Thanks you so much for your videos, for some reason, my teacher likes leaving questions that we have not learned before and make us suffer. You have just saved me from the suffering!!
Mr. Thornley, thanks a lot for all the helpful vids, they saved my life a few times already. But I've got a question - Why isn't the electronic configuration of Si an exception? Instead of 1s2 2s2 2p6 3s2 3p2 shouldn't it be 1s2 2s2 2p6 3s1 3p3, so that the two last orbitals were half-full?
In the case of silicon being an exception since the 3s orbital is lower than 3p so the electron configuration wont change But for Cu and Cr the 4s orbital is higher than the 3d so the electron could easily go down to a lower energy
Awesome video series! Thanks a lot for your help! However, it's quite a shame since you always stop at the edge of IB syllabus... Could you please talk more about chemistry out of IB, or are there additional materials recommended for further explorations? :o)
Hey, quick question. In the book they state the electron configuration for Selenium as following; 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4. However you've written 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4. This is a little confusing (looking at the 'd' orbit), there are several examples of this in the video that are stated a bit differently in the book. The way the electron configuration ends however is the same in both the video and the book. Is it that it doesnt matter if e.g. 3d is stated just before or after 4s as long as they are not the final component of the Elect Conf? Thanks in advance
Had a paper 2 mock a week ago and got asked about the orbital diagram of the Cobolt3+ ion. Why is there six electrons in 3d and none in 4s, if it is preferred to have full or half-full orbitals? I thought it would have one electron in 4s and 5 in 3d so that both orbitals would be half-full, instead of just a 3d orbital being slightly more than half-full.
Indeed - the 2.8.1 type electron arrangements have been removed (I have now added this in the notes) BUT knowing how to do it makes IB chemistry a lot easier -so I still teach it. I think this is an accidental omission on the part of the IB.
Hello Mr Thornley! a quick question: as Mo and Ag are in similar conditions to Cr and Cu respectively, and we are supposed to know up to Xe, should we assume the same happens to Mo and Ag even though it is not specified in the syllabus?
Hey, Richard! One question I've run into and haven't been able to rind a definitive answer. Does IB require students to reorganize the configuration with grouping the shells together (e.g. 1s2s22p63s23p63d104s1 for Cu) or can the students just leave the configuration in the order that they were filled (e.g. 1s22s22p63s23p64s13d10 for Cu)?
The only reason I ask is that Oxford, Cambridge, and Pearson texts all right the configurations by regrouping the orbitals by energy level, but never state whether or not it's required.
I tell the kids"ask your god why he made it that way!" - i work for the UN , we have lots of gods here. My understanding is that electrons will go where the energy is lowest = most stable. You question makes sense - I have no idea - but the IB want you to know the Cr Cu exceptions only.
![S1.3.6 Evidence of Energy Levels by 1st I.E. Trends Across a Period [HL IB Chemistry]](http://i.ytimg.com/vi/s5q_hFYmmrA/mqdefault.jpg)
Thanks you so much for your videos, for some reason, my teacher likes leaving questions that we have not learned before and make us suffer. You have just saved me from the suffering!!
Transition metals ions have some wierd extra patterns to learn (eg Cr and Cu are odd).
Love all of your videos, as a chemistry student, these help A LOT!
Mr. Thornley, thanks a lot for all the helpful vids, they saved my life a few times already. But I've got a question - Why isn't the electronic configuration of Si an exception? Instead of 1s2 2s2 2p6 3s2 3p2 shouldn't it be 1s2 2s2 2p6 3s1 3p3, so that the two last orbitals were half-full?
Mr. Thornley,
you are an angel sent from heaven above
I believe in the 2016 syllabus when you write the configurations for the transition metals you have to list the 3d before 4s2
In the case of silicon being an exception since the 3s orbital is lower than 3p so the electron configuration wont change
But for Cu and Cr the 4s orbital is higher than the 3d so the electron could easily go down to a lower energy
Awesome video series! Thanks a lot for your help! However, it's quite a shame since you always stop at the edge of IB syllabus... Could you please talk more about chemistry out of IB, or are there additional materials recommended for further explorations? :o)
did you find the element???
