ceaglex/VisualTTS_Chem · Datasets at Hugging Face

text stringlengths 19 206
0JyN9PH2oNg-008\|Now, this equilibrium is always true in water solution.
0JyN9PH2oNg-009\|Remember regardless of what other equilibria are occurring, all equilibria work together in a solution to satisfy themselves.
0JyN9PH2oNg-010\|So in water, this is always true.
0JyN9PH2oNg-014\|Acid-base forms of water have a very small K.
0JyN9PH2oNg-015\|So this reaction very much favors the water.
0JyN9PH2oNg-020\|So pure liquid water in equilibrium, the H3O+ and OH- concentrations are equal.
0JyN9PH2oNg-023\|And recall, when you take the log, you're taking the exponent, log base 10, of 10 to the exponent is just the exponent.
0JyN9PH2oNg-024\|So minus log of 10 to the minus 7 is 7.
0JyN9PH2oNg-025\|So the pH of pure liquid water is 7.
0JyN9PH2oNg-026\|The pOH of pure liquid water is 7 due to the autoionization and autodissociation of water.
f8b4i8DtA1Y-000\|An interesting application of the ideal gas law is swimming and diving.
f8b4i8DtA1Y-001\|When you dive beneath the surface of water, your body experiences an increase in pressure.
f8b4i8DtA1Y-002\|That's because the water has mass, and that mass, pushing down on your body, increases pressure.
f8b4i8DtA1Y-003\|The increase in pressure goes, for every 10 meters in depth, you get an additional 1 atmosphere of pressure.
f8b4i8DtA1Y-004\|So if you're at depth and you hold your breath, with a fixed amount of air in your lungs, and you ascend, that can actually be dangerous, as that volume expands.
f8b4i8DtA1Y-005\|Which is the most dangerous, is the question I have for you?
f8b4i8DtA1Y-015\|We're talking about diving, and when you dive beneath the surface of water, the pressure changes one atmosphere for every 10 meters in change of depth.
f8b4i8DtA1Y-016\|So how can I calculate the volume in my lungs, how that will change?
f8b4i8DtA1Y-017\|If I hold my breath and fix the amount of air, then the volume will expand or contract with the pressure changes.
f8b4i8DtA1Y-018\|As I ascend, the volume wants to increase, because the pressure decreases.
f8b4i8DtA1Y-019\|And if I hold my breath, that increase in volume can actually damage my lung tissues and my chest cavity.
f8b4i8DtA1Y-022\|So P2 times V2 is P1 times V1.
f8b4i8DtA1Y-025\|Let's do that for each ascent.
f8b4i8DtA1Y-030\|So this is a change of 2-- a factor of 2 in volume.
f8b4i8DtA1Y-031\|The volume will double if I do this ascent.
f8b4i8DtA1Y-032\|These two are a factor of 1 and 1/2.
f8b4i8DtA1Y-033\|So it's interesting that the greatest change in volume occurs nearest the surface.
f8b4i8DtA1Y-034\|And since that's where we do most of our swimming, that's where we have to be most careful.
f8b4i8DtA1Y-035\|So the greatest danger in holding your breath, you get the greatest volume change due to pressure, is from 10 meters to the surface.
wihnb2KZ1Bs-001\|For instance, here's two entries carbon-12 and naturally occurring carbon.
wihnb2KZ1Bs-002\|They have different relative masses.
wihnb2KZ1Bs-003\|That's because I could take a sample of pure carbon-12, where every atom is carbon-12, and that would have mass 12.
wihnb2KZ1Bs-004\|But in naturally occurring carbon, 1 out of every 100 atoms is a carbon-13, it's slightly more massive.
wihnb2KZ1Bs-005\|So if I took this piece of carbon and I started picking out atoms, 1 in 100 would be that carbon-13 with a slightly more massive nucleus.
wihnb2KZ1Bs-006\|That's what gives this naturally occurring carbon that slightly higher relative mass.
wihnb2KZ1Bs-007\|It's the mass weighted average of all the isotopes.
wihnb2KZ1Bs-008\|And you can see many elements have a potpourri of different isotopes.
wihnb2KZ1Bs-009\|They don't have integer molecular masses and atomic masses, because of the presence of all the different isotopes.
wihnb2KZ1Bs-010\|Now for the most part, isotopes are chemically similar, that is they do the same chemical reactions, but of course they have different masses.
wihnb2KZ1Bs-011\|A lot of times the mass difference is very small.
wihnb2KZ1Bs-012\|For hydrogen, there's hydrogen with mass 1 and deuterium with mass 2.
wihnb2KZ1Bs-013\|That's a factor of 2 in mass-- that's very large.
wihnb2KZ1Bs-014\|But for carbon already, carbon-12 versus carbon-13, that's a 1% difference in mass.
wihnb2KZ1Bs-015\|That's relatively small.
wihnb2KZ1Bs-017\|That's a very small percentage difference in mass.
wihnb2KZ1Bs-018\|Now you can separate pure isotopes and this is very common.
