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

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Identify the group number of each element in the periodic table.

Determine the number of valence electrons for each element based on its group number.

Predict whether the element will lose or gain electrons to achieve a stable electron configuration, typically a full outer shell.

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.

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.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ion Formation

Ion formation occurs when atoms gain or lose electrons to achieve a stable electron configuration, typically resembling that of the nearest noble gas. Elements tend to form ions to reach a full outer shell, which is often achieved by losing or gaining a specific number of electrons.

Electronegativity and Ion Charges

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Elements with high electronegativity, like oxygen, tend to gain electrons and form negative ions (anions), while those with low electronegativity, like potassium and rubidium, tend to lose electrons and form positive ions (cations).

Group Trends in the Periodic Table

The periodic table is organized into groups (columns) that share similar chemical properties. Elements in Group 1 (alkali metals) typically form +1 ions, while those in Group 2 (alkaline earth metals) form +2 ions. Nonmetals, such as oxygen in Group 16, usually form anions with a charge of -2.

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