People also ask


  • What is the trend in ionization energy from left to right?

  • Ionization energies are dependent upon the atomic radius. Since going from right to left on the periodic table, the atomic radius increases, and the ionization energy increases from left to right in the periods and up the groups. Exceptions to this trend is observed for alkaline earth metals (group 2) and nitrogen group elements (group 15).

  • How does the ionization energy change with the atomic radius?

  • The ionization energy increases as each electron is removed. Ionization energies are dependent upon the atomic radius. Since going from right to left on the periodic table, the atomic radius increases, and the ionization energy increases from left to right in the periods and up the groups.

  • Why do elements down the periodic table have a lower ionization energy?

  • The chemical elements down the periodic table have a much lower ionization energy (due to electrons being farther away from the atom with increasing atomic radius). The ionization energy increases as each electron is removed. Ionization energies are dependent upon the atomic radius.

  • Why is the first ionization energy lower on the outermost electrons?

  • Since the outermost electrons are further away, they are less strongly attracted by the nucleus, and are easier to remove, corresponding to a lower value for the first ionization energy. From left to right across a period, more protons are being added to the nucleus, but the number of electrons in the inner, lower-energy shells remains the same.

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