Effective Nuclear Charge, Shielding effect, & Periodic Properties Tutorial; Crash Chemistry Academy

This video is a crash course on what shielding is, what effective nuclear charge is, how they are related, how they produce specific atomic properties including the size of atoms and trends in atomic size, and electronegativy and electronegativity trends, and how shielding and effective nuclear charge determine periodicity of atomic properties.

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[@CrashChemistryAcademy]

Thanks so much, I appreciate the comment!

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[@CrashChemistryAcademy]

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[@CrashChemistryAcademy]

You're welcome and thank you! Glad it was helpful!

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Incredibly helpful!! Had to leave a comment because I have been looking for videos to explain Zeff and this is the only on I came across that explained it not only in detail but in a way I completely understand it now. Thank you so much!!

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These videos really provide clarification.

[@agustinjaysoncadag]

The two are very important concepts to understand periodicity. I struggled understanding shielding and Zeff but you made it easier.

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thanks to this video, i finally understand this concept. have been staring at my notes for hours...

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[@CrashChemistryAcademy]

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[@viively7]

FINALLY! a video that explains all the essentials of Zeff without complicating it

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[@CrashChemistryAcademy]

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[@CrashChemistryAcademy]

Thanks for your very nice comment!

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[@CrashChemistryAcademy]

Thanks!

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The Best way to calculate Zeff. You are really Great SIr. Thank you soooooo much

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[@df4250]

Again. Where were you when I needed you? :) Beautiful explanations. The content of this video is related to a question I asked about your video on metallic element electron behaviour. Asked in terms of ionisation energy, is it this energy that determines whether the valence electrons of an element behave by forming covalent bonds as against the less defined wanderings of electrons in metals?

[@CrashChemistryAcademy]

Not exactly. That is more in the realm of electronegativity, although the two are related. See my reply to your comment in the metallic bonding video.

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Well explained. I finally understand this concept!! Huge thanks.

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Up to the point & concise. Thanks for uploading this. Helped me alot

[@CrashChemistryAcademy]

Thanks!

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Tq sir it was very interesting topic

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This video is so much better than my lecture on this.

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pictures just hit different thanks!

[@thetruedjlivewire]

so the loose valence electrons act like iron surrounding a magnet or otherwise core structure valence electrons. that being said, aside from shielding specifically, the domain of said electrons would abide by formations of macro motive force.

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[@CrashChemistryAcademy]

You're welcome! Thanks for your comment.

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In fact, sir you are the best!

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[@CrashChemistryAcademy]

شكرا على تعليقك، شكرا على المشاهدة.

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Thankyou sir to make us understand about the concept

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Amazing explanation for such a complicated chem topic. This helped me soooo much. THANK YOU!!

[@CrashChemistryAcademy]

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[@hunterthorne4671]

Why don't we always say zeff is the number of Valence electrons instead of calculating it all the time...?

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[@user-pv3cn7xo1i]

core electrons are electrons that are not in outermost shell?

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[@CrashChemistryAcademy]

You're welcome, I'm glad it helped!

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[@tb2748]

Could you explain the lanthanide contraction? I don't get why Au has a smaller bonding atomic radius than Sc. My textbook says it has to do with shielding and that 4f orbitals are being filled, which causes an increase in Zeff. But I thought that the increase in core electrons, 4f electrons, would cause more repulsion, making Au have a bigger radius.

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[@ripan110]

very well explained!! thank you so much

[@MrMikael1337]

when you talk about Z_eff, you take into account both the shielding and the attractive force from the nucleus, but when you talk about IE you only take into account the shielding and NOT the attractive force. how come?

[@60pluscrazy]

Fantastic

[@CrashChemistryAcademy]

Thanks!

[@thechosen123isme]

Very clear explanation! Thanks.

[@sulezakaria7312]

Excellent work

[@NehPandya]

According to our theory atomic size should increase in groups from top to bottom but in group 13 Aluminium has atomic radius 143 pm and Gallium has atomic radius 135 pm which is less WHY??????

[@CrashChemistryAcademy]

Since size is intimately related to shielding and the number of protons, lets look there. Aluminum has no d electrons, and so the shielding of its three valence electrons comes only from the core ten electrons of the neon configuration. With gallium you have suddenly added another 18 electrons and protons. Ten of those are d electrons (three are valence--s2p1), but the d orbital energy is quite close to that of s, and the d electron positions are also, on average, close to the s electrons, which reduce the effect of their shielding. The result is those added 18 protons have a larger attractive affect (greater Zeff), bringing the electrons closer to the nucleus and reducing the radius. So to sum it up, the difference is the presence of d electrons.

[@CrashChemistryAcademy]

Because there is such a wide variety of ways to measure/calculate radii, you may be comparing two different methods. Almost all methods have Ga larger than Al. Look at webelements.com for a comprehensive list.

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[@JohannaPoysti]

Why did my teacher teach to find effective nuclear charge is -10 for all element after neon and -2 for all elements before neon? So eg Cl with atomic number 17 you -10=7+ is the effective nuclear charge...

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[@cinderellab4410]

What about the "decreased attractive force as distance increases with energy level" aka "inverse square law" argument used to explain trends down a group?

[@CrashChemistryAcademy]

I specifically state that among the factors in the trends discussed are distance from the nucleus and the resulting change in attractive force. This is Coulomb's Law, although I did not specifically state the law, but things were getting a bit complicated.

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Cool

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[@CrashChemistryAcademy]

You are welcome!

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[@mohammedali]

Thanks!!! Great detailed explanation!! My chemistry teacher explained something with 0.35 x the electrons?? I didn't understand that. If you would explain that would be great.

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[@CrashChemistryAcademy]

Thanks! You're very welcome.

[@piyushaspiretoachieve3179]

I would like to interrupt you that you have not mentioned the exception of noble gases and trend of noble gases shown in your video. Is wrong.I came here to know the exception of 3de- … if you have made video on this how these electron change the trend then please share thank you!!

[@CrashChemistryAcademy]

You may be thinking of covalent radius. I have presented the trend in atomic radius which is slightly different. The covalent radius has noble gases larger than their halogen neighbors, which disrupts the trend. However I have used atomic radius, not covalent radius, which keeps the period trend in size all the way to noble gases.

[@piyushaspiretoachieve3179]

@@CrashChemistryAcademy but bro atomic radius types are only covalent , metallic , ionic radius… etc then I didn’t understand how you depicted the atomic radius and for noble gases at its basic level only it’s van der wal radius can be measured ….. if am I not right at any point you can point out me

[@CrashChemistryAcademy]

@@piyushaspiretoachieve3179 Van der Waals is what I used (sorry I was not more specific) and while more accurate for noble gases, the Van der Waals radius for other atoms can be reliably reported via theoretical calculations.

[@piyushaspiretoachieve3179]

@@CrashChemistryAcademy yes thanks 👍

[@Ravenwest19]

why the electrons do not fall into the nucleus?

[@cantthinkofausername5642]

Bcoz the core electrons show repulsive force to the Valence electrons

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[@CrashChemistryAcademy]

It will be interesting to see how things play out with using online resources. As a teacher myself I see these kinds of videos as review or supplementary material, not as primary teaching material, because the interpersonal experience is essential and enhances teaching & learning. Anyway, you are welcome, thanks for the comment!

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