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The Hydrogen Atom Example Problems III
Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.
- Intro 0:00
- Example I: Show That ψ₂₁₁ is Normalized 0:07
- Example II: Show That ψ₂₁₁ is Orthogonal to ψ₃₁₀ 11:48
- Example III: Probability That a 1s Electron Will Be Found Within 1 Bohr Radius of The Nucleus 18:35
- Example IV: Radius of a Sphere 26:06
- Example V: Calculate <r> for the 2s Orbital of the Hydrogen-like Atom 36:33
Physical Chemistry Online Course
Transcription: The Hydrogen Atom Example Problems III
Hello, and welcome to www.educator.com, welcome back to Physical Chemistry.0000
We are going to continue our example problems for the hydrogen atom.0004
Let us get started.0006
The first example is show that the ψ 211 is normalized.0010
Now we are dealing with the entire wave function.0014
A function of R, a function of θ, and a function of φ.0019.2 We want to show that it is normalized.0017
Let us go ahead and write down what ψ 211.0023
Las time we are dealing with spherical harmonics, so now we are dealing with a full 3 quantum numbers 211, N, L, and M.0033
This particular wave function is equal to 1/ 64 π to ½ power Z/ α sub 0³/2 σ E ⁻σ/ 2 × sin θ E ⁺I φ,0041
where σ is actually equal to ZR/ Α sub 0.0070
Different books and different lists have some variation in how they actually list of functions,0079
depending on what they want to express as constants.0086
Whether they want to use exponents here or that I want to use √ signs, things like that.0088
If the wave functions in your book or in the particular list that you have to be looking at,0094
do not look exactly like this, do not worry about it.0097
They are the same wave function, I promise you that.0100
When you integrate them, you are going to get the same answer.0105
I would not worry too much.0108
This is Z here, Z is just is the atomic number.0111
These are the orbitals, the wave functions for what they call hydrogen like atoms.0114
Basically, anything that something like helium, where why the electrons is been taken off.0120
It is a helium atom but it has been ionized so you are still talking about the 1 electron.0126
For our purposes, we are just going to take Z equal to 1 because the atomic number of hydrogen is 1.0131
We just wan to write the general equation for the hydrogen like orbital,0137
that we are going to take Z equal to 1 and A sub 0 is the bohr radius.0142
We want to form the normalization integral which is the integral of ψ 211 conjugate × ψ 211.0148
We want this integral to equal 1 because we are trying to show that it is normalized.0167
We want this integral to equal 1.0174
Let us go ahead and write all this out.0184
Ψ 211 conjugate the integrand × ψ 211 is going to equal,0187
Let me see, the conjugate of this looks exactly the same except it is going to be E ⁻I φ instead of E ⁺I φ.0196
The 1/ 64 π to ½, 1/64 π gives us 1/ 64 π.0206
Again, we are taking Z equal to 1, 1/ A sub 0³/2 × 1/α sub 0³/2 is going to be 1/ Α sub 0³.0214
S σ is equal to Z R/α so this is just R/ A sub 0 E ⁻σ/ 2.0231
This is going to be -R/ 2 A0 sin of θ E ⁻I φ.0242
Yes, we still have some more, I think I have enough room here.0261
So × R/ A sub 0 E ⁻R/ 2 A sub 0 × sin θ × E ⁺I φ.0267
This, I multiply all the constants together.0282
This is for the conjugate and this is for the ψ 211.0286
When I put all this together, I get 1/ 64 φ A sub 0⁵ R² E ⁻R/ α sub 0.0294
R2 and R2 is going to be -2R.0318
Then, we have sin², sin θ sin θ is sin² θ E ⁺I φ E ⁻I φ × E ⁺I φ is just equal to 1.0323
This is our integrand.0334
The integral of ψ 211 conjugate × to ψ 211 is going to equal the integral from 0 to infinity.0339
Now, we are including R 0 to 2 π, 0 to π of this function which is 1/ 64 π A sub 0⁵ R² E ⁻R/Α sub 00351
sin² θ × the factor R² sin θ.0375
We are doing D θ D φ, we are going to do our last, D φ DR, inside to outside.0383
We have a function of R, a function of θ.0398
It does not look like we have a function of φ.0402
Let us go ahead and separate this out, = to 1/ 64 π A sub 0⁵ the integral from 0 to infinity, R² × R² is μ R⁴ E ⁻R A sub 0.0404
I’m going to separate out the variables, the R, θ, and φ, DR.0428
The integral from 0 to 2 π of D φ because there is no function of φ.0434
The integral from 0 to π if sin² θ sin θ, so we have our sin³ θ D θ.0439
We just put everything together.0450
All of the R’s we have put together with the r’s, under one integral.0452
The φ under one integral, the θ under one integral.0456
Now, we are going to solve these 3 integrals.0459
Integral number 1, our first integral which is equal to 0 to infinity of R⁴ E ⁻R/ Α sub 0 DR.0464
If you either let your software do it or if you look it up on a table, which is going to be on the inside cover back cover of your book0484
or the inside front cover of your book, because this integral shows up a lot so it is definitely an integral that you are going to need.0491
I think you have actually seen it before, it is 4 !/ 1/α sub 0⁵.0497
It is going to end up being 24 Α sub 0⁵.0507
That takes care of the first integral.0512
The second integral, integral number 2 that is nothing more than 0 to 2 π of D φ and that is equal to 2 π.0514
That is the second integral.0526
The third integral, integral number 3 is equal to the integral from 0 to π of sin³ θ D θ.0530
I do not know if I have done it here manually but I think at this point it is best for you to just go ahead and put it into your software.0545
I do not necessarily know if I want to go through.0552
That is fine, I will go ahead and go through this process.0554
It is it is not a problem.0557
D θ =, I going to separate this out so I will go ahead and do the manual.0558
You do not need to, but this is what it looks like, in case you would do it.0564
0 to π sin² θ sin θ.0567
I have separated this out and I'm going to use a U substitution.0572
I'm going to let, sin² θ is actually equal to 1/ π is equal to 1 - cos² θ sin θ D θ.0577
I will use a U substitution on that.0589
I will let U equal cos θ.0592
Therefore, DU = - sin θ D θ.0594
Therefore, this integral is going to actually end up equaling - the integral from 0 to π 1 - U² DU,0599
which is equal to - U – U³/ 3 from 0 to π, which is nothing more than U³/ 3 - U from 0 to π,0612
which is equal to cos³ θ/ 3 – cos θ from 0 to π.0623
And this is going to equal -1/ 3, -and -1 I hope that I have done this correctly.0642
-1/3 -1 which is going to end up equaling 4/3, this is our third integral.0650
Now that we have the first integral, the second and third.0660
When we put this together, it is going to be this × that × that × the constant.0663
We have 1/ 64 π A sub 0⁵ × 24 A sub 0⁵ × 2 π × 4/3.0670
Everything comes up to 192/ 192 is equal to 1.0690
Yes, ψ 211 is normalized as written, good, very nice.0695
Example 2, we want to show that ψ 211 is orthogonal to ψ 310.0710
Let us write out what they are.0716
Ψ 211 is equal to 1 / √ 64 π × Z/ A sub 0³/2 ZR/ A sub 0 E ⁻Z R/ 2 A sub 0 sin θ E ⁺I φ.0719
Then, we have ψ of 310 that is going to equal 1/ 81 × 2/ π.0749
I think this is going to be to the ½ and then we have Z/ A sub 0³/2.0761
This time we have 6 ZR/ A sub 0 - Z² R²/ A sub 0² × E ⁻ZR/ A sub 0.0774
Actually, it is going to be 3 A sub 0 × cos of θ.0792
Those are the two wave functions ψ 211 and ψ 310.0800
We want to form the integral to show that they are orthogonal.0805
We want to take ψ 211 the conjugate multiply by ψ 310, we want to integrate that and we want to equal 0.0815
We want this to equal 0 because we are trying to demonstrate orthogonality.0830
Ψ 211 conjugate, I’m not going to go through in every step,0842
at this point you should be reasonably familiar with taking conjugates when there is a complex there negated.0846
The ψ 211 × ψ 310 which is the integrand is going to equal,0853
I’m not going to write out all these constants over and over again.0860
I'm just going to call it the constant for 211 so let us call it ψ 211.0863
Again, we are taking Z equal to 1, the hydrogen atom.0867
R/ A0 E ⁻R/ 2 A sub 0 sin of θ E ⁻I φ because we are doing the conjugate × the constant for 310 × 6 R/0871
A 0 - R²/ A 0² × E ⁻R/ 3 A0 × the cos θ.0892
All of this is equal to ψ 211 × ψ 310 6.0909
I multiply the constants R, I'm going to get 6 R²/ A 0² – R³/ A 0³.0921
I just multiply everything together, E⁻⁵ R/ 6 A sub 0 sin θ cos θ E ⁻I φ.0934
That is my integrand.0961
Therefore, my integral of ψ 211 conjugate × ψ 310 is going to equal,0966
I'm going to go ahead, this is what I’m integrating in spherical coordinates.0977
I’m going to go ahead and just separate them at once, instead of doing it in 2 steps.0981
I'm going to have the integral from 0 to infinity of the R part.0985
6 R²/ A sub 0² – R³/ A sub 0³ E⁻⁵ R/ 6 A sub 0.0991
It is going to be R² DR 0 to 2 π of E ⁻I φ D φ × the integral from 0 to π of sin θ cos θ sin θ D θ.1001
Let us take a look at this.1038
I have this thing, this thing, and this thing.1040
The second integral is equal to 0, we have seen that before.1043
Integral number 2 is equal to 0.1047
Let me write what integral number 2 is, 0 to 2 π of E ⁻I φ D φ.1057
This is equal to 0, we know this from a previous example.1066
Therefore, our ψ 211 conjugate ψ 310 is equal to 0, which means they are orthogonal.1070
Exactly as we wanted.1087
You see that a lot of times you would not have to solve any integral.1090
The integral was very complicated but it is not complicated because a piece of it is really simple.1093
We already know that N = 0.1098
In one case it is this function.1100
In some other cases, you may have even and odd functions.1102
