Using the periodic table, predict the charge of the most stable ion of the following elements: d. Br

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Identify the group number of bromine (Br) in the periodic table. Bromine is in Group 17, also known as the halogens.

Understand that elements in Group 17 typically gain one electron to achieve a full outer shell, similar to the nearest noble gas configuration.

Recognize that gaining one electron results in a negative charge. Therefore, the most stable ion of bromine will have a charge of -1.

Write the electron configuration of bromine: [Ar] 3d^{10} 4s^{2} 4p^{5}.

By gaining one electron, bromine achieves the electron configuration of krypton: [Ar] 3d^{10} 4s^{2} 4p^{6}, resulting in a Br^- ion.

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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 bromine (Br) are in Group 17 and typically gain one electron to achieve a stable electron configuration, resulting in a charge of -1.

Ion Formation and Stability

Ions are charged particles formed when atoms gain or lose electrons. The stability of an ion is often related to achieving a noble gas electron configuration, which is energetically favorable. For bromine, gaining one electron to form Br- allows it to mimic the electron configuration of the nearest noble gas, krypton, thus making it a stable ion.

Electronegativity and Electron Affinity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons, while electron affinity refers to the energy change when an electron is added to a neutral atom. Bromine has high electronegativity and a significant electron affinity, indicating a strong tendency to gain an electron and form a stable anion (Br-), which is crucial for predicting its charge.