Predict the charge of the ion formed by each element. a. O b. K c. Al d. Rb

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1. Identify the group number of each element in the periodic table.
2. Determine the number of valence electrons for each element based on its group number.
3. Predict whether the element will lose or gain electrons to achieve a stable electron configuration, typically a full outer shell.
4. For elements that lose electrons, the charge of the ion is positive and equal to the number of electrons lost. For elements that gain electrons, the charge is negative and equal to the number of electrons gained.
5. Apply this logic to each element: a. Oxygen (O) is in Group 16, b. Potassium (K) is in Group 1, c. Aluminum (Al) is in Group 13, d. Rubidium (Rb) is in Group 1.