And if it ends up being the integral of an odd function/ a symmetric interval, that is going to equal 0.1105
Definitely makes life a lot easier.1112
Let us go ahead and go to example 3.1115
What is the probability that a 1S electron will be found within 1 bohr radius of the nucleus.1117
We want to evaluate this following integral.1123
The probability integral, we want to evaluate the integral from 0 to A sub 0.1129
Now, we are specifying an outer radius so it is no longer infinity of the ψ 1S conjugate ψ 1S.1140
This is the probability integral.1153
Normally, we just integrate it over the entire space and we want it equal to 1 to show normalization.1155
This is a normalization condition but now we are calculating the probability.1162
There is going to be some upper limit on this integral.1167
1S means that N is equal to 1 and S means that L is equal to 0.1172
Therefore, N is equal to 0.1182
What we are looking for is the ψ 100 function.1185
We need to form the ψ 100 conjugate × Ψ 100 the integrand.1191
Well, that is going to equal 1/ √ π × Z/ Α sub 0³/2 E ⁻ZR/ α sub 0 × 1/ √ π Z/ α sub 0³/2 E ⁻ZR / α sub 0.1200
Again, we are taking Z equal to 1.1230
Therefore, the Ψ 100 is going to equal,1233
This is 1 and this is 1, so it is going to equal 1/, π is taken care of, and A sub 0³ and1245
it is going to be E ⁻R/α 0 –R/ Α 0 -2R/ Α 0.1255
The integral from 0 to Α sub 0 Ψ 100 conjugate ψ 100 is going to equal 1/ π Α 0³.1273
The integral from 0 to Α sub 0 of E ⁻2R / A sub 0 and this is R² DR.1286
That is the R version.1297
We have 0 to 2 π of our D φ and we have the integral from 0 to π of, we have sin θ D θ.1299
We already know what this is, this is 2 π.1318
We already know what this is, this is just 2.1322
We have 4 π over here, this integral right here.1325
Let us go ahead and do a little something with that particular integral.1329
Should I do it on the next page?1338
I’m just going to go ahead and take care of it here.1348
The first integral, integral number 1 is the integral from 0 to A sub 0 of R² E ⁻2R/ A sub 0 D R.1351
We would actually do a little bit of a U substitution here.1365
I'm going to call U, I'm going to call it R/ A sub 0.1369
Therefore, DU is equal to 1/ A sub 0 which means that A sub 0 × DU is equal to DR.1376
I’m going to put this into the DR and then when I do R², that is going to equal A sub 0² U².1391
I'm going to put that into there.1403
This integral, when I put 0 in for here into R, I get 0.1405
U = 0.1413
This lower limit of integration is going to end up becoming 0.1415
When I put A sub 0 into R, I'm going to get the upper integral of 1.1419
When I do the substitution, I’m end up getting the following.1424
I'm going to get the integral from 0 to 1 R² is A sub 0² U².1428
This is going to be E ⁻2U and then × DR, which is A sub 0 × DU, which ends up being A sub 0² × A sub 0.1441
We have A sub 0³ × the integral from 0 to 1 of U² DU.1459
I'm sorry, U² E ⁻2U DU.1467
When I go ahead and put this into my mathematical software, I'm going to end up getting 0.08083 × A sub 0³.1476
This is my first integral.1487
My integral number 2, which was the integral from 0 to 2 π of D φ, that is equal to 2 π.1489
And then my integral number 3, which is the integral from 0 to π of sin θ D θ, that is going to actually end up equaling 2.1502
When we put all of the 3 together, we have 1/ the constant π A sub 0³ × 0.08083 A sub 0³ × 2 π × 2.1515
That that, that that, what I end up getting is 0.3233.1540
There you go, that is my probability.1550
My probability is roughly 1/3 of finding the 1S electron within 1 bohr radius.1552
Let us try example number 4, what is the radius of the sphere that encloses a 60% probability of finding the hydrogen 1S electron?1565
Express your answer in terms of A sub 0, the bohr radius.1582
They are telling us that the probability is equal to 0.6.1588
The integral that we just solve, we are going to set that integral equal to 0.61591
and we are actually going to look for that upper limit of the integral on R.1596
We want to know what that is, what is the radius that encloses a 60% probability.1604
Let me go ahead and go to blue, change this up a little bit.1610
From the previous problem and if you want you can do the integral all over again, it is not a problem.1613
From the previous problem, which also concern the 1S orbital, we found that the probability1624
was equal to 1/ π A sub 0³ 0 to some constant × A sub 0.1638
We are going to be looking for this constant ψ.1647
R² E ⁻2R/ Α sub 0 DR the integral from 0 to 2 π of D φ, the integral from 0 to π of sin θ D θ.1651
We found that all this is going to equal, this is 2, this is 2 π.1671
4 π 4 π, for on top the π cancel.1678
We are going to get 4/ A sub 0³ × the integral from 0 C A sub 0 R² E ⁻2R/ α sub 0 DR.1682
The probability integral is this, we are going to solve this integral.1699
We are going to get some equation in C and I’m going to set that C equal to our 60%,1705
because we want the probability = 60%, I want to find out what C is1710
because we want our answer expressed in terms of the A sub 0.1715
That is what we are going to do.1718
We will solve this integral then set it equal to 0.60 then solve for C.1720
Let us see what we have got.1752
Our probability integral is going to equal, I'm going to go ahead and do a little bit of U substitution here.1753
I’m going to go ahead and go to red.1766
Up here, I'm going to call U equal to R/ α sub 0 like I did before.1768
Which means that U² Α sub 0² is equal to R².1777
DU is going to equal 1/ α sub 0 DR means that DR is going to equal Α sub 0 DU.1783
When I put all of these into here, when I put DR, when I put this into DR.1793
When I put this in for R², I'm going to end up with 4 Α sub 0³/ Α sub 0³ × the integral from 0 to C.1796
When I put 0 into here, I'm going to get 0.1813
And then when I put C α sub 0 into here, I'm going to get C.1819
Now I have a new upper limit of integration and it is going to be U² E⁻² U DU.1826
This is by probability integral, I have converted this into this so I could deal with the C alone.1839
I'm going to go ahead and this cancels.1845
I’m going to go ahead and solve this integral by hand and so you can see it.1852
4 × the integral 0 to C U² E ⁻2U DU.1857
Just go ahead and do it with software but I would like you to go ahead and see it.1866
In this particular case, we have a function × a function so we are going to use something called integration by parts.1871
Integration by parts tends to get long, there is a short hand version of integration by parts called tabular integration.1876
Tabular integration, it works when your particular integration by parts integral is such that one of your functions,1886
I will go ahead and go back to blue.1893
When one of your functions differentiates down to 0 and the other one of your functions just integrates infinitely over and over again.1895
Integrals like this, where you have some polynomial and some exponential, they are perfect for tabular integration.1903
And what you actually do is this, you do U² over here, you do E ⁻TU, this is our U and this our DV.1910
Integration by parts notation, we differentiate this to TU.1920
We differentiate this down to 2 and we differentiate this down to 0.1926
We integrate this up to -1/2 E ⁻TU.1930
We integrate up to ¼ E ⁻2U and we integrate one more time up to -1/8 E⁻² U.1946
Now, we put them together like this.1952
We put that together with that one.1954
This together with that one, and this together with that one change in signs + - +.1956
This integral ends up actually equaling, it is going to be 4 × -1/2 U² E ⁻TU.1961
U is going to be this time this, this × this, this × this.1980
-U² E ⁻TU/ 2 - 2 U E⁻² U/ 4 -2 E ⁻TU/ 8.1986
This is going to equal – E⁻² U × 2U² + 2 U + 1, from 0 to C, by the way.2015
2U + 1 from 0 to C, it is going to equal - E⁻² C × 2 C² + 2 C + 1 - A -1 × 0 + 0 + 1.2034
We are going to get this integral equal to 1 - E⁻² C × 2 C² + 2 C + 1.2061
This is our probability, this is the solution to the integral.2076
We are going to set that equal to 0.6.2080
1 –E⁻² C × 2 C² + 2 C + 1 = 0.60.2084
When we go ahead and solve this equation, just put it in your software or just use a graphical calculator.2098
We end up with C equaling, E ⁻2C 2C² + 2 C + 1 = -0.40.2104
Move the 1over that side so I'm going to get E⁻² C × 2 C² + 2 C + 1.2128
These negatives cancel and I bring it back to the left.2138
It is going to be -0.40 is equal to 0.2141
This is the equation that I put my software or into my graphing calculator and I end up with C = 1.553.2146
For a 60% probability, our radius is equal to 1.553 α sub 0.2156
There you go, that is it.2174
Tedious math, but nothing that is straightforward math for the most part.2177
Of a 0.40, let us make that a little bit more clear.2183
What do we got next?2189
Calculate the average value of R for the 2S orbital of the hydrogen like atom.2202
Again, hydrogen like just means that you actually include the Z, the atomic number of the wave function.2208
You put in there for like hydrogen is just Z equal to 1.2213
This is what is going to leave the Z there.2216
Calculate the average value of R for the 2S orbital of the hydrogen like atom.2220
Let us see what we have got.2225
2S means that N is equal to 2.2227
It means that L is equal to 0, which means that M is equal to 0.2234
What we are looking at is our ψ 200.2241
The average value of R for 200 is going to equal the integral of ψ 200 conjugate × R operating on ψ 200.2249
This is the basic form for the average value of whatever it is we happen to be looking at.2265
