Question

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form. a. 53 b. 38 c. 55 d. 88 e. 9 f. 13

Short answer

a. \(I^{-}\) b. \(Sr^{2+}\) c. \(Cs^{+}\) d. \(Ra^{2+}\) e. \(F^{-}\) f. \(Al^{3+}\)

Step-by-step solution

Find the elements corresponding to the given atomic numbers

Use a periodic table to identify the elements with the given atomic numbers: a. 53 - Iodine (I) b. 38 - Strontium (Sr) c. 55 - Cesium (Cs) d. 88 - Radium (Ra) e. 9 - Fluorine (F) f. 13 - Aluminum (Al)

Determine the common oxidation states

Common oxidation states for elements depend on their group in the periodic table: a. Iodine (I) - Group 17, Halogens: Oxidation state of -1 b. Strontium (Sr) - Group 2, Alkaline Earth Metals: Oxidation state of +2 c. Cesium (Cs) - Group 1, Alkali Metals: Oxidation state of +1 d. Radium (Ra) - Group 2, Alkaline Earth Metals: Oxidation state of +2 e. Fluorine (F) - Group 17, Halogens: Oxidation state of -1 f. Aluminum (Al) - Group 13: Oxidation state of +3

Write the formula and charge for each ion

Based on the common oxidation states found in Step 2, write the formula and charge for each ion: a. Iodine (I) - \(I^{-}\) b. Strontium (Sr) - \(Sr^{2+}\) c. Cesium (Cs) - \(Cs^{+}\) d. Radium (Ra) - \(Ra^{2+}\) e. Fluorine (F) - \(F^{-}\) f. Aluminum (Al) - \(Al^{3+}\)