You Mr. Masley are the coolest human being alive on this planet! thank you for saving the lives of thousands of IB kids. also more people should be seeing your videos!!
You are truly the best teacher on earth Mr. Masley!! No teacher has taught me in such a logical and clear way as you do. Thank you very much for the hard work you do!
ok wow. i watched this video the day of my physics exam while i was getting ready, not knowing any of it beforehand. not only did i get it, but i was able to re-explain what you had said in this video in the exam, getting me full marks in the section on spectra, and making me first in the class! THANKYOU !
THANK YOU, THANK YOU, THANK YOU !!! BRILLIANT, BRILLIANT, BRILLIANT VIDEO... VERY EASY TO UNDERSTAND... AMAZING AND THANK YOU FOR THE SHARING YOUR KNOWLEDGE... GOD BLESS !!!
Hi Andy, That is a simplified explanations for a starter spectroscopy. Please, permit me to ask. Do you know how I can get available spectral finger print datasets for carbon? Emphasis on C7 - C18 compounds.
When the particles absorb the wavelengths and send a photon out, does that photon have the same wavelength as when it was absorbed? And is it possible for the photon that got emitted to reach the detector nonetheless? Since photons are emitted why is it impossible for it to still reach the detector?Are they only emitted in certain directions?
This might be a dumb question, but does this atomic behavior describe how we see any material's color. Do different materials composed of multiple elements create a composed absorption spectra, and when white light is shun on that material, the reflected spectra associated to those atoms is the pigment of color we see on any given object/material? Like, does this behavior describe the color of any object and material that we see in the world?
Not a dumb question at all! That's great. This is actually similar to what happens when light is reflected. I'm actually not super knowledgeable about this but this thread might be a good place to start: www.quora.com/What-happen-at-an-atomic-scale-when-light-is-reflected
At 5:15, your wavelengths are wrong. 890 nm and 1400 nm are both infrared and 540 nm is green. At 7:30, this would also mean that atoms could emit any wavelength and electrons could collapse onto the nucleus. Visible hydrogen lines have lower integer 2 and upper integer 3, 4, 5, and 6.
I wasn't super careful with the wavelengths corresponding to the actual colors here correct, I didn't mean to advertise them as "this is the wavelength for purple, blue, and red" and would assume students wouldn't pay attention to the specific numbers.
Great explanation! It was very clear. Maybe this is covered in a further video, if not, can you explain the width of the absorption lines? If the levels are quantized and only photons with the exact energy are emmited/absorbed then those lines should be infinitesimally small in width. Does this quantization allows for a small margin? Is it the same for all elements?
I don't understand how can an atom absorb every single photon of a specific frequency that a star emits. There are huge numbers of photons emitted at the same time, all the time. And then you have a few atoms of sodium lying around, and they take all of the photons of that specific frequency? And once they take all of them, they never release them again? All those photons are released back instantaneously (or almost), and not withheld by the atom, so they should still reach the light detector. And while the atom is busy absorbing and releasing one photon, another one has time to pass by unabsorbed. And besides, there are so many other photons don't pass in the vicinity of that atom and they don't get absorbed, it's not as if they are attracted. They only get absorbed if they happen to hit the atom. So I am confused as to how the spectrum can be completely black in places, and not just maybe a bit faded.
Thanks for the clear explanation. Better explain than my chemistry teacher lol. I have a quick question, you explain that the absorption spectrum is make off photons with all wavelengths, does that just mean white light? Because white light is made up of all wavelengths of photons.
THE GREATEST EXPLANATION ON ABSORPTION AND EMISSION OF THE ATOMIC SPECTRA. JUST LOVING IT!!!!!!!!
Thanks so much!!
You Mr. Masley are the coolest human being alive on this planet! thank you for saving the lives of thousands of IB kids. also more people should be seeing your videos!!
You are truly the best teacher on earth Mr. Masley!! No teacher has taught me in such a logical and clear way as you do. Thank you very much for the hard work you do!
