Hey! The only atom in which shielding does not occur is hydrogen, and that is because it has one electron. Speaking in very basic terms, you are absolutely right. The two electrons are found in the 1s orbital. But lets examine the ionization energies of the two electrons in hydrogen. If shielding does not occur in helium, that would mean that both electrons should require the same amount of energy to remove them. In reality (through experiments), the ionization energy of the first electron is
exactly!! most teachers force their students to memorize the trends because they either do not quite understand the effective nuclear charge themselves or cannot quite present it in a way that their students will understand it! I am glad to see that you understood the concept! Cheers
EXCELLENT video. You did a great job at explaining this concept. The Zeff explains all of the periodic trends that teachers teach students to memorize. This background information really allowed me to really understand the trends, not just memorize them. Thanks!!!
electron (the one further away) is only 1.34 while the effective nuclear charge on the first electron (after removing the second one) is 2. And this is once again, due to the fact that the first electron partly shields the second one from the full charge.
Your chemistry lesson was so good!!!! I did not understand Zeff and shielding at all, and you explained it so well. I am now confident with the information. Thank you.
dang, this a great explanation. gonna watch this a few times! my professor is really good, but the class is kinda short so he doesn't have time to spend explaining things as well as you do. thank you Professor AK!
24.6 electron volts and the ionization energy of the second electron is 54.4 eV. Why is this the case? Why does it require more than twice as much energy to remove the second electron than the first? The fact that the second electron is less tightly bound can be interpreted as a shielding effect!! This means that the other electron shields the second electron from the full charge of the proton nucleus. Once again, through experiments, we know that the effective nuclear charge on the second
honestly this was great. Thanks a lot. I also copied down the notes you had on the whiteboard . Some really good stuff . The greatest way to teach is to always put things in a simple way because than it shows real understanding and you have doen that.
lol thank you for your clarification. fortunately, it was not wrong but merely a simplification that I and many others before me have made for the purpose of explaining effective nuclear charge.
Great video. My only question/problem is why did you use helium? In helium, both electrons are in the 1s orbital so shielding doesn't occur. dont they have to be in different sublevels for that to take place? Like in lithium for instance, one of the electrons is in the 2s orbital and is shielded by the 1s electrons.
This drawing makes it look as if He has 2 principle energy levels and 1 valance electron, instead of 2 valence electrons in 1principle energy level. Is there a reason you drew it that way? Thanks!
Madeleinebel I did that so that you could differentiate between the two different electrons, so it was simply a matter of convenience. Remember that these two electrons are not found in the same location in space and so its possible that the second electron will be found slightly farther away than the first electron. In fact, according to quantum mechanics, electrons do not actually exist in orbits, like you are taught in general chemistry. But if you stick to the Bohr model description of the atom, then you are absolutely right. The two electrons should be on the same exact energy level. Hope that helped!
How about comparison of elements in the same group? Zeff should essentially be the same due to the same proton/electron ratio although I've seen that Zeff is presumed to decrease going down a given group. Could you clarify?
Very clear explanation! But I think the falloff of the radii of atoms from left to right in periodic table's row not only depends on the decreasing of the shielding effect,but also the increasing of nucleus right? These two aspects should work together to explain the falloff of those radii. Anyway,your video is very helpful: )
Yes, that is correct. That can be easily seen by examining Coulomb's Law (assuming the electrons and protons at stationary), which states that for a greater quantity of positive charge within the nucleus, the electrons will experience a greater net force. So when the number of protons in the nucleus increases, the greater amount of positive charge pulls those electrons closer, thereby decreasing the radius.
I would suggest you use Radial Probability Density. According to RPD, 1s electrons are closer to the nucleus in H than He's 2s ( 2s has 2 nodes, not 2 energy levels). The two electrons are degenerate. Don't put them in different levels. Good video though.
shouldn't both electrons in He feel the same force since they are both on the 1s2 orbital? aren't they both occupying the exact same energy level? in the seconds chart, Li has 2 electrons on the 1s2 orbital , how come this wasn't the same situation for He's electrons? or was that He atom excited?
even if helium wasn't excited, the electrons still would not feel the same force because they would not be found at the same location (but to understand this requires quantum mechanics). since we do not want to get into that right now, lets just say we are assuming helium is in its excited state.