wihnb2KZ1Bs-019\|For instance, uranium is a good example because we take uranium-238 and we separate out the other isotopes and we make pure uranium-238.
wihnb2KZ1Bs-020\|It's called depleted uranium because the radioactive fissible nuclei are removed.
wihnb2KZ1Bs-022\|Uranium-235 is the fissible nucleus.
wihnb2KZ1Bs-023\|It's used in nuclear reactors.
wihnb2KZ1Bs-024\|So we have different properties of the nuclei that are different isotopes.
wihnb2KZ1Bs-025\|Chemically they're very similar, but sometimes their mass gives them different physical properties that we can use.
wihnb2KZ1Bs-026\|In general, we catalog them based on the potpourri, the mass weighted average of all the isotopes in the mixture.
wihnb2KZ1Bs-027\|And that's how we achieve relative atomic and molecular masses.
JOjrtRHsozI-000\|Let's look at some naturally-occurring polychromic acids, amino acids.
JOjrtRHsozI-001\|Amino acids are found in your body.
JOjrtRHsozI-002\|They're the building blocks of the proteins in your body.
JOjrtRHsozI-003\|They're called amino acids because each one has an amino group and an acid group.
JOjrtRHsozI-004\|Here's the amino group and the carboxylic COOH group.
JOjrtRHsozI-005\|Now, I've drawn them at pH 7.
JOjrtRHsozI-006\|And I draw them at pH 7, that means this carboxylic acid group with pKa 2 will be in its basic form.
JOjrtRHsozI-011\|Here, tyrosine, as well, has a side group.
JOjrtRHsozI-016\|And in this case, that will be a neutral charge.
JOjrtRHsozI-017\|Notice, when I protonate the amino group here at the end of lysine, that attains a positive charge.
JOjrtRHsozI-022\|That's going to be in its basic form at pH 7.
JOjrtRHsozI-024\|Here's histidine.
JOjrtRHsozI-028\|And notice, I'm very close here.
JOjrtRHsozI-029\|There's just a factor of one pH unit.
JOjrtRHsozI-030\|So you know there's a factor of 10.
JOjrtRHsozI-031\|There's 10 times as much of the unprotonated basic form as the protonated form.
JOjrtRHsozI-033\|Now, that's very important, because the charge on amino acids, especially their side groups, affects the structure of proteins.
JOjrtRHsozI-034\|Proteins are molecules in your body that do all the catalysis in your body.
JOjrtRHsozI-035\|They help your chemical reactions go.
JOjrtRHsozI-036\|And proteins are long chains of amino acids, and one of the reasons proteins can operate is their three-dimensional structure.
JOjrtRHsozI-038\|One of the things that holds those structures together are charges on the side groups.
JOjrtRHsozI-039\|You have a positively-charged side group here, a negatively-charged side group here.
JOjrtRHsozI-040\|Those are attracted coulombically, and can anchor the three-dimensional structure, hold it together by that coulombic attraction.
JOjrtRHsozI-042\|If the molecule falls apart, it can't perform its catalytic operation anymore.
JOjrtRHsozI-043\|And I can actually demonstrate that for you.
JOjrtRHsozI-044\|There's enzymes, one of them peroxidase, which are very common in nature.
JOjrtRHsozI-045\|In fact, in turnips.
JOjrtRHsozI-046\|I have some turnip here.
JOjrtRHsozI-048\|That is, it will break down hydrogen peroxide into water and oxygen. So I'm going to do that.
JOjrtRHsozI-049\|I'm going to bring in a blender here-- and I've already ground up some turnip in advance here, kind of in the Julia Child child style.
JOjrtRHsozI-050\|So I've got a slurry already.
JOjrtRHsozI-051\|I'm going to make a little more here.
JOjrtRHsozI-053\|To one of the beakers, I'm going to add HCL, a strong acid.
JOjrtRHsozI-054\|So let me get my safety glasses on here.
JOjrtRHsozI-055\|I'll add a strong acid.
JOjrtRHsozI-058\|So if I change the PH, I change the protonated state, and I should affect the activity of the peroxidase.
JOjrtRHsozI-059\|That molecule should denature.
JOjrtRHsozI-060\|So what I'm going to do now is add hydrogen peroxide to each flask, and we should see peroxidase activity, bubbling oxygen here.
wXt_tUPtAe8-000\|Let's look at some electronic configurations.
wXt_tUPtAe8-001\|Fluorine minus, sodium, or sodium plus.
wXt_tUPtAe8-002\|Which of those three can have the electronic configuration helium 2s2 2p5 3s1?
wXt_tUPtAe8-011\|Sodium plus has one fewer electrons, so it's a 10-electron system.
wXt_tUPtAe8-013\|Fluorine minus, same situation.
wXt_tUPtAe8-014\|It's a 10-electron species, and it's in a slightly excited state.
wXt_tUPtAe8-015\|The 2p electron promoted to the 3s.
wXt_tUPtAe8-016\|So what we have are two 10-electron species.