Let us see what we have got.2273
Our ψ 200 is equal to 1/ √ 32 π × Z / α sub 0³/2 × 2 - σ × E ⁻σ/ 2.2275
Again, the σ is equal to ZR/ Α sub 0.2307
The ψ 200 conjugate is the same as this because there is nothing complex about this.2315
Therefore, this R operator, it just means multiply by R.2322
It does not matter where we put it.2330
I do not have to operate on this one first and then multiply on the left by this 1.2331
I could just multiply these 2 and then multiply by R.2335
R × ψ 200² is going to equal R × 1/ 32 π.2341
It is going to be Z³/ α 0³ × 2 - σ² E ⁻σ.2354
This × itself.2369
It is going to equal, let us pull the constants out.2373
Z³/ 32 π Α sub 0³, let us multiply this out for -4 σ + σ² E ⁻σ × R.2377
This integral here, it is going to be Z³/ 32 π A sub 0³ 0 to infinity2408
0 to 2 π 0 to π of 4 -4 σ + σ² R × R² sin θ D θ DR.2431
It is actually going to be D φ DR.2453
This is going to equal.2466
The 0 to 2 π D φ and the 0 π of the sin θ D θ is going to equal of 4 π.2478
We end up with 4 π Z³/ 32 π A sub 0³.2488
The π go away and it is going to be integral from 0 to infinity of R³ × 4 - 4 σ + σ² E ⁻σ DR.2498
I'm going to go ahead and do a little substitution here.2526
Our σ is equal to ZR / A sub 0 which means that D σ is equal to Z/α sub 0 DR.2529
Therefore, DR is equal to Α sub 0 σ/ Z and R³ is going to equal Α sub 0³/ Z³ × σ³.2546
We just rearrange this and R³.2570
When we put all of these into this thing, we end up with a lot.2573
4 π Z³/ 32 π/ A sub 0³ × A sub 0³/ Z³ × A sub 0/ Z × the integral 02582
to infinity σ³ × 4 -4 σ + σ² E ⁻σ.2606
This × D σ =, all of these things cancel out.2620
That cancels that, that cancels that, + 8, we end up with A sub 0/ 8 Z, the integral from 02624
to infinity of σ⁵ and distribute this out and rearrange.2636
Σ⁵ -4 σ⁴ + 4 σ³ D σ.2643
We have that general integral formula, we have the integral formula, what we get from the table.2658
The integral from 0 to 8 of X ⁺N × E ⁻AX DX is equal to N!/ 8 ⁺M + 1.2669
When we do that for this one, this one, and this one.2685
I keep forgetting my exponential E ⁻σ D σ.2693
When I apply this formula to this integral, this × this, this × this, this × this, I end up with,2707
Let me go back to red.2717
I end up with A sub 0/ 8Z + 5! -4 × 4! + 4 × 3!.2719
I end up with 48 A sub 0/ 8 Z and I end up with 6 A sub 0/ Z.2733
There you go, that is what we wanted, our final answer .2744
The average value of R, on average the electron will be this far from the nucleus for the 2S electron.2752
We just went through the mathematics.2765
This goes here, this is that one.2769
Let us go ahead and give you some general formulas.2774
The average value of R sub NL is equal to N² A sub 0 / Z × 1 + ½ × 1 - L × L + 1/ this is that one and this is that one.2780
Now for hydrogen, Z is equal to 1 and this general formula reduces to A sub 0/ 2 × 3 N² - L × L + 1.2815
For example, if I wanted to find the average for the 3S orbital, N is equal to 3, L is equal to 0, M is equal to 0.2845
I will just put that in.2867
I will get A sub 0/ 2, N =3, 3² is 9, 3 × -27, 27 - L × L + 1 -0.2870
It is going to be 27/2 A sub 0.2881
If I were to do it for the 3P orbital, the 3P orbital here N =3 and P, we are talking about L is equal to 1.2887
We just plug these back into there.2898
The general formula for the hydrogen atom.2900
The general formula for any hydrogen like atom which includes Z.2902
Thank you so much for joining us here at www.educator.com.2910
We will see you next time, bye.2912

Raffi Hovasapian
The Hydrogen Atom Example Problems III
Slide Duration:Table of Contents
46m 5s
- Intro0:00
- Course Overview0:16
- Thermodynamics & Classical Thermodynamics0:17
- Structure of the Course1:30
- The Ideal Gas Law3:06
- Ideal Gas Law: PV=nRT3:07
- Units of Pressure4:51
- Manipulating Units5:52
- Atmosphere : atm8:15
- Millimeter of Mercury: mm Hg8:48
- SI Unit of Volume9:32
- SI Unit of Temperature10:32
- Value of R (Gas Constant): Pv = nRT10:51
- Extensive and Intensive Variables (Properties)15:23
- Intensive Property15:52
- Extensive Property16:30
- Example: Extensive and Intensive Variables18:20
- Ideal Gas Law19:24
- Ideal Gas Law with Intensive Variables19:25
- Graphing Equations23:51
- Hold T Constant & Graph P vs. V23:52
- Hold P Constant & Graph V vs. T31:08
- Hold V Constant & Graph P vs. T34:38
- Isochores or Isometrics37:08
- More on the V vs. T Graph39:46
- More on the P vs. V Graph42:06
- Ideal Gas Law at Low Pressure & High Temperature44:26
- Ideal Gas Law at High Pressure & Low Temperature45:16
46m 2s
- Intro0:00
- Math Lesson 1: Partial Differentiation0:38
- Overview0:39
- Example I3:00
- Example II6:33
- Example III9:52
- Example IV17:26
- Differential & Derivative21:44
- What Does It Mean?21:45
- Total Differential (or Total Derivative)30:16
- Net Change in Pressure (P)33:58
- General Equation for Total Differential38:12
- Example 5: Total Differential39:28
1h 6m 45s
- Intro0:00
- Properties of Thermodynamic State1:38
- Big Picture: 3 Properties of Thermodynamic State1:39
- Enthalpy & Free Energy3:30
- Associated Law4:40
- Energy & the First Law of Thermodynamics7:13
- System & Its Surrounding Separated by a Boundary7:14
- In Other Cases the Boundary is Less Clear10:47
- State of a System12:37
- State of a System12:38
- Change in State14:00
- Path for a Change in State14:57
- Example: State of a System15:46
- Open, Close, and Isolated System18:26
- Open System18:27
- Closed System19:02
- Isolated System19:22
- Important Questions20:38
- Important Questions20:39
- Work & Heat22:50
- Definition of Work23:33
- Properties of Work25:34
- Definition of Heat32:16
- Properties of Heat34:49
- Experiment #142:23
- Experiment #247:00
- More on Work & Heat54:50
- More on Work & Heat54:51
- Conventions for Heat & Work1:00:50
- Convention for Heat1:02:40
- Convention for Work1:04:24
- Schematic Representation1:05:00
1h 6m 33s
- Intro0:00
- The First Law of Thermodynamics0:53
- The First Law of Thermodynamics0:54
- Example 1: What is the Change in Energy of the System & Surroundings?8:53
- Energy and The First Law II, cont.11:55
- The Energy of a System Changes in Two Ways11:56
- Systems Possess Energy, Not Heat or Work12:45
- Scenario 116:00
- Scenario 216:46
- State Property, Path Properties, and Path Functions18:10
- Pressure-Volume Work22:36
- When a System Changes22:37
- Gas Expands24:06
- Gas is Compressed25:13
- Pressure Volume Diagram: Analyzing Expansion27:17
- What if We do the Same Expansion in Two Stages?35:22
- Multistage Expansion43:58
- General Expression for the Pressure-Volume Work46:59
- Upper Limit of Isothermal Expansion50:00
- Expression for the Work Done in an Isothermal Expansion52:45
- Example 2: Find an Expression for the Maximum Work Done by an Ideal Gas upon Isothermal Expansion56:18
- Example 3: Calculate the External Pressure and Work Done58:50
1h 2m 17s
- Intro0:00
- Compression0:20
- Compression Overview0:34
- Single-stage compression vs. 2-stage Compression2:16
- Multi-stage Compression8:40
- Example I: Compression14:47
- Example 1: Single-stage Compression14:47
- Example 1: 2-stage Compression20:07
- Example 1: Absolute Minimum26:37
- More on Compression32:55
- Isothermal Expansion & Compression32:56
- External & Internal Pressure of the System35:18
- Reversible & Irreversible Processes37:32
- Process 1: Overview38:57
- Process 2: Overview39:36
- Process 1: Analysis40:42
- Process 2: Analysis45:29
- Reversible Process50:03
- Isothermal Expansion and Compression54:31
- Example II: Reversible Isothermal Compression of a Van der Waals Gas58:10
- Example 2: Reversible Isothermal Compression of a Van der Waals Gas58:11
1h 4m 39s
- Intro0:00
- Recall0:37
- State Function & Path Function0:38
- First Law2:11
- Exact & Inexact Differential2:12
- Where Does (∆U = Q - W) or dU = dQ - dU Come from?8:54
- Cyclic Integrals of Path and State Functions8:55
- Our Empirical Experience of the First Law12:31
- ∆U = Q - W18:42
- Relations between Changes in Properties and Energy22:24
- Relations between Changes in Properties and Energy22:25
- Rate of Change of Energy per Unit Change in Temperature29:54
- Rate of Change of Energy per Unit Change in Volume at Constant Temperature32:39
- Total Differential Equation34:38
- Constant Volume41:08
- If Volume Remains Constant, then dV = 041:09
- Constant Volume Heat Capacity45:22
- Constant Volume Integrated48:14
- Increase & Decrease in Energy of the System54:19
- Example 1: ∆U and Qv57:43
- Important Equations1:02:06
16m 50s
- Intro0:00
- Joule's Experiment0:09
- Joule's Experiment1:20
- Interpretation of the Result4:42
- The Gas Expands Against No External Pressure4:43
- Temperature of the Surrounding Does Not Change6:20
- System & Surrounding7:04
- Joule's Law10:44
- More on Joule's Experiment11:08
- Later Experiment12:38
- Dealing with the 2nd Law & Its Mathematical Consequences13:52
43m 40s
- Intro0:00
- Changes in Energy & State: Constant Pressure0:20
- Integrating with Constant Pressure0:35
- Defining the New State Function6:24
- Heat & Enthalpy of the System at Constant Pressure8:54
- Finding ∆U12:10
- dH15:28
- Constant Pressure Heat Capacity18:08
- Important Equations25:44
- Important Equations25:45
- Important Equations at Constant Pressure27:32
- Example I: Change in Enthalpy (∆H)28:53
- Example II: Change in Internal Energy (∆U)34:19
32m 23s
- Intro0:00
- The Relationship Between Cp & Cv0:21
- For a Constant Volume Process No Work is Done0:22
- For a Constant Pressure Process ∆V ≠ 0, so Work is Done1:16
- The Relationship Between Cp & Cv: For an Ideal Gas3:26
