energy absorbed when jumps out = yes (electron moves to a higher energy level) energy (photon) released when jumps back - yes Ask away - and good luck with the self study - lucky I made all these vids eh!
Ilsa Wojt I make $20 every 30,000 views.If you watch each of the 300 vids 10 times = 3000, that means I just made a sweeeeet $2 before tax!Goood luck tomorrow.
I took SL for the first six months before sadly, jumping to HL. I have all the books and revision guides which have failed to save me. Thank you so much Richard Thornley, I shall send you chemistry magazines if I do well in my exams!
Thank you so so much i couldnt understand this for like 4 days while i read my textbook over and over and watched different videos. YOUrs has helped me the most thank you
Thank you very much for all your videos - I have my exams on Wednesday and Thursday for HL chem and you videos have helped me immensely throughout these two years :-) Thank you Richard Thornley.
The electrons can only jump up when they receive the exact amount of energy - but if you heat them then a wide array of energy is available (hot bit of flame, cold bit etc) - so heating gives all colours.
sir, you made me laugh while learning at the same time, thank you so much for this, i cannot express how grateful i am now that i understand fully how it works 😭💖
I'm not a Chemistry instructor, but I was taught (as I am staring at my text book for reference) that electrons DO NOT orbit around the shells, or rings, but rather bounce around INSIDE the ring. The orbits that electrons travel are actually areas of probability. That ring is where the electron can be found 90 percent of the time. So the information given about the electron shifting from one ring to the next is inaccurate, but rather the electron increases its radius of movement to the next energy level when excited. I enjoyed this video, but felt it needs clarification with so many views and all. Sources: Introductory Chemistry Zumdahl 7th Ed. ch. 11 pg. 332 The Wave-Mechanical Model
There is IB chemistry and then there is chemistry! This assumes the Bohr model of the atom where electrons are found on discrete shells. The more modern "molecular orbital" theory comes up a bit later in the course.
Thank you for your amazing videos. They are really helpful.There's just one thing that makes me wonder a bit. How come that these videos are for the new syllabus for the 2016 exams, but the video is from 2011?
I have a few questions and was wondering if you could answer them. 1)Why cant bohrs atom explain multi electrons systems? 2)In hydrogen atom , when the electron increases in energy level , does it go into a more outward orbital (further away from the nucleus) or does it just temporarily increase in the amount of energy it has 3) When gas is subjected to high voltage , how the electrons jump up an energy level? Is the voltage a very specific one?
1) I think it becomes the classic 3 body problem, then 4 body problem - very hard to solve mathematically. Electron A moves, this repels electron B, this attracts the nucleus more, which moves electron A and on and on. Also electrons like to pair up sometimes. Bohr works for He+ Li2+ though since there is only 1 electron remaining! 2) An excited electron has more energy and moves to a higher orbital further from the nucleus. 3) Hmm - in IB chemistry there is a specific energy needed to ionize a gaseous atom E=hf (topic 12). This assumes a jump to n =infinity for the electron. Since electrons can only exist at specific energies (they are quantum) the must have specific energy delivered to them. Any more or less will not cause the jump. BUT in reality the atoms have different speeds, rotational energies, LDF interactions, isotopes etc so I expect the energy required will be in a broader range.
1) cos there is more than 1 atom involved. (But you are right one atom can only produce one line at a time). 2) if the tom is given energy then other shells are available - only a "low" energy H atom has one shell.
Hi Richard, your video is awesome!!! I just have one question: do the electrons of an atom jump randomly to any higher energy level that they can even when a controlled amount of energy is given to excite them? For example, how come hydrogen produces all 5 lines in the line spectra when it just have 1 electron and a fixed amount of external energy? (Wouldn't it just show one strip of color at a time?) Thanks soooooo much
Hey! I have just started my IB journey and I’m very confused about some things in the syllabus. Just to confirm, do IB exams assess Nature of Science spec points? Do they assess the Utilization/International-mindedness as well? I can’t thank you enough for all of the amazing and easy to understand Chemistry resources. I’ll definitely be returning to watch them every once in a while!!
