What noble gas has the same election configuration as each of the ions in the following compounds? a. cesium sulfide \(\quad\) c. calcium nitride b. strontium fluoride \(\quad\) d. aluminum bromide

For each compound, identify the elements present, determine the corresponding ions and their charges. Remember that elements tend to gain or lose electrons to achieve a stable electron configuration like a noble gas. a. Cesium sulfide Cesium (Cs) has a +1 charge as it loses one electron, and Sulfide (S) has a -2 charge since it gains two electrons. The ions are Cs⁺ and S²⁻. b. Strontium fluoride Strontium (Sr) has a +2 charge when it loses two electrons, and Fluoride (F) has a -1 charge after gaining one electron. The ions are Sr²⁺ and F⁻. c. Calcium nitride Calcium (Ca) has a +2 charge after losing two electrons, and Nitride (N) has a -3 charge when it gains three electrons. The ions are Ca²⁺ and N³⁻. d. Aluminum bromide Aluminum (Al) has a +3 charge after it loses three electrons, and Bromide (Br) has a -1 charge when it gains one electron. The ions are Al³⁺ and Br⁻.

Using the ions' charges, find the electron configuration of each ion, as they gain or lose electrons to achieve a noble gas configuration. For example, Cs⁺ loses one electron from its outer shell. So, we need to find the electron configuration of Cs without its outermost electron to find the configuration of Cs⁺. Perform this process for all ions present in each compound.

Compare the electron configurations of the ions obtained in Step 2 to the electron configurations of noble gases, and identify the noble gas with the same electron configuration. a. Cesium sulfide: Cs⁺ has a similar electron configuration to Xenon (Xe). S²⁻ also has a similar electron configuration to Argon (Ar). b. Strontium fluoride: Sr²⁺ has a similar electron configuration to Krypton (Kr). F⁻ has a similar electron configuration to Neon (Ne). c. Calcium nitride: Ca²⁺ has a similar electron configuration to Argon (Ar). N³⁻ has a similar electron configuration to Neon (Ne). d. Aluminum bromide: Al³⁺ has a similar electron configuration to Neon (Ne). Br⁻ has a similar electron configuration to Argon (Ar). The electron configurations of ions are similar to noble gases as they have full outer electron shells, making them stable.