- The Relationship Between Cp & Cv: In Terms of Molar heat Capacities5:44
- Heat Capacity Can Have an Infinite # of Values7:14
- The Relationship Between Cp & Cv11:20
- When Cp is Greater than Cv17:13
- 2nd Term18:10
- 1st Term19:20
- Constant P Process: 3 Parts22:36
- Part 123:45
- Part 224:10
- Part 324:46
- Define : γ = (Cp/Cv)28:06
- For Gases28:36
- For Liquids29:04
- For an Ideal Gas30:46
39m 15s
- Intro0:00
- General Equations0:13
- Recall0:14
- How Does Enthalpy of a System Change Upon a Unit Change in Pressure?2:58
- For Liquids & Solids12:11
- For Ideal Gases14:08
- For Real Gases16:58
- The Joule Thompson Experiment18:37
- The Joule Thompson Experiment Setup18:38
- The Flow in 2 Stages22:54
- Work Equation for the Joule Thompson Experiment24:14
- Insulated Pipe26:33
- Joule-Thompson Coefficient29:50
- Changing Temperature & Pressure in Such a Way that Enthalpy Remains Constant31:44
- Joule Thompson Inversion Temperature36:26
- Positive & Negative Joule-Thompson Coefficient36:27
- Joule Thompson Inversion Temperature37:22
- Inversion Temperature of Hydrogen Gas37:59
35m 52s
- Intro0:00
- Adiabatic Changes of State0:10
- Adiabatic Changes of State0:18
- Work & Energy in an Adiabatic Process3:44
- Pressure-Volume Work7:43
- Adiabatic Changes for an Ideal Gas9:23
- Adiabatic Changes for an Ideal Gas9:24
- Equation for a Fixed Change in Volume11:20
- Maximum & Minimum Values of Temperature14:20
- Adiabatic Path18:08
- Adiabatic Path Diagram18:09
- Reversible Adiabatic Expansion21:54
- Reversible Adiabatic Compression22:34
- Fundamental Relationship Equation for an Ideal Gas Under Adiabatic Expansion25:00
- More on the Equation28:20
- Important Equations32:16
- Important Adiabatic Equation32:17
- Reversible Adiabatic Change of State Equation33:02
42m 40s
- Intro0:00
- Fundamental Equations0:56
- Work2:40
- Energy (1st Law)3:10
- Definition of Enthalpy3:44
- Heat capacity Definitions4:06
- The Mathematics6:35
- Fundamental Concepts8:13
- Isothermal8:20
- Adiabatic8:54
- Isobaric9:25
- Isometric9:48
- Ideal Gases10:14
- Example I12:08
- Example I: Conventions12:44
- Example I: Part A15:30
- Example I: Part B18:24
- Example I: Part C19:53
- Example II: What is the Heat Capacity of the System?21:49
- Example III: Find Q, W, ∆U & ∆H for this Change of State24:15
- Example IV: Find Q, W, ∆U & ∆H31:37
- Example V: Find Q, W, ∆U & ∆H38:20
1h 23s
- Intro0:00
- Example I0:11
- Example I: Finding ∆U1:49
- Example I: Finding W6:22
- Example I: Finding Q11:23
- Example I: Finding ∆H16:09
- Example I: Summary17:07
- Example II21:16
- Example II: Finding W22:42
- Example II: Finding ∆H27:48
- Example II: Finding Q30:58
- Example II: Finding ∆U31:30
- Example III33:33
- Example III: Finding ∆U, Q & W33:34
- Example III: Finding ∆H38:07
- Example IV41:50
- Example IV: Finding ∆U41:51
- Example IV: Finding ∆H45:42
- Example V49:31
- Example V: Finding W49:32
- Example V: Finding ∆U55:26
- Example V: Finding Q56:26
- Example V: Finding ∆H56:55
44m 34s
- Intro0:00
- Example I0:15
- Example I: Finding the Final Temperature3:40
- Example I: Finding Q8:04
- Example I: Finding ∆U8:25
- Example I: Finding W9:08
- Example I: Finding ∆H9:51
- Example II11:27
- Example II: Finding the Final Temperature11:28
- Example II: Finding ∆U21:25
- Example II: Finding W & Q22:14
- Example II: Finding ∆H23:03
- Example III24:38
- Example III: Finding the Final Temperature24:39
- Example III: Finding W, ∆U, and Q27:43
- Example III: Finding ∆H28:04
- Example IV29:23
- Example IV: Finding ∆U, W, and Q25:36
- Example IV: Finding ∆H31:33
- Example V32:24
- Example V: Finding the Final Temperature33:32
- Example V: Finding ∆U39:31
- Example V: Finding W40:17
- Example V: First Way of Finding ∆H41:10
- Example V: Second Way of Finding ∆H42:10
59m 7s
- Intro0:00
- Example I: Find ∆H° for the Following Reaction0:42
- Example II: Calculate the ∆U° for the Reaction in Example I5:33
- Example III: Calculate the Heat of Formation of NH₃ at 298 K14:23
- Example IV32:15
- Part A: Calculate the Heat of Vaporization of Water at 25°C33:49
- Part B: Calculate the Work Done in Vaporizing 2 Mols of Water at 25°C Under a Constant Pressure of 1 atm35:26
- Part C: Find ∆U for the Vaporization of Water at 25°C41:00
- Part D: Find the Enthalpy of Vaporization of Water at 100°C43:12
- Example V49:24
- Part A: Constant Temperature & Increasing Pressure50:25
- Part B: Increasing temperature & Constant Pressure56:20
49m 16s
- Intro0:00
- Entropy, Part 10:16
- Coefficient of Thermal Expansion (Isobaric)0:38
- Coefficient of Compressibility (Isothermal)1:25
- Relative Increase & Relative Decrease2:16
- More on α4:40
- More on κ8:38
- Entropy, Part 211:04
- Definition of Entropy12:54
- Differential Change in Entropy & the Reversible Path20:08
- State Property of the System28:26
- Entropy Changes Under Isothermal Conditions35:00
- Recall: Heating Curve41:05
- Some Phase Changes Take Place Under Constant Pressure44:07
- Example I: Finding ∆S for a Phase Change46:05
33m 59s
- Intro0:00
- Math Lesson II0:46
- Let F(x,y) = x²y³0:47
- Total Differential3:34
- Total Differential Expression6:06
- Example 19:24
- More on Math Expression13:26
- Exact Total Differential Expression13:27
- Exact Differentials19:50
- Inexact Differentials20:20
- The Cyclic Rule21:06
- The Cyclic Rule21:07
- Example 227:58
54m 37s
- Intro0:00
- Entropy As a Function of Temperature & Volume0:14
- Fundamental Equation of Thermodynamics1:16
- Things to Notice9:10
- Entropy As a Function of Temperature & Volume14:47
- Temperature-dependence of Entropy24:00
- Example I26:19
- Entropy As a Function of Temperature & Volume, Cont.31:55
- Volume-dependence of Entropy at Constant Temperature31:56
- Differentiate with Respect to Temperature, Holding Volume Constant36:16
- Recall the Cyclic Rule45:15
- Summary & Recap46:47
- Fundamental Equation of Thermodynamics46:48
- For Entropy as a Function of Temperature & Volume47:18
- The Volume-dependence of Entropy for Liquids & Solids52:52
31m 18s
- Intro0:00
- Entropy as a Function of Temperature & Pressure0:17
- Entropy as a Function of Temperature & Pressure0:18
- Rewrite the Total Differential5:54
- Temperature-dependence7:08
- Pressure-dependence9:04
- Differentiate with Respect to Pressure & Holding Temperature Constant9:54
- Differentiate with Respect to Temperature & Holding Pressure Constant11:28
- Pressure-Dependence of Entropy for Liquids & Solids18:45
- Pressure-Dependence of Entropy for Liquids & Solids18:46
- Example I: ∆S of Transformation26:20
23m 6s
- Intro0:00
- Summary of Entropy So Far0:43
- Defining dS1:04
- Fundamental Equation of Thermodynamics3:51
- Temperature & Volume6:04
- Temperature & Pressure9:10
- Two Important Equations for How Entropy Behaves13:38
- State of a System & Heat Capacity15:34
- Temperature-dependence of Entropy19:49
25m 42s
- Intro0:00
- Entropy Changes for an Ideal Gas1:10
- General Equation1:22
- The Fundamental Theorem of Thermodynamics2:37
- Recall the Basic Total Differential Expression for S = S (T,V)5:36
- For a Finite Change in State7:58
- If Cv is Constant Over the Particular Temperature Range9:05
- Change in Entropy of an Ideal Gas as a Function of Temperature & Pressure11:35
- Change in Entropy of an Ideal Gas as a Function of Temperature & Pressure11:36
- Recall the Basic Total Differential expression for S = S (T, P)15:13
- For a Finite Change18:06
- Example 1: Calculate the ∆S of Transformation22:02
43m 39s
- Intro0:00
- Entropy Example Problems I0:24
- Fundamental Equation of Thermodynamics1:10
- Entropy as a Function of Temperature & Volume2:04
- Entropy as a Function of Temperature & Pressure2:59
- Entropy For Phase Changes4:47
- Entropy For an Ideal Gas6:14
- Third Law Entropies8:25
- Statement of the Third Law9:17
- Entropy of the Liquid State of a Substance Above Its Melting Point10:23
- Entropy For the Gas Above Its Boiling Temperature13:02
- Entropy Changes in Chemical Reactions15:26
- Entropy Change at a Temperature Other than 25°C16:32
- Example I19:31
- Part A: Calculate ∆S for the Transformation Under Constant Volume20:34
- Part B: Calculate ∆S for the Transformation Under Constant Pressure25:04
- Example II: Calculate ∆S fir the Transformation Under Isobaric Conditions27:53
- Example III30:14
- Part A: Calculate ∆S if 1 Mol of Aluminum is taken from 25°C to 255°C31:14
- Part B: If S°₂₉₈ = 28.4 J/mol-K, Calculate S° for Aluminum at 498 K33:23
- Example IV: Calculate Entropy Change of Vaporization for CCl₄34:19
- Example V35:41
- Part A: Calculate ∆S of Transformation37:36
- Part B: Calculate ∆S of Transformation39:10
56m 44s
- Intro0:00
- Example I0:09
- Example I: Calculate ∆U1:28
- Example I: Calculate Q3:29
- Example I: Calculate Cp4:54
- Example I: Calculate ∆S6:14
- Example II7:13
- Example II: Calculate W8:14
- Example II: Calculate ∆U8:56
- Example II: Calculate Q10:18
- Example II: Calculate ∆H11:00
- Example II: Calculate ∆S12:36
- Example III18:47
- Example III: Calculate ∆H19:38
- Example III: Calculate Q21:14
- Example III: Calculate ∆U21:44
- Example III: Calculate W23:59
- Example III: Calculate ∆S24:55
- Example IV27:57
- Example IV: Diagram29:32
- Example IV: Calculate W32:27
- Example IV: Calculate ∆U36:36
- Example IV: Calculate Q38:32
- Example IV: Calculate ∆H39:00
- Example IV: Calculate ∆S40:27
- Example IV: Summary43:41
- Example V48:25
- Example V: Diagram49:05
- Example V: Calculate W50:58
- Example V: Calculate ∆U53:29
- Example V: Calculate Q53:44
- Example V: Calculate ∆H54:34
- Example V: Calculate ∆S55:01
57m 6s
- Intro0:00
- Example I: Isothermal Expansion0:09
