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(in simple terms), how much "pull" a valence electron "feels" from the nucleus, trend for effective nuclear charge (groups), constant down group, because atomic # increases, but so do the # of core electrons, trend for effective nuclear charge (periods), increasing from left to right because atomic # is increasing while inner core electrons are constant, electrons are attracted to the nucleus, but outer electrons experience less attraction because the inner ("core") electrons are blocking them, half the distance between the two of the same nuclei, increases down a group because there are more electron "shells" added as you descend, decreases going left to right across a period because of increasing effective nuclear charge, the energy required to remove a valence electron from an atom, decreases down a group because of greater distance from nucleus, increases going left to right across a period because of increasing effective nuclear charge, the ability of an atom in a covalent bond to attract electrons to itself, decreases down a group because of increasing atomic size, increases left to right across period because of increasing effective nuclear charge, the size of the most common ion of an element, increases down group because more electron shells are added, decreases left to right across the period because of the increasing effective nuclear charge, when anions form, electrons are gained with the same protons, but more electrons, the radius increases (pushing each other apart), when cations form, electrons are lost; there is less repulsion and the electrons are pulled closer to the nucleus; therefore, for positive ions, radius decreases, atoms that have the same number and configuration of electrons. 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