I wrote a Chemistry test about a month ago, based on ionization energy and I watched only this video before taking the test and believe it or not, I got an A+ (100%) for that test... I am so happy and grateful to you for making chemistry less complicated than everyone, including lecturer, makes it seem. Thank you so much! God Bless.
Exactly! I dont understand anything what my teachers "teach" but thanks to this man and his language, it helps me learn what I am not very able to learn in my native language and that's wonderful but also terrifying cos I just figured out that I dont understand a subject in my native language but understand in english :(
Sir your explanations are more than perfect you make chemistry so interesting. Thank you very much sir for working hard to produce these videos .May GOD bless you, I am forever grateful to you.
I cant thank you enough, I had no hope for my chemistry As Level but thanks to you i can finally understand what my school failed to do, I hope eveything amazing comes your way.
Professor Organic Chemistry Tutor, thank you for a Basic Introduction/Explanation into Ionization Energy in AP/General Chemistry. Once again, the practice problems/problem selections are off the learning charts from start to finish. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
Your explanations are so crystal clear and iam so grateful for your teaching. Thank You so much Sir! for this and for making it free for us to learn. Means a lot!
Thank you for making this so easy to understand!!! I'm honestly blown away at how easy it was for me to catch onto this. I went here to understand why ionization isn't used more as a clean propulsion method. Now I truly see why it's such a task. But I won't stop. Those noisy propellers will be a thing of the past! I'm going to build a prototype ion propulsion system for future AVs. Thanks for your time, and explanation. I'll subscribe to the rest of your lessons.
Ionization energy - is a measure of the capability of an element to enter into chemical reactions requiring ion formation or donation of electrons. It is also generally related to the nature of the chemical bonding in the compounds formed by the elements.
If you’re taking a course, your teacher will likely have provided you with a chart. If not, you can look one up. It’s all based on experimental evidence.
Woo we have to memorixe the entire chart because they wont let us use the chart which was made so people wouldnt have to memorize this during the university exam
Yea my teacher couldn't be bothered to explain the simplicity of the discontinuity. He acts like this level chemistry is advanced hyper rocket science and us lowlifes don't technically deserve to be in his presence. SMC chemistry is taught by old gatekeeping boomers who ruin the sciences. Thank you for actually treating us students with some decorum and respect.
I love that he talks so slowly and clearly when I’m doing my first round on a tricky topic, but I love that I can speed him up, too. I didn’t know I could do this. Thanks for the heads up.
i think there is contradiction. 19:00 the more the electron is stable, the more ionization energy it requires to remove it. im judjing by your drawings and explanations.
Thanks for pointing that out! Since distance from nucleus and energy needed to remove an electron are directly proportional, I guess it would be instability/repelling of the electrons ↑ ionization energy ↓ distance from nucleus ↓. I'll correct that in my notes.
I definitely think this was confusing. If I understand correctly, he was referring to the intrinsic energy of the electron and *not* the ionization energy. If an electron is in a more stable (and lower energy) state, then it would take *more* energy to ionize it (rip it away from the atom).
Quick question: Is it incorrect to say that there is more shielding with Na than Li because the effective nuclear charge is the same? If so, then that would mean the only reason why Li has greater ionization energy is that it has less distance from the nucleus. Thanks!
I think you’re right. Usually when I’ve heard about shielding, it’s in the context of moving across a row of the periodic table. Doing that, the shielding from the inner electrons stays constant but the nuclear charge increases, so the atom size generally decreases and the ionization energy generally increases.
I might be mistaken, but I think it’s easier to measure the ionization of gases. Also, if you’re putting in enough energy to rip electrons off of atoms, I imagine that things might melt and boil anyway…
The amount of ionization energy needed to remove an electron increases as you remove more electrons. P-2 has 2 extra electrons while P-3 has 3 extra electrons, so in a way P-2 has "removed" one more electron than P-3.
@@zlidyh5 but doesn't p3- have a noble gas configuration (Ar) and p2- has the configuration of Cl? Typically noble gas configurations require the highest ionization energy, and looking at 15:31 the ionization energy for Cl is lower than Ar, so shouldn't p3- have the higher IE?
