Problem 14 - Chemistry The Central Science

Question

What is the Lewis symbol for each of the following atoms or ions? (a) \(\mathrm{K},\) (b) As, (c) \(\mathrm{Sn}^{2+},(\mathbf{d}) \mathrm{N}^{3-}\) .

Step-by-Step Solution

Answer

The Lewis symbols for the given atoms and ions are: (a) \(\text{K}\bullet\) , (b) \[\begin{array}{c}\cdot \text{As} \cdot \\ | \end{array}\], (c) \(\bullet \text{Sn}^{2+} \bullet\), and (d) \[\begin{array}{c}\cdot \text{N}^{3-} \cdot \\ | \end{array}\].

Step 1: Determine valence electrons for each atom/ion

(a) Potassium (K) - As it belongs to the first group in the periodic table, it has only 1 valence electron. (b) Arsenic (As) - Being a member of Group 15 in the periodic table, it has 5 valence electrons. (c) Tin(II) ion (Sn²⁺) - Tin, as a Group 14 element, has 4 valence electrons. However, due to the 2+ charge, which means it loses 2 electrons, that leaves it with 2 valence electrons. (d) Nitride ion (N³⁻) - Nitrogen, as a Group 15 element, has 5 valence electrons. Since the ion has a 3- charge, it gains 3 electrons, thus giving it a total of 8 valence electrons.

Step 2: Represent elements and ions with their symbols and valence electrons

(a) Potassium (K) - \[\text{K}\bullet\] (b) Arsenic (As) - \[\begin{array}{c}\cdot \text{As} \cdot \\ | \end{array}\] (c) Tin(II) ion (Sn²⁺) - \[\bullet \text{Sn}^{2+} \bullet\] (d) Nitride ion (N³⁻) - \[\begin{array}{c}\cdot \text{N}^{3-} \cdot \\ | \end{array}\] The Lewis symbols for the given atoms and ions are: (a) K• , (b) ∙As∙| , (c) •Sn²⁺• , and (d) ∙N³⁻∙| .

Key Concepts

Valence Electrons

Valence electrons are the outermost electrons in an atom, which are crucial in determining how atoms interact with one another. These electrons play a significant role in chemical bonds, as they are the ones involved in gaining, losing, or sharing to form compounds.

• Valence electrons dictate how an element behaves chemically.
• They are located in the atom's highest energy level or shell.
• The number of valence electrons in an atom is often represented in Lewis symbols.

For example, potassium (K) has only one valence electron because it belongs to the first group of the periodic table. Arsenic (As), on the other hand, has five valence electrons since it is part of group 15.
The tin(II) ion (Sn²⁺) originally has four valence electrons, but due to its 2+ charge, it loses two. Thus, it has two valence electrons left. