MUCH. I was trying to think of how I could recycle my sodium bromide after i make ntiro alkane from a victor meyer reaction. I think i figured it out. Take iron metal and mix with the silver bromide to precip the silver out and make iron bromide. THEN I CAN JUST ADD NaOH to the iron bromide solution and filter out the iron hydroxide formed and i would be left with NaBr in solution. That way i can make more alkyl bromide to do the victor meyer reaction again
Great - hope it works out for you.
DrOrchard………..Curious about the transition metals now. How would the transition metal cation in a salt be reduced to metal by sulfuric acid? I mean sulfuric acid is an oxidizer right? Or did you mean the H2SO4 will oxidize the transition metal bromide salt to bromine?
Since TM can have various oxidation states, if you started with Iron (II), it could be oxidised to Iron (III). They will just complicate the chemistry.
a level chem unit 3 tom lmfaooo