Unformatted text preview: because of full orbitals because of full s orbitals in the former case and all ½ full p orbitals in the latter. Generally a group closer to fluorine will have, on the whole, a higher electronegativity than the group to the left of it. Also (but less a factor in magnitude) an element in one of the upper periods but in the same group will have a higher electronegativity. Generally covalent atomic radius decreases as you go up in period and as you get closer to the right, for these reasons: elements have fewer energy levels as you go up and as you go left there are more protons to pull in the electrons. Generally ionic radius depends on charge. The more positive a charge is the smaller the ionic radius, because there are more protons than electrons and the remaining electrons are pulled closer (Z eff is larger) to the nucleus....
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- Winter '08
- Ionization Energy, Metals Prelaboratory Questions, covalent radius increases, Ionization potential increases