- Example I: Calculate W1:19
- Example I: Calculate ∆U1:48
- Example I: Calculate Q2:06
- Example I: Calculate ∆H2:26
- Example I: Calculate ∆S3:02
- Example II: Adiabatic and Reversible Expansion6:10
- Example II: Calculate Q6:48
- Example II: Basic Equation for the Reversible Adiabatic Expansion of an Ideal Gas8:12
- Example II: Finding Volume12:40
- Example II: Finding Temperature17:58
- Example II: Calculate ∆U19:53
- Example II: Calculate W20:59
- Example II: Calculate ∆H21:42
- Example II: Calculate ∆S23:42
- Example III: Calculate the Entropy of Water Vapor25:20
- Example IV: Calculate the Molar ∆S for the Transformation34:32
- Example V44:19
- Part A: Calculate the Standard Entropy of Liquid Lead at 525°C46:17
- Part B: Calculate ∆H for the Transformation of Solid Lead from 25°C to Liquid Lead at 525°C52:23
54m 35s
- Intro0:00
- Entropy & Probability0:11
- Structural Model3:05
- Recall the Fundamental Equation of Thermodynamics9:11
- Two Independent Ways of Affecting the Entropy of a System10:05
- Boltzmann Definition12:10
- Omega16:24
- Definition of Omega16:25
- Energy Distribution19:43
- The Energy Distribution19:44
- In How Many Ways can N Particles be Distributed According to the Energy Distribution23:05
- Example I: In How Many Ways can the Following Distribution be Achieved32:51
- Example II: In How Many Ways can the Following Distribution be Achieved33:51
- Example III: In How Many Ways can the Following Distribution be Achieved34:45
- Example IV: In How Many Ways can the Following Distribution be Achieved38:50
- Entropy & Probability, cont.40:57
- More on Distribution40:58
- Example I Summary41:43
- Example II Summary42:12
- Distribution that Maximizes Omega42:26
- If Omega is Large, then S is Large44:22
- Two Constraints for a System to Achieve the Highest Entropy Possible47:07
- What Happened When the Energy of a System is Increased?49:00
35m 5s
- Intro0:00
- Volume Distribution0:08
- Distributing 2 Balls in 3 Spaces1:43
- Distributing 2 Balls in 4 Spaces3:44
- Distributing 3 Balls in 10 Spaces5:30
- Number of Ways to Distribute P Particles over N Spaces6:05
- When N is Much Larger than the Number of Particles P7:56
- Energy Distribution25:04
- Volume Distribution25:58
- Entropy, Total Entropy, & Total Omega Equations27:34
- Entropy, Total Entropy, & Total Omega Equations27:35
28m 42s
- Intro0:00
- Reversible & Irreversible0:24
- Reversible vs. Irreversible0:58
- Defining Equation for Equilibrium2:11
- Defining Equation for Irreversibility (Spontaneity)3:11
- TdS ≥ dQ5:15
- Transformation in an Isolated System11:22
- Transformation in an Isolated System11:29
- Transformation at Constant Temperature14:50
- Transformation at Constant Temperature14:51
- Helmholtz Free Energy17:26
- Define: A = U - TS17:27
- Spontaneous Isothermal Process & Helmholtz Energy20:20
- Pressure-volume Work22:02
34m 38s
- Intro0:00
- Transformation under Constant Temperature & Pressure0:08
- Transformation under Constant Temperature & Pressure0:36
- Define: G = U + PV - TS3:32
- Gibbs Energy5:14
- What Does This Say?6:44
- Spontaneous Process & a Decrease in G14:12
- Computing ∆G18:54
- Summary of Conditions21:32
- Constraint & Condition for Spontaneity21:36
- Constraint & Condition for Equilibrium24:54
- A Few Words About the Word Spontaneous26:24
- Spontaneous Does Not Mean Fast26:25
- Putting Hydrogen & Oxygen Together in a Flask26:59
- Spontaneous Vs. Not Spontaneous28:14
- Thermodynamically Favorable29:03
- Example: Making a Process Thermodynamically Favorable29:34
- Driving Forces for Spontaneity31:35
- Equation: ∆G = ∆H - T∆S31:36
- Always Spontaneous Process32:39
- Never Spontaneous Process33:06
- A Process That is Endothermic Can Still be Spontaneous34:00
30m 50s
- Intro0:00
- The Fundamental Equations of Thermodynamics0:44
- Mechanical Properties of a System0:45
- Fundamental Properties of a System1:16
- Composite Properties of a System1:44
- General Condition of Equilibrium3:16
- Composite Functions & Their Differentiations6:11
- dH = TdS + VdP7:53
- dA = -SdT - PdV9:26
- dG = -SdT + VdP10:22
- Summary of Equations12:10
- Equation #114:33
- Equation #215:15
- Equation #315:58
- Equation #416:42
- Maxwell's Relations20:20
- Maxwell's Relations20:21
- Isothermal Volume-Dependence of Entropy & Isothermal Pressure-Dependence of Entropy26:21
34m 6s
- Intro0:00
- The General Thermodynamic Equations of State0:10
- Equations of State for Liquids & Solids0:52
- More General Condition for Equilibrium4:02
- General Conditions: Equation that Relates P to Functions of T & V6:20
- The Second Fundamental Equation of Thermodynamics11:10
- Equation 117:34
- Equation 221:58
- Recall the General Expression for Cp - Cv28:11
- For the Joule-Thomson Coefficient30:44
- Joule-Thomson Inversion Temperature32:12
39m 18s
- Intro0:00
- Properties of the Helmholtz & Gibbs Energies0:10
- Equating the Differential Coefficients1:34
- An Increase in T; a Decrease in A3:25
- An Increase in V; a Decrease in A6:04
- We Do the Same Thing for G8:33
- Increase in T; Decrease in G10:50
- Increase in P; Decrease in G11:36
- Gibbs Energy of a Pure Substance at a Constant Temperature from 1 atm to any Other Pressure.14:12
- If the Substance is a Liquid or a Solid, then Volume can be Treated as a Constant18:57
- For an Ideal Gas22:18
- Special Note24:56
- Temperature Dependence of Gibbs Energy27:02
- Temperature Dependence of Gibbs Energy #127:52
- Temperature Dependence of Gibbs Energy #229:01
- Temperature Dependence of Gibbs Energy #329:50
- Temperature Dependence of Gibbs Energy #434:50
19m 40s
- Intro0:00
- Entropy of the Universe & the Surroundings0:08
- Equation: ∆G = ∆H - T∆S0:20
- Conditions of Constant Temperature & Pressure1:14
- Reversible Process3:14
- Spontaneous Process & the Entropy of the Universe5:20
- Tips for Remembering Everything12:40
- Verify Using Known Spontaneous Process14:51
54m 16s
- Intro0:00
- Example I0:11
- Example I: Deriving a Function for Entropy (S)2:06
- Example I: Deriving a Function for V5:55
- Example I: Deriving a Function for H8:06
- Example I: Deriving a Function for U12:06
- Example II15:18
- Example III21:52
- Example IV26:12
- Example IV: Part A26:55
- Example IV: Part B28:30
- Example IV: Part C30:25
- Example V33:45
- Example VI40:46
- Example VII43:43
- Example VII: Part A44:46
- Example VII: Part B50:52
- Example VII: Part C51:56
31m 17s
- Intro0:00
- Example I0:09
- Example II5:18
- Example III8:22
- Example IV12:32
- Example V17:14
- Example VI20:34
- Example VI: Part A21:04
- Example VI: Part B23:56
- Example VI: Part C27:56
45m
- Intro0:00
- Example I0:10
- Example II15:03
- Example III21:47
- Example IV28:37
- Example IV: Part A29:33
- Example IV: Part B36:09
- Example IV: Part C40:34
58m 5s
- Intro0:00
- Example I0:41
- Part A: Calculating ∆H3:55
- Part B: Calculating ∆S15:13
- Example II24:39
- Part A: Final Temperature of the System26:25
- Part B: Calculating ∆S36:57
- Example III46:49
25m 20s
- Intro0:00
- Work, Heat, and Energy0:18
- Definition of Work, Energy, Enthalpy, and Heat Capacities0:23
- Heat Capacities for an Ideal Gas3:40
- Path Property & State Property3:56
- Energy Differential5:04
- Enthalpy Differential5:40
- Joule's Law & Joule-Thomson Coefficient6:23
- Coefficient of Thermal Expansion & Coefficient of Compressibility7:01
- Enthalpy of a Substance at Any Other Temperature7:29
- Enthalpy of a Reaction at Any Other Temperature8:01
- Entropy8:53
- Definition of Entropy8:54
- Clausius Inequality9:11
- Entropy Changes in Isothermal Systems9:44
- The Fundamental Equation of Thermodynamics10:12
- Expressing Entropy Changes in Terms of Properties of the System10:42
- Entropy Changes in the Ideal Gas11:22
- Third Law Entropies11:38
- Entropy Changes in Chemical Reactions14:02
- Statistical Definition of Entropy14:34
- Omega for the Spatial & Energy Distribution14:47
- Spontaneity and Equilibrium15:43
- Helmholtz Energy & Gibbs Energy15:44
- Condition for Spontaneity & Equilibrium16:24
- Condition for Spontaneity with Respect to Entropy17:58
- The Fundamental Equations18:30
- Maxwell's Relations19:04
- The Thermodynamic Equations of State20:07
- Energy & Enthalpy Differentials21:08
- Joule's Law & Joule-Thomson Coefficient21:59
- Relationship Between Constant Pressure & Constant Volume Heat Capacities23:14
- One Final Equation - Just for Fun24:04
34m 25s
- Intro0:00
- Complex Numbers0:11
- Representing Complex Numbers in the 2-Dimmensional Plane0:56
- Addition of Complex Numbers2:35
- Subtraction of Complex Numbers3:17
- Multiplication of Complex Numbers3:47
- Division of Complex Numbers6:04
- r & θ8:04
- Euler's Formula11:00
- Polar Exponential Representation of the Complex Numbers11:22
- Example I14:25
- Example II15:21
- Example III16:58
- Example IV18:35
- Example V20:40
- Example VI21:32
- Example VII25:22
59m 57s
- Intro0:00
- Probability & Statistics1:51
- Normalization Condition1:52
- Define the Mean or Average of x11:04
- Example I: Calculate the Mean of x14:57
- Example II: Calculate the Second Moment of the Data in Example I22:39
- Define the Second Central Moment or Variance25:26
- Define the Second Central Moment or Variance25:27
- 1st Term32:16
- 2nd Term32:40
- 3rd Term34:07
- Continuous Distributions35:47
- Continuous Distributions35:48
- Probability Density39:30
- Probability Density39:31
- Normalization Condition46:51
- Example III50:13
- Part A - Show that P(x) is Normalized51:40
- Part B - Calculate the Average Position of the Particle Along the Interval54:31
- Important Things to Remember58:24
42m 5s
- Intro0:00
- Schrӧdinger Equation & Operators0:16
