I just realised that his tie is the periodic table, I adore this man so much! This whole series is so informative and wholesome I want to cry with joy!
absolutely LOVE these videos.. they always help me before my science exams. these concepts get clear because you can visualize it with the help of these videos
From what I remember from a brief attempt at chemistry, one of the funny things of buckyballs/fullerenes was that adding a group to one point of the ball, changed the energy (and usually making it easier) to add the group to the next position. Basically you got only a few products, all 60 positions reacted, or none at all. (or slightly less when there was steric hindrance)
I cannot thank you enough for this video. You are the first of about five videos that I've watched that explained carbon in a manner that was attainable thorough simplistic and helpful.
When you have hair like that, everyone just assumes you're a scientist. They'd probably get suspicious if his bag DIDN'T contain any weird-looking gadgets.
If they made videos one hour for each element, I would also watch all of them. Since I was a child I always wanted to know everything about elements and their chemistry. Totally fascinating
These videos are awesome! Thank you for taking the time to make a video for each element and not just one for the whole PT. It's super interesting and I'm really inspired by your dedication!
Really like the videos! I'm an undergraduate Computer Science student, but still love these videos! They spark my imagination and make me want to take a few Chemistry classes! I often think of Chemistry as the study of programming nature, and got to thinking about it, and was wondering how a Chemist thinks of Computer Science?
basically yes, considering electricity is the transfer of electrons, if something has strong bonds it is less likely if if not unwilling to give up electrons ..
No. It is just a rough explanation of why diamonds are transparent (because there are no electrons that can be excited by visible radiation). However there are plenty of clear/ colourless/ transparent substances with electrons in double bonds and other structures that might absorb light but they absorb in the UV eg perspex.
I love the new electron miscroskope images your showing usw... amazing how the molecules actually look exactly like the models you see at school when you take a close look at them in the scope... sounds stupid, but that kind of amazes me...
Interesting video on Carbon.. What a coincidence I happened to see this today! Only yesterday I was teaching a local school children on Carbon different forms as per their curriculum. Nothing will make the topic clearer than seeing this video!1 Today ia hope to show this to them. Great work by Martyn to young generations , possible future Noble Laureattes.
He didn't mention the use of Carbon to make steel. If you add 0.4% carbon to pure iron, you get a much harder, stronger metal which we call steel. Actually, there are hundreds of different alloys of steel that have other elements added. Maybe he mentions this in his video about Iron.
Something really want to ask: Silicon is in the same group of carbon, or other elements in that group as well. Why can't those elements also form these wide variety of molecule chains? just like the way carbon does? Especially for silicon regarding its huge abundance
Because Silcon-Silicon bonds are not as strong as Carbon-Carbon bonds. The reason for this is that the Silicon atoms are larger than Carbon atoms, so their electrons are a greater distance from the nucleus and require less energy to break. You can have chains of Silicon atoms, but they are limited to about seven atoms long before they become unstable. Credit to knockhardy.org.uk
i think it's due to its reactivity and larger size. Other atoms can interact with silicon atom through its d-orbitals which makes silicon atom more susceptible to nucleophilic reactions whereas carbon is more stable, especially if it is tetra-substituted.
Silicon can catenate (form long chains), however not as easily as carbon and the reason is carbon has a smaller atomic radius and the same shielding effect on its valence shell of electrons. Hence, carbon has a higher electronegativity and can more easily form the covalent bonds required to form these long chains. Silicon can as well, but the chains formed by carbon are far more stable because of its higher electronegativity, resulting from its smaller atomic radius.
Carbon has a huge amount of information and uses. He hasn't talked about its hybridized sp orbitals, 2s2 2p2 electrons have 4 electrons in hybridized sp orbitals. Are these talks about inorganic and not about organic chemistry? But buckyballs were covered in organic chemistry textbooks, too.
