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Periodic trends and electron characteristics
coulombic attraction
force of attraction between oppositely charged particles (protons and electrons)
coulombic potential
energy associated with coulombic attraction
atomic radius
distance from the center of the nucleus of an atom to the edge of the electron cloud
ionization energy
amount of energy required to remove the most loosely held electron from an atom — in the valence level (ionizing the atom into +1); opposite of coulombic
electron affinity
the amount of energy released when an electron is gained by a neutral atom in the gaseous state to form a (-) ion
electronegativity
ability of an atom to attract shared electrons away from another atom in a bond; how strongly an atom pulls on electrons from another atom while bonded
effective nuclear charge
number of protons - number of valence electrons; larger number means a greater core charge and stronger attraction to electrons
successive ionization
ionization energy increases for each electron removed from the electron cloud; dramatic increase for the electron following the final valence electron
group 2 → group 13 ionization trend exception
(s2) → (s2p1)
the p sublevel is higher in energy and farther from the nucleus, which is greater than the attraction from the additional proton; decreases the coulombic attraction/potential and therefore the ionization energy
group 15 → group 16 ionization trend exception
(p3 ↑ ↑ ↑) → (p4 ↑↓ ↑ ↑)
the paired electron spin level creates repulsion, which is greater than the attractive force from the additional proton; decreases the coulombic attraction/potential and therefore the ionization energy
