Believe me you are making wonders!!! I have a chemistry test tomorrow ans was hopeless I could learn anything more in couple hours before the test. But I did, and I learned a lot more than I did in several weeks. Thank you very much for your hard work, and please continue uploading your amazing videos. We do learn from them
Professor Organic Chemistry Tutor, thank you for a solid Introduction to Atomic Radius and Periodic Table Trends in AP/General Chemistry. From the practice problems , I found this material simple to follow and understand from start to finish. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
Thanku so much Bt vl u plz tell me any other method to find the atomic size bw mg and iodine because we are not always given the value and even cant remember the value of atomic radii for all elements
A higher effective nuclear charge (zeff) causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius (or size). Zeff is calculated by : Zeff = number of protons - number of inner electrons. So for magnesium Zeff = 12 - 10 = 2. For Iodine Zeff = 53 - 50 = 3. Even without memorizing the pm you know that Magnesium (2 Zeff) has a lower Zeff than Iodine ( 3 Zeff) and therefore has a larger atomic size than Iodine.If you have 2 elements where both Zeff are the same then the element with higher energy level (most shells) is larger.
There is no such as a specific trend along the P.T. Shielding effect varies with the density of electrons in an orbital (shape of the orbital) i.e. - (s, p, d, f). As e - are least diffused in s orbital, it has the strongest shielding effect whereas in f-orbital the e- are most diffused, it has the weakest shielding effect. Hope, this helps!
So in other words in case of flourine as electrons are very close to the nucleus so the nuclus excerts a greater Force of attraction that's why Sheilding effect is less right the inner electrons aren't repelling the valence electrons strongly because of s.e? Right
Radium has a higher effective nuclear charge which brings in the outer electrons closer to the nucleus thus counteracting the trending atomic radii increase.
A higher effective nuclear charge (zeff) causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius (or size). Zeff is calculated by : Zeff = number of protons - number of inner electrons. So for magnesium Zeff = 12 - 10 = 2. For Iodine Zeff = 53 - 50 = 3. Even without memorizing the pm you know that Magnesium (2 Zeff) has a lower Zeff than Iodine ( 3 Zeff) and therefore has a larger atomic size than Iodine. If you have 2 elements where both Zeff are the same then the element with higher energy level (most shells) is larger.
number of protons in magnesium is twelve in number. On the contrary, the number of protons in iodine is 53. The atomic radius of magnesium is 173 pm and the atomic radius of iodine is 198 pm. Hence, iodine has a larger atomic radius.
You would go based on its position in the periodic table. From Left to right they get smaller. So Li would be bigger than C because it's further to the left. They get larger moving down the column so Li would be smaller than Na because it's Li is listed higher.
@@regista_09 maybe determine both of their electronic configurations, see the number of electrons in the last shells and then compare according to the trends ;-;
And yet all particles are compressed together by opposing electromagnetic fields so F would actually have a combined electromagnetic field strength that was combined from the collection of the distinct matter. 1800's understanding to today's known small particle observations is a stretch of my mind.
there are charts most likely in your textbook, or you can also find them on google. You can look up and print periodic tables with the size of each atom listed under or in the place of where the mass would be.
Final Exams and Video Playlists: www.video-tutor.net/
Chemistry 1 Final Exam Review: th-cam.com/video/5yw1YH7YA7c/w-d-xo.html
Believe me you are making wonders!!! I have a chemistry test tomorrow ans was hopeless I could learn anything more in couple hours before the test. But I did, and I learned a lot more than I did in several weeks. Thank you very much for your hard work, and please continue uploading your amazing videos. We do learn from them
This is wonderful
True very true 🙏🏽
th-cam.com/video/taFyYTpxcUY/w-d-xo.html
how did you do?
I have a chem test tommorow and this helped so much!!!