- Relation Between a Photon's Momentum & Its Wavelength0:17
- Louis de Broglie: Wavelength for Matter0:39
- Schrӧdinger Equation1:19
- Definition of Ψ(x)3:31
- Quantum Mechanics5:02
- Operators7:51
- Example I10:10
- Example II11:53
- Example III14:24
- Example IV17:35
- Example V19:59
- Example VI22:39
- Operators Can Be Linear or Non Linear27:58
- Operators Can Be Linear or Non Linear28:34
- Example VII32:47
- Example VIII36:55
- Example IX39:29
30m 26s
- Intro0:00
- Schrӧdinger Equation as an Eigenvalue Problem0:10
- Operator: Multiplying the Original Function by Some Scalar0:11
- Operator, Eigenfunction, & Eigenvalue4:42
- Example: Eigenvalue Problem8:00
- Schrӧdinger Equation as an Eigenvalue Problem9:24
- Hamiltonian Operator15:09
- Quantum Mechanical Operators16:46
- Kinetic Energy Operator19:16
- Potential Energy Operator20:02
- Total Energy Operator21:12
- Classical Point of View21:48
- Linear Momentum Operator24:02
- Example I26:01
21m 34s
- Intro0:00
- The Plausibility of the Schrӧdinger Equation1:16
- The Plausibility of the Schrӧdinger Equation, Part 11:17
- The Plausibility of the Schrӧdinger Equation, Part 28:24
- The Plausibility of the Schrӧdinger Equation, Part 313:45
56m 22s
- Intro0:00
- Free Particle in a Box0:28
- Definition of a Free Particle in a Box0:29
- Amplitude of the Matter Wave6:22
- Intensity of the Wave6:53
- Probability Density9:39
- Probability that the Particle is Located Between x & dx10:54
- Probability that the Particle will be Found Between o & a12:35
- Wave Function & the Particle14:59
- Boundary Conditions19:22
- What Happened When There is No Constraint on the Particle27:54
- Diagrams34:12
- More on Probability Density40:53
- The Correspondence Principle46:45
- The Correspondence Principle46:46
- Normalizing the Wave Function47:46
- Normalizing the Wave Function47:47
- Normalized Wave Function & Normalization Constant52:24
45m 24s
- Intro0:00
- Free Particle in a Box0:08
- Free Particle in a 1-dimensional Box0:09
- For a Particle in a Box3:57
- Calculating Average Values & Standard Deviations5:42
- Average Value for the Position of a Particle6:32
- Standard Deviations for the Position of a Particle10:51
- Recall: Energy & Momentum are Represented by Operators13:33
- Recall: Schrӧdinger Equation in Operator Form15:57
- Average Value of a Physical Quantity that is Associated with an Operator18:16
- Average Momentum of a Free Particle in a Box20:48
- The Uncertainty Principle24:42
- Finding the Standard Deviation of the Momentum25:08
- Expression for the Uncertainty Principle35:02
- Summary of the Uncertainty Principle41:28
48m 43s
- Intro0:00
- 2-Dimension0:12
- Dimension 20:31
- Boundary Conditions1:52
- Partial Derivatives4:27
- Example I6:08
- The Particle in a Box, cont.11:28
- Operator Notation12:04
- Symbol for the Laplacian13:50
- The Equation Becomes…14:30
- Boundary Conditions14:54
- Separation of Variables15:33
- Solution to the 1-dimensional Case16:31
- Normalization Constant22:32
- 3-Dimension28:30
- Particle in a 3-dimensional Box28:31
- In Del Notation32:22
- The Solutions34:51
- Expressing the State of the System for a Particle in a 3D Box39:10
- Energy Level & Degeneracy43:35
46m 18s
- Intro0:00
- Postulate I0:31
- Probability That The Particle Will Be Found in a Differential Volume Element0:32
- Example I: Normalize This Wave Function11:30
- Postulate II18:20
- Postulate II18:21
- Quantum Mechanical Operators: Position20:48
- Quantum Mechanical Operators: Kinetic Energy21:57
- Quantum Mechanical Operators: Potential Energy22:42
- Quantum Mechanical Operators: Total Energy22:57
- Quantum Mechanical Operators: Momentum23:22
- Quantum Mechanical Operators: Angular Momentum23:48
- More On The Kinetic Energy Operator24:48
- Angular Momentum28:08
- Angular Momentum Overview28:09
- Angular Momentum Operator in Quantum Mechanic31:34
- The Classical Mechanical Observable32:56
- Quantum Mechanical Operator37:01
- Getting the Quantum Mechanical Operator from the Classical Mechanical Observable40:16
- Postulate II, cont.43:40
- Quantum Mechanical Operators are Both Linear & Hermetical43:41
39m 28s
- Intro0:00
- Postulate III0:09
- Postulate III: Part I0:10
- Postulate III: Part II5:56
- Postulate III: Part III12:43
- Postulate III: Part IV18:28
- Postulate IV23:57
- Postulate IV23:58
- Postulate V27:02
- Postulate V27:03
- Average Value36:38
- Average Value36:39
35m 32s
- Intro0:00
- The Postulates & Principles of Quantum Mechanics, Part III0:10
- Equations: Linear & Hermitian0:11
- Introduction to Hermitian Property3:36
- Eigenfunctions are Orthogonal9:55
- The Sequence of Wave Functions for the Particle in a Box forms an Orthonormal Set14:34
- Definition of Orthogonality16:42
- Definition of Hermiticity17:26
- Hermiticity: The Left Integral23:04
- Hermiticity: The Right Integral28:47
- Hermiticity: Summary34:06
29m 55s
- Intro0:00
- The Postulates & Principles of Quantum Mechanics, Part IV0:09
- Operators can be Applied Sequentially0:10
- Sample Calculation 12:41
- Sample Calculation 25:18
- Commutator of Two Operators8:16
- The Uncertainty Principle19:01
- In the Case of Linear Momentum and Position Operator23:14
- When the Commutator of Two Operators Equals to Zero26:31
54m 25s
- Intro0:00
- Example I: Three Dimensional Box & Eigenfunction of The Laplacian Operator0:37
- Example II: Positions of a Particle in a 1-dimensional Box15:46
- Example III: Transition State & Frequency29:29
- Example IV: Finding a Particle in a 1-dimensional Box35:03
- Example V: Degeneracy & Energy Levels of a Particle in a Box44:59
46m 58s
- Intro0:00
- Review0:25
- Wave Function0:26
- Normalization Condition2:28
- Observable in Classical Mechanics & Linear/Hermitian Operator in Quantum Mechanics3:36
- Hermitian6:11
- Eigenfunctions & Eigenvalue8:20
- Normalized Wave Functions12:00
- Average Value13:42
- If Ψ is Written as a Linear Combination15:44
- Commutator16:45
- Example I: Normalize The Wave Function19:18
- Example II: Probability of Finding of a Particle22:27
- Example III: Orthogonal26:00
- Example IV: Average Value of the Kinetic Energy Operator30:22
- Example V: Evaluate These Commutators39:02
44m 11s
- Intro0:00
- Example I: Good Candidate for a Wave Function0:08
- Example II: Variance of the Energy7:00
- Example III: Evaluate the Angular Momentum Operators15:00
- Example IV: Real Eigenvalues Imposes the Hermitian Property on Operators28:44
- Example V: A Demonstration of Why the Eigenfunctions of Hermitian Operators are Orthogonal35:33
35m 33s
- Intro0:00
- The Harmonic Oscillator0:10
- Harmonic Motion0:11
- Classical Harmonic Oscillator4:38
- Hooke's Law8:18
- Classical Harmonic Oscillator, cont.10:33
- General Solution for the Differential Equation15:16
- Initial Position & Velocity16:05
- Period & Amplitude20:42
- Potential Energy of the Harmonic Oscillator23:20
- Kinetic Energy of the Harmonic Oscillator26:37
- Total Energy of the Harmonic Oscillator27:23
- Conservative System34:37
43m 4s
- Intro0:00
- The Harmonic Oscillator II0:08
- Diatomic Molecule0:10
- Notion of Reduced Mass5:27
- Harmonic Oscillator Potential & The Intermolecular Potential of a Vibrating Molecule7:33
- The Schrӧdinger Equation for the 1-dimensional Quantum Mechanic Oscillator14:14
- Quantized Values for the Energy Level15:46
- Ground State & the Zero-Point Energy21:50
- Vibrational Energy Levels25:18
- Transition from One Energy Level to the Next26:42
- Fundamental Vibrational Frequency for Diatomic Molecule34:57
- Example: Calculate k38:01
26m 30s
- Intro0:00
- The Harmonic Oscillator III0:09
- The Wave Functions Corresponding to the Energies0:10
- Normalization Constant2:34
- Hermite Polynomials3:22
- First Few Hermite Polynomials4:56
- First Few Wave-Functions6:37
- Plotting the Probability Density of the Wave-Functions8:37
- Probability Density for Large Values of r14:24
- Recall: Odd Function & Even Function19:05
- More on the Hermite Polynomials20:07
- Recall: If f(x) is Odd20:36
- Average Value of x22:31
- Average Value of Momentum23:56
41m 10s
- Intro0:00
- Possible Confusion from the Previous Discussion0:07
- Possible Confusion from the Previous Discussion0:08
- Rotation of a Single Mass Around a Fixed Center8:17
- Rotation of a Single Mass Around a Fixed Center8:18
- Angular Velocity12:07
- Rotational Inertia13:24
- Rotational Frequency15:24
- Kinetic Energy for a Linear System16:38
- Kinetic Energy for a Rotational System17:42
- Rotating Diatomic Molecule19:40
- Rotating Diatomic Molecule: Part 119:41
- Rotating Diatomic Molecule: Part 224:56
- Rotating Diatomic Molecule: Part 330:04
- Hamiltonian of the Rigid Rotor36:48
- Hamiltonian of the Rigid Rotor36:49
30m 32s
- Intro0:00
- The Rigid Rotator II0:08
- Cartesian Coordinates0:09
- Spherical Coordinates1:55
- r6:15
- θ6:28
- φ7:00
- Moving a Distance 'r'8:17
- Moving a Distance 'r' in the Spherical Coordinates11:49
- For a Rigid Rotator, r is Constant13:57
- Hamiltonian Operator15:09
- Square of the Angular Momentum Operator17:34
- Orientation of the Rotation in Space19:44
- Wave Functions for the Rigid Rotator20:40
- The Schrӧdinger Equation for the Quantum Mechanic Rigid Rotator21:24
- Energy Levels for the Rigid Rotator26:58
35m 19s
- Intro0:00
- The Rigid Rotator III0:11
- When a Rotator is Subjected to Electromagnetic Radiation1:24
- Selection Rule2:13
- Frequencies at Which Absorption Transitions Occur6:24
- Energy Absorption & Transition10:54
- Energy of the Individual Levels Overview20:58
- Energy of the Individual Levels: Diagram23:45
- Frequency Required to Go from J to J + 125:53
