Wow! blown away. I didn't expect this video would keep me riveted to the screen more than your videos on physics! But it did. Chemistry used to give me cold sweats in high school. But you made it sound so interesting. Bravo and thank you.
Sorry some issue with YT app. Not able to create new comment so replying here. What a great video. This solved many of my questions firein l from my highschool days. I am 47yrs old now. This clears my phy chem bio doubts. This clears multiple years of fundamentals and touched many concepts. Acid bases, pH values, periodic table, energy levels, phy concepts of electron clouds, orbitals, bonds. One question I have may be it is the way animation is made. You mentioned about covalent bond where electrons are shared, and ionic bond where electrons are transferred, HCl has covalent bond but when dissolved in water it breaks covalent bond and becomes ionic bond? Since hydrogen is transferred to water molecule?
Although higher electronegativity leads to polarity, the large atoms like iodine an xenon can be *polarized* because they are "soft" in the sense that outermost shells are bound weakly and can be squished or displaced with respect to nucleus - this is why e.g. xenon can form various compounds and iodine can become hypervalent, violating the octet rule.
Pedantic commenter here. First of all, great overview. I have some comments. 1. Thank you for using the latest periodic table. But that might need to be updated in a few years. 2. Technically it was de Broglie, not Schrodinger that first treated electron as wave. 3. Regarding polar molecule, difference in electronegativity by itself is not enough. For example, methane is CH4. C-H bond is polar. But CH4 molecule is non polar. 4. Regarding acid and base, that was a great example. I personally prefer Lewis model over Bronsted-Lowry. But BL model is quite useful by itself. P.S. I am a physical (computational, to be more precise) chemist by training. So I can relate to the video.
The difference in electronegativity between carbon and hydrogen is not that big to be considered polar but i think you mean something like BF3 not being polar due to the cancellation of dipole moments, right?
CH4 does have an octupole moment, however. Also, H2O wouldn't have a dipole moment if it didn't have a bent shape, due to sp3 hybridized orbitals. But the bent shape is slightly modified by Bent's rule.
@@edgardodeleon7058 As far as I know, every time I calculate the partial charges of C in CH4, it had always been negative. Might be small, but still nonzero. Hence, polar bond.
Hi Dr. Ash, I have a question for you that intrigues myself quite a bit: If protons and neutrons are both composed of quarks (UUD and UDD, respectively), why do we refer to protons and neutrons instead of the total number of quarks when we talk about atomic nuclei? Isn't it the strong nuclear force that holds the atomic nucleus together, as well as the quarks inside the nucleon? Don't the quarks in one nucleon have the possibility of interacting with the quarks in another nucleon directly? I mean, in the same way that they interact within the nucleon itself? Thx for your meaningful explanations about the underlyings of the world we see everyday!
Great question! There is a phenomenon called "color confinement" that keeps the three quarks of the nucleon tied to each other. have two videos about it here if you want more details: th-cam.com/video/WF2c_jzefKc/w-d-xo.html th-cam.com/video/KnbrRhkJCRk/w-d-xo.html -- essentially, three quarks help to maintain a "neutral" color charge which is confined within each nucleon. If the quarks try to get apart from each other, they are pulled back. If they stretch too far apart, the energy creates a new quark/antiquark pair or meson. In fact there is a residual, non direct interaction from one nucleon to another via these mesons. This is called the residual strong force or strong nuclear force. This is the force that keeps nucleons bound to each other inside a nucleus. If you watch the videos at the links, I think this will make more sense.
@@ArvinAsh ohh, nice! I knew about the meson formation but I didn't know they're responsible for the indirect strong force between the nucleons! Thx for the links, I'll watch ASAP 🥰🥰
@@mrtienphysics666 Eating food is a biological process. Ultimately, all of those biological processes are chemistry. Ultimately, all of that chemistry is physics. Ultimately, all of that physics is math.
I wish I had this video way back in high school. Struggled in my chemistry class because I never got a good explanation for why anything did what it did.
I am going to watch this 20 times, it is so relevant to my study of archival knowledge of oil paintings. This is the basic physics to which governs things for PH and its link to deteriorating bonds, and the reason things with lower PH are reactive to moisture.
Damn! I felt the same way: I didn't understand High School Chemistry until I studied the Schrödinger Equation in my Senior Year as a Physics Major. "General Chemistry" by Linus Pauling (Dover, 1970) is a great read. It starts with a good discussion of the Atomic Theory of Matter before diving into Chemistry.
