ionization energy - measures amount of energy needed to lose an electron
- more difficult to remove electrons w/ greater ionization energy
- more energy needed to remove each subsequent electron
- sharp increase in ionization energy needed to remove inner shell electrons
- inner shell electrons much closer to nucleus
- I1 generally increases w/ atomic number on each row
- I1 decreases as atomic number increases down a group
- representative elements have larger range of I1 than transition elements
- smaller atoms tend to have higher ionization energies (electrons closer to nucleus)
ion electron configurations - electrons removed from largest available quantum number first
- electrons added to lowest available quantum number first
electron affinity - energy change when electron is added to a gaseous atom
- measures attraction of atom for added electron
- usually negative (energy usually released when electron is added), but can be positive for noble gases (anion higher in energy than separated atom/electron)
- halogens have the most negative electron affinities
- noble gases have positive electron affinities (when adding an electron would place it on a new energy subshell)
- group 5A (w/ 1/2 filled subshells) have electron affinities either positive or less negative than group 4A
- doesn't change much going up/down a group
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