NOS - yes this is tested as is IM (but only one point- the answers is @replication of experiments, different points of view lead to better experiments etc). TOK and Utilisation are not needed. Good luck on the journey!
they converge because there is less difference in energy levels as you go up, the difference in energy decreases. for example, the energy emitted in the jump from n=2 to n=1 is greater than the jump from n=infinity to n=2.
Okay. Sometimes it gets confusing when you pronounce something differently; the difference in the way it's pronounced is infinitesimal and leads to ambiguity in the lesson. For instance, the "ultra-violet" in this video.
hey richard, i understand the bit on the energy levels being convergent but I dont get how they are concentric, what does that even mean, how re they within one another. Btw thanks for all the help.
The hydrogen atom has 1 e- going around on one energy level but it turns out if you heat it up then the electron jumps out further from the nucleus and continues moving around in a "circle" but further from the nucleus. These energy levels are centered on the nucleus and get closer together the further from the nucleus they are. Concentric just means that they are within one another with the same center.
so it absorbs energy to jump out and release energy when jump back? or both release energy. sorry if I ask too much questions. I'm self-studying IB Chem so I don't have a teacher.
awesome video: just a few questions 1) theres only one electron in an Hydrogen atom - how does it show all 5 lines in the visible light (Balmer's series) at the same time 2) how does an electron 'return' to n=2 or n=3 when they fall from a higher energy level as the electron at is ground state in a Hydrogen atom is only at the first shell as there is only one electron?
I think that higher frequencies may cause ionisation AND give the electron an extra kick of speed! But the quantized nature of reality may not work like that.
I have a question! Why do different elements when lighted have different coloured flames? So for example why is it that Sodium has a yellow flame and copper a green one??
Hi Mr Thornley, thank you for these great videos. I was just wondering whether n can equal infinity because my teacher told me that there is a limit to the number of shells due to convergence.
Hey, Richard! My students and I love using your videos, but I would correct this video as "spectra" is the plural of "spectrum." If you're referring to a single spectrum, you shouldn't use the term "spectra."
. Visable is a disruptive, next-generation recruiting tool for students and employers to engage in a meaningful and efficient way to create significantly improved hiring outcomes
I wouldn't even want to imagine what Chemistry HL would be like without you.
You, Mr. Thornley, are the man.
Exactly, my IB chem teacher is ass at explaining stuff.
May 2015 session final revision with Thornley. I cannot thank you enough, sir :)
George Kalostypis no problem - gooood luck in May
energy absorbed when jumps out = yes (electron moves to a higher energy level)
energy (photon) released when jumps back - yes
Ask away - and good luck with the self study - lucky I made all these vids eh!
Omagadd i couldn't thank you enough. You are a complete life saver. if only there was something like this for other ib subjects.
STEEZ fan??
Thank you for this crystal-clear explanation!
My final exam is tomorrow and I've watched all these videos maybe 10 times thank you so much!! They are extremely comprehensible
Ilsa Wojt I make $20 every 30,000 views.If you watch each of the 300 vids 10 times = 3000, that means I just made a sweeeeet $2 before tax!Goood luck tomorrow.
I took SL for the first six months before sadly, jumping to HL. I have all the books and revision guides which have failed to save me. Thank you so much Richard Thornley, I shall send you chemistry magazines if I do well in my exams!
Thank you so so much i couldnt understand this for like 4 days while i read my textbook over and over and watched different videos. YOUrs has helped me the most thank you
OMG I'm so glad I found this channel!! Great video and hugee info and you made it so easy to understand! Thank you sooo much sir!
Thank you very much for all your videos - I have my exams on Wednesday and Thursday for HL chem and you videos have helped me immensely throughout these two years :-) Thank you Richard Thornley.
finally after watching so many videos this one is the perfect one
The electrons can only jump up when they receive the exact amount of energy - but if you heat them then a wide array of energy is available (hot bit of flame, cold bit etc) - so heating gives all colours.
your videos are legendary
i can never thank you enough for these vids
sir, you made me laugh while learning at the same time, thank you so much for this, i cannot express how grateful i am now that i understand fully how it works 😭💖
I can't thank you enough :)
This was extremely helpful ..