Arvin, I'm so glad I stumbled upon you. I'm 75 and I need a review of chemistry. I I asked it when I was young. The details have gotten foggy, not the fundamental ideas. Thanks!
"General Chemistry" by Linus Pauling (Dover, 1970) is a great read. It starts with a good discussion of the Atomic Theory of Matter before diving into Chemistry.
This video is actually really great its such an underrated crossroad that helps with understanding both sides of pH and oxidation clearly through atomic interaction. 👏👍
I wish that I had heard his introduction 50 years ago. I also hated chemistry, which just seemed like an uncoordinated memory exercise as Arvin describes, so I packed it in at the first opportunity. But it was fundamentally different at A level and some familiarity might have been pretty useful later. It was a long time ago though, and there are a few other subjects I wish I'd hung on to. The UK system encouraged over-specialisation at the time, and possibly still does.
4:31 Sir, I think it's not the electrostatic attraction, as both sodium and chlorine have attained there nearest Nobel gas configurations (i.e., Ne and Ar respectively) ,but it's the lowering of lattice energy which brings them together. Correct me if I am wrong👉👈
The electrostatic force keeps them tightly together no matter whether a crystal has been formed or the salt is in an amorphous state. The lattice energy comes in play a little bit later when the actual lattice forms. Also, a small observation, the lattice energy can't be lowered, it's pretty much a constant. Its release lowers the overall energy of the system, which stabilises it, would be a more correct explanation.
@@satyajeetbose2931 don't worry, it often happens that we get a concept slightly wrong (although we get the hang of it), but most of these issues will be solved in the long run. Good luck and happy new year!
Thank you so much for this video Arvin, if this video existed back when I was in high school chemistry class I would have gotten a better grade than a D
I find it fascinating that atoms are layered like little Matryoshka dolls (the russian stacking dolls) because every element has the exact electron configuration of the nearest noble gas before it and inside that is electron configuration of the previous noble gas etc. So xenon contains krypton inside it which contains argon, which contains neon, which contains helium buried deep inside. The magnesium ion, for example, looks like neon, except having two more protons in its nucleus, binding the full shell even stronger (magnesium is so "hard" that even two hydride ions won't stretch it). That's why removing two electrons off the magnesium metal is easy (about 700 and 1 400 kJ/mol) but the next electron would take a whopping 7 700 kJ to remove as it is bound several times more strongly than the outermost electron in neon.
2:00 sir but aren't the matter waves just an area where a matter is bound to be found, so isn't this statement incorrect as it should be it actually is matter which happens to be seen like a wave Please respond sir
See I LOVED the theory portion of my Physical Chemistry courses. I could talk and listen abut quantum mechanics and thermodynamics, but I sucked at remembering the formulas and when to use them and when to manipulate them into other equations. So I ended up disliking the courses overall, which kinda sucked. I can do differential calculus but I can't do it straight from memory, just not how my brain works I guess. I passed well enough, but I wish I was better at it.
@Arvin - Hello. It seems you've incorrectly depicted electrons existing in flight again 1:48. Excited electrons actually barely move. You can verify this as measuring the current on the anode and cathode of the emitter and finding the same relative amount of current on both. Electrons are not being emitted. Virtual photons are.
Arvin has these whole library of super interesting videos. He has the ability to explain complicated things in an entertaining yet serious manner. I just can’t help but enjoy these videos immensely . Thank you Arvin!! ❤🎉😊
Haha. Indeed. At my college, it was voted "the most difficult undergrad class" at the school. I'm was he only person i know that enjoyed that class. Most people suffered through it because it was required for their major. So don't feel so bad.
Terrific video. In my freshman year, I threw my chemistry text against the wall because I couldn't understand any of the explanations. I hated chemistry. But now was a biologist, I love it. In retrospect, it was a very poorly written book.
Does H3O+ have less polarity (electron distribution more uniform) compared to HCl? If so, can it be said that acid-base reactions occur so that molecules can have more uniform electron distributions (even if some of those molecules end up having net charge)?
But why do Hydrogens bind to Oxygen in water in such a way that the molecule becomes polar? Why doesn't one Hydrogen attach on the other end of the molecule?
Hydrogen is placed in the leftmost column of the Periodic Table because it has one electron in its outermost (valence) shell. But because two electrons would fill that shell (as in the helium atom), a hydrogen atom is also one electron short of having its outermost shell filled, just like the elements in the column containing chlorine and fluorine. So it would be helpful to discuss why hydrogen doesn't behave chemically like chlorine.
