how do i find what the element is when i've been given ionisation energys Watch

Ray_Shadows
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first IE= 577
second IE=1820
third IE=2740
fourth IE=11600

how do i find out what element it is
thanks
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CheeseIsVeg
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(Original post by Ray_Shadows)
first IE= 577
second IE=1820
third IE=2740
fourth IE=11600

how do i find out what element it is
thanks
Look for jumps between successive ionisation energies which are exceptionally large
this gives you an idea for their electron configuration ie: higher ionisation energies mean more energy is required for this electron to be removed which could be due to going down a shell etc.

Therefore if you take a look at your IE's there, you should be able to work out some info

Hope this helps
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Ray_Shadows
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(Original post by CheeseIsVeg)
Look for jumps between successive ionisation energies which are exceptionally large
this gives you an idea for their electron configuration ie: higher ionisation energies mean more energy is required for this electron to be removed which could be due to going down a shell etc.

Therefore if you take a look at your IE's there, you should be able to work out some info

Hope this helps
i still don't understand
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CheeseIsVeg
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(Original post by Ray_Shadows)
i still don't understand
ok, read this and then let me know if there is anything specific troubling you!
http://www.chemguide.co.uk/atoms/pro...s/moreies.html
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alyttelton
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(Original post by Ray_Shadows)
i still don't understand
The jumps being referred to are the differences between each of the ionisation energies.

From 1st to 2nd there's an increase of 1243.
From 2nd to 3rd it is 920.
From 3rd to 4th it is 8860.

The biggest increase is from 3rd to 4th, much larger than the others. You would have learnt from class that the lowest the energy level (the closest the shell is to the nucleus), the more energy is required to remove the electron. If the 4th electron requires a LOT more energy, then it is in another shell. This means that there are 3 electrons in the outermost shell of that atom, hence it is in group 3.
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Ray_Shadows
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(Original post by c.lorenzoni)
The jumps being referred to are the differences between each of the ionisation energies.

From 1st to 2nd there's an increase of 1243.
From 2nd to 3rd it is 920.
From 3rd to 4th it is 8860.

The biggest increase is from 3rd to 4th, much larger than the others. You would have learnt from class that the lowest the energy level (the closest the shell is to the nucleus), the more energy is required to remove the electron. If the 4th electron requires a LOT more energy, then it is in another shell. This means that there are 3 electrons in the outermost shell of that atom, hence it is in group 3.
yeh that's true , i figured out it was i period three , but how do i pinpoint the highest IE level to one specific element
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Ray_Shadows
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(Original post by c.lorenzoni)
The jumps being referred to are the differences between each of the ionisation energies.

From 1st to 2nd there's an increase of 1243.
From 2nd to 3rd it is 920.
From 3rd to 4th it is 8860.

The biggest increase is from 3rd to 4th, much larger than the others. You would have learnt from class that the lowest the energy level (the closest the shell is to the nucleus), the more energy is required to remove the electron. If the 4th electron requires a LOT more energy, then it is in another shell. This means that there are 3 electrons in the outermost shell of that atom, hence it is in group 3.

(Original post by CheeseIsVeg)
ok, read this and then let me know if there is anything specific troubling you!
http://www.chemguide.co.uk/atoms/pro...s/moreies.html


thanks guys i got it eventually
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