@@mht4908 I think things can be confusing because usually only the *first* ionization energies are talked about. While it’s true that ripping one electron off of an electrically neutral argon atom would require more energy than ripping one electron off a neutral chlorine atom, ripping the *second* electron off of a (now positive) argon atom would require even more energy. You can take a look at the different ionization energies here ( en.m.wikipedia.org/wiki/Molar_ionization_energies_of_the_elements ). And also, by removing electrons from a negative ion (anion), you’d be reducing the electrostatic repulsion and making things more stable, which would help to decrease the ionization energies.
There is something I don't understand from your explanation in I. E (this particular video). Here, you said the reason why the first ionisation energy of Mg2+ is bigger than the ionisation energy of Al3+ is because there is a decrease inionisation energy whenever there is a move from the S-block to the P-block , but why didn't this works for Be (beryllium) and fluorine, where Be with electronic configuration ending with 2S² (S-Block), while the fluorine ending with 2p5 (P-block)
If it's easier to remove pair electrons, then why is the ionization energy of Na (unpaired- 3s1) smaller than Mg's (paired-3s2)? How is this one different than P and S's ionization energy? Does anyone reading this know?
so am i right when i say this. I am answering a question, the question is why the jump from the second to the third ionization energy higher than the third and fourth ionization energy? It is easier to remove a 3p electron than a 3s electron because the 3p electron is the furthest from the nucleus so it decreases and also the shielding decreases which makes it easier for the valence electron to get attracted to the nucleus because there are less electrons now that will repel the valence electron
Can u explain why electron configuration of Silicon is [Ne] 3S2 3P2 and not [Ne] 3S1 3P3? Like the chromium.. Why the 1S2 electon not jump to the 3P energy level although it have 1 empty space there? Can someone explain this to me. Thank you
When electrons are unpaired, it is in a more stable situation and "stability" means it will be harder to remove that electron which implies that we need a higher energy to remove that electron(i.e a stable or unpaired electron) so as Stability 'increases' Energy 'increases' . You said otherwise that its inversely related??.
The Expression of Energy here is the "Neutral Atom Energy". To Clarify things up the energy of an atom is determined with respect to the attraction and repulsion forces present inside an atom. As the number of electrons increases, Hence the energy increases. For example P ends with 3p3 and S(Sulfur)ends with 3p4 with no doubt S has higher energy than P(phosphorus) And P is more Stable than S. Hope this answers your question :)
Final Exams and Video Playlists: www.video-tutor.net/
Chemistry 1 Final Exam Review: ua-cam.com/video/5yw1YH7YA7c/v-deo.html
I absolutely love it when we're asked how to do stuff that were never taught in lecture
every single time
Every damn lesson
Yep. Those teachers have absolutely no business collecting their paychecks. It makes me so mad they get paid to s**t all over science.
Mhmm!
U devil😂 same as me too😈
I wrote a Chemistry test about a month ago, based on ionization energy and I watched only this video before taking the test and believe it or not, I got an A+ (100%) for that test... I am so happy and grateful to you for making chemistry less complicated than everyone, including lecturer, makes it seem. Thank you so much! God Bless.
These lectures get through to my soul man, I'm serious. I cannot keep up with my professor's pace, but your videos clarify everything.
Exactly! I dont understand anything what my teachers "teach" but thanks to this man and his language, it helps me learn what I am not very able to learn in my native language and that's wonderful but also terrifying cos I just figured out that I dont understand a subject in my native language but understand in english :(
Sir your explanations are more than perfect you make chemistry so interesting. Thank you very much sir for working hard to produce these videos .May GOD bless you, I am forever grateful to you.
I agree with you
how you act one day before Chem Finals and see this vid
hahahaha How do you know my Chemistry final is coming
@@idkwhttosay912 lol
Not only in chemistry but also perfect in mathematics and physics
I cant thank you enough, I had no hope for my chemistry As Level but thanks to you i can finally understand what my school failed to do, I hope eveything amazing comes your way.
dude im studying for my As level rn as well..... well 2 years later than u
@@chrissysher0680 me too! i just started my AS levels a few months ago
@@scarlett6541 keep us updated lolol
@@chrissysher0680 how was it bro
@@nick2aim431probably not good since they never replied
my lecturer is a doctor, you and her have the same tone to your voice, constant. But the thing is I UNDERSTAND WHAT YOU ARE TEACHING thank god
how r u doing in life now?