- Using Separation Between Lines on the Spectrum to Calculate Bond Length28:02
- Example I: Calculating Rotational Inertia & Bond Length29:18
- Example I: Calculating Rotational Inertia29:19
- Example I: Calculating Bond Length32:56
33m 48s
- Intro0:00
- Equations Review0:11
- Energy of the Harmonic Oscillator0:12
- Selection Rule3:02
- Observed Frequency of Radiation3:27
- Harmonic Oscillator Wave Functions5:52
- Rigid Rotator7:26
- Selection Rule for Rigid Rotator9:15
- Frequency of Absorption9:35
- Wave Numbers10:58
- Example I: Calculate the Reduced Mass of the Hydrogen Atom11:44
- Example II: Calculate the Fundamental Vibration Frequency & the Zero-Point Energy of This Molecule13:37
- Example III: Show That the Product of Two Even Functions is even19:35
- Example IV: Harmonic Oscillator24:56
46m 43s
- Intro0:00
- Example I: Harmonic Oscillator0:12
- Example II: Harmonic Oscillator23:26
- Example III: Calculate the RMS Displacement of the Molecules38:12
40m
- Intro0:00
- The Hydrogen Atom I1:31
- Review of the Rigid Rotator1:32
- Hydrogen Atom & the Coulomb Potential2:50
- Using the Spherical Coordinates6:33
- Applying This Last Expression to Equation 110:19
- Angular Component & Radial Component13:26
- Angular Equation15:56
- Solution for F(φ)19:32
- Determine The Normalization Constant20:33
- Differential Equation for T(a)24:44
- Legendre Equation27:20
- Legendre Polynomials31:20
- The Legendre Polynomials are Mutually Orthogonal35:40
- Limits37:17
- Coefficients38:28
35m 58s
- Intro0:00
- Associated Legendre Functions0:07
- Associated Legendre Functions0:08
- First Few Associated Legendre Functions6:39
- s, p, & d Orbital13:24
- The Normalization Condition15:44
- Spherical Harmonics20:03
- Equations We Have Found20:04
- Wave Functions for the Angular Component & Rigid Rotator24:36
- Spherical Harmonics Examples25:40
- Angular Momentum30:09
- Angular Momentum30:10
- Square of the Angular Momentum35:38
- Energies of the Rigid Rotator38:21
36m 18s
- Intro0:00
- The Hydrogen Atom III0:34
- Angular Momentum is a Vector Quantity0:35
- The Operators Corresponding to the Three Components of Angular Momentum Operator: In Cartesian Coordinates1:30
- The Operators Corresponding to the Three Components of Angular Momentum Operator: In Spherical Coordinates3:27
- Z Component of the Angular Momentum Operator & the Spherical Harmonic5:28
- Magnitude of the Angular Momentum Vector20:10
- Classical Interpretation of Angular Momentum25:22
- Projection of the Angular Momentum Vector onto the xy-plane33:24
33m 55s
- Intro0:00
- The Hydrogen Atom IV0:09
- The Equation to Find R( r )0:10
- Relation Between n & l3:50
- The Solutions for the Radial Functions5:08
- Associated Laguerre Polynomials7:58
- 1st Few Associated Laguerre Polynomials8:55
- Complete Wave Function for the Atomic Orbitals of the Hydrogen Atom12:24
- The Normalization Condition15:06
- In Cartesian Coordinates18:10
- Working in Polar Coordinates20:48
- Principal Quantum Number21:58
- Angular Momentum Quantum Number22:35
- Magnetic Quantum Number25:55
- Zeeman Effect30:45
51m 53s
- Intro0:00
- The Hydrogen Atom V: Where We Are0:13
- Review0:14
- Let's Write Out ψ₂₁₁7:32
- Angular Momentum of the Electron14:52
- Representation of the Wave Function19:36
- Radial Component28:02
- Example: 1s Orbital28:34
- Probability for Radial Function33:46
- 1s Orbital: Plotting Probability Densities vs. r35:47
- 2s Orbital: Plotting Probability Densities vs. r37:46
- 3s Orbital: Plotting Probability Densities vs. r38:49
- 4s Orbital: Plotting Probability Densities vs. r39:34
- 2p Orbital: Plotting Probability Densities vs. r40:12
- 3p Orbital: Plotting Probability Densities vs. r41:02
- 4p Orbital: Plotting Probability Densities vs. r41:51
- 3d Orbital: Plotting Probability Densities vs. r43:18
- 4d Orbital: Plotting Probability Densities vs. r43:48
- Example I: Probability of Finding an Electron in the 2s Orbital of the Hydrogen45:40
51m 53s
- Intro0:00
- The Hydrogen Atom VI0:07
- Last Lesson Review0:08
- Spherical Component1:09
- Normalization Condition2:02
- Complete 1s Orbital Wave Function4:08
- 1s Orbital Wave Function4:09
- Normalization Condition6:28
- Spherically Symmetric16:00
- Average Value17:52
- Example I: Calculate the Region of Highest Probability for Finding the Electron21:19
- 2s Orbital Wave Function25:32
- 2s Orbital Wave Function25:33
- Average Value28:56
- General Formula32:24
34m 29s
- Intro0:00
- The Hydrogen Atom VII0:12
- p Orbitals1:30
- Not Spherically Symmetric5:10
- Recall That the Spherical Harmonics are Eigenfunctions of the Hamiltonian Operator6:50
- Any Linear Combination of These Orbitals Also Has The Same Energy9:16
- Functions of Real Variables15:53
- Solving for Px16:50
- Real Spherical Harmonics21:56
- Number of Nodes32:56
43m 49s
- Intro0:00
- Example I: Angular Momentum & Spherical Harmonics0:20
- Example II: Pair-wise Orthogonal Legendre Polynomials16:40
- Example III: General Normalization Condition for the Legendre Polynomials25:06
- Example IV: Associated Legendre Functions32:13
1h 1m 57s
- Intro0:00
- Example I: Normalization & Pair-wise Orthogonal0:13
- Part 1: Normalized0:43
- Part 2: Pair-wise Orthogonal16:53
- Example II: Show Explicitly That the Following Statement is True for Any Integer n27:10
- Example III: Spherical Harmonics29:26
- Angular Momentum Cones56:37
- Angular Momentum Cones56:38
- Physical Interpretation of Orbital Angular Momentum in Quantum mechanics1:00:16
48m 33s
- Intro0:00
- Example I: Show That ψ₂₁₁ is Normalized0:07
- Example II: Show That ψ₂₁₁ is Orthogonal to ψ₃₁₀11:48
- Example III: Probability That a 1s Electron Will Be Found Within 1 Bohr Radius of The Nucleus18:35
- Example IV: Radius of a Sphere26:06
- Example V: Calculate <r> for the 2s Orbital of the Hydrogen-like Atom36:33
48m 33s
- Intro0:00
- Example I: Probability Density vs. Radius Plot0:11
- Example II: Hydrogen Atom & The Coulombic Potential14:16
- Example III: Find a Relation Among <K>, <V>, & <E>25:47
- Example IV: Quantum Mechanical Virial Theorem48:32
- Example V: Find the Variance for the 2s Orbital54:13
48m 33s
- Intro0:00
- Example I: Derive a Formula for the Degeneracy of a Given Level n0:11
- Example II: Using Linear Combinations to Represent the Spherical Harmonics as Functions of the Real Variables θ & φ8:30
- Example III: Using Linear Combinations to Represent the Spherical Harmonics as Functions of the Real Variables θ & φ23:01
- Example IV: Orbital Functions31:51
59m 18s
- Intro0:00
- Quantum Numbers Specify an Orbital0:24
- n1:10
- l1:20
- m1:35
- 4th Quantum Number: s2:02
- Spin Orbitals7:03
- Spin Orbitals7:04
- Multi-electron Atoms11:08
- Term Symbols18:08
- Russell-Saunders Coupling & The Atomic Term Symbol18:09
- Example: Configuration for C27:50
- Configuration for C: 1s²2s²2p²27:51
- Drawing Every Possible Arrangement31:15
- Term Symbols45:24
- Microstate50:54
34m 54s
- Intro0:00
- Microstates0:25
- We Started With 21 Possible Microstates0:26
- ³P State2:05
- Microstates in ³P Level5:10
- ¹D State13:16
- ³P State16:10
- ²P₂ State17:34
- ³P₁ State18:34
- ³P₀ State19:12
- 9 Microstates in ³P are Subdivided19:40
- ¹S State21:44
- Quicker Way to Find the Different Values of J for a Given Basic Term Symbol22:22
- Ground State26:27
- Hund's Empirical Rules for Specifying the Term Symbol for the Ground Electronic State27:29
- Hund's Empirical Rules: 128:24
- Hund's Empirical Rules: 229:22
- Hund's Empirical Rules: 3 - Part A30:22
- Hund's Empirical Rules: 3 - Part B31:18
- Example: 1s²2s²2p²31:54
38m 3s
- Intro0:00
- Spin Quantum Number: Term Symbols III0:14
- Deriving the Term Symbols for the p² Configuration0:15
- Table: MS vs. ML3:57
- ¹D State16:21
- ³P State21:13
- ¹S State24:48
- J Value25:32
- Degeneracy of the Level27:28
- When Given r Electrons to Assign to n Equivalent Spin Orbitals30:18
- p² Configuration32:51
- Complementary Configurations35:12
57m 49s
- Intro0:00
- Lyman Series0:09
- Spectroscopic Term Symbols0:10
- Lyman Series3:04
- Hydrogen Levels8:21
- Hydrogen Levels8:22
- Term Symbols & Atomic Spectra14:17
- Spin-Orbit Coupling14:18
- Selection Rules for Atomic Spectra21:31
- Selection Rules for Possible Transitions23:56
- Wave Numbers for The Transitions28:04
- Example I: Calculate the Frequencies of the Allowed Transitions from (4d) ²D →(2p) ²P32:23
- Helium Levels49:50
- Energy Levels for Helium49:51
- Transitions & Spin Multiplicity52:27
- Transitions & Spin Multiplicity52:28
1h 1m 20s
- Intro0:00
- Example I: What are the Term Symbols for the np¹ Configuration?0:10
- Example II: What are the Term Symbols for the np² Configuration?20:38
- Example III: What are the Term Symbols for the np³ Configuration?40:46
56m 34s
- Intro0:00
- Example I: Find the Term Symbols for the nd² Configuration0:11
- Example II: Find the Term Symbols for the 1s¹2p¹ Configuration27:02
- Example III: Calculate the Separation Between the Doublets in the Lyman Series for Atomic Hydrogen41:41
- Example IV: Calculate the Frequencies of the Lines for the (4d) ²D → (3p) ²P Transition48:53
18m 24s
- Intro0:00
- Quantum Mechanics Equations0:37
- De Broglie Relation0:38
- Statistical Relations1:00
- The Schrӧdinger Equation1:50
- The Particle in a 1-Dimensional Box of Length a3:09
- The Particle in a 2-Dimensional Box of Area a x b3:48
- The Particle in a 3-Dimensional Box of Area a x b x c4:22
- The Schrӧdinger Equation Postulates4:51
- The Normalization Condition5:40
- The Probability Density6:51
- Linear7:47
- Hermitian8:31
- Eigenvalues & Eigenfunctions8:55
- The Average Value9:29
- Eigenfunctions of Quantum Mechanics Operators are Orthogonal10:53
