Smallest ionic radius  [ENDORSED]

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Smallest ionic radius

Postby 305174946 » Sun Oct 28, 2018 1:10 pm

If you're comparing P^-3, Cl^-, S^-2, which would have the smallest ionic radius? Would you have to compare their protons at this point?

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Re: Smallest ionic radius  [ENDORSED]

Postby 305113590 » Sun Oct 28, 2018 1:42 pm

Cl^2- because of the bigger proton count. Since they are isoelectronic (where they both achieve the noble gas configuration), you should look at which has more protons to attract the negatively charged electrons. This will, consequently, lead to a smaller radius.

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Re: Smallest ionic radius

Postby mbaker4E » Sun Oct 28, 2018 2:24 pm

Atomis radius increases down and to the left, and since they are all in the same Period you would check for which is closest the the right hand side to find the smallest.

Mhun-Jeong Isaac Lee 1B
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Re: Smallest ionic radius

Postby Mhun-Jeong Isaac Lee 1B » Sun Oct 28, 2018 11:33 pm

Just to add on to the above responses, as you go from the bottom left to the top right of the periodic table, the atomic radius generally gets smaller because there are less energy levels as you go up and more protons as you go to the right. More protons means that there is a stronger positive attraction, pulling the electrons closer to the nucleus, and thus a smaller radius.

Aili Ye 4L
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Re: Smallest ionic radius

Postby Aili Ye 4L » Mon Oct 29, 2018 10:16 am

The more positive charge for the same negative charge on isoelectronic atoms, the stronger the attraction and thus the smaller the radius.

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Re: Smallest ionic radius

Postby 105085381 » Mon Oct 29, 2018 1:15 pm

Elements increase in atomic size down the periodic table, as they gain shells, and decrease across the periodic table (from left to right)!

Sophia Ding 1B
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Re: Smallest ionic radius

Postby Sophia Ding 1B » Wed Oct 31, 2018 12:12 pm

In class it was discussed that anions are always larger than their parents ions (and cations are smaller). Phosphorus is the the largest anion now with the addition of 3 electrons to shield the attraction by the nucleus, whereas the chloride anion only has one extra election, providing not as much shielding and thus the nucleus has a greater attraction to pull them in for the smallest ionic radius out of the three. But the number of protons is also significant, contributing to the attraction of electrons to the nucleus for the factor of atomic radius as well!

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