I would guess that that has a lot to do with the nuclear force. Hydrogen has only 1 proton and 1 shell. Chlorine has 17 and Flourine has 9. They also need one electron to fill the outershell but have valence electrons close enough to the nucleus and enough of a nuclear charge to pull in electrons much stronger. As to why it doesn't behave chemically like the halogens, hydrogen is sometimes considered to be part of its own category, they just kinda fit it up there at the top. I don't know enough for that specific of chemistry but id try taking to some really smart people on quora.
>andrewrazzano3118 : The problem with your explanation is that the protons' attraction is "cancelled" by the repulsion by the equal number of electrons that surround the nucleus. An atom is electrically neutral.
Great video that really built on my basic understanding of molecular bonds. I'd love to see a follow-up that explains how the sub-atomic processes lead to the macroscopic effects that we're familiar with when it comes to acids
One thing not mentioned in this video is orbital hybridization and bonding/anti-bonding orbitals. It's definitely more complicated than what this video is going for, but that really helped explain what was happening when things bonded.
Strong acids disrupt the chemical bonds holding the structure together, but donating H+ which causes new chemical bonds, causing the substances existing bonds to break. This breaks down the substance into smaller parts which then dissolve in water.
What always blows my mind is that no one understood any of this as late as the end of the 19th century. It would have been so frustrating to study chemistry back then.
I attempted to comprehend an Iodine clock reaction at the quantum mechanical level and it almost pulverized my brain. Varying redox, proton transfer mechanisms & the interplay with the bulk water matrix were a rabbit hole I would still be stuck in if I had not walked away from attempting a quantum level understanding.........but I KNOW it's ultimately the driving effect behind the kinetics.
@@oszb Nothing to smoke. I have aspergers and imagine 4D geometry. Specufucally Hyperspheres / cardioids. No need to be rude. I think you were trying to be rude?
There are more factors involved. With HF, it's not such a strong acid because the H-F bond is so strong that the F does not give up the proton in aqueous solution very easily.
There's one thing you're missing when it comes to strenght of acids. One might think that hydrofluoric acid is stronger acid than hydrochloric acid because fluorine is more electronegative than chlorine. It's vice versa HCl is magnitudes stronger than HF. In fact the strongest of hydrohalogen acids is hydroiodic acid the least electronegative of the halogens! This is because the stability of the conjugate base matters. Fluoride ion has the highest charge density and is thus the least stable. The largest iodide ion is the most stable due to its lower charge density.
Dearest Marvin, thank you for ALL your wonderful work. Please note: It is common in, the Physicist Community, to make this same overstatement. The Schrodinger Equation determines NOTHING... The Schrodinger Equation DESCRIBES... Existence will got along just fine without the EXISTENCE of Schrodinger, let alone his Equations...... Respectfully, 🙂 Jason Miller
Teaching by attributing "wants" to electrons, protons, atoms, or molecules seems problematic. Can't we use probability, likelihood, or tendency instead?
You hint at the quantum mechanics underpinning and mentionn electron probability clouds and then proceed to use all conventional terms, visual models etc. that are found in chemistry text books since ages. I don´t get it! What is the new here that makes chemistry more comprensible?
Question: What determines if two atoms will form a covalent bond or an ionic bond? Does it have to do with relative sizes, as in the Sodium/Chlorine example being about the same size and the oxygen/hydrogen example being very different sizes (maybe number of electrons in the outer shell)? I very much liked the total explanation. Happy Holidays to me (us)!
It's been a long time since I studied Chemistry, but unless I'm mistaken, the group 1 and 2 metals have a propensity to give up an electron because doing so can result in a more energetically stable outer shell configuration. If you have 1 or 2 electrons in the outer shell it is more likely that you will "give them" ionically to an atom that is 1 or 2 electrons short of a full outer shell, rather than gaining another 6 or 7 through covalent bonding. However I believe that certain metals can form bonds that may be more covalent than ionic in character if I recall correctly (which I might not).
Ionic bonds are an abstraction that don't really exist. You can have a perfect covalent bond if your bond is symmetrical, but the electron will never be totally stripped away, otherwise there would be no bond anymore. Covalent bonds can be more or less polarized, and in NaCl for example, about 2/3 of the bond energy can be described by the attraction between Na+ and Cl-, which is why we say it is mainly ionic. But the vast majority of bonds are mainly covalent and this ionic contribution is generally small.