I love your teaching. I really appreciate it. You are gifted and also have perfect voice- warm, clear, right speed, clear explanation.
Professor Organic Chemistry Tutor, thank you for a Basic Introduction/Explanation into Ionization Energy in AP/General Chemistry. Once again, the practice problems/problem selections are off the learning charts from start to finish. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
i hope there will be more people like you in the future
here i am in 2021
This man is single-handedly saving my grades in Chem
The last example u gave ... Was the most difficult for me to identify untill I watched your video... Thanks for such a good explanation
Your explanations are so crystal clear and iam so grateful for your teaching. Thank You so much Sir! for this and for making it free for us to learn. Means a lot!
Thank you for making this so easy to understand!!! I'm honestly blown away at how easy it was for me to catch onto this. I went here to understand why ionization isn't used more as a clean propulsion method. Now I truly see why it's such a task. But I won't stop. Those noisy propellers will be a thing of the past! I'm going to build a prototype ion propulsion system for future AVs. Thanks for your time, and explanation. I'll subscribe to the rest of your lessons.
How has this gone? Any progress?
2x speed for finals
amen to that one
I use 1.5x and 1.75x lol
I'm so scareddd
I think 1.5 is better
Amen😂😂😂😂😂😂😂
I understood your lessons more than my professor even I'm not good at English
Because of the difference in language. Good efforts ☺️🌸
Once In a life time polymath, and best teacher ever
I luv u mr. organic chemistry tutor theres no words as to how much i appreciate u
where are you getting these values my guy
Periodic table
You can found it in general chamistry book
google
20:19
Ohh my God,am ready for my exam now.May God richly bless you
I wish I could like this more than once. So helpful
This is such an amazing channel and series of videos. More people need to have their ion you 😎
Thank you very much, sir. You explain so perfectly. I am very grateful for the time you take to make these videos.
Thanks for your videos you make chemistry less complicated for me I really appreciate your hard work
Ionization energy - is a measure of the capability of an element to enter into chemical reactions requiring ion formation or donation of electrons. It is also generally related to the nature of the chemical bonding in the compounds formed by the elements.
I have a Chem test tomorrow and I was legit about to have a panic attack because I could not figure this out. Thanks for helping me!
How did it go?
@@PunmasterSTP well I passed out in the middle of studying from stress but I got an A so it was fucking worth it
@@skykrasher4475 I’m sorry you passed out, but I’m glad you got an A!
Thank you so much, words cant describe how grateful I am to you.
Great explaination.... I love it now it is very clear this can only possible because of so many examples
On a test when we are not given a periodic table with the ionization energies on them, how would I be able to know different exceptions to the rule?
Thanks dude! U went pretty dept in every details but I just needed 1st 5 mins.
where are you getting those values?
If you’re taking a course, your teacher will likely have provided you with a chart. If not, you can look one up. It’s all based on experimental evidence.
Woo we have to memorixe the entire chart because they wont let us use the chart which was made so people wouldnt have to memorize this during the university exam
Sucks that there doesnt seem to be a way to find the kj/mol without just knowing it
Yea my teacher couldn't be bothered to explain the simplicity of the discontinuity. He acts like this level chemistry is advanced hyper rocket science and us lowlifes don't technically deserve to be in his presence. SMC chemistry is taught by old gatekeeping boomers who ruin the sciences. Thank you for actually treating us students with some decorum and respect.
Teacher thanks
I'm from Somalia 🇸🇴 when watching this lesson very very I understood this lesson thanks much
Than I gave you subscrip and like
Amazing. Well explained. Thank you.
simply amazing!
Thanks so much sir 🙏✌️✨ Since I entered form one I have been using your lessons and explations to write my exams. Thanks so much sir❤
Your voice makes the video good!!😁
these are the best study videos
i think u made a mistake at 18:30 (?) isnt the more stable an orbit, the greater its IE? you said P with 1060 has less energy than S with 1005
watch at 1.25x speed
1.5 w/ the captions on does enough lol
1.75 is working just fine for me, if I use 2.0 then I'll need captions on for sure.
