Ionic and Atomic Radius - Periodic Trends
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- Опубликовано: 12 сен 2024
- This chemistry video focuses on periodic trends such as ionic radius and atomic radius. It explains fundamental concepts of why some ions are smaller than atoms while others are larger.
Ionization Energy: • Ionization Energy - Ba...
Electron Affinity:
• Electron Affinity Tren...
Atomic Radius:
• Atomic Radius - Basic ...
Bond Energy & Bond Length:
• Bond Energy & Bond Len...
Electronegativity:
• Electronegativity, Bas...
Periodic Trends:
• Ionization Energy Elec...
__________________________________
Polar & Nonpolar Covalent Bonding:
• Polar Covalent Bonds a...
Bond Polarity & Dipole Moment:
• Bond Polarity, Electro...
Ionic Radius:
• Ionic Radius Trends, B...
Lattice Energy:
• Lattice Energy of Ioni...
Born Haber Cycle:
• Born Haber Cycle, Basi...
Bond Energy Calculations:
• Bond Energy Calculatio...
___________________________________
Lewis Structures - Mega Review:
• Lewis Structures, Intr...
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Full-Length Videos and Worksheets:
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I think you should emphasise that ions become bigger when increasing in electrons because the number of protons stay the same. Kept me confused for a bit before I figured that out.
May the parents that raised you be blessed mahn ❤️❤️❤️I just don't know how to appreciate you .
I think if you get paid for this , then am sure what you do is more than what they pay you evn if I don't know how much but this is more than someone working for virtue of being paid
thank you for always saving me in my tests! more power to your channel !
Thank you! I had a hard time understanding the trends of ionic radii but u cleared it up! Thank you for this video!
Thank you for that notice on Cation and Anion difference size.... you literally solved one of my 9 wonders of the world (not its 8)
Hi there! Your videos are great and very educational. It is easy to understand the contents as well. I would like to know the tools you use to make them. I'm trying to start something for the local schools in my area, a tutoring program if I may call it. I want to use a method where I can help as many schools as I possibly can without having to be physically present and I think making videos your method will be most effective. I'd really appreciate your help. Thank you.
Hi! I know this is kind of late - 5 years later, to be exact, but maybe this video might help, since it's a list of his equipment and stuff. ruclips.net/video/rBSuMooMYrs/видео.html
gotta put x1.5 speed for every one of his vids else i would get like no work done
1.25 is better lol
Fr
@@Satori-g4v taking things slowly is better for understanding, especially for new concepts
how u gonna dislike the guy passing you for chemistry
Cuz i dislike chemistry
do you think you have enough adds? you probably could have added 2-3 more...
were fluorine and chlorine mixed up?
I have a question. Why did you say that P and F have same energy levels when they’re in different periods? Shouldn’t they be P and Cl?
That made so much sense! Thank you so much!!
Thanks for the video!!! It helped me clear some doubts🙏🙏👍👍
wait so why are atomic and ionic radius so hard to describe?
Wow. So informative! you give me such a relief. sending good vibrations your way!
I love your videos, thank you. Your videos help a lot❤❤❤❤
You teach better than all my 8 teachers combined thxs bro
are there anyone else like me who didn't understand a word on Chemistry class, came to watch a youtube video and then just BOOM, fully understood? I can't be the only one, right ;)
You teach better than my college Professor
So atomic radii increases downwards the group and decreases rightwards. But what about the trend in a diagonal direction?
Thank you for the clear and concise explanation!
9:15 in cation Na+ isn't the effective charge supposed to be Zeff=10-2=+8 and not Zeff=11-2=+9? Need answers thanks!
I'm not entirely sure about this but I think that it is supposed to be Zeff=11-2=+9 because Na+ still has the 11 protons that Na has. The only difference is the number of electrons in the core which changes from 10 in Na to 2 in Na+. So the equation should be Na: Zeff = 11(protons) - 10(core electrons) = +1 and Na+: Zeff = 11(protons) - 2(core electrons) = +9.
