Predict the charge of the ion formed by each element. a. Mg b. N d. Na

Verified step by step guidance

1. Step 1: Identify the position of the element in the periodic table. Magnesium (Mg) is in the second group (alkaline earth metals) of the periodic table.
2. Step 2: Determine the number of valence electrons. Elements in the second group have two valence electrons.
3. Step 3: Remember that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration, usually that of the nearest noble gas. For Magnesium, the nearest noble gas is Neon (Ne).
4. Step 4: Determine the easiest way for the atom to achieve a stable electron configuration. In the case of Magnesium, it's easier to lose two electrons than to gain six.
5. Step 5: The charge of the ion is determined by the number of electrons gained or lost. Since Magnesium loses two electrons, it forms a +2 ion.

Key Concepts

Ion Formation

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

Magnesium's Position in the Periodic Table

Magnesium (Mg) is located in Group 2 of the periodic table, which consists of alkaline earth metals. These elements have two valence electrons, and they tend to lose these electrons during chemical reactions, resulting in a +2 charge for the ion formed.

Charge of Ions

The charge of an ion is determined by the difference between the number of protons and electrons. For magnesium, losing two electrons results in a net positive charge of +2, leading to the formation of the Mg²⁺ ion, which is common in various compounds.