At this point you saved my education
This is actually easier than I thought! You made it seem easier tbh, thx
The fact that you are so popular shows schools are doing what they're supposed to well. Thx anyway bro
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
I love you so much, my teacher gave me a self learning assignment that will come in a quiz and this literally is saving my life thank you
pickle meters
Pico meters
Pistol meters
Pico meters . 😊
Professor Organic Chemistry Tutor, thank you for a solid Introduction to Atomic Radius and Periodic Table Trends in AP/General Chemistry. From the practice problems , I found this material simple to follow and understand from start to finish. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
Where did you get the PM of every atom?
periodictable.com/Properties/A/AtomicRadius.v.html
@@FR0SBYTES bruh you saved my life in chem
Your videos are helping me feel soo much more prepared for my 1st chemistry exam than when my professor explains it in class. THANK YOU!!!!!!
My man JG always has my back when it comes to chemistry
How are you figuring out what they are in PM??
Hi i like to know how do i get the distance between the nucleic atom of a molecule
I was getting confused on this, untill I watched this video. Thanks so much JG.
wait so i have to momreis all the pm numbers ?
Thank you, my teacher, may God bless you You are the best teacher ❤❤
I hope you make a lot of money through ads. Thank you
Thank you so much. You explain everything so well.
you really are my saviourrrr
needed revision, came here. DONE!!
Thanku so much
Bt vl u plz tell me any other method to find the atomic size bw mg and iodine because we are not always given the value and even cant remember the value of atomic radii for all elements
And plz tell me abt si abd Ge
A higher effective nuclear charge (zeff) causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius (or size). Zeff is calculated by : Zeff = number of protons - number of inner electrons. So for magnesium Zeff = 12 - 10 = 2. For Iodine Zeff = 53 - 50 = 3. Even without memorizing the pm you know that Magnesium (2 Zeff) has a lower Zeff than Iodine ( 3 Zeff) and therefore has a larger atomic size than Iodine.If you have 2 elements where both Zeff are the same then the element with higher energy level (most shells) is larger.
where can i get a chart with all the pm of every atom?
@phil0820 phil0820 A little, more like 8 months lol
❤❤❤ you're the best
Why you wrote that in Na atom in the second shell there’s ten electron, but it is 8 electrons, 2s^2 2p^6, am i right?
i have the same question, so if someone knows pls explain !!
how do you know the radius of Br2 was 228 is that something to be memorized?
Across the period, does the shielding effect remain constant because of the same number of electron shell?
There is no such as a specific trend along the P.T. Shielding effect varies with the density of electrons in an orbital (shape of the orbital) i.e. - (s, p, d, f). As e - are least diffused in s orbital, it has the strongest shielding effect whereas in f-orbital the e- are most diffused, it has the weakest shielding effect. Hope, this helps!
Guys best of luck of ur exam 🤣
Hahaha u sigma
Lol thanks man
So in other words in case of flourine as electrons are very close to the nucleus so the nuclus excerts a greater Force of attraction that's why Sheilding effect is less right the inner electrons aren't repelling the valence electrons strongly because of s.e? Right
I can't thank you enough
God Bless you💜
How do i calculate the pm?
how did you get the number of atomic radius?
same thing I'm trying to figure out.
Hey, can u explain why radium is smaller in size than potassium, It would be very helpful.
Radium has a higher effective nuclear charge which brings in the outer electrons closer to the nucleus thus counteracting the trending atomic radii increase.
You're a life saver!
Good as always 💯
keep up the fantastic work!
Brilliant video mate
how did you calculate the PMs?
Same I didn't understand also
Thanks , you help me a lot
But the atomic radius of Mg is 173 and that of iodine is 198 so it should be bigger according to google
I have a chemistry test tomorrow, wish me luck!
how was it
@@brozams08 I honestly do not remember, i passed chem 1 with a 89, and chem 2 with a 98. Chem 2 was a lot easier.
where do y’all find the measure of each elements radius
You can’t type atomic radii for elements and u will find it
periodictable.com/Properties/A/AtomicRadius.v.html
Yeah I using the periodic table that the school gave me
Yu are best teacher from 🇮🇳
Sir how mg is bigger than iodine sir?? Explanation needed
It’s because the radii is a lot bigger
A higher effective nuclear charge (zeff) causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius (or size). Zeff is calculated by : Zeff = number of protons - number of inner electrons. So for magnesium Zeff = 12 - 10 = 2. For Iodine Zeff = 53 - 50 = 3. Even without memorizing the pm you know that Magnesium (2 Zeff) has a lower Zeff than Iodine ( 3 Zeff) and therefore has a larger atomic size than Iodine. If you have 2 elements where both Zeff are the same then the element with higher energy level (most shells) is larger.