Excellent explaination
No, I disagree with that
Nuclear attraction & Shielding effect both increase down the group, only that effect of the shielding effect outweighs that of the nuclear charge
The video is so amazing. actually the contain is so understandable.
saved my chem grades from dropping! bless u
😂 15:33 phosphide is huuuge
Can't stop laughing...
Best teaching on Periodic table ever!!!
dose the anions increase across the periodic table ???????????
plz ans :)
Yep
@@booksandsomemagic2536 That was quick fast as an response.
@@tahategin6969 well, that was the time I first saw this vid. Btw, hi there👋
@@booksandsomemagic2536 🤗
Thank you so much! Your video is very helpful. 💙💙💙💙💙💙💙💙
How to compare the ionic radius of I with a negative bar and S with 2negative bar?
Very helpful. Thank you.
Hii
how you formulated That sodium's Effective charge of nucleus
subtract the number of electrons excluding those in the valence shell from the number of protons
That's awesome buddy!
You are awesome!!!
Wow I really enjoyed it
Thanks 👍
Great work!!!
What about the cations of parent element with different charges?
nice vid as always.Thankyou!
yooo thanks man you saved me
Is F- smaller than Na+ or larger?
larger
F- is larger since its an anion, and anions are larger since the repulsion of electrons increase
Thanks a bunch!
Thank you :) very muchhhh
Anions are always bigger than cations?
O-2 is bigger than Mg+2?
Pleeeease answer
??
No..not always..it depends whether the set of ions is isoelectronic..I hope yk what's the concept of isoelectronic, ryt?
هل علينا حفظ الجدول الدورى؟
who's the voice behind ths vid?
amazing job
thanks
ADS on this video 2-2 seconds ughhh
Thank you!!
Thank for you help
The goat!
thank you so much :)
Thanks Teacher
Educative indeed
You are a star 🙏
Great
The explanation of the atomic radius doesn't ryme
This video just made me think of a chemistry joke! But it involves Nitrogen and Oxygen. Do you want to hear it?
"N O"
Great explanation
i love it
This makes no sense. You say that when there are more electrons on the outer shell (all else being equal, protons, energy levels, etc.), the radius will be smaller because there are more electrons being attracted inwards towards the protons...but then at 15:25 you say that anions are BIGGER than their neutral version because they have more electrons. Well which one is it??? We can say that more valence electrons - all else being equal - causes a bigger radius because there are more electrons repelling each other and therefore expanding (ie. increasing) the radius BUT we can also say that there are more electrons being attracted to the protons therefore compressing (ie. shrinking) the radius...So which one is it???? Which one takes precedence over the other, the fact that more electrons mean more repelling among themselves or the fact that more electrons mean more attraction towards the protons??? You can argue both! How do we know which takes precedence? This needs to be explained and made clear or else it all seems contradictory......
I think that he didn’t say that when there are more electrons, the radius will be smaller because there are more electrons being attracted inwards towards the protons. He said that when there are more protons, the radius will be smaller because the electrons are attracted more towards the nucleus because the nucleus has a higher positive charge, resulting in the valence electron(s) having a higher effective nuclear charge, which means the electrons are pulled closer toward the nucleus compared to that in an atom with lower effective nuclear charge. That is the trend of the atomic radii. However, for the trend of the ionic radii, the anions are bigger than the parent atoms because they have more electrons, which means there is electron repulsion which causes the electron cloud to expand, making the size bigger.
Ye
When there are more protons than usual the size decreases, but in a anion it has a negative charge which means it has more electrons in the outermost shell then usual , so it gets repelled more so it has a larger size
DIFFICULT to understand the DIFFÉRENCE BETWEEN THE 2 OXYGEN AND SODIUM. I DONT SEE THE DIFFÉRENCE.
❤😢
MG is smaller than Al
Good vid but TOO MUCH adds
Terrible video. Wayyyy drawn out for watchtime and way too many ads.
thank you soo muchhhh
Thanks
Thanks