Using the periodic table, predict the charge of the most stable ion of the following elements: (a) Li (b) Ba (c) Po (d) I

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Identify the group number of iodine (I) in the periodic table. Iodine is in Group 17, also known as the halogens.

Recall that elements in Group 17 typically gain one electron to achieve a stable electron configuration, similar to the nearest noble gas.

Determine the electron configuration of iodine. Iodine has the electron configuration [Kr] 4d^{10} 5s^{2} 5p^{5}.

To achieve a stable electron configuration, iodine will gain one electron to fill its 5p orbital, resulting in the electron configuration [Kr] 4d^{10} 5s^{2} 5p^{6}, which is the same as xenon (Xe), a noble gas.

Conclude that by gaining one electron, iodine forms an anion with a charge of -1, denoted as I^{-}.

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Periodic Table and Group Trends

The periodic table organizes elements based on their atomic number and properties. Elements in the same group (column) exhibit similar chemical behaviors, including their tendency to gain or lose electrons. For example, halogens like iodine (I) are found in Group 17 and typically gain one electron to achieve a stable electron configuration, resulting in a charge of -1.

Ion Formation

Ions are charged particles formed when atoms gain or lose electrons. The charge of an ion reflects the difference between the number of protons and electrons. For iodine, which has seven valence electrons, it tends to gain one electron to complete its octet, forming a negatively charged ion (I⁻) that is more stable.

Stability of Ions

The stability of an ion is influenced by its electron configuration. Ions that achieve a noble gas configuration are generally more stable. For iodine, gaining an electron to form I⁻ allows it to mimic the electron configuration of xenon, a noble gas, thus enhancing its stability and making I⁻ the most stable ion for iodine.