I enjoy watching your videos, usually. but today I'm just disappointed... 01:45 covalent bonds are definitely NOT stronger than ionic bonds... in fact ionic bonds have the highest bond energy (lattice energy) of any bonds thus being BY FAR the strongest! 03:12 WRONG! like so wrong it really hurts (again)! the carbon still has only 4 bonds it just crystalizes in a hexagonal structure. for carbon to have 5 bonds (which is technically possible, kinda...) you need VERY different conditions and these compounds are not as stable as to survive entering earths atmosphere, by far.
Hardness isn’t isotropic nor isobaric, thus nc-TiN/a-Si3N4 I rad is harder. Everything occurs naturally; you mean natively, wildly. thin → fine; would → should; There..here: pick one; big → great.
A thought experiment for you...we know what will happen if two planets collide, we know what happens if two planets enter the Roche limit of another...but what if we magically side step reality for a second and place a rocky planet directly on the surface of another planet? For example, what would happen if Mars suddenly appeared on the surface of the Earth in lets say the middle of relatively flat Australia? What happens to Mars? Will it roll due to its shape, compositions, or Earth's movements? Will it start to sink to the center with its weight/mass and gravity? Will it just crumble creating the biggest volcanic mountain pile in the solar system? What happens to the Earth? Its gravity, atmosphere, land/water, core.......?
Its great to wake up, have breakfast, and see a video about a paper you worked on for a decade! Thanks SciShow for spreading the word about our weird little rocks!
Small correction about the Lonsdaleite. It doesn't have carbon atoms with 6 bonds. It still has 4 bonds since carbon can can only form 4 bonds. The difference in material properties is entirely from the shape of its bonds. Diamond makes a cubic grids while lonsdaleite makes hexagonal grids.
That just sounds like a rad plot point for many Sci-Fi / Disaster stories: maniacal dudes who REQUIRE MORE MINERALS and can only figure out how to synthesize their spooky isotopes by going the old fashioned way and blowing up star systems. Then again, if you have enough power to smash two planets together, wouldn’t you have more than enough know-how to just synthesize it in a controlled lab environment? I guess that’s where the maniacal part comes in.
Might as well take this precious opportunity to tell people to listen to Fun City (Shadowrun Actual Play podcast GM’d by Mike Rugnetta) where alchemically systhesizing radioactive isotopes of magical elements and planets colliding are not only major plot points but also the most incredible narrative experiences I’ve had all year.
@@TheYuleTube i know someone who owns around 120 thousand carrots of Australian black opal he has been cutting them for around 40 years and has a absolutely insane mineral collection.
@@RalseiGaming That's super nice! I have a good bit, but nothing at all like that! Most of mine is lower cost Andamooka stones, still in the rough. I am learning how to process it myself. Still some nice stones to be had!
I remember having to do w report on this when I was in Chemistry in High School. It's one of those substances like Graphine is that when they figure out how to make itannd make it cheaply could have a massive impact on how we are manufacturing things.
Carbon in Londaleite bond to 4 neighboring carbons as well. What changes is the disposition of atoms through the planes (similar, but not exactly equal, as the close packing of similar spheres problem). The problem with the hexagonal packing is its anisotropic properties, which means that they change depending on orientation. That can be a big no no for some technical applications. Even though it's cool that there's a "harder" diamond, it's probably too expensive, rare and its properties probably arent different enough to justify its economical exploration. I might be wrong, though.
Actually graphite is very similar to diamond and is made up of the same bonds. The difference is that they form 2D plates of single carbon atoms and while the bonds holding the plates together are hard as diamond the forces keeping the plates together are extremely weak. This mix of hardness on a molecular level and softness on a physics level has led graphite to have some unique uses. For example the largest machines in the world use graphite as a lubericant. The strong bonds between the atoms allow them to support massive forces while the weak forces between the sheets means there isn't too much heat created. This is important cause carbon nanotubes are actually the exact same thing as graphite but instead of forming into flat sheets they form into tubes. Carbon nanotubes have the main advantage of being an excellent conductor of electricity while also being very resistant to being affected by chemicals as well as being very light weight. It's also exceptionally fireproof and will hold it's structure even under extreme temperatures. This makes it very useful in the space industry as their corrosion resistance makes them more reliable and their light weight and high conductivity is very nice when every single gram counts. On a rocket weight scales exponentially since a bigger rocket needs more thrust to lift itself so taking a few kg off a sattatile will scale down to the other parts and be very significant. The extreme heat resistance also means they are a conductor that can withstand the heat and pressures of atmospheric reentry. Another advantage that they have is that they are bio-compatible which means they have a lot of application in medicine. Very often it's the wires inside peacemakers and other prosthetics that are at the greatest risk of being biologically rejected. Carbon nanotubes can also be used in trains and other vehicles that rely on an external power source. Today they usually use graphite but this wears off quickly so trains need to go into expensive maintenance fairly often. A layer of carbon nanotubes, even if it's very thin could significantly cut down the maintenance needed.
@@MrMarinus18 Graphite is very different. It has sp2 hibridization in a resonance structure (just like benzene) on the plane, and Van der Waals bonds between planes, while both cubic diamond and Lonsdaleite are formed by sp3 hybridized carbon tetrahedra, but stacked differently.