I love that he talks so slowly and clearly when I’m doing my first round on a tricky topic, but I love that I can speed him up, too. I didn’t know I could do this. Thanks for the heads up.
2.0x is usually fine for review but I think he talks faster than others so I have to hit rewind sometimes
I watch at 1.5x, especially for the videos closer to an hour long.
Where do you get the ionization energy numbers in kj/mol that’s the part I’m confused about
i think there is contradiction. 19:00 the more the electron is stable, the more ionization energy it requires to remove it. im judjing by your drawings and explanations.
I realized that as well thanks for pointing it out
Thanks for pointing that out! Since distance from nucleus and energy needed to remove an electron are directly proportional, I guess it would be instability/repelling of the electrons ↑ ionization energy ↓ distance from nucleus ↓. I'll correct that in my notes.
I definitely think this was confusing. If I understand correctly, he was referring to the intrinsic energy of the electron and *not* the ionization energy. If an electron is in a more stable (and lower energy) state, then it would take *more* energy to ionize it (rip it away from the atom).
sir thanks you explain everything well.
Thx very much, this video is much more understandable!!
thx a lot . ur explanation is so accurate to the point. really hleps alot 😄
you actually said all the questions i had to ask
thank you so much for this!!
Hi, to cationise a ion (P -3) won’t it require more energy coz it’s already stable?
what is that mean pair and unpaired electron you got make everything crystal clear
this was a great explanation
Sir I have a doubt .. the ba is more electronegative than fe because the d orbitals in ba provide poor shielding effect...........🙏🙏🙏 please help me
Quick question: Is it incorrect to say that there is more shielding with Na than Li because the effective nuclear charge is the same? If so, then that would mean the only reason why Li has greater ionization energy is that it has less distance from the nucleus. Thanks!
I think you’re right. Usually when I’ve heard about shielding, it’s in the context of moving across a row of the periodic table. Doing that, the shielding from the inner electrons stays constant but the nuclear charge increases, so the atom size generally decreases and the ionization energy generally increases.
Great video, but could you pls explain why Al+3 has more IE than Al+2 even though it is jumping from p to s sublevel for Al+2?
Do we need to memorize the energies and the exceptions in the periods??
My problem is how did you find the values of the ionization energy? Where are the numbers being made from?
Why ionization energy measured in gases phase ?
I might be mistaken, but I think it’s easier to measure the ionization of gases. Also, if you’re putting in enough energy to rip electrons off of atoms, I imagine that things might melt and boil anyway…
Sir! Please can you please explain why some elements show variable valencies 🙏
What books do you use? Can you please tell I need recomendations for studying purposes
note that +2 will be oxidation state, so it should 2+ as a charge when you write it on the upper right
But how do you even get the first ionization of 780 kj/mol?? everyone seems to skip that part and show no equation.
Thank you sir ❤🎉
I dont get the P-2 and P-3 example. Ionization Energy of P-3 looks more to me because it is 18 electrons.
The amount of ionization energy needed to remove an electron increases as you remove more electrons. P-2 has 2 extra electrons while P-3 has 3 extra electrons, so in a way P-2 has "removed" one more electron than P-3.
@@zlidyh5 but doesn't p3- have a noble gas configuration (Ar) and p2- has the configuration of Cl? Typically noble gas configurations require the highest ionization energy, and looking at 15:31 the ionization energy for Cl is lower than Ar, so shouldn't p3- have the higher IE?
@@mht4908 I think things can be confusing because usually only the *first* ionization energies are talked about. While it’s true that ripping one electron off of an electrically neutral argon atom would require more energy than ripping one electron off a neutral chlorine atom, ripping the *second* electron off of a (now positive) argon atom would require even more energy. You can take a look at the different ionization energies here ( en.m.wikipedia.org/wiki/Molar_ionization_energies_of_the_elements ).
And also, by removing electrons from a negative ion (anion), you’d be reducing the electrostatic repulsion and making things more stable, which would help to decrease the ionization energies.