- Commutator of Two Operators10:56
- The Uncertainty Principle11:41
- The Harmonic Oscillator13:18
- The Rigid Rotator13:52
- Energy of the Hydrogen Atom14:30
- Wavefunctions, Radial Component, and Associated Laguerre Polynomial14:44
- Angular Component or Spherical Harmonic15:16
- Associated Legendre Function15:31
- Principal Quantum Number15:43
- Angular Momentum Quantum Number15:50
- Magnetic Quantum Number16:21
- z-component of the Angular Momentum of the Electron16:53
- Atomic Spectroscopy: Term Symbols17:14
- Atomic Spectroscopy: Selection Rules18:03
50m 2s
- Intro0:00
- Spectroscopic Overview: Which Equation Do I Use & Why1:02
- Lesson Overview1:03
- Rotational & Vibrational Spectroscopy4:01
- Frequency of Absorption/Emission6:04
- Wavenumbers in Spectroscopy8:10
- Starting State vs. Excited State10:10
- Total Energy of a Molecule (Leaving out the Electronic Energy)14:02
- Energy of Rotation: Rigid Rotor15:55
- Energy of Vibration: Harmonic Oscillator19:08
- Equation of the Spectral Lines23:22
- Harmonic Oscillator-Rigid Rotor Approximation (Making Corrections)28:37
- Harmonic Oscillator-Rigid Rotor Approximation (Making Corrections)28:38
- Vibration-Rotation Interaction33:46
- Centrifugal Distortion36:27
- Anharmonicity38:28
- Correcting for All Three Simultaneously41:03
- Spectroscopic Parameters44:26
- Summary47:32
- Harmonic Oscillator-Rigid Rotor Approximation47:33
- Vibration-Rotation Interaction48:14
- Centrifugal Distortion48:20
- Anharmonicity48:28
- Correcting for All Three Simultaneously48:44
59m 47s
- Intro0:00
- Vibration-Rotation0:37
- What is Molecular Spectroscopy?0:38
- Microwave, Infrared Radiation, Visible & Ultraviolet1:53
- Equation for the Frequency of the Absorbed Radiation4:54
- Wavenumbers6:15
- Diatomic Molecules: Energy of the Harmonic Oscillator8:32
- Selection Rules for Vibrational Transitions10:35
- Energy of the Rigid Rotator16:29
- Angular Momentum of the Rotator21:38
- Rotational Term F(J)26:30
- Selection Rules for Rotational Transition29:30
- Vibration Level & Rotational States33:20
- Selection Rules for Vibration-Rotation37:42
- Frequency of Absorption39:32
- Diagram: Energy Transition45:55
- Vibration-Rotation Spectrum: HCl51:27
- Vibration-Rotation Spectrum: Carbon Monoxide54:30
46m 22s
- Intro0:00
- Vibration-Rotation Interaction0:13
- Vibration-Rotation Spectrum: HCl0:14
- Bond Length & Vibrational State4:23
- Vibration Rotation Interaction10:18
- Case 112:06
- Case 217:17
- Example I: HCl Vibration-Rotation Spectrum22:58
- Rotational Constant for the 0 & 1 Vibrational State26:30
- Equilibrium Bond Length for the 1 Vibrational State39:42
- Equilibrium Bond Length for the 0 Vibrational State42:13
- Bₑ & αₑ44:54
29m 24s
- Intro0:00
- The Non-Rigid Rotator0:09
- Pure Rotational Spectrum0:54
- The Selection Rules for Rotation3:09
- Spacing in the Spectrum5:04
- Centrifugal Distortion Constant9:00
- Fundamental Vibration Frequency11:46
- Observed Frequencies of Absorption14:14
- Difference between the Rigid Rotator & the Adjusted Rigid Rotator16:51
- Adjusted Rigid Rotator21:31
- Observed Frequencies of Absorption26:26
30m 53s
- Intro0:00
- The Anharmonic Oscillator0:09
- Vibration-Rotation Interaction & Centrifugal Distortion0:10
- Making Corrections to the Harmonic Oscillator4:50
- Selection Rule for the Harmonic Oscillator7:50
- Overtones8:40
- True Oscillator11:46
- Harmonic Oscillator Energies13:16
- Anharmonic Oscillator Energies13:33
- Observed Frequencies of the Overtones15:09
- True Potential17:22
- HCl Vibrational Frequencies: Fundamental & First Few Overtones21:10
- Example I: Vibrational States & Overtones of the Vibrational Spectrum22:42
- Example I: Part A - First 4 Vibrational States23:44
- Example I: Part B - Fundamental & First 3 Overtones25:31
- Important Equations27:45
- Energy of the Q State29:14
- The Difference in Energy between 2 Successive States29:23
- Difference in Energy between 2 Spectral Lines29:40
1h 1m 33s
- Intro0:00
- Electronic Transitions0:16
- Electronic State & Transition0:17
- Total Energy of the Diatomic Molecule3:34
- Vibronic Transitions4:30
- Selection Rule for Vibronic Transitions9:11
- More on Vibronic Transitions10:08
- Frequencies in the Spectrum16:46
- Difference of the Minima of the 2 Potential Curves24:48
- Anharmonic Zero-point Vibrational Energies of the 2 States26:24
- Frequency of the 0 → 0 Vibronic Transition27:54
- Making the Equation More Compact29:34
- Spectroscopic Parameters32:11
- Franck-Condon Principle34:32
- Example I: Find the Values of the Spectroscopic Parameters for the Upper Excited State47:27
- Table of Electronic States and Parameters56:41
33m 47s
- Intro0:00
- Example I: Calculate the Bond Length0:10
- Example II: Calculate the Rotational Constant7:39
- Example III: Calculate the Number of Rotations10:54
- Example IV: What is the Force Constant & Period of Vibration?16:31
- Example V: Part A - Calculate the Fundamental Vibration Frequency21:42
- Example V: Part B - Calculate the Energies of the First Three Vibrational Levels24:12
- Example VI: Calculate the Frequencies of the First 2 Lines of the R & P Branches of the Vib-Rot Spectrum of HBr26:28
1h 1m 5s
- Intro0:00
- Example I: Calculate the Frequencies of the Transitions0:09
- Example II: Specify Which Transitions are Allowed & Calculate the Frequencies of These Transitions22:07
- Example III: Calculate the Vibrational State & Equilibrium Bond Length34:31
- Example IV: Frequencies of the Overtones49:28
- Example V: Vib-Rot Interaction, Centrifugal Distortion, & Anharmonicity54:47
33m 31s
- Intro0:00
- Example I: Part A - Derive an Expression for ∆G( r )0:10
- Example I: Part B - Maximum Vibrational Quantum Number6:10
- Example II: Part A - Derive an Expression for the Dissociation Energy of the Molecule8:29
- Example II: Part B - Equation for ∆G( r )14:00
- Example III: How Many Vibrational States are There for Br₂ before the Molecule Dissociates18:16
- Example IV: Find the Difference between the Two Minima of the Potential Energy Curves20:57
- Example V: Rotational Spectrum30:51
1h 1m 15s
- Intro0:00
- Statistical Thermodynamics: The Big Picture0:10
- Our Big Picture Goal0:11
- Partition Function (Q)2:42
- The Molecular Partition Function (q)4:00
- Consider a System of N Particles6:54
- Ensemble13:22
- Energy Distribution Table15:36
- Probability of Finding a System with Energy16:51
- The Partition Function21:10
- Microstate28:10
- Entropy of the Ensemble30:34
- Entropy of the System31:48
- Expressing the Thermodynamic Functions in Terms of The Partition Function39:21
- The Partition Function39:22
- Pi & U41:20
- Entropy of the System44:14
- Helmholtz Energy48:15
- Pressure of the System49:32
- Enthalpy of the System51:46
- Gibbs Free Energy52:56
- Heat Capacity54:30
- Expressing Q in Terms of the Molecular Partition Function (q)59:31
- Indistinguishable Particles1:02:16
- N is the Number of Particles in the System1:03:27
- The Molecular Partition Function1:05:06
- Quantum States & Degeneracy1:07:46
- Thermo Property in Terms of ln Q1:10:09
- Example: Thermo Property in Terms of ln Q1:13:23
47m 23s
- Intro0:00
- Lesson Overview0:19
- Monatomic Ideal Gases6:40
- Monatomic Ideal Gases Overview6:42
- Finding the Parition Function of Translation8:17
- Finding the Parition Function of Electronics13:29
- Example: Na17:42
- Example: F23:12
- Energy Difference between the Ground State & the 1st Excited State29:27
- The Various Partition Functions for Monatomic Ideal Gases32:20
- Finding P43:16
- Going Back to U = (3/2) RT46:20
54m 9s
- Intro0:00
- Diatomic Gases0:16
- Diatomic Gases0:17
- Zero-Energy Mark for Rotation2:26
- Zero-Energy Mark for Vibration3:21
- Zero-Energy Mark for Electronic5:54
- Vibration Partition Function9:48
- When Temperature is Very Low14:00
- When Temperature is Very High15:22
- Vibrational Component18:48
- Fraction of Molecules in the r Vibration State21:00
- Example: Fraction of Molecules in the r Vib. State23:29
- Rotation Partition Function26:06
- Heteronuclear & Homonuclear Diatomics33:13
- Energy & Heat Capacity36:01
- Fraction of Molecules in the J Rotational Level39:20
- Example: Fraction of Molecules in the J Rotational Level40:32
- Finding the Most Populated Level44:07
- Putting It All Together46:06
- Putting It All Together46:07
- Energy of Translation51:51
- Energy of Rotation52:19
- Energy of Vibration52:42
- Electronic Energy53:35
48m 32s
- Intro0:00
- Example I: Calculate the Fraction of Potassium Atoms in the First Excited Electronic State0:10
- Example II: Show That Each Translational Degree of Freedom Contributes R/2 to the Molar Heat Capacity14:46
- Example III: Calculate the Dissociation Energy21:23
- Example IV: Calculate the Vibrational Contribution to the Molar heat Capacity of Oxygen Gas at 500 K25:46
- Example V: Upper & Lower Quantum State32:55
- Example VI: Calculate the Relative Populations of the J=2 and J=1 Rotational States of the CO Molecule at 25°C42:21
57m 30s
- Intro0:00
- Example I: Make a Plot of the Fraction of CO Molecules in Various Rotational Levels0:10
- Example II: Calculate the Ratio of the Translational Partition Function for Cl₂ and Br₂ at Equal Volume & Temperature8:05
- Example III: Vibrational Degree of Freedom & Vibrational Molar Heat Capacity11:59
- Example IV: Calculate the Characteristic Vibrational & Rotational temperatures for Each DOF45:03
0 answers
Post by Van Anh Do on December 14, 2015
For example IV and V would it make sense to use only the radial part to calculate the radius of a sphere and <r> since those values are for R and only the radial part contains R?