Awesome presentation!
I'm not a Chemistry instructor, but I was taught (as I am staring at my text book for reference) that electrons DO NOT orbit around the shells, or rings, but rather bounce around INSIDE the ring. The orbits that electrons travel are actually areas of probability. That ring is where the electron can be found 90 percent of the time. So the information given about the electron shifting from one ring to the next is inaccurate, but rather the electron increases its radius of movement to the next energy level when excited.
I enjoyed this video, but felt it needs clarification with so many views and all.
Sources:
Introductory Chemistry Zumdahl 7th Ed. ch. 11 pg. 332
The Wave-Mechanical Model
There is IB chemistry and then there is chemistry! This assumes the Bohr model of the atom where electrons are found on discrete shells.
The more modern "molecular orbital" theory comes up a bit later in the course.
Thank you for your amazing videos. They are really helpful.There's just one thing that makes me wonder a bit.
How come that these videos are for the new syllabus for the 2016 exams, but the video is from 2011?
Omg u r the best. I Won't fail tommorows exam. 😊
Big jump = Big energy, this is exactly what i need in my life
I was the 1k like -my friend
thanks for this fr I forgot everything about atomic structure
you are a genius!!!! an excellent teacher thank youuuuu
Good video :) just one question. Who put a shower in a chemistry room?
I have a few questions and was wondering if you could answer them.
1)Why cant bohrs atom explain multi electrons systems?
2)In hydrogen atom , when the electron increases in energy level , does it go into a more outward orbital (further away from the nucleus) or does it just temporarily increase in the amount of energy it has
3) When gas is subjected to high voltage , how the electrons jump up an energy level? Is the voltage a very specific one?
1) I think it becomes the classic 3 body problem, then 4 body problem - very hard to solve mathematically. Electron A moves, this repels electron B, this attracts the nucleus more, which moves electron A and on and on. Also electrons like to pair up sometimes. Bohr works for He+ Li2+ though since there is only 1 electron remaining!
2) An excited electron has more energy and moves to a higher orbital further from the nucleus.
3) Hmm - in IB chemistry there is a specific energy needed to ionize a gaseous atom E=hf (topic 12). This assumes a jump to n =infinity for the electron. Since electrons can only exist at specific energies (they are quantum) the must have specific energy delivered to them. Any more or less will not cause the jump. BUT in reality the atoms have different speeds, rotational energies, LDF interactions, isotopes etc so I expect the energy required will be in a broader range.
1) cos there is more than 1 atom involved. (But you are right one atom can only produce one line at a time).
2) if the tom is given energy then other shells are available - only a "low" energy H atom has one shell.
wow my doubts are now!! Thumbs UP!!
Dude I love u.. Thank u lol
Hi Richard, your video is awesome!!! I just have one question: do the electrons of an atom jump randomly to any higher energy level that they can even when a controlled amount of energy is given to excite them? For example, how come hydrogen produces all 5 lines in the line spectra when it just have 1 electron and a fixed amount of external energy? (Wouldn't it just show one strip of color at a time?) Thanks soooooo much
Hey! I have just started my IB journey and I’m very confused about some things in the syllabus. Just to confirm, do IB exams assess Nature of Science spec points? Do they assess the Utilization/International-mindedness as well? I can’t thank you enough for all of the amazing and easy to understand Chemistry resources. I’ll definitely be returning to watch them every once in a while!!
NOS - yes this is tested as is IM (but only one point- the answers is @replication of experiments, different points of view lead to better experiments etc). TOK and Utilisation are not needed. Good luck on the journey!
@@ibchemvids thank you so much for the help!
Thank you for making me understand, not just rewriting things from the book (which is completely useless for me)
You are the best!! Thank u!
