Predict the charge of the ion formed by each element. c. I

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Identify the group number of iodine (I) in the periodic table. Iodine is in Group 17, also known as the halogens.

Understand that elements in Group 17 typically gain one electron to achieve a full outer shell, similar to the noble gases.

Recognize that gaining one electron results in a negative charge because electrons are negatively charged.

Conclude that iodine will form an ion with a charge of -1 when it gains one electron.

Express the ion formed by iodine as \( \text{I}^- \), indicating a single negative 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. Understanding this process is crucial for predicting the charge of ions formed by different elements.

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Ion Formation

Periodic Table Trends

The periodic table displays trends in element properties, including electronegativity, ionization energy, and atomic radius. As you move across a period from left to right, elements tend to gain electrons and become more electronegative, leading to the formation of anions. Conversely, moving down a group generally results in larger atomic radii and lower ionization energies, influencing the charge of the ions formed.

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Periodic Trends

Charge of Iodine Ion

Iodine (I) is a halogen located in Group 17 of the periodic table. It typically gains one electron to achieve a stable octet configuration, resulting in the formation of an iodide ion (I⁻) with a charge of -1. This characteristic behavior of halogens is essential for predicting the charge of ions they form.

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