Thanks a lot for the great work
Hey, quick question. In the book they state the electron configuration for Selenium as following; 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4. However you've written 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4. This is a little confusing (looking at the 'd' orbit), there are several examples of this in the video that are stated a bit differently in the book. The way the electron configuration ends however is the same in both the video and the book. Is it that it doesnt matter if e.g. 3d is stated just before or after 4s as long as they are not the final component of the Elect Conf?
Thanks in advance
Had a paper 2 mock a week ago and got asked about the orbital diagram of the Cobolt3+ ion. Why is there six electrons in 3d and none in 4s, if it is preferred to have full or half-full orbitals? I thought it would have one electron in 4s and 5 in 3d so that both orbitals would be half-full, instead of just a 3d orbital being slightly more than half-full.
Thank you so much before this i knew nothing everything was so complicated,
now i finally know how to do this.
Can the trick you showed us at the beginning of the video be used for transition metal ions too?
Thanks
it is in the 5th period = 5 energy levels
Thanks so much! Wish I would have taken HL chem, but I only did SL. Your HL videos are coming in handy in my first year uni chem course. :)
YOU DID SL CHEM BUT CAN STILL DO CHEM IN UNI???
hahah am working on it ... no pls we have enough :P
Does the IB accept the short hand representations of the electron configurations?
Hey do you still alive? 7 years passed notification
is this removed form the 2018 syllabus?
Indeed - the 2.8.1 type electron arrangements have been removed (I have now added this in the notes) BUT knowing how to do it makes IB chemistry a lot easier -so I still teach it. I think this is an accidental omission on the part of the IB.
Omg you actually replyed i just wanna thank u alot alot alottttttttttttt alot alot as many electrons in the universe
+ANAS Hallak Uhhh, "alot" is literally not a word.
me no speak English roski rush b yes?
thanks!! helpful review for me!
i have a question why does tin have 5 energy level instead of four
Richard, how about writing electron configurations for the new syl SL?
André Amaral New syllabus goes not have 2:8:8:2 (unbelievably) for either SL or HL. spdf is used.
thanks a lot!!!!!!!!!!
Hello Mr Thornley! a quick question: as Mo and Ag are in similar conditions to Cr and Cu respectively, and we are supposed to know up to Xe, should we assume the same happens to Mo and Ag even though it is not specified in the syllabus?
Covadonga Menéndez Acebal Yup - you need to know Ag+ for sure
Hey, Richard! One question I've run into and haven't been able to rind a definitive answer. Does IB require students to reorganize the configuration with grouping the shells together (e.g. 1s2s22p63s23p63d104s1 for Cu) or can the students just leave the configuration in the order that they were filled (e.g. 1s22s22p63s23p64s13d10 for Cu)?
The only reason I ask is that Oxford, Cambridge, and Pearson texts all right the configurations by regrouping the orbitals by energy level, but never state whether or not it's required.
I don't think it matter. I don't think they'll cut off points because you didn't order them properly
The IB have given both ways in their questions.
ur awesome tysm
Hi Richard, do I need to know everything in this video for SL?
yup
Thanks (:
I tell the kids"ask your god why he made it that way!" - i work for the UN , we have lots of gods here.
My understanding is that electrons will go where the energy is lowest = most stable. You question makes sense - I have no idea - but the IB want you to know the Cr Cu exceptions only.
Hey Mr. Thornley,
Does this video cover everything for HL Chem now?
Thanks!
+Sabeet Raza yup
So, tell us, Was "Thornlenium" element that ends in 2d1 already discovered by you? 😃
3:16 Are you still working on Mr. T? 😂
Oh the usefull-ness of these videos are so good. :D:D:D:D:D:D
Im doing applied science and its asking me all of this....... why have so many a level chemistry/biology/physics topics in my module?
Hmm so would I - I am curious - can you message me the question or web address?
so for chem sl I dont need to know the configurations (1s2, 2s2)? or..
+Jenna Z All changed for the new syllabus - SL and HL now - I have added a note now - cheers.
yup (that's what I said!)
How do I write the electorn configuration for Co2+? Why is it not [Ar]4s^2 3d^5? Why is it [Ar]3d^7?
It's because when d-block elements (transition metals) form ions, the 4s electrons are lost first.
Bond angel 120 degrees!
watching this 10 years later
Done with topic 2! 17 hours left ...
Actually you say in the video 2d1
Wahsha
man i have no idea what he’s saying