atomic structure cont. Flashcards
(IB) psuedo stable
a full 3d sublevel
(IB) ISOELECTRONIC
same electron configuration
(IB) which is removed first: 4s or 3d?
4s
(IB) ATOMIC RADIUS
measured as the 1/2 distance between nuclei of 2 adjacent atoms
(IB) why does atomic radius inc. as you go down a group
as “n” inc., more energy levels of a electron shield (repel) the valence electron
(IB) why does atomic radius dec. as you go across a period
protons inc. and number of electrons inc. but are more attracted to the nucleus
(IB) IONIZATION ENERGY (IE)
amount of energy required to completely remove one mole of electron from one mole of gaseous atoms (or ions)
(IB) IE down a group, why?
dec., more energy levels shield the valence electron, meaning less attraction required to overcome
(IB) IE across a period, why?
inc., stronger attraction to the nucleus, more energy required to overcome
(IB) SUCCESSIVE IE, trend, why?
IE inc., more energy required as each electron is closer to the nucleus
(IB) ELECTRON AFFINITY (EA)
energy released when 1 mole of electron is added to 1 mole of gaseous atom
(IB) EA down a group, why?
dec. (less energy released), more energy levels, more shielding, less attraction to overcome
(IB) EA across a period, why?
inc. (more energy released), incoming electron experiences less shielding and more attraction.
(IB) REACTIVE METALS IE
dec.
not much energy required to move
(IB) REACTIVE METALS EA
dec.
not much energy being released
(IB) what are reactive metals good at?
losing electrons
doesn’t require much E to lose and not getting much energy back
(IB) REACTIVE NON-METALS IE
inc.
require a lot of energy to lose
(IB) REACTIVE NON-METALS EA
inc.
releases a lot of energy to gain
(IB) what are reactive non-metals good at?
gaining electrons
(IB) NOBLE GASES IE AND EA
IE: too high
EA: too low
good at keeping electrons