You are perfect at explaining. Step by step ,with nothing is missing. Thank you so much)
Youre an amazing teacher ive been trying to find someone who can explain this good u make it simple and easy to understand thank u so much
You legit explained it better than my textbook and teachers! Thanks alot, your videos mean alot to students like me 😢
If this was how every TH-camr explained it we wouldn't have suffered this much
Thanks sir🙏
U're the best
This is what I've been looking for to fully understand the absorption and emission spectra. Thank you very much!
ok wow. i watched this video the day of my physics exam while i was getting ready, not knowing any of it beforehand. not only did i get it, but i was able to re-explain what you had said in this video in the exam, getting me full marks in the section on spectra, and making me first in the class! THANKYOU !
Aaah that's amazing! So happy it was helpful!
THANK YOU, THANK YOU, THANK YOU !!! BRILLIANT, BRILLIANT, BRILLIANT VIDEO... VERY EASY TO UNDERSTAND... AMAZING AND THANK YOU FOR THE SHARING YOUR KNOWLEDGE... GOD BLESS !!!
Love your teaching style and the way you present key points!!
Best lecture about emission and absorption spectra .
Thank you very much for this amazing lecture! I understand it much better now. Keep inspiring us, students.
thank you so much sir, i never understood how absorption and emission spectra work until now :)
Perfect explanation! Thank you
Hi Andy,
That is a simplified explanations for a starter spectroscopy.
Please, permit me to ask.
Do you know how I can get available spectral finger print datasets for carbon?
Emphasis on C7 - C18 compounds.
greatest explanation ever, your videos are amazing
When the particles absorb the wavelengths and send a photon out, does that photon have the same wavelength as when it was absorbed? And is it possible for the photon that got emitted to reach the detector nonetheless? Since photons are emitted why is it impossible for it to still reach the detector?Are they only emitted in certain directions?
great videos. Hels me learn ally my physics and chem classes even better. Thx so much.
this was a perfectly detailed explanation, thank you!
This might be a dumb question, but does this atomic behavior describe how we see any material's color. Do different materials composed of multiple elements create a composed absorption spectra, and when white light is shun on that material, the reflected spectra associated to those atoms is the pigment of color we see on any given object/material? Like, does this behavior describe the color of any object and material that we see in the world?
Not a dumb question at all! That's great. This is actually similar to what happens when light is reflected. I'm actually not super knowledgeable about this but this thread might be a good place to start: www.quora.com/What-happen-at-an-atomic-scale-when-light-is-reflected
Amazing lesson
At 5:15, your wavelengths are wrong. 890 nm and 1400 nm are both infrared and 540 nm is green. At 7:30, this would also mean that atoms could emit any wavelength and electrons could collapse onto the nucleus. Visible hydrogen lines have lower integer 2 and upper integer 3, 4, 5, and 6.
I wasn't super careful with the wavelengths corresponding to the actual colors here correct, I didn't mean to advertise them as "this is the wavelength for purple, blue, and red" and would assume students wouldn't pay attention to the specific numbers.
Great explanation! It was very clear. Maybe this is covered in a further video, if not, can you explain the width of the absorption lines? If the levels are quantized and only photons with the exact energy are emmited/absorbed then those lines should be infinitesimally small in width. Does this quantization allows for a small margin? Is it the same for all elements?
Very good explanation...... hats off.......
That was excellent
Great 👍 Sir
What do you mean by all possible wavelengths? At 2:32
All the wavelengths of all radiations to ever exist
Excellent!
I don't understand how can an atom absorb every single photon of a specific frequency that a star emits. There are huge numbers of photons emitted at the same time, all the time. And then you have a few atoms of sodium lying around, and they take all of the photons of that specific frequency? And once they take all of them, they never release them again? All those photons are released back instantaneously (or almost), and not withheld by the atom, so they should still reach the light detector. And while the atom is busy absorbing and releasing one photon, another one has time to pass by unabsorbed. And besides, there are so many other photons don't pass in the vicinity of that atom and they don't get absorbed, it's not as if they are attracted. They only get absorbed if they happen to hit the atom. So I am confused as to how the spectrum can be completely black in places, and not just maybe a bit faded.
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Thanks for the clear explanation. Better explain than my chemistry teacher lol. I have a quick question, you explain that the absorption spectrum is make off photons with all wavelengths, does that just mean white light? Because white light is made up of all wavelengths of photons.
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Nice
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Thank you sir...
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I love you please accept my love
Accepted!
OMG HII YOU RESPONDED! My exam is in like 12 hours but you have not only helped revise but like u deadass helped teach me
Thank you sir nice explanation love from India