which will have a higher ionization energy

[IWantH2O]

1)K+ or Ne
2)Kr or F

and why

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[futuredent22]

1. Ne
2. F

For the first, K+ is basically just Ar. Ne has a larger ionization energy than Ar because it is smaller.

For second, -Kr is really just Rb. F has a much, much greater ionization energy than Rb.

 

[IWantH2O]

1. Ne
2. F

For the first, K+ is basically just Ar. Ne has a larger ionization energy than Ar because it is smaller.

For second, -Kr is really just Rb. F has a much, much greater ionization energy than Rb.

ya but for K+, theres more protons then electrons, doesnt that mean that there will be that much stonger force holding the electrons?

and sorry the second one is a neutral Kr

 

[Albuterol]

http://en.wikipedia.org/wiki/Ionization_energies_of_the_elements

also knowing the period trend of ionization energy will help u answer this question.

i think the answers are K+ and F
K+ because it has already lost an electron and established the noble gas state. In order to lose another electron it will require even MORE energy than it did to lose its 1st electron (basically u are looking at the 2nd ionization energy for K+).

F because its F... high ionization energy than Kr according to the periodic trend.

just curious, where did u get these questions from?

 

[flycd05]

1 - K+ b/c cations take more ionization energy to remove an e- b/c theres a more positive charge so e- are held in more closely to the nucleus

2 - F b/c the trend increases up and to the right

 

[excusezmoi]

This is a random website but it shows a good ionization graph

http://www.iun.edu/~cpanhd/C101webnotes/modern-atomic-theory/ionization-energy.html

I'd say remember that Noble gases has the highest first ionization energy...when you know this basic concept then this will help you through the rest

 

[IWantH2O]

http://en.wikipedia.org/wiki/Ionization_energies_of_the_elements

also knowing the period trend of ionization energy will help u answer this question.

i think the answers are K+ and F
K+ because it has already lost an electron and established the noble gas state. In order to lose another electron it will require even MORE energy than it did to lose its 1st electron (basically u are looking at the 2nd ionization energy for K+).

F because its F... high ionization energy than Kr according to the periodic trend.

just curious, where did u get these questions from?

lol I made them up to better understand the concept

 

[futuredent22]

I still think Ne has a higher ionization energy than K+. K+ is basically the same thing as Ar. Both have 18 electrons, and while K+ will be slightly smaller because of its extra proton as compared to Ar, this doesn't make up for the fact that Ar is much bigger than Ne. Ne is smaller so has its electrons much closer, thus a higher ionization energy.

 

[Albuterol]

yes but K+ now needs to overcome the 2nd ionization energy which is MUCH greater than the 1st ionization energy of Ar and will be greater than the 1st ionization energy of Ne.

 

[futuredent22]

yes but K+ now needs to overcome the 2nd ionization energy which is MUCH greater than the 1st ionization energy of Ar and will be greater than the 1st ionization energy of Ne.

I agree that K's 2nd ionization energy is much higher than its first, but that doesn't mean its greater than Ne's 1st. Would you argue that Cs's 2nd ionization energy is greater than Ne's? No, because it is so much bigger that its electrons are much easier to take off than Ne.

 

[Albuterol]

i understand what you are saying about the atomic size of Ne being very small drawing the electrons tightly. i thought of it this way...since Ar is right below Ne their difference in ionization cannot be that much and we know K+ has much greater 2nd ionization energy than Ar so it probably has a much greater ionization energy than Ne. If you take a look at the wiki table of ionization energies K+> Ne.

 

[futuredent22]

i understand what you are saying about the atomic size of Ne being very small drawing the electrons tightly. i thought of it this way...since Ar is right below Ne their difference in ionization cannot be that much and we know K+ has much greater 2nd ionization energy than Ar so it probably has a much greater ionization energy than Ne. If you take a look at the wiki table of ionization energies K+> Ne.

Yeah I just looked at the table, you are indeed correct. Its weird to me though that K+ has double the ionization energy of Ar when both have the same electron configuration. I guess that extra proton really does make that much of a difference. In fact, looking at the table, even Cs+ has a higher ionization energy than Ne, even though its much larger.

Thanks for sticking to what you knew to be the correct answer and for being patient with my stubbornness haha. Now I hope this type of question will come on the test so I'll be able to get it right.

 

[Albuterol]

its all good man, atleast now u will never get an ionization question wrong!
good luck w/the studying