In conclusion, the secret of acid-base quantum mechanics lies in the powerful combination of quantum mechanical principles and acid-base chemistry. This synergy enables researchers to gain deeper insights into the intricate world of acid-base reactions.
Polypeptides are not absorbed. They have to be further broken down into amino acids or at least tripeptides in the small intestine (with the use of other enzymes like trypsin and chymotrypsin) to be absorbed. But thank you for the video.
Go to mudwtr.com/ARVINASH to try your new morning ritual.
LOVE AND RESPECT ❤️❤️❤️❤️❤️❤️❤️❤️❤️
Wow! blown away. I didn't expect this video would keep me riveted to the screen more than your videos on physics! But it did. Chemistry used to give me cold sweats in high school. But you made it sound so interesting. Bravo and thank you.
Sorry some issue with YT app. Not able to create new comment so replying here.
What a great video. This solved many of my questions firein l from my highschool days. I am 47yrs old now. This clears my phy chem bio doubts. This clears multiple years of fundamentals and touched many concepts. Acid bases, pH values, periodic table, energy levels, phy concepts of electron clouds, orbitals, bonds.
One question I have may be it is the way animation is made. You mentioned about covalent bond where electrons are shared, and ionic bond where electrons are transferred, HCl has covalent bond but when dissolved in water it breaks covalent bond and becomes ionic bond? Since hydrogen is transferred to water molecule?
I always thought Arvin was a bit of a Square, but I read the title and found out he's doing physics on acid now. What a wild guy, good for him.
He can smell colors now!
Yes, I can now smell colors, fly without wings, see stars inside a flower, and have conversations with myself.
Your comment gave a me good chuckle 😂👏
What does a Square mean?
@hozukimaru nerd someone who studies a lot
Although higher electronegativity leads to polarity, the large atoms like iodine an xenon can be *polarized* because they are "soft" in the sense that outermost shells are bound weakly and can be squished or displaced with respect to nucleus - this is why e.g. xenon can form various compounds and iodine can become hypervalent, violating the octet rule.
Xenon lightbulb.
Pedantic commenter here.
First of all, great overview. I have some comments.
1. Thank you for using the latest periodic table. But that might need to be updated in a few years.
2. Technically it was de Broglie, not Schrodinger that first treated electron as wave.
3. Regarding polar molecule, difference in electronegativity by itself is not enough.
For example, methane is CH4. C-H bond is polar. But CH4 molecule is non polar.
4. Regarding acid and base, that was a great example.
I personally prefer Lewis model over Bronsted-Lowry. But BL model is quite useful by itself.
P.S. I am a physical (computational, to be more precise) chemist by training. So I can relate to the video.
Nice comments! Thank you.
The difference in electronegativity between carbon and hydrogen is not that big to be considered polar but i think you mean something like BF3 not being polar due to the cancellation of dipole moments, right?
CH4 does have an octupole moment, however. Also, H2O wouldn't have a dipole moment if it didn't have a bent shape, due to sp3 hybridized orbitals. But the bent shape is slightly modified by Bent's rule.
@@edgardodeleon7058 As far as I know, every time I calculate the partial charges of C in CH4, it had always been negative. Might be small, but still nonzero. Hence, polar bond.
@@afriedrich1452 Exactly.
I think only highly symmetrical molecules have no octupole moment.
Like, they must have octahedral symmetry or higher.
Hi Dr. Ash, I have a question for you that intrigues myself quite a bit: If protons and neutrons are both composed of quarks (UUD and UDD, respectively), why do we refer to protons and neutrons instead of the total number of quarks when we talk about atomic nuclei? Isn't it the strong nuclear force that holds the atomic nucleus together, as well as the quarks inside the nucleon? Don't the quarks in one nucleon have the possibility of interacting with the quarks in another nucleon directly? I mean, in the same way that they interact within the nucleon itself?
Thx for your meaningful explanations about the underlyings of the world we see everyday!
Great question! There is a phenomenon called "color confinement" that keeps the three quarks of the nucleon tied to each other. have two videos about it here if you want more details: th-cam.com/video/WF2c_jzefKc/w-d-xo.html th-cam.com/video/KnbrRhkJCRk/w-d-xo.html -- essentially, three quarks help to maintain a "neutral" color charge which is confined within each nucleon. If the quarks try to get apart from each other, they are pulled back. If they stretch too far apart, the energy creates a new quark/antiquark pair or meson. In fact there is a residual, non direct interaction from one nucleon to another via these mesons. This is called the residual strong force or strong nuclear force. This is the force that keeps nucleons bound to each other inside a nucleus. If you watch the videos at the links, I think this will make more sense.