The Mohs hardness scale is calibrated to diamond. Diamond is always 10. Its like how if the international kilo looses mass its still a kilo, because that item IS a kilo. Similarly, a Mohs hardness of 10 is always diamond.
The kilo was actually redefined in 2019 and can no longer be varied (due to exactly the issue mentioned above) It's now based on a constant, i think it was on the plank number, but it may have been something else.
Whats also funny about mohs scale is how it gives a warped sense of hardness, it makes it sound like corundum is almost as hard as diamond since its a 9, when you look at a scale used by gem lapidaries that relates hardness to time spent for surface area removed, corundum is at 1000 while diamond sits at a whopping 140000 (and Topas at 8 only has 175)
Although might I ask why Carbon couldn't say, bond to 8 other carbons? If they each have 4 valence electrons out of 8 spots, they could hypothetically lend out and accept 4 electrons no.? I suppose the forces are such that any atom lending (to share) its electron to a neighboring Carbon will always be taking (to share) an electron from the same atom.
@@castonyoung7514 Yeah, covalent bonds are typically a pair of shared electrons, one from each atom. Each lends and accepts an electron from the other.
@@massimocole9689 Oh, yeah, duh. I guess it was just the way that she said it that... Well okay I guess I should have known that before starting the video... I mean you can kind of see it from the graphics so I guess I have no excuse Other than she said that it could be bonded to 6 other atoms, so by that logic 8 made sense.
Just a simple correction: Ionic Bonds ARE stronger than equivalent covalent bonds. In fact, Ionic Bonds are the strongest bonds between atoms and the strength of any bond can be measured by the energy required to break them apart. And Ionic bonds requires significantly more energy than Covalent bonds.
Lonsdaleite atoms do NOT have 6 first neighbours. Lonsdaleite has exactly the same number of first neighbours and in (approximately) the same positions relative to the center atom than diamond. It's precisely in the second, third and succesive neighbours where we find a difference between diamond and lonsdaleite, changing the properties of the crystal! The same is true of FCC and HCP crystal lattices. Actually, this is where this all comes from, as diamond cubic cell (also called sphalerite structure) is a FCC structure with a two atom base, and lonsdaleite has a wurtzite structure, HCP with a two atom base. PS: I love SciShow, I've been a fan for many years but PLEASE try double check your sources. I happen to know a bit of crystallography (I'm a physics grad), but I don't know much biology or chemistry, so this makes me wonder if I've overlooked errors in other fields.
I had the same thought. I've seen videos where they use a photo of the wrong species of plant. It does make you wonder what other errors they might repeat or explain wrong without knowing.
3:08 - "Each carbon atom is covalently bonded to 6 other atoms." - This is not correct. It's 4 just as in diamond. Only the layering is different. ABAB rather than ABCABC. Putting 2 more non-bonded(!) carbons more near. This is coordination not covalent bonds. Thus only a moderately higher stiffness & hardness is to expect. Mostly more directional variation (aka anisotropy) as there is just one preferred axis now rather than four.
Interesting trivia: Moissanite (gem grade transparent silicon carbide SiC) has a layer ordering which is fluctuating between cubic and hexagonal. Its like a diamind to lonsdaleite crossover ("dialoneite") with every second carbon replaced by silicon.
Ech carbon is bonded to three other atoms of the layer only, they form a hexagonal lattice however and that's the error or way too simplified explanation.
@@LuisAldamiz - You are referring to graphite. There it's 3 bonds in plane. Aromatic bonds. Each counting as one plus a bit from the added delocalized pi-bonding from sp2 hybridization. Diamond & lonsdaleite form 4 covalent bonds per atom. Bonds are out of plane in tetrahedral symmetry (as orbitals are sp3 hybridized).
@@pallasiteroid Aromatic bonds? That's new for me, I'll look it up... I'll try to smell them if possible. Anyway, I thought you meant graphite indeed, were you talking about diamonds instead? If so the bonds are four.
@@LuisAldamiz - Yeah. I talked about diamond and lonsdaleite. I guess I got you confused with me talking about layering in those two. It's just a way to keep track of recurring placement and orientation of atoms. ABAB hexagonal sphere stacking (hcp) covers both graphite and lonsdaleite. The latter not layered by lack of covalent bonds but layered in the sense of a preferrential crystal direction. Side-note: ABCABC stacking in graphite is probably weakly metastable and hard or not to reach by anything but pick and place. Just a guess.
From the PhysOrg link in the description, there's a quote: "If somebody said to you, 'look, I'm going to give you the choice of two diamonds: one is lot more rare than the other one.' Which one would you pick?" ~ Yogendra Gupta, director of the Institute for Shock Physics and corresponding author on the study. "Frankly, I would rather have something like black opal, instead. Clear rocks are boring." ~ me. Seriously, I've never had a diamond, and don't want one. Gimme a sapphire or amethyst, or like I said, a black opal, any day over a boring old diamond. I prefer my diamonds on the tips of saw blades or drill bits, instead. 😄
"Dogs are a girl's best friend". I laughed my ass off at that turn of phrase. If Lorelei had figured that out, instead of diamonds, she would have been a whole lot happier. Nice writing, SciShow team!
