anonymous
  • anonymous
Two atoms have the electron configurations 1s2 2s2 sp6 and 1s2 2s2 2p6 3s1. The first ionization energy of one is 2080 kJ/mol and that of the other is 496 kJ/mol Match each ionization energy with one of the given electron configurations. Justify your choice. The answer is 1s2 2s2 2p6: 2080 k/mol I can't figure out how to get this answer. Please help!! :(
Chemistry
  • Stacey Warren - Expert brainly.com
Hey! We 've verified this expert answer for you, click below to unlock the details :)
SOLVED
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
chestercat
  • chestercat
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
anonymous
  • anonymous
look p has 3 orbitals which can accomodate a max of 6 electrons . Hence when you have a fully filled outer shell (here 2p6) the molecule tends to become much more stable and it is difficult to remove electrons from a stable configuration... so a higher energy has to be given to the system to remove the electron, hence its higher I.E. value. the other one having half-filled configuration, needs less energy to remove an electron from the outer most shell, hence a comparatively lower I.E.

Looking for something else?

Not the answer you are looking for? Search for more explanations.