@@ArvinAsh ohh, nice! I knew about the meson formation but I didn't know they're responsible for the indirect strong force between the nucleons! Thx for the links, I'll watch ASAP 🥰🥰
wow. physics, chemistry and biology in one single breath. salute.
All biology is chemistry.
All chemistry is physics.
All physics is math.
Math is everything, everything is math.
@@rockets4kids math is everything, so you can eat math when you are hungry? lol
@@mrtienphysics666 Eating food is a biological process. Ultimately, all of those biological processes are chemistry. Ultimately, all of that chemistry is physics. Ultimately, all of that physics is math.
@@rockets4kids you are confusing 3 apples with the number 3. Math is not physics.
@@mrtienphysics666 Learn to read. I never said math was physics. I said physics was ultimately math.
I wish I had this video way back in high school. Struggled in my chemistry class because I never got a good explanation for why anything did what it did.
Yea most people will feels like this
Well thats the school system
@berlinisvictorious school system kinda makes it harder, but I understand we need to ”short cut” it
I am going to watch this 20 times, it is so relevant to my study of archival knowledge of oil paintings. This is the basic physics to which governs things for PH and its link to deteriorating bonds, and the reason things with lower PH are reactive to moisture.
Please share more
I raise 10!
LOVED this explanation Arvin! Wish you (and TH-cam) were around when I took high school chemistry class.
I'm glad you found it helpful! I wish YT was around too!
Same!!!! I sure could have used TH-cam in general when I was in college (96-02)!
We mean digital video public sharing right. Because TH-cam's monopoly and censorship combo is a huge problem
Damn! I felt the same way: I didn't understand High School Chemistry until I studied the Schrödinger Equation in my Senior Year as a Physics Major.
"General Chemistry" by Linus Pauling (Dover, 1970) is a great read. It starts with a good discussion of the Atomic Theory of Matter before diving into Chemistry.
This explains sssssooooo much. 66 years on earth before understanding acids😩
In high school you were a classical student and in the college level you changed to quantum student. Got it!
Arvin, I'm so glad I stumbled upon you. I'm 75 and I need a review of chemistry. I I asked it when I was young. The details have gotten foggy, not the fundamental ideas. Thanks!
I asked my organic chemistry professor to teach us more quantum mechanics!
"General Chemistry" by Linus Pauling (Dover, 1970) is a great read. It starts with a good discussion of the Atomic Theory of Matter before diving into Chemistry.
That's not their job. Stop being selfish and expect someone else to bend to your whim
Only quantum chemistry knowledge you need in ochem is the concept of HOMO, LUMO and orbitals
This video is actually really great its such an underrated crossroad that helps with understanding both sides of pH and oxidation clearly through atomic interaction. 👏👍
im doing industrial chemistry and atleast i can make sense of what this polarity means in water ,salute sir i love your intuition
I wish that I had heard his introduction 50 years ago. I also hated chemistry, which just seemed like an uncoordinated memory exercise as Arvin describes, so I packed it in at the first opportunity. But it was fundamentally different at A level and some familiarity might have been pretty useful later.
It was a long time ago though, and there are a few other subjects I wish I'd hung on to. The UK system encouraged over-specialisation at the time, and possibly still does.
Excellent explanations! Thank you so much, this is beautiful to see.
You are a very good teacher, Arvin. Keep it up.
Cordyceps? Do you want a zombie apocalypse? Cause that's how you get a zombie apocalypse.
Dude, it ain't like the last of us.😂
Zombies are the most impossible sci-fi characters.
Great vid! Me, MD for 30 years, undergrad Biochemistry (now called Molecular Biology). Thanks for refreshing my memory on Chemistry!
4:31 Sir, I think it's not the electrostatic attraction, as both sodium and chlorine have attained there nearest Nobel gas configurations (i.e., Ne and Ar respectively) ,but it's the lowering of lattice energy which brings them together.
Correct me if I am wrong👉👈
The electrostatic force keeps them tightly together no matter whether a crystal has been formed or the salt is in an amorphous state. The lattice energy comes in play a little bit later when the actual lattice forms. Also, a small observation, the lattice energy can't be lowered, it's pretty much a constant. Its release lowers the overall energy of the system, which stabilises it, would be a more correct explanation.
