What is the Lewis symbol for each of the following atoms or ions: c. Sn²⁺

Verified step by step guidance

1. <strong>Step 1:</strong> Understand the concept of a Lewis symbol. A Lewis symbol represents the valence electrons of an atom or ion using dots around the element's symbol.
2. <strong>Step 2:</strong> Identify the element and its position in the periodic table. Tin (Sn) is in Group 14, which means it has 4 valence electrons in its neutral state.
3. <strong>Step 3:</strong> Consider the charge of the ion. Sn²⁺ indicates that the tin atom has lost 2 electrons.
4. <strong>Step 4:</strong> Calculate the remaining valence electrons. Since Sn has lost 2 electrons, it now has 2 valence electrons left.
5. <strong>Step 5:</strong> Draw the Lewis symbol for Sn²⁺. Place the element symbol 'Sn' and arrange 2 dots around it to represent the remaining valence electrons.

Key Concepts

Lewis Symbols

Lewis symbols, also known as Lewis dot structures, represent the valence electrons of an atom or ion. Each dot corresponds to a valence electron, and the arrangement of these dots around the chemical symbol indicates how the atom can bond with others. Understanding Lewis symbols is essential for visualizing electron sharing and transfer in chemical bonding.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom interacts with others. For main group elements, the number of valence electrons corresponds to the group number in the periodic table. In the case of Sn (tin), it has four valence electrons, but when it forms a Sn²⁺ ion, it loses two of these electrons.

Ionic Charge

Ionic charge refers to the electrical charge that an atom or ion carries due to the loss or gain of electrons. A positive charge, such as in Sn²⁺, indicates that the atom has lost electrons, resulting in a net positive charge. This concept is vital for understanding how ions form and how they are represented in Lewis symbols.