Ionisation energy

Ionisation energies come up a lot in A Level Chemistry. This video gives you a basic introduction to the definition of ionisation energy, showing this as equations and what affects how easily an atom is ionised. All this in under 10 minutes!

[@saadpatel2734]

2 HOURS LESSON IN 8 MINUTES..AMAZING SUMMARY

[@ismaeladen2582]

What an incredible teacher. Bravo! So clear to understand!

[@AlleryChemistry]

Thanks. Pleased you found it helpful.

[@dania.adil20]

I sleep in class without worrying, as you explain it all way better than anything

[@azehnuuuuu1846]

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[@cao1x]

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[@yebany9662]

Nice summary!
Going down a group : ionisation decreases because the atomic radius increases, and the electron shielding also increases; as a result of the increased radius the nuclear charge's effect on the electrons decreases as it's more distant.
Going across a period: ionisation increaes because the atomic radius slighty decreases at every ionisation, the nuclear charge's effect on the electron is greater as there are more protons. The electron shielding remains the same when going across a period(?)

[@captainmesh]

No. Ionisation energy is the energy required to overcome the attraction between the electron being removed and the atom's protons. This depends on two factors: the number of protons (more protons in nucleus = greater attraction) and shielding (more electrons between the electron being removed and the nucleus = greater repulsion). Across a period (L to R) number of protons increases but shielding remains roughly constant, so attraction increases and so IE increases. Down a group, number of protons increases but shielding also increases AND has a greater effect, so attraction decreases and so IE decreases.

[@David-yv4li]

You Truly helped me man! I really appreciate what you've done for us students. Bless!

[@Shaun.1]

Ikr I wish I decided to check this first

[@karenm8529]

Ahh I'm so glad I found you early. These explainations are perfect so thank yoouuu!

[@pearlhotto949]

Thank you soo much❤️short and straight forward

[@AlleryChemistry]

No problem!

[@jalajarora2331]

Hi, great video but I had one question: In my spec (I do OCR A) and in my textbook it says that the definition of ionisation energy is the amount of energy required to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions. Is this not a very good definition?

[@alwahastoodent1234]

basically the same thing. But you have to remember the key words

[@sadekur]

So, shielding basically refers to the total number of the electrons present in an atom ? the higher the number the higher the shielding affect ?

[@AlleryChemistry]

Shielding is mainly concerned with the amount of shells and subshells that exist between the nucleus and the outer shell. You're right in some ways, these shells and subshells contain electrons and the more shells you have, the more shielding you get. Hope this helps.

[@captainmesh]

Shielding is simply the repulsion between inner electrons and outer electrons, because all electrons are negatively charged and like charges repel.

[@zainbhally9347]

thank you for making these videos :D

[@abneyabbdy5116]

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[@saadpatel2734]

LOve you
BEst teacher..makes it so easy

[@Yohanmiracle]

I don't like the assumption of the sodium as a gas. Please clarify

[@chambochaz3950]

would it be correct to say... As you move across a period, the nuclear charge is greater therefore the ionisation energy increases because it's harder to remove the electrons from the outer shell??

[@AlleryChemistry]

+Chambo Chaz That's correct! This would represent the general trend.

[@captainmesh]

Absolutely, and no need to mention that pesky misconception "distance from the nucleus"!

[@tondcbeasts9173]

does the atomic radius remain the same across a period??

[@AlleryChemistry]

No. Atomic radius decreases. As you go across the period the nuclear charge increases due to more Protons in nucleus. Shielding is similar so the outer electrons are pulled in towards the nucleus. Hope this helps.

[@captainmesh]

@@AlleryChemistry yes, so "distance from the nucleus" depends on the overall attraction of the electron to the nucleus, it is not a separate factor as you claim in your video. Here's a question for you: what happens to the 1s orbital radius as you go across a period and down a group?
Answer: it decreases, as does the radius of any shell, subshell or orbital. Shielding is constant but number of protons increases, so attraction to the nucleus increases and so radius decreases. "Distance from the nucleus" is a consequence of overall attraction, not a factor in its determination.

[@Imranq-cf3ie]

Thanks so much, this is great!!

[@sea5205]

Great video!

[@thatoneguy7646]

Thank You Very Much.

[@anakinskywalker3777]

finally got to see him, also thank you for the extremely helpful videos. Please make videos where you answer exam questions plzzzz thx.

[@jennyb.9237]

Thank you very much😭😍

[@zebroar4630]

Does this cover OCR A?

[@AlleryChemistry]

Yes it does

[@nancygorman2241]

Thank you so much

[@sajdahamad9980]

why does the electron configuration 1s2, 2s2 have a smaller I.E. than 1s2, 2s2, 2p6...??

[@captainmesh]

Neon has 10 protons in the nucleus whereas Beryllium only has 4. Shielding is approximately the same as both atoms' outer electrons are in second energy level (shell). Hence, there is a much greater attraction of the outer electron to the nucleus in a Ne atom than in a Be atom.

[@dannyk5166]

Which atom in the periodic table is the biggest?

[@AlleryChemistry]

+Danny K Caesium has the biggest atomic radius.

[@dannyk5166]

Thanks!

[@captainmesh]

Aah, but why not francium, eh? (A:relativity)

[@keeweeow624]

Pogu

[@marinette299]

I dont get it it isnt even that good like he doesnt mention the decrease in ionization enegy of group 3 ,6 elements...

[@hi-pg9bp]

In the next vid babe

[@JBLPB110]

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