This was really helpful and detailed 🌚
we love you johnathan
This helped so much! Thank you :)
Ratha use Zeff to distinguish atomic radius between atoms then at the end you will notice that Zeff is inversely related to AR
Hello please are we to learn all the picometer stuff
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
Thank a lot for ur amazing video it really helped
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
What is electronic configuration
Thank you so much I was lost and now I get it
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
Sir you were wrong about Magnesium and iodine.
Iodine has a greater atomic radius. Apart from that I think this video was great.
No magnesium is bigger he’s correct
@@lukechang1037 Dude Please study the concept You are wrong and so is he magnesium is smaller
@@lukechang1037 Dude Iodine is 198pm and magnesium is 178pm
Magnesium is more to the left
You are wrong. Magnesium is 173pm and iodine is 140pm
number of protons in magnesium is twelve in number. On the contrary, the number of protons in iodine is 53. The atomic radius of magnesium is 173 pm and the atomic radius of iodine is 198 pm. Hence, iodine has a larger atomic radius.
what if your teacher only expects you to know which one is bigger by eyeing it out because they haven't taught you any values yet???
You would go based on its position in the periodic table. From Left to right they get smaller. So Li would be bigger than C because it's further to the left. They get larger moving down the column so Li would be smaller than Na because it's Li is listed higher.
Thank you!
Thank you so much! This video is so helpful for me
It is very good. TNX
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
thank u again dudee
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
@@regista_09 maybe determine both of their electronic configurations, see the number of electrons in the last shells and then compare according to the trends ;-;
@@redw4n So you mean, will have to memorise whole table ;(
How do I compare the atomic radius of two elements from different group as well as period. For eg Be and Al, do i have to memorise?
Thanks you sir❤❤
what is "Zeff,"
Thank you 🙏
Thank you sir
How to find the pickle meter
And yet all particles are compressed together by opposing electromagnetic fields so F would actually have a combined electromagnetic field strength that was combined from the collection of the distinct matter. 1800's understanding to today's known small particle observations is a stretch of my mind.
Great video but,how do you know abot Atomic radi in down right and down left😢❤
Thanks man
can someone pls explain why he put 10 electrons in the second outer shell of Na, when the maximum electron in the second outer shell is 8 ?
It was probably a mistake, slip of tounge
The way id not listen in class if it wasnt for u sir😭😭 i would have failed
How to find the "pm"?
periodictable.com/Properties/A/AtomicRadius.v.html
he posted this 3 years ago, goodluck buddy
@@babybird9255 thankss 😆
Thank you!
Dude, quit your day job and become a professor already, I'd love school if every teacher taught like you
thanks.
Make more video
Congrats 👌
you are the best 🥹🥲🥲🥲🌸🌸🌸🌸🌸✅✅✅✅✅
I love you man
i love u i love u i love u a trillion times
INFINITELY
Love from India❤️
Ok I don’t get the part of the radius how u know the number of every single element radius
there are charts most likely in your textbook, or you can also find them on google. You can look up and print periodic tables with the size of each atom listed under or in the place of where the mass would be.
periodictable.com/Properties/A/AtomicRadius.v.html
Great
13:04 nice
My eyes are open now
What periodic trend exists for atomic radius?
Who else heard "116" at 9:16? 😂
thank you
Beryllium-111
Wtf
thx
Sen var ya adamsın
Senin ne isin var la burda
Fast pls I have exam tomorrow
Increase the speed, I hope your last minute worked well 😢
how did u find out the radius was 228?? nobody is saying this shit!
ur accent sounds like Peter Parker's (Tom Holland)
It is very help full for me sir thank you but i need another way its not simple and cool to find the atomic radius
❤
Valoeant
Why does silver have a larger atomic radius than gold?
152 किसे आया
I owe you the fees I pay the university
😁😁😁
2:32
like 69......