It can't and it isn't: it's bonded (in graphite/graphene) to three other atoms and one bond is free to keep the layered structure not falling apart. In diamonds it's bound to four other carbon atoms in a 3D structure and no electrons remain free for anything else.
I found your video on the mineral from space that's harder than diamond fascinating! It's amazing to think that such a small, extraterrestrial object could hold so much power. The fact that this mineral is harder than diamond is truly mind-boggling. Diamond has long been considered the hardest mineral on Earth, so it's remarkable to discover that there is something even harder out there in the universe. I appreciate how you explained the science behind this discovery in a way that was easy to understand, and the visuals you used really helped to illustrate the point. It's exciting to think about what other discoveries are waiting for us out there in space. Overall, this video was both informative and engaging. I look forward to watching more of your content in the future! [Diamond Hunter Tv]
I mean... Neutron Stars exist, and there are some that form such strong electromagnetic fields that could produce some of the sturdiest materials out there
I find this very exciting. I see the development of techniques to synthesize Lonsdaleite as bringing us one step closer to synthesizing Quantium-40 and thereby developing hyperspace Jumpgate technology. Not to mention *even more effective* saw blades. Woo!
@1:36 I'm surprised (and not at all surprised) that the list of bond types entirely skips metallic bonding. Almost all introductory chemistry textbooks do the same. Exceedingly frustrating to those of us with degrees in metallurgy.
What I remember from my research, was that Lonsdaleite didn't over-bond carbon, but instead followed a different cell lattice, which was stronger than diamond along one axis, though slightly softer along the perpendicular plane
This was something I did not know anything about and the odd forms of carbon was something I was keeping an eye on for a while. Guess I stopped digging just as things get really interesting after synthetic diamond coating surfaces and all the uses for bucky balls. Harder than diamond material could be very useful for material science.
Typically, ionic bonds are much stronger than covalent bonds, but bond strength is not black and white. As with most things in life, chemical bond strength varies greatly depending on the substance bonded. If you measure with something as simple as melting point (assuming no chemical reactions like decomposition are happening), then diamond is an example of a covalently bonded substance with an extremely high mp. To qualify that last statement you must understand that the diamond allotrope of carbon does not melt at normal atmospheric pressure (1 atm) it sublimes directly to vapour (gas state). Given enough pressure (about 100,000x atmospheric pressure) it will melt at about 5000ºC. Of course, the gas compressing the diamond must not be air, as the oxygen in the air will cause the diamond to burn. A classic ionic crystal, NaCl, will melt at a mere 801ºC. Bond strength is a continuum of strength that varies with type of bond and substance. Side note on diamond. Since all the carbon atoms are covalently bonded in a tetrahedral lattice and there is no molecular boundary, a diamond is a single molecule. It is probably the only single molecule that you can see with the naked eye. Very cool…
I was about to comment something similar about the bind strengths because generally the breaking of an ionic bond releases more energy than a covalent one which is only the case if the broken bond was stronger
I loooove rocks and minerals! I'm not from the US but from what I've seen, the States has so many great places to go fossicking! In particular, the loads of old abandoned mines up in the mountains in the western states. Some outcrops and streams up in the hills seem to be good too.
Tom - "I'm not to keen on foreign food." Becca - "Trust me this meal goes 'hard'! You'll love it!" Tom - "Okay, okay. What's it called again?" Becca - "Lon's Delight." You heathens are welcome.
So... the statement "diamonds are the hardest substance ON EARTH" is mostly true since natural londsdalite seems to be from space...? This was a nifty, very interesting video!
Even for industrial uses, it's not necessarily going to be a clear "this is better, we're going to switch to this" situation. From the sounds of it, lonsdalite might end up being a lot more difficult and expensive to produce, which would force businesses to decide whether the extra durability will be worth the extra cost -- and in many cases, continuing to use the diamond-tipped blades will likely be the more cost-effective option.
Very cool! It makes me wonder if there are other minerals out there in the void of space that we know nothing about because it doesn't occur naturally on Earth and we'll only discover it if it ends up crashing into Earth on a meteor or something... just goes to show how little we really know about our world around us and how much more there is still to learn!
How can a carbon atom bond to 6 others, when it has only 4 valence electrons? And that illustration at 3:16 doesn't make it clear either, as the highest # of bonds i can see, is 3.
The hypothesis that Lonsdaleite was made from an exploding planet, or released from an exploding planet is typical crazy man guesswork. Dragons make minerals, check out the Safire project to see Dragons making elements
Imagine a carbon structure made up of triangular pyramidal forms all bonding as a single super molecule rather than individual segments of loosely bonded groups. Almost nothing could break that.
With the way I go through drill bits and saw blades, put me down for a couple of boxes of each. Now hopefully I won’t burn out another drill in the meantime.
This video was awesome, I like the chemistry explanation, this is good content, like all you guys do but is an even greater improvement. Add more sciences!!!
diamonds have a tetrahydral lattice structure each carbon atom is bonded to 4 covalant bonds it can take and disperse force out along the whole structure thats why
My uncle found a meteorite. We tried to plane one side flat with a ceramic hardwheel on a grinder. It remains the hardest object I've ever tried working.
In addition to meteorites, Lonsdaleite has been found occurring naturally in locations that had nothing to do with meteorites. However, its hardness is still an open question. The Wikipedia page for Lonsdaleite says that a certain face of diamond is harder than Lonsdaleite.