0JyN9PH2oNg-008|Now, this equilibrium is always true in water solution.

0JyN9PH2oNg-009|Remember regardless of what other equilibria are occurring, all equilibria work together in a solution to satisfy themselves.

0JyN9PH2oNg-010|So in water, this is always true.

0JyN9PH2oNg-014|Acid-base forms of water have a very small K.

0JyN9PH2oNg-015|So this reaction very much favors the water.

0JyN9PH2oNg-020|So pure liquid water in equilibrium, the H3O+ and OH- concentrations are equal.

0JyN9PH2oNg-023|And recall, when you take the log, you're taking the exponent, log base 10, of 10 to the exponent is just the exponent.

0JyN9PH2oNg-024|So minus log of 10 to the minus 7 is 7.

0JyN9PH2oNg-025|So the pH of pure liquid water is 7.

0JyN9PH2oNg-026|The pOH of pure liquid water is 7 due to the autoionization and autodissociation of water.

f8b4i8DtA1Y-000|An interesting application of the ideal gas law is swimming and diving.

f8b4i8DtA1Y-001|When you dive beneath the surface of water, your body experiences an increase in pressure.

f8b4i8DtA1Y-002|That's because the water has mass, and that mass, pushing down on your body, increases pressure.

f8b4i8DtA1Y-003|The increase in pressure goes, for every 10 meters in depth, you get an additional 1 atmosphere of pressure.

f8b4i8DtA1Y-004|So if you're at depth and you hold your breath, with a fixed amount of air in your lungs, and you ascend, that can actually be dangerous, as that volume expands.

f8b4i8DtA1Y-005|Which is the most dangerous, is the question I have for you?

f8b4i8DtA1Y-015|We're talking about diving, and when you dive beneath the surface of water, the pressure changes one atmosphere for every 10 meters in change of depth.