Hey! The only atom in which shielding does not occur is hydrogen, and that is because it has one electron. Speaking in very basic terms, you are absolutely right. The two electrons are found in the 1s orbital. But lets examine the ionization energies of the two electrons in hydrogen. If shielding does not occur in helium, that would mean that both electrons should require the same amount of energy to remove them. In reality (through experiments), the ionization energy of the first electron is
exactly!! most teachers force their students to memorize the trends because they either do not quite understand the effective nuclear charge themselves or cannot quite present it in a way that their students will understand it! I am glad to see that you understood the concept! Cheers
EXCELLENT video. You did a great job at explaining this concept. The Zeff explains all of the periodic trends that teachers teach students to memorize. This background information really allowed me to really understand the trends, not just memorize them. Thanks!!!
Thanks for watching! Im glad it helped :)
electron (the one further away) is only 1.34 while the effective nuclear charge on the first electron (after removing the second one) is 2. And this is once again, due to the fact that the first electron partly shields the second one from the full charge.
seriously one of the best explanations I have ever seen on youtube--thank you so much!
Your chemistry lesson was so good!!!! I did not understand Zeff and shielding at all, and you explained it so well. I am now confident with the information. Thank you.
That is great to hear Ashlee! :)
dang, this a great explanation. gonna watch this a few times! my professor is really good, but the class is kinda short so he doesn't have time to spend explaining things as well as you do. thank you Professor AK!
Hey! That is wonderful to hear. You are most welcome :)
24.6 electron volts and the ionization energy of the second electron is 54.4 eV. Why is this the case? Why does it require more than twice as much energy to remove the second electron than the first? The fact that the second electron is less tightly bound can be interpreted as a shielding effect!! This means that the other electron shields the second electron from the full charge of the proton nucleus. Once again, through experiments, we know that the effective nuclear charge on the second
Thanks! awesome to hear that!
honestly this was great. Thanks a lot. I also copied down the notes you had on the whiteboard . Some really good stuff . The greatest way to teach is to always put things in a simple way because than it shows real understanding and you have doen that.
lol thank you for your clarification. fortunately, it was not wrong but merely a simplification that I and many others before me have made for the purpose of explaining effective nuclear charge.
finally I understood the idea of effective nuclear charge,,thanks sir
Thank you. Thats exactly what I was trying to do, glad to hear it worked :)
doesnt the helium have both electrons in same 1s2 orbital. How can we assume there wil be this shielding thing
Thank you! Awesome that it helped :)
a very precise explanation which can be understood by anyone thank you looking forward to more such videos
neel patel Thanks Neel!
Thank You, sir. You are an absolute Legend.
Emile Heskey you're welcome! thanks for watching! :)
Brilliant! Simply BRILLIANT!
wow this guy is the best teacher
beautifully explained. Great teacher.
wow. very clearly explained! thanks! i hope you do more tutorials like this!!!
sir i'm really very pleased to see your chemisry channal on you tube....
thanks AK sir
Madhukant Vashishtha you're very welcome! :-) Thanks for watching.
Thank You sir........I am glad to find ur channel on UA-cam.....at last....thank you sir
Thank you a lot for using you time in such a helpful way!
Your videos really made my day. XD
excellent explanation! I think I'm finally beginning to understand this subject. Many, many thanks
Great video. My only question/problem is why did you use helium? In helium, both electrons are in the 1s orbital so shielding doesn't occur. dont they have to be in different sublevels for that to take place? Like in lithium for instance, one of the electrons is in the 2s orbital and is shielded by the 1s electrons.
If you were my instructor, I would hug the shit outta you. Thanks for the help!
You are just too awesome! It helped me a lot. I was so confused abt all of this but now it seems simple :D
hey this actually helped thanks!
to ease your worry, pretend the electron has been bumped up to the 2s orbital.
I need him as my chemistry professor
Thank you sir you are using a very precise explanations that are easly undestood
This one was a real help to me! Thanks
Sanjeev Asgekar You're welcome! :-)
This drawing makes it look as if He has 2 principle energy levels and 1 valance electron, instead of 2 valence electrons in 1principle energy level. Is there a reason you drew it that way? Thanks!