At 3:16 the speaker claims that “each carbon atom in Lonsdaleite is covalently bound to six other atoms” - this is factually incorrect, we are not dealing with hypervalent carbon. Each carbon still forms only four bonds, it’s just that the unit cell is now hexagonal, being extremely stable six carbon rings in the chair conformation.
Pencil lead is not pure graphite, but a graphite and clay mix. By altering the ratio of clay to graphite they can create pencils with different hardnesses.
My partner and i had fun playing "spot the animal" with your sweat shirt. 🤠 Edit: My partner wants to ask if you could please wear it backwards next time?
Minerals rock! ❤ I like that it sounds like laundry-ite & in a volatile place like Star Wars' Kessel, such a mineral could be common. So at least we understand some smuggling & gathering methods in that galaxy. Yet it tells us of probable practices in the past & future of our own galaxy! So; YOU ROCK! ❤ TY!
3:15 I don’t believe it’s possible for a carbon atom to bond with 6 other carbon atoms. Carbon only has 4 bonding sites, not 6. It can form hexagonal structures in 3D but this is still done using 4 bonds per carbon atom. Think of it as graphite but with a strong bond between layers. You rightly said carbon in graphite bonds with 3 other carbon atoms. The remaining bond is a weak bond between the layers.
And you don't believe correctly. What she probably meant is that 6 carbons form a hexagon while each is attached to other three atoms in that hexagonal lattice only (there's a fourth electron doing the inter-layer connection anyhow).
Thank you to Wondrium for sponsoring today’s video! Signup for your FREE trial to Wondrium here: ow.ly/4Hl450N4T1g
I enjoy watching your videos, usually. but today I'm just disappointed...
01:45 covalent bonds are definitely NOT stronger than ionic bonds...
in fact ionic bonds have the highest bond energy (lattice energy) of any bonds thus being BY FAR the strongest!
03:12 WRONG! like so wrong it really hurts (again)! the carbon still has only 4 bonds it just crystalizes in a hexagonal structure. for carbon to have 5 bonds (which is technically possible, kinda...) you need VERY different conditions and these compounds are not as stable as to survive entering earths atmosphere, by far.
Hardness isn’t isotropic nor isobaric, thus nc-TiN/a-Si3N4 I rad is harder. Everything occurs naturally; you mean natively, wildly. thin → fine; would → should; There..here: pick one; big → great.
A thought experiment for you...we know what will happen if two planets collide, we know what happens if two planets enter the Roche limit of another...but what if we magically side step reality for a second and place a rocky planet directly on the surface of another planet? For example, what would happen if Mars suddenly appeared on the surface of the Earth in lets say the middle of relatively flat Australia? What happens to Mars? Will it roll due to its shape, compositions, or Earth's movements? Will it start to sink to the center with its weight/mass and gravity? Will it just crumble creating the biggest volcanic mountain pile in the solar system? What happens to the Earth? Its gravity, atmosphere, land/water, core.......?
@@savage069 the earth is full of dirt-cheap diamond dust.
Its great to wake up, have breakfast, and see a video about a paper you worked on for a decade! Thanks SciShow for spreading the word about our weird little rocks!
You're a legend
Yoooo, thank YOU for your research!
You rock fancy man!
Keep up the good work!
Epic af!
so you're saying hexagons are the bestagons
CGP Grey Would be Proud
Always has been
Vihart
I use that as a hashtag... when I make hexagonal artwork #hexagonsarethebestagons
Truth
Small correction about the Lonsdaleite. It doesn't have carbon atoms with 6 bonds. It still has 4 bonds since carbon can can only form 4 bonds. The difference in material properties is entirely from the shape of its bonds. Diamond makes a cubic grids while lonsdaleite makes hexagonal grids.
Thanks so much
Looking 3min 14 secs into the video, I noticed the same thing
Came here to say this. 👏
I was wondering the same thing! I was looking at both pictures they showed and both had 4 bonds. Thanks
Lonsdelite is something I saw in a Minecraft mod. I had no idea it was a real mineral until this video. It turns out to be really awesome IRL, too!
Nice to see another Minecraft player
My people.
Now try unbelievium...
oh which mod?
@@SunroseStudios Environmental Tech is the mod name, IIRC.
Auto-generated captions kept saying the hardest thing is Lawn's Delight and I think that was just wonderful.
my brain-generated caption did it too 😇.
This feels like the plot to a spy movie where the bad guy wants the super space crystal so he's got to smash to planets together.
That just sounds like a rad plot point for many Sci-Fi / Disaster stories: maniacal dudes who REQUIRE MORE MINERALS and can only figure out how to synthesize their spooky isotopes by going the old fashioned way and blowing up star systems. Then again, if you have enough power to smash two planets together, wouldn’t you have more than enough know-how to just synthesize it in a controlled lab environment? I guess that’s where the maniacal part comes in.
That does actually sound super legit. After all, the plot of Avatar exists because humans need to mine "unobtainium" out of the surface of Pandora
Might as well take this precious opportunity to tell people to listen to Fun City (Shadowrun Actual Play podcast GM’d by Mike Rugnetta) where alchemically systhesizing radioactive isotopes of magical elements and planets colliding are not only major plot points but also the most incredible narrative experiences I’ve had all year.