@Noovil25 you see the color that it didn't absorb. The color it reflects. The best example ist if you look at dichromatic mirrors (or short "dichro") widely used in laser applications. They only reflect one certain color, so they look like the color they reflect. The light they let through, is "the rest" which was not reflected.
Can someone tell where to get such super quality molecular model set at reasonable cost? Several available on Amazon and I ordered one. But it is hopeless.
I'm very hopeful of breakthroughs concerning graphene in the near future. Carbon has so much significance in our lives, yet only up until now scientists have started unlocking its full potential. I'm glad to have been born in this day and age.
I've never thought before why diamond is transparent. Now I understand it clearly. Once we are able to manufacture sheets of it, how effective would a window made from diamond be?
@@winter4505 Depends on the form (allotrope) Many countries have Coal, Anthracite is probably the purest form of carbon that is a coal type. Africa and some other countries have Diamond, it occurs in ancient volcanic pipes in a rock type called kimberlite. Graphite occurs in metamorphic rocks, thus it too will be associated with igneous rocks to some extent as it is the presence of such along with the heat and pressure that causes the alteration of carbon into graphite, not sure exactly how but google will pull that one up.
Boyle is one of my favorites. You can change what temp things freeze at or turn into gas or even plasma just by changing the pressure of the air. I think one of the gases close to neon does something cool if you give it less then normal air pressure, it turns into plasma if you electrify it. Sure water crystalizes at 32F so you think of coldness when you think of freezing but other things can freeze and crystalize at room temperature or even higher
in a hexagonal carbon ring, can each carbon atom form a molecular bond with another element, and if so, than how many electrons does each atom need to fill outer electron shell?
Is that a black and white drawing/artwork of Sri lankan/Kandyan Perahara left to the clock..? BTW, I'm binge watching the whole playlist of periodic table this time.
Who remembers the Star Trek movie, where the ...villain robot (V'ger) refers to the humans as "Carbon Units" ? Hahahahaha ! Dear Professor, and the rest of the Team, thank you so much for this excellent video. One of your best.
@pawningcity C60/70 are discrete molecules. The solvent can move around between the individual molecules and interact with them, which allows them to dissolve. In something like graphite/diamond you have big huge sheets/structures of carbon, these wont dissolve simply because the structures are so large the solvent cant get in between to break anything up.
Capacity might not be the right word, but the unprecedented capability of any organism to produce fine chemicals is indeed amazing. Even more so given that organisms have only a limited supply of catalysts and reagents, and yet they can always make them. Of course when one considers the 4.3 or so thousand million years of evolution that have lead to this, it becomes a little less impressive, but nevertheless still immensely amazing.
don't know why C-50 wasn't mentioned. i discussed this cool video on my enviroblog the other day, see the Hazard Hot Sheet, the post titled "The Sixth Element," for the tip of the hat. i love u guys! wish i could win a Nobel with some tape.
@giltine002 You have a point there... i hadn't even thought about that. About the mesomeric structures you are partly right,but you should look at it more like delocalized bonds. They can be delocalized in a way that forms a C=C bond for a short amount of time, but that is rather improbable. They way our teacher wanted us to look at it was like 1 1/2 bond between carbon atoms. But since you made your point, i'm unsure if my theory is right because the rings are not really defined.
There is one more allotrope called Lonsdaleite - also known as "hexagonal diamond" - which is diamond with hexagonal crystal lattice instead of normal cubic lattice - such cramped structure might make it over 50% harder than normal diamond. This kind of diamond can be formed under the most extreme conditions, like meteorite impact.
What material is in the type of grey pencil that turns blue and bitter when licked? It made a poor pencil because for it to leave any mark it had to be pressed real hard to the paper.
Could have mentioned that C60 and C70 are named "fullerenes" after Buckminster Fuller, because the molecules resemble his geodesic domes. C60 is called Buckminsterullerene ore "Bucky balls."
So Carbon absorbs all visible wavelengths of light so it appears black. But how far into the infrared and/or ultraviolet does it also absorb through too?
