The video is very useful for few last days before the exam and congratulations on effort! One small mistake is at 30:00, the atomic radius increases down the group and decreases across the period.
Hiya, Firstly, amazing video thank you so much!!! Found it really useful Secondly, I did something that might help. Below is a time-topic list, so if you're looking for a specific topic you can skip. Hope it helps. 0:00 - introduction *2.1* 0:35 - Atoms and Subatomic Particles 1:11 - How Each Element Is Laid Out On The Periodic Table 1:24 - Isotopes 1:45 - Relative Masses And Formula To Calculate 2:19 - Elements, Compounds, Molecules And Ion Definitions 2:41 - The Periodic Table And Ions 3:30 - Polyatomic Ions To Memorise 3:50 - Ionic Compounds And Diatomic Molecules 4:32 - The Mole And Avagadro's Constant 5:27 - Empirical And Molecular Formula 6:06 - Water Of Crystallisation 6:38 - Mole Equations: Concentation And Volume 7:09 - The Ideal Gas Equation 7:59 - Percentage Yield And Atom Economy 9:16 - Acids 9:45 - Bases, Alkalis And Neutralisation Equations 10:48 - Making A Standard Solution 11:44 - Titration And Percentage Uncertainty Formula 12:50 - REDOX *2.2* 14:41 - Electron Configuration 18:43 - Ionic Bonding And Properties 19:52 - Covalent Bonding And Properties 20:54 - Shapes Of Molecules 22:48 - Electronegativity 25:05 - Dipole-Dipole Interactions 25:49 - Permanent-Permanent Dipole Interactions 26:32 - Hydrogen Bonding *3.1* 27:40 - The Periodic Table Over Time 28:42 - Ionisation Energy 29:16 - Ionisation Energy Trends 30:20 - Exceptions For Ionisation Energy Trends 30:54 - Ionisation Energy Graph 31:13 - Metallic Bonding 32:57 - Group 2 34:42 - Group 7 36:05 - Group 7 Tests 36:28 - Disproportionation Reactions 36:56 - Ion Testing *3.2* 38:15 - Enthalpy 38:33 - Standard Conditions 39:57 - Enthalpy Equation 40:52 - Enthalpy Definitions 41:36 - Average Bond Enthalpy/Bond Energies 42:07 - Hess' Law 43:22 - Rate Of Reaction 45:00 - Catalysts 45:57 - Boltzmann Distribution: Effects Of Temperature And Catalyst 47:23 - Equilibrium 47:41 - Le Chatelier's Principle And Factors Affecting Equilibirum's Position 48:59 - Equilibrium Constant 50:08 - End Of Lecture Message *separated by module as according to contents page from textbook link below* *www.worldofbooks.com/en-gb/books/victoria-stutt/ocr-as-a-level-chemistry-a-student-book-1-activebook/9781447990789?gclid=Cj0KCQjw7pKFBhDUARIsAFUoMDYIuvD5dVjbfSQO4UgOcjJZpuWC9NwOtLCoSrzhPqHDPUjoZu-zJVkaAsKhEALw_wcB*
Thank you so much! This helped me to consolidate all my knowledge of the Year 1 topics in one go and in a short amount of time. I'm was super stressed out because my end of year's start next week but this run through thorough all the topics has honestly really helped me. Thank youuuu :)
can u make this for the year 2 content too ? it’ll be rlly useful for students having summer exams in 2022 thanks for all the support & ur hard work ❤️
@Tanush ! That is not the issue at all. When writing the electron config, you can write it either way around, and yes, it is preferred to write the 3d before the 4s. Surprisingly, the issue isn't that she said 3d before 4s. No, the issue is somehow worse, and very clear if you just click the timestamp in the comment - she specifically states that "the order of filling therefore is 1s, 2s, 2p, 3s, 4s, 3p, 4p, 4d." She doesn't even say 3d. I've compiled a playlist of chemistry revision and haven't watched this video yet, but going by the comments and the sheer amount of errors, I think I'll be removing this one from the playlist. If only we had a way to show others with a simple counter that a video is bad, like a dislike button, _RU-vid_
thank you for the video!!! one question , the energy of the 4s energy level is not less than the energy of 3p it is more... this is how it goes 1s,2s,2p,3s,sp,4s,3d
Amazed you saw OCR A-Level Year 1, a whole english exam board with a spec called inorganic chem, and thought ah yea sure mate thisll be perfect for my college course. Fam this is for us stupid fuckers doing the eponymous OCR A-Level 🤧
collision theory is basically: A reaction will not take place between two particles unless: - they collide in the right direction and orientation - they collide with an energy greater than the activation energy