Is there a way to know the kj/mol witout a periodic table? Here during the exam which matters they dont let us use it
This man who's talking in this video looks like nothing he doesn't know sometimes...😊😊😊 That includes mathematics, technology even science
I've been confused by this quetion the quetion was
The first ionization energy of aluminium is slightly less than that of magnesium, why?
I'm in 6th grade and working on 8th this really helped
good on you
That’s awesome! I hope your studies are going well.
You laid a very strong foundation on IE in me......
You are so much better than my teacher
Does e- mean ionisation energy like a constant?
Is the nuclear charge means the positive protons or the negative electrons
nuclear charge is the total positive charge in the nucleus of an atom
Thank you 💝
Quality videos you can trust.
How did you get the values of Ionization energy? I am kinda confuse here.
He looked them up. They have to be determined experimentally.
We really appreciate you 😊
How can distance decrease if energy has decreased???
There is something I don't understand from your explanation in I. E (this particular video). Here, you said the reason why the first ionisation energy of Mg2+ is bigger than the ionisation energy of Al3+ is because there is a decrease inionisation energy whenever there is a move from the S-block to the P-block , but why didn't this works for Be (beryllium) and fluorine, where Be with electronic configuration ending with 2S² (S-Block), while the fluorine ending with 2p5 (P-block)
I don't understand a single thing, like how tf did u get those numbers🧐
RIGHT??? he just pulling them outta no where
Theyre calculated using mathematical formulas
@@user-ic5hi9fg3g we wanted to know how🤦🏻♀️🤦🏻♀️
How do you calculate the KJ/Mol?
Futang ina modules fak yo
HAHAHAHA
and how does nuclear charge if directly proportion to ionization energy how ?
I'm looking for a analytical chemistry books!! Do you have any recommendations?? Please 🙏🏻
Schaum's analytical chemistry
How can I calculate the ionization energy?
what apps did you use to make this video?
If it's easier to remove pair electrons, then why is the ionization energy of Na (unpaired- 3s1) smaller than Mg's (paired-3s2)? How is this one different than P and S's ionization energy? Does anyone reading this know?
Thanks sir for making it clear
so am i right when i say this. I am answering a question, the question is why the jump from the second to the third ionization energy higher than the third and fourth ionization energy?
It is easier to remove a 3p electron than a 3s electron because the 3p electron is the furthest from the nucleus so it decreases and also the shielding decreases which makes it easier for the valence electron to get attracted to the nucleus because there are less electrons now that will repel the valence electron
What do thé 3p and 2s mean I’m so confused
When he said remove a valence electro on the silicon example, why dis he put + e- when he removed it?
its the same as saying - one electron
where do you get these values or whatever it is?????????
Why valency is more in between 3_4 than 1_2?
If an unpaired electron is more stable, why does Mg has bigger ionization energy than Na?
im really confused on this
guys were can i get magnitudes of first and second ionization energy
From where we can find the kj/mol?? Help me pls
Thank you sir
Thank you so much sir
U are the best love you !!!!!
Can u explain why electron configuration of Silicon is [Ne] 3S2 3P2 and not [Ne] 3S1 3P3? Like the chromium.. Why the 1S2 electon not jump to the 3P energy level although it have 1 empty space there? Can someone explain this to me. Thank you
It is explained a bit in this video, hopefully this helps clarify ua-cam.com/video/NIwcDnFjj98/v-deo.html
you can watch my videos too
Bro how you calucate ionization value
thank you😀🙏🙏🙏🙏
I don't get it how'd u get the numbers
Thank you thank you thank you thank you thank you thank you thank youuuuuuuuu
When electrons are unpaired, it is in a more stable situation and "stability" means it will be harder to remove that electron which implies that we need a higher energy to remove that electron(i.e a stable or unpaired electron) so as Stability 'increases' Energy 'increases' . You said otherwise that its inversely related??.
Yeah i was confused too
You can watch my videos too
The Expression of Energy here is the "Neutral Atom Energy". To Clarify things up the energy of an atom is determined with respect to the attraction and repulsion forces present inside an atom. As the number of electrons increases, Hence the energy increases. For example P ends with 3p3 and S(Sulfur)ends with 3p4 with no doubt S has higher energy than P(phosphorus) And P is more Stable than S. Hope this answers your question :)
You are blessing from god