@dariusalendru7479
Thank you so much Sir for taking the time to correct my comment.❤
It seems that school taught me a wrong concept.😢
@@satyajeetbose2931 don't worry, it often happens that we get a concept slightly wrong (although we get the hang of it), but most of these issues will be solved in the long run. Good luck and happy new year!
@@dariusalexandru7479 Happy New Year to you too Sir🥰🎊!
Thanks for these encouraging lines🫂☺️
I hated chemistry class in school, I wish we watched this video first! Really good explanation and visuals to go along.
4:17 Doesn’t make sense because Sodium (Na) has 11 protons and electrons, not 12.
Thank you so much for this video Arvin, if this video existed back when I was in high school chemistry class I would have gotten a better grade than a D
I totally get where you're coming from!
I can relate. I wish I would've studied more, but I settled for the D for diploma.😢
As always Arvin you exceed your peers in excellence.
This was quite informative. I didn’t like chemistry in college either but Arvin is a great teacher.
I find it fascinating that atoms are layered like little Matryoshka dolls (the russian stacking dolls) because every element has the exact electron configuration of the nearest noble gas before it and inside that is electron configuration of the previous noble gas etc. So xenon contains krypton inside it which contains argon, which contains neon, which contains helium buried deep inside.
The magnesium ion, for example, looks like neon, except having two more protons in its nucleus, binding the full shell even stronger (magnesium is so "hard" that even two hydride ions won't stretch it). That's why removing two electrons off the magnesium metal is easy (about 700 and 1 400 kJ/mol) but the next electron would take a whopping 7 700 kJ to remove as it is bound several times more strongly than the outermost electron in neon.
When you look at things that way, it is beautiful. I'm far less thoughtful, to me its all hydrogen, helium and a whooooole lotta heat
russians have stolen the idea from Japanese Daruma dolls. Don't give those bastards a credit
Wow it was like visualizing acid base with quantum perspective. Very good nice detailing.
2:00 sir but aren't the matter waves just an area where a matter is bound to be found, so isn't this statement incorrect as it should be it actually is matter which happens to be seen like a wave
Please respond sir
See I LOVED the theory portion of my Physical Chemistry courses. I could talk and listen abut quantum mechanics and thermodynamics, but I sucked at remembering the formulas and when to use them and when to manipulate them into other equations. So I ended up disliking the courses overall, which kinda sucked. I can do differential calculus but I can't do it straight from memory, just not how my brain works I guess. I passed well enough, but I wish I was better at it.
The combo of your description and your imagery is really illuminating! I love this
@Arvin - Hello. It seems you've incorrectly depicted electrons existing in flight again 1:48. Excited electrons actually barely move. You can verify this as measuring the current on the anode and cathode of the emitter and finding the same relative amount of current on both. Electrons are not being emitted. Virtual photons are.
I was expecting something else when I read Acid and Quantum Mechanics
😂😂😂
Good presentation. It raises other questions in a student’s mind, which affirms the value of the talk.
Arvin has these whole library of super interesting videos. He has the ability to explain complicated things in an entertaining yet serious manner. I just can’t help but enjoy these videos immensely . Thank you Arvin!! ❤🎉😊
You have to be some sort of sadist to fall in love with college P-Chem. I still have PTSD from that class
Haha. Indeed. At my college, it was voted "the most difficult undergrad class" at the school. I'm was he only person i know that enjoyed that class. Most people suffered through it because it was required for their major. So don't feel so bad.
I like the way an ad comes in without interrupting with the video
Really good visual and animation ❤ made so easy to understand
You are incredible and your knowledge and enthusiasm are praiseworthy
I’ve been waiting for this video for 20+ years
Million subscribers, congratulations!
Thank you! 🙏
As Don Lincoln would say: physics is everything 💜 great video, Arvin!
@2:45 you refer to a valance shell, this should read valence shell.
Thanks for that. Wish you were my video editing checker!
Great video, now I understand better the nature of bonds. In 4:44 can you explain also why the H2O bonds are not straight but angled?
Incredible explanation and visuals. Thank you.
thank you. i have learned a lot from this
Terrific video. In my freshman year, I threw my chemistry text against the wall because I couldn't understand any of the explanations. I hated chemistry. But now was a biologist, I love it. In retrospect, it was a very poorly written book.