Hell yeah, I always wanted to be able to tell diamonds that there are always bigger fish.
There already are. Opals are way more rare, way more unique, and way more attractive in jewelry. Just, you know, not *harder*.
@@TheYuleTube i know someone who owns around 120 thousand carrots of Australian black opal he has been cutting them for around 40 years and has a absolutely insane mineral collection.
@@RalseiGaming That's super nice! I have a good bit, but nothing at all like that! Most of mine is lower cost Andamooka stones, still in the rough. I am learning how to process it myself. Still some nice stones to be had!
Dogfish.
@@TheYuleTube Ehh🤷♂️ I don’t think opal is that great.
I remember having to do w report on this when I was in Chemistry in High School. It's one of those substances like Graphine is that when they figure out how to make itannd make it cheaply could have a massive impact on how we are manufacturing things.
"IF you went through a rocks snd minerals phase as a kid." Well, I'm perpetually stuck in that phase and now I'm studying to become a geologist 😂
Same but not studying
Have fun!!! 😊
Carbon in Londaleite bond to 4 neighboring carbons as well. What changes is the disposition of atoms through the planes (similar, but not exactly equal, as the close packing of similar spheres problem). The problem with the hexagonal packing is its anisotropic properties, which means that they change depending on orientation. That can be a big no no for some technical applications. Even though it's cool that there's a "harder" diamond, it's probably too expensive, rare and its properties probably arent different enough to justify its economical exploration. I might be wrong, though.
Best comment so far. TY.
Actually graphite is very similar to diamond and is made up of the same bonds. The difference is that they form 2D plates of single carbon atoms and while the bonds holding the plates together are hard as diamond the forces keeping the plates together are extremely weak. This mix of hardness on a molecular level and softness on a physics level has led graphite to have some unique uses. For example the largest machines in the world use graphite as a lubericant. The strong bonds between the atoms allow them to support massive forces while the weak forces between the sheets means there isn't too much heat created.
This is important cause carbon nanotubes are actually the exact same thing as graphite but instead of forming into flat sheets they form into tubes. Carbon nanotubes have the main advantage of being an excellent conductor of electricity while also being very resistant to being affected by chemicals as well as being very light weight. It's also exceptionally fireproof and will hold it's structure even under extreme temperatures. This makes it very useful in the space industry as their corrosion resistance makes them more reliable and their light weight and high conductivity is very nice when every single gram counts. On a rocket weight scales exponentially since a bigger rocket needs more thrust to lift itself so taking a few kg off a sattatile will scale down to the other parts and be very significant. The extreme heat resistance also means they are a conductor that can withstand the heat and pressures of atmospheric reentry.
Another advantage that they have is that they are bio-compatible which means they have a lot of application in medicine. Very often it's the wires inside peacemakers and other prosthetics that are at the greatest risk of being biologically rejected.
Carbon nanotubes can also be used in trains and other vehicles that rely on an external power source. Today they usually use graphite but this wears off quickly so trains need to go into expensive maintenance fairly often. A layer of carbon nanotubes, even if it's very thin could significantly cut down the maintenance needed.
@@MrMarinus18 Graphite is very different. It has sp2 hibridization in a resonance structure (just like benzene) on the plane, and Van der Waals bonds between planes, while both cubic diamond and Lonsdaleite are formed by sp3 hybridized carbon tetrahedra, but stacked differently.
Aaah thanks I was wondering how this would even work regarding hybridisation
Yeah, that's another item in the long list of easily checkable falsehood spread by this channel...
The Mohs hardness scale is calibrated to diamond. Diamond is always 10. Its like how if the international kilo looses mass its still a kilo, because that item IS a kilo. Similarly, a Mohs hardness of 10 is always diamond.
The kilo was actually redefined in 2019 and can no longer be varied (due to exactly the issue mentioned above) It's now based on a constant, i think it was on the plank number, but it may have been something else.
Let's rock! Take it up to 11!
Loses, not looses.
Whats also funny about mohs scale is how it gives a warped sense of hardness, it makes it sound like corundum is almost as hard as diamond since its a 9, when you look at a scale used by gem lapidaries that relates hardness to time spent for surface area removed, corundum is at 1000 while diamond sits at a whopping 140000 (and Topas at 8 only has 175)
Lol that's a logarithmic scale for you
At 3:18, carbon has a different lattice structure but its still bonding with 4 other atoms, not 6
+
Wikipedia seems to agree.
Although might I ask why Carbon couldn't say, bond to 8 other carbons? If they each have 4 valence electrons out of 8 spots, they could hypothetically lend out and accept 4 electrons no.? I suppose the forces are such that any atom lending (to share) its electron to a neighboring Carbon will always be taking (to share) an electron from the same atom.
@@castonyoung7514 Yeah, covalent bonds are typically a pair of shared electrons, one from each atom. Each lends and accepts an electron from the other.
@@massimocole9689 Oh, yeah, duh.
I guess it was just the way that she said it that... Well okay I guess I should have known that before starting the video... I mean you can kind of see it from the graphics so I guess I have no excuse Other than she said that it could be bonded to 6 other atoms, so by that logic 8 made sense.
