What is the Lewis symbol for each of the following atoms or ions? (c) Sn²⁺

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Step 1: 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.

Step 2: Determine the number of valence electrons for a neutral tin (Sn) atom. Tin is in group 14 of the periodic table, so it has 4 valence electrons.

Step 3: Consider the charge of the ion. Sn²⁺ indicates that the tin ion has lost 2 electrons.

Step 4: Subtract the 2 lost electrons from the 4 valence electrons of the neutral tin atom. This results in 2 remaining valence electrons for Sn²⁺.

Step 5: Draw the Lewis symbol for Sn²⁺ by placing 2 dots around the symbol 'Sn' to represent the 2 remaining valence electrons.

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Key Concepts

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

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. The number of valence electrons influences an atom's reactivity and the types of bonds it can form. For tin (Sn), which is in group 14 of the periodic table, it has four valence electrons, but the ion Sn²⁺ has lost two of these electrons.

Ionic Charge

The ionic charge of an atom or ion indicates the number of electrons lost or gained compared to its neutral state. In the case of Sn²⁺, the positive charge signifies that the tin atom has lost two electrons, resulting in a total of two valence electrons remaining. This change in electron count is crucial for determining the Lewis symbol, as it directly affects the number of dots shown.

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Textbook Question

(c) Ti and Hf behave as though they possess the same number of valence electrons. Which of the subshells in the electron configuration of Hf behave as valence orbitals? Which behave as core orbitals?

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