Excuse me... Why do the lines always converge toward higher energy levels? (PS: Awesome video! :o))
they converge because there is less difference in energy levels as you go up, the difference in energy decreases. for example, the energy emitted in the jump from n=2 to n=1 is greater than the jump from n=infinity to n=2.
U are a genius
Sir, You are a life saver ....
Give me your post, I want to send you a thank you card after exams...
thank you so much :-)
Okay. Sometimes it gets confusing when you pronounce something differently; the difference in the way it's pronounced is infinitesimal and leads to ambiguity in the lesson. For instance, the "ultra-violet" in this video.
Thanks so much
Thank you that was helpful! Is that Half Life you are using as an example xD
lauralol98 Nah, fam. That’s Gmod, which which is a Half Life sandbox game.
yah. thank you very much. Does anyone tell you that you're a good Chem teacher before?
hey richard, i understand the bit on the energy levels being convergent but I dont get how they are concentric, what does that even mean, how re they within one another.
Btw thanks for all the help.
The hydrogen atom has 1 e- going around on one energy level but it turns out if you heat it up then the electron jumps out further from the nucleus and continues moving around in a "circle" but further from the nucleus. These energy levels are centered on the nucleus and get closer together the further from the nucleus they are. Concentric just means that they are within one another with the same center.
so it absorbs energy to jump out and release energy when jump back? or both release energy.
sorry if I ask too much questions. I'm self-studying IB Chem so I don't have a teacher.
awesome video: just a few questions
1) theres only one electron in an Hydrogen atom - how does it show all 5 lines in the visible light (Balmer's series) at the same time
2) how does an electron 'return' to n=2 or n=3 when they fall from a higher energy level as the electron at is ground state in a Hydrogen atom is only at the first shell as there is only one electron?
same question :|
You are the best! :)
omg that was soo incredibly helpfull
The G.O.A.T
7:22 so are there higher frequencies of visible light that can be absorbed by the electron?
I think that higher frequencies may cause ionisation AND give the electron an extra kick of speed! But the quantized nature of reality may not work like that.
brilliant!
"oh! we are losing contact" 😁👽
google it - they took a photo 5 days ago!
I have a question! Why do different elements when lighted have different coloured flames? So for example why is it that Sodium has a yellow flame and copper a green one??
Because the electrons jump down towards the nucleus different distances = different energies of photon released = different colours.
can you explain what quantization means? its on this chapter
in this case, it means that the electron can only jump up certain energy levels (never half levels) - only certain quantities of energy are allowed.
Hi Mr Thornley, thank you for these great videos. I was just wondering whether n can equal infinity because my teacher told me that there is a limit to the number of shells due to convergence.
The limit is (weirdly) infinity. When the electron moves to the infinite level it has popped off (ionisation).
How is there multiple colors if Hydrogen has 1 electron
There are many atoms, each has electrons jumping to different energy levels depending on how much energy they recieve.
thank you! :D
I think the shower is there in case someone has to wash off anything dangerous that might've spilled on them in the chemistry lab
why does it say not UV?
Oh what fantastic help :D:D:D
Hey, Richard! My students and I love using your videos, but I would correct this video as "spectra" is the plural of "spectrum." If you're referring to a single spectrum, you shouldn't use the term "spectra."
thanka ya!
Electrons don't orbit in a circular path otherwise they would be accelerating and lose energy and crash into the nucleus.
Indeed, but this theory uses the Bohr model. Every model is wrong, but some are useful.
Gmod explanations > Every other teaching method
UNIS, 2450 FDR Drive, New York, NY,10010
couple 'o' people!
Asad habibi - that is the last thing I want! - good luck in the exams (The journal of chemical education rejected my article 2 or 3 times)
i love you
HA you cant fool me. i know there SHOULD be a shower in a chemestry room incase a student gets potentionaly dangerous liquids on him. :3
visable.... hmm sounds like product placement ;)
For hydrogen n =1 only
"who put a shower inn a chemistry room"
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don't you take her
OOK I WILL NOT STAND FOR THIS OK
sir, you are the shit
When you spelt visible wrong lmao
skert
America has win zat ho oqat ho