The decrease at sulfur: In this case something other than the transition from a 3s orbital to a 3p orbital must offset the effect of an extra proton. Both of these factors offset the effect of the extra proton. The 3p electron is slightly farther from the nucleus than the 3s electron, and partially screened by the 3s electrons as well as the inner electrons. However, this effect is offset by the fact that the outer electron of aluminum occupies a 3p orbital rather than a 3s orbital. The decrease at aluminum: The value for aluminum might be expected to be greater than that of magnesium due to the extra proton. The increasing nuclear charge also pulls the outer electrons toward the nucleus, further increasing ionization energies across the period. This creates greater attraction between the nucleus and the electrons and thus increases the ionization energies. The determining factor in the increase in energy is the increasing number of protons in the nucleus from sodium across to argon. These electrons are at approximately the same distance from the nucleus, and are screened by corresponding electrons in orbitals with principal atomic numbers n=1 and n=2. The upward trend: In the whole of period 3, the outer electrons are in 3-level orbitals. whether the electron is alone in an orbital or one of a pair.the amount of screening by inner electrons.the distance of the outer electron from the nucleus.It covers ionization energy, atomic radius, electronegativity, electrical conductivity, melting point and boiling point.įirst ionization energy is dependent on four factors: This page describes and explains the trends in atomic and physical properties of the Period 3 elements from sodium to argon. The pattern of first ionization energies across Period 3.
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