Great animated illustrations in this one
Thanks for the lesson, good work Paul
So cool! Never heard a talk like this before that used the Shröedinger equation to explain the action of protons and electrons in chemistry.
Does H3O+ have less polarity (electron distribution more uniform) compared to HCl?
If so, can it be said that acid-base reactions occur so that molecules can have more uniform electron distributions (even if some of those molecules end up having net charge)?
Please more of such videos about chemistry
But why do Hydrogens bind to Oxygen in water in such a way that the molecule becomes polar? Why doesn't one Hydrogen attach on the other end of the molecule?
It's the most optimal arrangement to minimize repulsion between hydrogen atoms while maintaining attraction with the oxygen atom.
As always another awesome intuitive video ❤ from India
Hydrogen is placed in the leftmost column of the Periodic Table because it has one electron in its outermost (valence) shell. But because two electrons would fill that shell (as in the helium atom), a hydrogen atom is also one electron short of having its outermost shell filled, just like the elements in the column containing chlorine and fluorine. So it would be helpful to discuss why hydrogen doesn't behave chemically like chlorine.
I would guess that that has a lot to do with the nuclear force. Hydrogen has only 1 proton and 1 shell. Chlorine has 17 and Flourine has 9. They also need one electron to fill the outershell but have valence electrons close enough to the nucleus and enough of a nuclear charge to pull in electrons much stronger. As to why it doesn't behave chemically like the halogens, hydrogen is sometimes considered to be part of its own category, they just kinda fit it up there at the top. I don't know enough for that specific of chemistry but id try taking to some really smart people on quora.
>andrewrazzano3118 : The problem with your explanation is that the protons' attraction is "cancelled" by the repulsion by the equal number of electrons that surround the nucleus. An atom is electrically neutral.
Hmmm... this is the exact same explanation as we get in schools in Sweden. I was hoping for a bit more quantum mechanics and math.
Great video that really built on my basic understanding of molecular bonds. I'd love to see a follow-up that explains how the sub-atomic processes lead to the macroscopic effects that we're familiar with when it comes to acids
One thing not mentioned in this video is orbital hybridization and bonding/anti-bonding orbitals. It's definitely more complicated than what this video is going for, but that really helped explain what was happening when things bonded.
3:25 Also can you explain the reason behind the auf-bau rule(n+l rule).Why do orbitals whuch have a greater value of (n+l) have higher energy.
THANKS FOR THE VIDEO BROTHER ❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️
All these year i have been waiting for this topic
0:08 if i got the same explanation in high school i wouldnt have failed chemistry twice 😂😂
Thank you! So why/how do acids dissolve stuff?
Strong acids disrupt the chemical bonds holding the structure together, but donating H+ which causes new chemical bonds, causing the substances existing bonds to break. This breaks down the substance into smaller parts which then dissolve in water.
@ Of course! Thank you for that clear concise and prompt answer!
I learned all of this in Highschool chemistry, I guess my chemistry teacher was greater than I thought he was.
although I already got after studying but I appreciate the illustration that makes easier to grasp things.
Thankyou. Your fascination is catching.
What always blows my mind is that no one understood any of this as late as the end of the 19th century. It would have been so frustrating to study chemistry back then.
I attempted to comprehend an Iodine clock reaction at the quantum mechanical level and it almost pulverized my brain. Varying redox, proton transfer mechanisms & the interplay with the bulk water matrix were a rabbit hole I would still be stuck in if I had not walked away from attempting a quantum level understanding.........but I KNOW it's ultimately the driving effect behind the kinetics.
petrol can burn in three ways : oxidation (chemical reaction with oxygen), thermo nuclear fission or interaction with anti-matter petrol. Correct?
Thanks - enjoyed this very much.
It's all charge. And charge is curvature of space-time. Electrons intersecting everywhere. It's like a 4D moire pattern
This is nonsense, but hit me up if you got any of that stuff left to smoke.
@@oszb Nothing to smoke. I have aspergers and imagine 4D geometry. Specufucally Hyperspheres / cardioids. No need to be rude. I think you were trying to be rude?
Can you visualize your life in the last 24 hours as a 4D pattern viewed from different angles and distances?
I know this is a pretty crazy thing to ask, but I thought it was worth a try😜
Wish I had you in high school.
This helped me so much, thank you!
I’m just pleased to see Arvin on the gloomy London day.
8:35 with that logic HF must be the strongest acid, H2O must be stronger acid than H2S, etc.
