Predict the charge of the ion formed by each element. a. Sr

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Identify the group number of the element in the periodic table. Strontium (Sr) is in Group 2.

Recall that elements in Group 2 are alkaline earth metals, which typically form ions with a +2 charge.

Understand that this is because Group 2 elements have two valence electrons, which they tend to lose to achieve a stable electron configuration similar to the nearest noble gas.

Write the electron configuration of Sr: [Kr] 5s². By losing two electrons, it achieves the electron configuration of krypton (Kr), a noble gas.

Conclude that the ion formed by strontium (Sr) is Sr²⁺, indicating it has lost two electrons and has a +2 charge.

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Ion Formation

Ion formation occurs when atoms gain or lose electrons to achieve a stable electron configuration, often resembling that of the nearest noble gas. Metals typically lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions.

Group Trends in the Periodic Table

Elements in the same group of the periodic table exhibit similar chemical properties, including their tendency to form ions. For example, alkaline earth metals like strontium (Sr), which is in Group 2, typically lose two electrons to form a +2 charge when they ionize.

Charge of Common Ions

The charge of common ions can often be predicted based on the element's position in the periodic table. Strontium, being an alkaline earth metal, commonly forms a Sr²⁺ ion by losing two electrons, resulting in a +2 charge, which is characteristic of this group.