This is because, with 7 valence electrons, halogens want to gain one more electron to form an octet. On the opposite end of the spectrum, group 17 elements have very high ionization energies. It takes very little energy to remove an electron because the atom can be more stable without it. Thus, group 1 elements have very low ionization energies. It is very easy to remove an electron from an atom that is very far from an octet.Ī group 1 element that has one valence electron will readily lose its electron in order to have an octet of electrons. So, removing an electron becomes harder and harder, and the ionization energy increases, as atoms approach an octet. As elements have successively more electrons across a period, atoms get closer and closer to their goal. As mentioned before, elements strive to have complete octets of valence electrons. Period TrendĪcross a period, ionization energies increase. Let’s see this relationship directly with the ionization energy period trend. How does the octet rule relate to the trend of ionization energies on the periodic table? Since atoms strive to have an octet, each atom’s ionization energy differs based on how many electrons they have. Noble gas atoms do not react with other elements because they are already extremely stable, due to the octet of electrons they have. Group 18 noble gases have an octet of electrons, which causes them to be chemically inert and nonreactive. This is because this configuration provides the most stability for the atom. The Octet RuleĪccording to the octet rule, atoms strive to have a complete set of 8 valence electrons. Before we break down the trend into its period and group trends, let’s talk about a major contributing factor to this trend: the octet rule. In general, (first) ionization energies increase toward the top right corner of the periodic table, with helium having the highest ionization energy. Ionization Energy Trend on the Periodic Tableįor the ionization energy trend on the periodic table, we will assume that we are always referring to elements’ first ionization energy.
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