There are more factors involved. With HF, it's not such a strong acid because the H-F bond is so strong that the F does not give up the proton in aqueous solution very easily.
This is a common discussion in advanced chem classes.
Thank you so much for this illuminating presentation. However , need more ...what about bases,salts etc! A kind of short series...
Plz have a video on Earth's magnetic field 😢😢
We got we need to talk about the poly exclusion principle. Nobody understood electrons not collapse to the lowest energy level before Wolfgang Pauli.
I now am thinking of an electron as a negative energy wave rather than a particle, a cousin of a photon.
There's one thing you're missing when it comes to strenght of acids. One might think that hydrofluoric acid is stronger acid than hydrochloric acid because fluorine is more electronegative than chlorine. It's vice versa HCl is magnitudes stronger than HF. In fact the strongest of hydrohalogen acids is hydroiodic acid the least electronegative of the halogens!
This is because the stability of the conjugate base matters. Fluoride ion has the highest charge density and is thus the least stable. The largest iodide ion is the most stable due to its lower charge density.
Dearest Marvin, thank you for ALL your wonderful work. Please note: It is common in, the Physicist Community, to make this same overstatement. The Schrodinger Equation determines NOTHING... The Schrodinger Equation DESCRIBES... Existence will got along just fine without the EXISTENCE of Schrodinger, let alone his Equations...... Respectfully, 🙂 Jason Miller
I useless at Chemistry but I wonder what difference there would be if our atmosphere was different.
0:53 i have this exactly the same illustration of the Periodic Table of Elements Showing Electron Shells in my room 😮
Mud water. What an appetizing name!
Did you make any vid related to quantum reason of covalent bonding? If yes then please tell which one and it no can you make one?
Excellent!!
We had quantum mechanics in chemistry in high school. But the professor was nothing short of a wizard.
"All About That Base (No Acid)" ~ acapellascience2
th-cam.com/video/IAJsZWhj6GI/w-d-xo.html
Teaching by attributing "wants" to electrons, protons, atoms, or molecules seems problematic. Can't we use probability, likelihood, or tendency instead?
I never can understand that how electron clouds produce exact spectral lines and with only 1/137 difference.
You hint at the quantum mechanics underpinning and mentionn electron probability clouds and then proceed to use all conventional terms, visual models etc. that are found in chemistry text books since ages. I don´t get it! What is the new here that makes chemistry more comprensible?
You had that in University? In germany we have that in the higher classes of normal school.
Quantum mechanics in high school! That's impressive.
Physics is everything. :)
indeed!
You know so much, incredible
0:02 it’s all about the cones
Question: What determines if two atoms will form a covalent bond or an ionic bond? Does it have to do with relative sizes, as in the Sodium/Chlorine example being about the same size and the oxygen/hydrogen example being very different sizes (maybe number of electrons in the outer shell)? I very much liked the total explanation. Happy Holidays to me (us)!
It's been a long time since I studied Chemistry, but unless I'm mistaken, the group 1 and 2 metals have a propensity to give up an electron because doing so can result in a more energetically stable outer shell configuration. If you have 1 or 2 electrons in the outer shell it is more likely that you will "give them" ionically to an atom that is 1 or 2 electrons short of a full outer shell, rather than gaining another 6 or 7 through covalent bonding. However I believe that certain metals can form bonds that may be more covalent than ionic in character if I recall correctly (which I might not).
Ionic bonds are an abstraction that don't really exist. You can have a perfect covalent bond if your bond is symmetrical, but the electron will never be totally stripped away, otherwise there would be no bond anymore.
Covalent bonds can be more or less polarized, and in NaCl for example, about 2/3 of the bond energy can be described by the attraction between Na+ and Cl-, which is why we say it is mainly ionic.
But the vast majority of bonds are mainly covalent and this ionic contribution is generally small.
@@shiuay6165 Well that's how long it's been for me: Either I learnt that and forgot it, or it was never taught to me, even at university level.
@@shiuay6165 Thanks for the scoop :-)
@@80ssynthfan48 Thanks for the response :-)
In conclusion, the secret of acid-base quantum mechanics lies in the powerful combination of quantum mechanical principles and acid-base chemistry. This synergy enables researchers to gain deeper insights into the intricate world of acid-base reactions.
Polypeptides are not absorbed. They have to be further broken down into amino acids or at least tripeptides in the small intestine (with the use of other enzymes like trypsin and chymotrypsin) to be absorbed. But thank you for the video.
Banger outro music