f8b4i8DtA1Y-016|So how can I calculate the volume in my lungs, how that will change?

f8b4i8DtA1Y-017|If I hold my breath and fix the amount of air, then the volume will expand or contract with the pressure changes.

f8b4i8DtA1Y-018|As I ascend, the volume wants to increase, because the pressure decreases.

f8b4i8DtA1Y-019|And if I hold my breath, that increase in volume can actually damage my lung tissues and my chest cavity.

f8b4i8DtA1Y-022|So P2 times V2 is P1 times V1.

f8b4i8DtA1Y-025|Let's do that for each ascent.

f8b4i8DtA1Y-030|So this is a change of 2-- a factor of 2 in volume.

f8b4i8DtA1Y-031|The volume will double if I do this ascent.

f8b4i8DtA1Y-032|These two are a factor of 1 and 1/2.

f8b4i8DtA1Y-033|So it's interesting that the greatest change in volume occurs nearest the surface.

f8b4i8DtA1Y-034|And since that's where we do most of our swimming, that's where we have to be most careful.

f8b4i8DtA1Y-035|So the greatest danger in holding your breath, you get the greatest volume change due to pressure, is from 10 meters to the surface.

wihnb2KZ1Bs-001|For instance, here's two entries carbon-12 and naturally occurring carbon.

wihnb2KZ1Bs-002|They have different relative masses.

wihnb2KZ1Bs-003|That's because I could take a sample of pure carbon-12, where every atom is carbon-12, and that would have mass 12.

wihnb2KZ1Bs-004|But in naturally occurring carbon, 1 out of every 100 atoms is a carbon-13, it's slightly more massive.

wihnb2KZ1Bs-005|So if I took this piece of carbon and I started picking out atoms, 1 in 100 would be that carbon-13 with a slightly more massive nucleus.

wihnb2KZ1Bs-006|That's what gives this naturally occurring carbon that slightly higher relative mass.

wihnb2KZ1Bs-007|It's the mass weighted average of all the isotopes.

wihnb2KZ1Bs-008|And you can see many elements have a potpourri of different isotopes.

wihnb2KZ1Bs-009|They don't have integer molecular masses and atomic masses, because of the presence of all the different isotopes.

wihnb2KZ1Bs-010|Now for the most part, isotopes are chemically similar, that is they do the same chemical reactions, but of course they have different masses.

wihnb2KZ1Bs-011|A lot of times the mass difference is very small.

wihnb2KZ1Bs-012|For hydrogen, there's hydrogen with mass 1 and deuterium with mass 2.

wihnb2KZ1Bs-013|That's a factor of 2 in mass-- that's very large.

wihnb2KZ1Bs-014|But for carbon already, carbon-12 versus carbon-13, that's a 1% difference in mass.

wihnb2KZ1Bs-015|That's relatively small.

wihnb2KZ1Bs-017|That's a very small percentage difference in mass.

wihnb2KZ1Bs-018|Now you can separate pure isotopes and this is very common.

wihnb2KZ1Bs-019|For instance, uranium is a good example because we take uranium-238 and we separate out the other isotopes and we make pure uranium-238.

wihnb2KZ1Bs-020|It's called depleted uranium because the radioactive fissible nuclei are removed.

wihnb2KZ1Bs-022|Uranium-235 is the fissible nucleus.

wihnb2KZ1Bs-023|It's used in nuclear reactors.

wihnb2KZ1Bs-024|So we have different properties of the nuclei that are different isotopes.

wihnb2KZ1Bs-025|Chemically they're very similar, but sometimes their mass gives them different physical properties that we can use.

wihnb2KZ1Bs-026|In general, we catalog them based on the potpourri, the mass weighted average of all the isotopes in the mixture.

wihnb2KZ1Bs-027|And that's how we achieve relative atomic and molecular masses.

JOjrtRHsozI-000|Let's look at some naturally-occurring polychromic acids, amino acids.