Madeleinebel I did that so that you could differentiate between the two different electrons, so it was simply a matter of convenience. Remember that these two electrons are not found in the same location in space and so its possible that the second electron will be found slightly farther away than the first electron. In fact, according to quantum mechanics, electrons do not actually exist in orbits, like you are taught in general chemistry. But if you stick to the Bohr model description of the atom, then you are absolutely right. The two electrons should be on the same exact energy level. Hope that helped!
Hi, I am searching for one of your videos that explained the electromagnetic excitation in atoms and the conditions for that. Thanks
The shielding of S orbital electrons is higher due to the fact that the electrons can penetrate the nucleus.
Great one really helped
thanks so much this lecture is the best
How about comparison of elements in the same group? Zeff should essentially be the same due to the same proton/electron ratio although I've seen that Zeff is presumed to decrease going down a given group. Could you clarify?
Thanks sir. This helped a lot.
Very clear explanation! But I think the falloff of the radii of atoms from left to right in periodic table's row not only depends on the decreasing of the shielding effect,but also the increasing of nucleus right? These two aspects should work together to explain the falloff of those radii. Anyway,your video is very helpful: )
Yes, that is correct. That can be easily seen by examining Coulomb's Law (assuming the electrons and protons at stationary), which states that for a greater quantity of positive charge within the nucleus, the electrons will experience a greater net force. So when the number of protons in the nucleus increases, the greater amount of positive charge pulls those electrons closer, thereby decreasing the radius.
In helium,,both the electrons are in the same shell,,,i.e. the 1st or K shell,,,but you have explained wrong, One in 1st and other in 2nd.
I am also confused. Thanks
Why did you place the 2 electrons of He separately? (had thought is 1s2. ) Thanks
I would suggest you use Radial Probability Density. According to RPD, 1s electrons are closer to the nucleus in H than He's 2s ( 2s has 2 nodes, not 2 energy levels). The two electrons are degenerate. Don't put them in different levels.
Good video though.
thanks a lot!! ur video really helps it's awesome!!
You're welcome! Glad to hear it
you my nigga. i wish you would be my AP chem teacher. you make it so much more clear
can you do a video on how to CALCULATE EFFECTIVE NUCLEUR CHARGE for outermost electron
hey its gr8. ionization energy of nitrogen is more than oxygen so does nitrogen has less shielding effect than oxygen?plse answer.
How in the He atom, does one electron get pulled away first if they are both in the 1s orbital?
why does helium own two energy levels instead of one
****But lets examine the ionization energies of the two electrons in HELIUM. (not hydrogen)
shouldn't both electrons in He feel the same force since they are both on the 1s2 orbital?
aren't they both occupying the exact same energy level? in the seconds chart, Li has 2 electrons on the 1s2 orbital , how come this wasn't the same situation for He's electrons? or was that He atom excited?
even if helium wasn't excited, the electrons still would not feel the same force because they would not be found at the same location (but to understand this requires quantum mechanics). since we do not want to get into that right now, lets just say we are assuming helium is in its excited state.
thanks pro
thanks
wiil any one tell me taht s orbotal shielding effect is more or d orbital and y??????????????
howw
Can you do Hf vs Zr
You move your hands sooo much :p
Btw great explanation..thnq
Yeah I didn't realize it at first :-P
Glad you found it helpful.
:)
You got some videos on general organic chemistry?
Do you mean the organic chemistry you cover in an AP chemistry course?
I don't know about the ap course
I am from India ..passed class 12 and preparing for mbbs entrance exam
Oh I see. Well I am not sure but you can check out my website for my organic chemistry lectures. You can find my website in the description.
Why is f-orbital shielded poorly??
thank you sir
you're welcome! :)
Respected sir u explain well but He contain on one shell which has two electrons.
Umm.. Can you explain this as we go down the group? Pleaseee
I love you
mamamia.
Thanks.
you save me from tmr's midterm
Gordon Tan Good luck Gordon! Let me know how it goes :)
the test was really easy. i over studied it. haha
lol well thats always the better case scenario! congrats :)
LOL you're welcome
but hydrogen has no neutron
sometimes it does... ;-)
hydrogen has only 1 proton bro!!!!! wtf
Gana angrez na bane
can you speak faster? this is way too slow...sorry