Oh my god I was looking for this the other day because I hate how group 7 exam equations are since I struggle to really understand halogens. words cant explain how happy i am that youve posted this THANK YOU!!
Thank you so much for the kind words. This document of all my videos might be useful? drive.google.com/file/d/1s3I5prjbJRR1U1lcKpXO9TQpQMaVoP66/view?usp=drivesdk
Another life saving video honestly making me so confident for my year 12 mock resits in 2 weeks, now all thats left are doing past paper questions Thanks sir for everything!!!
We add the 10H+ to balance the H from the RHS and then we had 10 H+ and one SO4^2- so the overall charge was currently +8. Then we add the 8e- to bring the charge on LHS down to zero
Great question... There's three reasons 1) it already contains the nitrate ion that is the same as the second ion in silver nitrate. 2) it doesn't contain Cl- (and HCl does) 3) it doesn't contain a second ion that could get involved in redox. SO4^2- can be reduced by Iodide ions and so side reactions can occur
hello, this was so helpful. btw sir, can i ask a question? so can you explain how to find angles when you are given a molceule such as ethanol or butanol? is there a easier way to find it...pls answer this, i have my exams next month
I'm pleased it was useful. I'm not sure I know exactly what you mean. This is my video about shapes.... ru-vid.com/video/%D0%B2%D0%B8%D0%B4%D0%B5%D0%BE-SkUmNLGWS5o.html Alternatively, you can think about the electron pairs around an atom. So the oxygen in ethanol has a bond to an H and one to the C. It also has 2 lone pairs. So 2 Bonding pairs and 2 lone pairs, means the bond angle between the 2 bonds will be the same as in water, so 104.5
Well, I teach AQA, so I make sure the videos cover everything for that exam board. Every topic for each exam board will be 98% identical. Its mostly the exam paper structure and question styles that vary 😀
That section is to show you that they can react with the acid in a simple acid-base reaction producing similar products. On the next page, I then go on to beginning the redox interactions of Br^1- That's when SO2 is a product
@@chemistrytutor does that mean the reaction of h2so4 with NaBr could either be redox or acid-base? do we need to know what causes the difference? and thankyou for the quick reply :)
@glo457 in reality it's probably best to assume that both will happen simultaneously or even one after the other. Which is why in the redox equation you can see H+ and Br- on the left hand side... so effectively the HBr produced in the acid-base reaction can then reduce the S
That’s sir , fantastic video very helpful ….. I’ll subscribe and watch your video s because you re very good at simplifying complex content for your students (like me) to understand !!
Thank you, that's really kind and great to hear! This document of links will probably be useful! drive.google.com/file/d/1s3I5prjbJRR1U1lcKpXO9TQpQMaVoP66/view?usp=drivesdk
@hasaanjunaid1842 That's a great question! When reacting sodium or potassium halides with concentrated sulfuric acid, it's important to use the halide in its solid form rather than aqueous solution for a few reasons: 1. Chemical Reactivity: In their solid state, the halide ions are more reactive with concentrated sulfuric acid. This is because the reaction involves a redox process where the halide ions act as reducing agents. When the halides are in aqueous solution, the presence of water can interfere with the redox reaction, potentially diluting the acid and reducing its effectiveness as an oxidizing agent. 2. Gas Evolution: The reaction between solid halides and concentrated sulfuric acid typically results in the evolution of gases such as hydrogen halides (HX) or other gases depending on the halide used. If the halides were in solution, the evolved gases might dissolve back into the solution, which would not only reduce the yield but also make it difficult to collect and observe the gases. 3. Temperature Control: The reaction between solid halides and concentrated sulfuric acid is exothermic. Using a solid allows for better control over the reaction temperature. An aqueous solution could lead to a more rapid and less controlled reaction, increasing the risk of splattering and making it harder to manage. Additionally concentrated acids react very exothermically with water, and a small volume of solution in a test tube might not have enough water to dissipate all the heat energy. 4. Product Purity: Using solid halides helps in obtaining purer products. In an aqueous solution, side reactions can occur, leading to impurities in the final products.
@@chemistrytutor so reactions of cr and Mn in year 13? Sorry I'm just future international students and i want brush everything up before my bachelor degree. And in my country we cover an array of reaction and I'm a little bit lost
That's a great question! When reacting sodium or potassium halides with concentrated sulfuric acid, it's important to use the halide in its solid form rather than aqueous solution for a few reasons: 1. Chemical Reactivity: In their solid state, the halide ions are more reactive with concentrated sulfuric acid. This is because the reaction involves a redox process where the halide ions act as reducing agents. When the halides are in aqueous solution, the presence of water can interfere with the redox reaction, potentially diluting the acid and reducing its effectiveness as an oxidizing agent. 2. Gas Evolution: The reaction between solid halides and concentrated sulfuric acid typically results in the evolution of gases such as hydrogen halides (HX) or other gases depending on the halide used. If the halides were in solution, the evolved gases might dissolve back into the solution, which would not only reduce the yield but also make it difficult to collect and observe the gases. 3. Temperature Control: The reaction between solid halides and concentrated sulfuric acid is exothermic. Using a solid allows for better control over the reaction temperature. An aqueous solution could lead to a more rapid and less controlled reaction, increasing the risk of splattering and making it harder to manage. Additionally, concentrated acids react very exothermically with water, and a small volume of solution in a test tube might not have enough water to dissipate all the heat energy. 4. Product Purity: Using solid halides helps in obtaining purer products. In an aqueous solution, side reactions can occur, leading to impurities in the final products.
Also Extremely sorry to disturb again and again. So what i understood was that, the reaction wont occur if metal halides were aq Could u then please help me with a past paper question about this? Its from chemistry AS level 9701, february march 2023, qp22, q2 d (i) In this strontium iodide (aq) is used along with concentrated sulfuric acid. But the reaction still occurs, according to the marking scheme. Shouldnt no reaction occur
That was a stepping stone calculation. RHS is 0 charge, the left *before electrons are added* The 4H+ ions and SO4^2- together have a 2+ charge which is why 2e needed to be added to make the charge zero
