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Any chemistry experts/fellow student available to help damsel in distress?

Mrs.Z Avatar
7y, 3m agoPosted 7 years, 3 months ago
To do with ionisation energy and periodicity

Thank you!!!
Mrs.Z Avatar
7y, 3m agoPosted 7 years, 3 months ago
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#1
Sure thing! Hit me with it! I'll try my best! :thumbsup:
#2
hdizzle
Sure thing! Hit me with it! I'll try my best! :thumbsup:


Found it now, you want it still?
#3
Mrs.Z
Found it now, you want it still?


Oh I thought you needed help, I thought I may be able to, did my Chem A-level last year
#4
hdizzle
Oh I thought you needed help, I thought I may be able to, did my Chem A-level last year


I did when I posted OP, but carried on searching :-D

http://www.iun.edu/~cpanhd/C101webnotes/modern-atomic-theory/images/ionization-energy.jpg
Needed to explain the slight drops in ionisation energy between 'Be' and 'B' - and 'Mg' and 'Al' :thumbsup:
#5
Ahh coolio. Well i'm glad you found it! Just a tip...if you have any chemistry issues you should try this site:

http://www.chemguide.co.uk/

It's so so useful, it got me through A-level Chem!

So I'm guessing your doing Module one? Good luck !
#6
hdizzle
Ahh coolio. Well i'm glad you found it! Just a tip...if you have any chemistry issues you should try this site:

http://www.chemguide.co.uk/

It's so so useful, it got me through A-level Chem!

So I'm guessing your doing Module one? Good luck !


Ooh, thank you!
I am actually doing BTEC Applied Science as I unfortunately couldn't work the A-Level timetable around the kids school times :oops:
Maybe you can help me after all :-D
I can explain the decrease in energy between groups 2&3 but not the slight decrease between groups 5&6 :thinking:
#7
For Mg I have 1S2 2S2 2P6 3S2
For Al I have 1S2 2S2 2P6 3S2 3P1
so that explains the lower ionization energy for Al

but with groups 5 & 6 I have for example

P (phosphorous) - 1S2 2S2 2P6 3S2 3P3
S (Sulphur) - 1S2 2S2 2P6 3S2 3P4

:?

Maybe I should go to bed :giggle:

Ah, sorry got it - it's because of the pairs :oops:
#8
ok i know this, let me just get some images on here so i can explain it
#9
hdizzle
ok i know this, let me just get some images on here so i can explain it


I have got it, trying to put it down in words without makung a separate essay, so images would be great :-D
1 Like #10
Ok, phosphorous has 3 electrons in 3p, which are all unpaired (singly occupied orbitals), whereas Sulphur has 4 electrons making one of them orbitals paired:
http://image.tutorvista.com/content/atomic-structure/electronic-configuration-sodium-aluminium-phosphorous-sulphur.gif

There is some repulsion with the paired electrons in sulphur, which lessens their attraction to the nucleus. Therefore its easier to remove one of these paired electrons from sulphur than an unpaired 3p electron from phosphorus. Hence the decrease in energy.

Hope that helps :thumbsup:
#11
hdizzle
Ok, phosphorous has 3 electrons in 3p, which are all unpaired (singly occupied orbitals), whereas Sulphur has 4 electrons making one of them orbitals paired:
http://image.tutorvista.com/content/atomic-structure/electronic-configuration-sodium-aluminium-phosphorous-sulphur.gif

There is some repulsion with the paired electrons in sulphur, which lessens their attraction to the nucleus. Therefore its easier to remove one of these paired electrons from sulphur than an unpaired 3p electron from phosphorus. Hence the decrease in energy.

Hope that helps :thumbsup:


Wow, it sure does, I was contemplating drawing that box myself on the computer so you just saved me about 3 hours work :giggle:
#12
Mrs.Z
Wow, it sure does, I was contemplating drawing that box myself on the computer so you just saved me about 3 hours work :giggle:


coolio, hope my explanation was clear, its been a long time since i did this stuff!

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