Just a simple correction: Ionic Bonds ARE stronger than equivalent covalent bonds. In fact, Ionic Bonds are the strongest bonds between atoms and the strength of any bond can be measured by the energy required to break them apart. And Ionic bonds requires significantly more energy than Covalent bonds.
This video is filled with errors. I appreciate the news they’re trying to convey but the inaccuracies are just a bit too much.
Lonsdaleite atoms do NOT have 6 first neighbours. Lonsdaleite has exactly the same number of first neighbours and in (approximately) the same positions relative to the center atom than diamond. It's precisely in the second, third and succesive neighbours where we find a difference between diamond and lonsdaleite, changing the properties of the crystal! The same is true of FCC and HCP crystal lattices. Actually, this is where this all comes from, as diamond cubic cell (also called sphalerite structure) is a FCC structure with a two atom base, and lonsdaleite has a wurtzite structure, HCP with a two atom base.
PS: I love SciShow, I've been a fan for many years but PLEASE try double check your sources. I happen to know a bit of crystallography (I'm a physics grad), but I don't know much biology or chemistry, so this makes me wonder if I've overlooked errors in other fields.
I had the same thought. I've seen videos where they use a photo of the wrong species of plant. It does make you wonder what other errors they might repeat or explain wrong without knowing.
@ i wondered. How can an atom with 4 valence atoms couple to more than 4 other atoms. Involving the 2 of the inner shell, seriously?
And there I was wondering if someone had found a source for Netherite ... thanks for the great presentation of this really cool information.
I believe either MatPat or Austin (blue text thumbnails) made a video saying exactly that
Link to the video I meantioned ruclips.net/video/3Bxf2o27ykM/видео.html
3:08 - "Each carbon atom is covalently bonded to 6 other atoms." - This is not correct. It's 4 just as in diamond. Only the layering is different. ABAB rather than ABCABC. Putting 2 more non-bonded(!) carbons more near. This is coordination not covalent bonds. Thus only a moderately higher stiffness & hardness is to expect. Mostly more directional variation (aka anisotropy) as there is just one preferred axis now rather than four.
Interesting trivia: Moissanite (gem grade transparent silicon carbide SiC) has a layer ordering which is fluctuating between cubic and hexagonal. Its like a diamind to lonsdaleite crossover ("dialoneite") with every second carbon replaced by silicon.
Ech carbon is bonded to three other atoms of the layer only, they form a hexagonal lattice however and that's the error or way too simplified explanation.
@@LuisAldamiz - You are referring to graphite. There it's 3 bonds in plane. Aromatic bonds. Each counting as one plus a bit from the added delocalized pi-bonding from sp2 hybridization. Diamond & lonsdaleite form 4 covalent bonds per atom. Bonds are out of plane in tetrahedral symmetry (as orbitals are sp3 hybridized).
@@pallasiteroid Aromatic bonds? That's new for me, I'll look it up... I'll try to smell them if possible.
Anyway, I thought you meant graphite indeed, were you talking about diamonds instead? If so the bonds are four.
@@LuisAldamiz - Yeah. I talked about diamond and lonsdaleite. I guess I got you confused with me talking about layering in those two. It's just a way to keep track of recurring placement and orientation of atoms. ABAB hexagonal sphere stacking (hcp) covers both graphite and lonsdaleite. The latter not layered by lack of covalent bonds but layered in the sense of a preferrential crystal direction.
Side-note: ABCABC stacking in graphite is probably weakly metastable and hard or not to reach by anything but pick and place. Just a guess.
Really enjoying Savannah Geary's presentation in this video! Great host!
"Minerals rock" - These two words made me like this video.
From the PhysOrg link in the description, there's a quote:
"If somebody said to you, 'look, I'm going to give you the choice of two diamonds: one is lot more rare than the other one.' Which one would you pick?" ~ Yogendra Gupta, director of the Institute for Shock Physics and corresponding author on the study.
"Frankly, I would rather have something like black opal, instead. Clear rocks are boring." ~ me. Seriously, I've never had a diamond, and don't want one. Gimme a sapphire or amethyst, or like I said, a black opal, any day over a boring old diamond. I prefer my diamonds on the tips of saw blades or drill bits, instead. 😄
What a strange "im not like other girls" comment
"Dogs are a girl's best friend". I laughed my ass off at that turn of phrase. If Lorelei had figured that out, instead of diamonds, she would have been a whole lot happier. Nice writing, SciShow team!
It all sounds potentially dubious...
Yikes
It scratches at level 10, with deeper grooves at level 11
Was looking for this, thank you.
3:16 each carbon cannot be covalently bonded to six other atoms
Correct, it's arranged into a hexagonal lattice rather than a cubic one by having the bonds be aligned rather than staggered.
It can't and it isn't: it's bonded (in graphite/graphene) to three other atoms and one bond is free to keep the layered structure not falling apart. In diamonds it's bound to four other carbon atoms in a 3D structure and no electrons remain free for anything else.
This channel has taught me so much!
Can't wait to see Lonsdaleite in a future Minecraft update
I'm surprised by the fact that I wasn't the only one thinking about this.
I found your video on the mineral from space that's harder than diamond fascinating! It's amazing to think that such a small, extraterrestrial object could hold so much power.
