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Found 6 results

  1. Guys and Gals, I'm seven months into my IBDP (wow, time flies like anything) and my second cyclic tests are starting soon with Chemistry being the first one (in 2 weeks). The latest chapter that was taught to us is bonding, however the concepts are not yet clear to me (especially the whole hybridisation and sigma/pi bond thing) so I thought I would just do some questions. The problem is, that I don't want to do past papers because our tests are made out of them and there is a chance that I might have already solved some questions on my test which would inflate my score - the last thing I need. So if any of you know of a resource/website that has questions on the 2016 Chemistry syllabus which will help me cement my concepts, I'll be really grateful. Thanks, Aniruddh
  2. Aesop

    Chemistry Bonding Notes

    Here are my Chemistry Bonding notes.
  3. efelectron

    Bonding Practice Questions

    If any of you are interested in more bonding practice questions, whether it be for your next quiz, or test, exam or final, I found this website, and it has a lot of documents with hundreds of questions. I am sharing because I think many of you might find this useful. There's chem 20, 30, 35 more for hl, but obviously will do for sl, and some university level questions in there. Enjoy, and good luck! Link: http://highschoolchemresources.blogspot.ca/
  4. Hi guys! I have a homework to give in and I'm stuck on this question: Describe the bonding in iron and explain the electrical conductivity and malleability of the metal. I'm confused and don't understand what they mean by 'bonding in iron'... the way it takes electrons to complete their shell? the angle of bond? I'm very confused... Could you help me? Thanks very much! Note: I'm taking chem SL
  5. EmmonsBrooke

    Design Lab- Bonding

    Does anyone have a good idea for a Chemistry SL lab? It's topic is bonding. Thanks!!
  6. AustralianIB

    Bonding Angles Explained

    I have been tutoring Chemistry for over 2 years now and one of the topics students continually struggle with is Bonding, especially with regards to bond angles and VSEPR Theory. The key points to remember from VSEPR Theory are: - Electrons repel each other and thus spread out to minimise repulsion - Lone pairs further compress the bonding angle (I use 2 degrees as a rule of thumb) Throughout this explanation, I will be referring to negative charge centres, defined as: - A Single, Double or Triple Bond (Counts as one negative charge centre) - A non-bonding pair HL students can use this definition: - sigma bond - non-bonding pair The hard part is working out how many bonding and non-bonding pairs there are. This comes through practice and being able to recognise molecules from experience (I'll give a few tips about this at the end) The easy part is memorising is knowing what to do after you know how many negative charge centres and non-bonding pairs there are. Let's go through this now: Note - when I write say 4 negative charge centres, 2 non-bonding pairs, I mean: - 4 negative charge centres, of which 2 are non-bonding pairs - NOT 4 negative charge centres and 2 non-bonding pairs 1 negative charge centre: If there is only 1 negative charge centre, the shape can only be linear (180 degrees) Examples include H2, O2 Cl2 F2 N2 etc. 2 Negative charge centres: 0 non-bonding pairs If there are 2 negative charge centres, e.g. CO2, the charge centres will automatically repel each other to be as far apart as possible. Hence: Linear, 180 degrees 1 non- bonding pair This essentially means that there is only 1 bond, so linear, 180 degrees 3 Negative charge centres: 0 non-bonding pairs 3 negative charge centres trying to spread out to minimise repulsion means basically 360 degrees/3 = 120 degrees. Shape: trigonal planar 1 non-bonding pair Using the rule of thumb of -2, this would be 118 degrees Shape: Bent 4 negative charge centres: 0 non-bonding pairs Regular tetrahedron - 109.5 degrees 1 non-bonding pair Trigonal pyramidal - 107 degrees (-2 and rounding down) 2 non-bonding pairs V-shaped - 105 degrees 5 negative charge centres: 0 non-bonding pairs Trigonal Bi-pyramidal - 120 degrees and 90 degrees (Note that there are 2 different angles here) 1 non-bonding pair See-saw - 118 degrees and 90 degrees 2 non-bonding pairs T - shaped - 90 degrees (Think T) 6 negative charge centres: 0 non-bonding pairs Octahedral - 90 degrees 1 non-bonding pair Square pyramid - 88 degrees 2 non-bonding pairs Square planar - 90 degrees Now for a little bit to help ease the hard part: For SL students, if you see a 4 at the end, e.g. NH4, CH4 - this is tetrahedral 109.5 degrees. Why? Because 5 and 6 negative charge centres are not examinable in SL. BF3 is trigonal planar - 120 degrees NH3 is trigonal pyramidal - 107 degrees H2O has 4 negative charge centres, of which 2 are non-bonding - V-shaped, 105 degrees For HL Students, if you see a 6, it is octahedral. As 7+ negative charge centres are not examinable. Be careful when you see 2s however, as it can be linear or V-shaped. For HL students, be careful when you see 4, as it is not necessarily tetrahedral. Hope this helps!

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