JOjrtRHsozI-001|Amino acids are found in your body.

JOjrtRHsozI-002|They're the building blocks of the proteins in your body.

JOjrtRHsozI-003|They're called amino acids because each one has an amino group and an acid group.

JOjrtRHsozI-004|Here's the amino group and the carboxylic COOH group.

JOjrtRHsozI-005|Now, I've drawn them at pH 7.

JOjrtRHsozI-006|And I draw them at pH 7, that means this carboxylic acid group with pKa 2 will be in its basic form.

JOjrtRHsozI-011|Here, tyrosine, as well, has a side group.

JOjrtRHsozI-016|And in this case, that will be a neutral charge.

JOjrtRHsozI-017|Notice, when I protonate the amino group here at the end of lysine, that attains a positive charge.

JOjrtRHsozI-022|That's going to be in its basic form at pH 7.

JOjrtRHsozI-024|Here's histidine.

JOjrtRHsozI-028|And notice, I'm very close here.

JOjrtRHsozI-029|There's just a factor of one pH unit.

JOjrtRHsozI-030|So you know there's a factor of 10.

JOjrtRHsozI-031|There's 10 times as much of the unprotonated basic form as the protonated form.

JOjrtRHsozI-033|Now, that's very important, because the charge on amino acids, especially their side groups, affects the structure of proteins.

JOjrtRHsozI-034|Proteins are molecules in your body that do all the catalysis in your body.

JOjrtRHsozI-035|They help your chemical reactions go.

JOjrtRHsozI-036|And proteins are long chains of amino acids, and one of the reasons proteins can operate is their three-dimensional structure.

JOjrtRHsozI-038|One of the things that holds those structures together are charges on the side groups.

JOjrtRHsozI-039|You have a positively-charged side group here, a negatively-charged side group here.

JOjrtRHsozI-040|Those are attracted coulombically, and can anchor the three-dimensional structure, hold it together by that coulombic attraction.

JOjrtRHsozI-042|If the molecule falls apart, it can't perform its catalytic operation anymore.

JOjrtRHsozI-043|And I can actually demonstrate that for you.

JOjrtRHsozI-044|There's enzymes, one of them peroxidase, which are very common in nature.

JOjrtRHsozI-045|In fact, in turnips.

JOjrtRHsozI-046|I have some turnip here.

JOjrtRHsozI-048|That is, it will break down hydrogen peroxide into water and oxygen. So I'm going to do that.

JOjrtRHsozI-049|I'm going to bring in a blender here-- and I've already ground up some turnip in advance here, kind of in the Julia Child child style.

JOjrtRHsozI-050|So I've got a slurry already.

JOjrtRHsozI-051|I'm going to make a little more here.

JOjrtRHsozI-053|To one of the beakers, I'm going to add HCL, a strong acid.

JOjrtRHsozI-054|So let me get my safety glasses on here.

JOjrtRHsozI-055|I'll add a strong acid.

JOjrtRHsozI-058|So if I change the PH, I change the protonated state, and I should affect the activity of the peroxidase.

JOjrtRHsozI-059|That molecule should denature.

JOjrtRHsozI-060|So what I'm going to do now is add hydrogen peroxide to each flask, and we should see peroxidase activity, bubbling oxygen here.

wXt_tUPtAe8-000|Let's look at some electronic configurations.

wXt_tUPtAe8-001|Fluorine minus, sodium, or sodium plus.

wXt_tUPtAe8-002|Which of those three can have the electronic configuration helium 2s2 2p5 3s1?

wXt_tUPtAe8-011|Sodium plus has one fewer electrons, so it's a 10-electron system.

wXt_tUPtAe8-013|Fluorine minus, same situation.

wXt_tUPtAe8-014|It's a 10-electron species, and it's in a slightly excited state.

wXt_tUPtAe8-015|The 2p electron promoted to the 3s.

wXt_tUPtAe8-016|So what we have are two 10-electron species.