The fact that this mineral is harder than diamond is truly mind-boggling. Diamond has long been considered the hardest mineral on Earth, so it's remarkable to discover that there is something even harder out there in the universe.
I appreciate how you explained the science behind this discovery in a way that was easy to understand, and the visuals you used really helped to illustrate the point. It's exciting to think about what other discoveries are waiting for us out there in space.
Overall, this video was both informative and engaging. I look forward to watching more of your content in the future!
[Diamond Hunter Tv]
I mean... Neutron Stars exist, and there are some that form such strong electromagnetic fields that could produce some of the sturdiest materials out there
Her shirt also rocks. Makes me feel like I'm playing Cascadia.
2:13 - 2:25 The diamond reference photo is a Herkimer diamond (double-terminated quartz crystal)
I find this very exciting. I see the development of techniques to synthesize Lonsdaleite as bringing us one step closer to synthesizing Quantium-40 and thereby developing hyperspace Jumpgate technology.
Not to mention *even more effective* saw blades. Woo!
@1:36 I'm surprised (and not at all surprised) that the list of bond types entirely skips metallic bonding.
Almost all introductory chemistry textbooks do the same.
Exceedingly frustrating to those of us with degrees in metallurgy.
Today's classrooms should be absolutely lit with this kind of information floating around the way it does.
What I remember from my research, was that Lonsdaleite didn't over-bond carbon, but instead followed a different cell lattice, which was stronger than diamond along one axis, though slightly softer along the perpendicular plane
I always enjoy Savannah’s videos, their explanation is always clear and concise!
Give me hank!!!
Great. Now we’re gonna find some alien civilization with Lonsdaleite armor and we’re gonna have no way to pierce it and get conquered.
This was something I did not know anything about and the odd forms of carbon was something I was keeping an eye on for a while. Guess I stopped digging just as things get really interesting after synthetic diamond coating surfaces and all the uses for bucky balls. Harder than diamond material could be very useful for material science.
"Minerals ROCK!"
HA!
Good One!
scientists recreate force that shatters planets in order to make better sandpaper
Best abstract ever.
Typically, ionic bonds are much stronger than covalent bonds, but bond strength is not black and white. As with most things in life, chemical bond strength varies greatly depending on the substance bonded. If you measure with something as simple as melting point (assuming no chemical reactions like decomposition are happening), then diamond is an example of a covalently bonded substance with an extremely high mp.
To qualify that last statement you must understand that the diamond allotrope of carbon does not melt at normal atmospheric pressure (1 atm) it sublimes directly to vapour (gas state). Given enough pressure (about 100,000x atmospheric pressure) it will melt at about 5000ºC. Of course, the gas compressing the diamond must not be air, as the oxygen in the air will cause the diamond to burn.
A classic ionic crystal, NaCl, will melt at a mere 801ºC.
Bond strength is a continuum of strength that varies with type of bond and substance.
Side note on diamond. Since all the carbon atoms are covalently bonded in a tetrahedral lattice and there is no molecular boundary, a diamond is a single molecule. It is probably the only single molecule that you can see with the naked eye. Very cool…
Best comment so far. There was another one but yours is even better, I thought something was not quite right in the electron explanation, thank you.
I was about to comment something similar about the bind strengths because generally the breaking of an ionic bond releases more energy than a covalent one which is only the case if the broken bond was stronger
Villian: Your name?
Bond: Bond, Chemical Bond.
Villian: Here comes Oxygen!
Bond: Oh oh!
I love how the image of the two planets colliding says “artist concept”.. darn I was hoping for a real photo of that event.
I'm going through a rocks and minerals phase as an adult thank you very much
Learn so much from this channel 💯
I loooove rocks and minerals!
I'm not from the US but from what I've seen, the States has so many great places to go fossicking! In particular, the loads of old abandoned mines up in the mountains in the western states. Some outcrops and streams up in the hills seem to be good too.
Great delivery! Thanks for the info.
I learnt more about hardness in 1 minute than my entire materials course 😭😁
Why are education institutions so bad at teaching? that's their only job.
The new world of business models of education means we win :)
Sounds like a skill issue. Like fr
Best presenter yet. Slightly more calm tone makes it easier to follow. Many others are a bit “hyper?”-sounding to me.
Hurray! A new Sci Show... ..show
Tom - "I'm not to keen on foreign food."
Becca - "Trust me this meal goes 'hard'! You'll love it!"
Tom - "Okay, okay. What's it called again?"
Becca - "Lon's Delight."
You heathens are welcome.
This narrator is an EXCELLENT teacher.
Your animal jumper is amazing!
"Check out how hard my rock is, bro" was probably how geology got started as a science
Some dude probably scratched it with his braces 😬 😅
Industrial scale shocking of carbon into lonsdaleite can also be obtained by letting the carbon know that dogs are not all girls best friends
Coal is then?
Bruh, I'm still in my rocks and minerals phase
That "phase" never ended for me!
So... the statement "diamonds are the hardest substance ON EARTH" is mostly true since natural londsdalite seems to be from space...?
This was a nifty, very interesting video!
Every time I heard "Lon's delight", I kept thinking of spoo from Babylon 5.
FYI: Hexagonal boron-nitride is harder than diamond and is found as volcanic mineral. Its probably also harder than lonsdaleite.
*snort* "Dogs are a girl's best friend."
