Currently unavailable: until 15/12/2016
Degree: Chemistry (Bachelors) - Edinburgh University
I am currently an (environmental) chemistry student at the University of Edinburgh, and I will be the first to admit I am a science geek. Now, if science is not your thing, I hope that by the end of one of my sessions you might start to appreciate it's finesse as much as I do.
I always find it difficult to describe myself, but I guess one word that would definitely describe me is determined. I am, and always have been determined to succeed- whether that takes me five minutes to achieve or five months, I will not stop. And that is a skill that I will not only apply to my tutees but will try to pass on to them as well. Giving up is never an option!
In terms of teaching style, I am definitely someone who appreciates tutees taking initiative. I can only help so much as they allow me to. I have found that such sessions are much more fruitful when the tutee knows exactly what it is that they need help with, if they want to go over questions I can do that, if they want the best results it would be good to send them to me earlier, so that I can prepare answers to them- otherwise I will go over it during the session, but again, that will take away from the time they could be using to ask other questions. Of course I will also go over concepts, and try my best to explain any concepts they are having issues with. When it comes to chemistry I find anologies incredibly helpful so that is something that I will usuually incorporate into my teaching as well, as I find it really helps to put things into perspective and allows people to look at things in a different light.
|IB Math Standard Level||Baccalaureate||6|
|IB English Lang & Lit A Standard Level||Baccalaureate||6|
|IB Spanish B Standard Level||Baccalaureate||7|
|IB Biology Higher Level||Baccalaureate||7|
|IB Chemistry Higher Level||Baccalaureate||7|
|IB Economics Higher Level||Baccalaureate||7|
|Before 12pm||12pm - 5pm||After 5pm|
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Ammonia acts as the Lewis base in this reaction by donating its lone pair of electrons, whilst Cu2+ (which is an electron deficient, electrophile) accepts the lone pair of electrons from the ammonia, making it a Lewis acid. The bond between Cu2+ and NH3 is a coordinate bond (also known as a dative bond), whereby the electrons in the bond are both donated by one species (in this case NH3). Thus NH3 is a ligand. Cu2+ is the electrophile (electron deficient) and NH3 is the nucleophile (electron rich).see more