Atomic Radius - Basic Introduction - Periodic Table Trends, Chemistry
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- Опубліковано 7 вер 2024
- This chemistry video tutorial provides a basic introduction into atomic radius which is one of the four main periodic table trends you need to know. Atomic radius increases as you down a group and to the left across the periodic table. Atomic radius decreases with effective nuclear charge but increases with each successive energy level added to an atom as you go down a group.
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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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 🙏🏽
ua-cam.com/video/taFyYTpxcUY/v-deo.html
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I have a chem test tommorow and this helped so much!!!
This is actually easier than I thought! You made it seem easier tbh, thx
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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
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 UA-cam TV with the Organic Chemistry Tutor.
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?
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!!!!!!
Where did you get the PM of every atom?
periodictable.com/Properties/A/AtomicRadius.v.html
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Thank you so much. You explain everything so well.
I was getting confused on this, untill I watched this video. Thanks so much JG.
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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.
Brilliant video mate
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.
Thanks , you help me a lot
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!
This was really helpful and detailed 🌚
Ratha use Zeff to distinguish atomic radius between atoms then at the end you will notice that Zeff is inversely related to AR
Hi i like to know how do i get the distance between the nucleic atom of a molecule
keep up the fantastic work!
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?
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 !!
Good as always 💯
Thank you!
This helped so much! Thank you :)
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
wait so i have to momreis all the pm numbers ?
Thank you so much! This video is so helpful for me
Thank you!
Yu are best teacher from 🇮🇳
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!
Thank you sir
How are you figuring out what they are in PM??
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where can i get a chart with all the pm of every atom?
@phil0820 phil0820 A little, more like 8 months lol
Thanks man
Thank you 🙏
thanks.
Guys best of luck of ur exam 🤣
Thanks you sir❤❤
But the atomic radius of Mg is 173 and that of iodine is 198 so it should be bigger according to google
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.
how did you get the number of atomic radius?
same thing I'm trying to figure out.
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.
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
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 you
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?
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how do you know the radius of Br2 was 228 is that something to be memorized?
how did you calculate the PMs?
Same I didn't understand also
Great
How to count protons, electrons, and nuetrons in an element
Make more video
thx
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
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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
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.
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
How can you find the pm of the element?
How to find the pickle meter
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?
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
Love from India❤️
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.
The way id not listen in class if it wasnt for u sir😭😭 i would have failed
13:04 nice
what is "Zeff,"
Sen var ya adamsın
Senin ne isin var la burda
Beryllium-111
Wtf
What periodic trend exists for atomic radius?
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
Saturated and unsaturated,
Valoeant
How to find the "pm"?
periodictable.com/Properties/A/AtomicRadius.v.html
he posted this 3 years ago, goodluck buddy
@@babybird9255 thankss 😆
My eyes are open now
Dude, quit your day job and become a professor already, I'd love school if every teacher taught like you
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Neon is smaller than fluorine
Why does silver have a larger atomic radius than gold?
how did u find out the radius was 228?? nobody is saying this shit!
Fast pls I have exam tomorrow
Increase the speed, I hope your last minute worked well 😢
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How do i calculate the pm?