F*ing love it!
This stuff is fascinating
If I squint I can hear Lon's Delight. Lon is here for the hardest
Sr. Lonsdaleite, knight of the hard table
Even for industrial uses, it's not necessarily going to be a clear "this is better, we're going to switch to this" situation. From the sounds of it, lonsdalite might end up being a lot more difficult and expensive to produce, which would force businesses to decide whether the extra durability will be worth the extra cost -- and in many cases, continuing to use the diamond-tipped blades will likely be the more cost-effective option.
Thanks for the show.
Glimmering, glistening, bone-chilling, slow-burn, genre-defining Gemerald!
Very cool! It makes me wonder if there are other minerals out there in the void of space that we know nothing about because it doesn't occur naturally on Earth and we'll only discover it if it ends up crashing into Earth on a meteor or something... just goes to show how little we really know about our world around us and how much more there is still to learn!
Guys the netherite update is here.
How can a carbon atom bond to 6 others, when it has only 4 valence electrons? And that illustration at 3:16 doesn't make it clear either, as the highest # of bonds i can see, is 3.
You are right, they made a mistake. Each carbon in Lonsdaleite is still bound to 4 other carbons. What's different is the angle that these bonds make.
Lon's Delight. Sounds like a good name for a future-tech jewelry store.
So who is Lon, and why is this stuff his delight?
Very good explanation
I'm gonna name my landscaping business lawns-delight
Because it's a hard job, but someone's gotta do it.
'Decay into diamond' sounds so strange for some reason.
"Sorry everyone, our experiment to create Lonsdelite failed miserably. All we ended up with was this lousy pile of diamonds."
The hypothesis that Lonsdaleite was made from an exploding planet, or released from an exploding planet is typical crazy man guesswork. Dragons make minerals, check out the Safire project to see Dragons making elements
Imagine a carbon structure made up of triangular pyramidal forms all bonding as a single super molecule rather than individual segments of loosely bonded groups. Almost nothing could break that.
With the way I go through drill bits and saw blades, put me down for a couple of boxes of each. Now hopefully I won’t burn out another drill in the meantime.
I want Lonsdaleite Tools! Really cool wonder if there are even harder minerals out there.
Plot twist: the space mineral isn’t natural
I think David Bowie would have a really good time singing about starman's rock.
This video was awesome, I like the chemistry explanation, this is good content, like all you guys do but is an even greater improvement. Add more sciences!!!
Lonsdalite? HA! I could gum through that with my dentures behind my back. My trademarked Diamondium is twice as hard!
Ok Farnsworth
diamonds have a tetrahydral lattice structure each carbon atom is bonded to 4 covalant bonds it can take and disperse force out along the whole structure thats why
My uncle found a meteorite. We tried to plane one side flat with a ceramic hardwheel on a grinder. It remains the hardest object I've ever tried working.
NASA astronaut Lodewijk van den Berg should be credited here for his research in the 1980’s of the growth of crystals in zero G.
I mean, if it only occurs in meteors, then that means that diamond is still the hardest natural material on _earth._
In addition to meteorites, Lonsdaleite has been found occurring naturally in locations that had nothing to do with meteorites. However, its hardness is still an open question. The Wikipedia page for Lonsdaleite says that a certain face of diamond is harder than Lonsdaleite.
Reality is like modded Minecraft, you keep finding things that make better gear than diamond
minerals rock and this video was a gem!
Geology Rocks! But Fluvial Geomorphology is pretty groovy...
Gesundheit
Space, well the universe in general has all the answers.
But what are the questions?
At 3:16 the speaker claims that “each carbon atom in Lonsdaleite is covalently bound to six other atoms” - this is factually incorrect, we are not dealing with hypervalent carbon. Each carbon still forms only four bonds, it’s just that the unit cell is now hexagonal, being extremely stable six carbon rings in the chair conformation.
Uh oh. I smell a geek off!
Minerals rock
Never thought I'd see a diamond anvil.
Pencil lead is not pure graphite, but a graphite and clay mix. By altering the ratio of clay to graphite they can create pencils with different hardnesses.
My partner and i had fun playing "spot the animal" with your sweat shirt. 🤠
Edit:
My partner wants to ask if you could please wear it backwards next time?
Wow! Super cool.
Minerals rock! ❤ I like that it sounds like laundry-ite & in a volatile place like Star Wars' Kessel, such a mineral could be common. So at least we understand some smuggling & gathering methods in that galaxy. Yet it tells us of probable practices in the past & future of our own galaxy! So; YOU ROCK! ❤ TY!
3:13 No, each atom is not covalently bound to six others.
3:15 I don’t believe it’s possible for a carbon atom to bond with 6 other carbon atoms. Carbon only has 4 bonding sites, not 6. It can form hexagonal structures in 3D but this is still done using 4 bonds per carbon atom. Think of it as graphite but with a strong bond between layers. You rightly said carbon in graphite bonds with 3 other carbon atoms. The remaining bond is a weak bond between the layers.
And you don't believe correctly. What she probably meant is that 6 carbons form a hexagon while each is attached to other three atoms in that hexagonal lattice only (there's a fourth electron doing the inter-layer connection anyhow).
Leave it to the hexagon to out-diamond a diamond.
So, we finally got the netherite update