From which of the following atoms is it easiest to remove an electron?

Question

a. Mg b. Na c. K d. Be e. Li

The answer is K. But why? Which trend does this have to do with? Please help i have a test tomorrow!

Thanks!

Answer 1

Ionization energy is the amount of energy an atom needs to lose an electron. The general pattern in which it increases is up a column and to the right of a row. so the highest IE would be He or F. the Lowest would be Fr meaning its easiest to take an electron away from it (low energy needed to remove electron)

therefore since K, Na, and Li both have a unpaired s electron orbital its easiest to remove from these elements. Be and Mg have paired electrons in the s orbital making them not want to break up this pair.

Out of K, Na and Li. Even though K has the highest positive charge on it, it also has more electrons that tend to "shield" the outer electrons from being pulled in by the positive charge on the nucleus. The more electrons you have the more shielding you will get. So as you go down a column the shielding will increase and the ionization energy will decrease.

i hope that remotely makes sense. when in doubt think of hte patterns. IE = increase up and right
electron affinity (gain electron) = increase up and right

there are exceptions though remember that.

Answer 2

I'll give it a try. It has to do with the electron configuration of the atom. For instance, Mg is a 1s(^2)2s(^2)2p(^6)3s(^2), because it has a complete outer orbit (3s) it is essentially happy and doesn't want to take or give up any electrons. K on the other hand has only one electron in it's outermost shell (4s) and would gladdly give up an electron to have a complete outer orbit. Li is in the same position as K (one electron short in the outer orbit) but because it is the 2s orbit, and closer to the nucleus, it has more attraction, and is harder to remove. That is extremely over simplified. I would suggest reading your Chemistry book over the section of electron configurations.

Answer 3

Radium is a plenty extra beneficial atom. the interior electrons look after the outer ones from the nucleus, so there is far less effectual nuclear cost attracting the outer electrons inwards. this means that much less power is mandatory to do away with an outer electron.

Answer 4

I answered your other question about which atoms are most likely to lose an electron. The other responders did not give very accurate information.

But on this question, both of the first two responses are right on target. You should listen to these people.

Good luck on the test!

Answer 5

Seams like you know that the periodic table farther left easier to remove electron, it also goes farther down it is easier.

Hence K is easier than Na. (If you know about electronegativity that will tell you also)

As for grabbing an electron, top right of periodic table will grab the most (except the inert nobel gasses do not count)

Answer 6

hey i'll give you a simpler answer.

potassium (K) is higher up than the other 3 elements in the reactivity series. which also goes to mean that its ionisation power is greater and hence it is more reactive and is easiest to remove an electron.

good luck for your test! :)

Answer 7

Fr ,Xe ,F,H,S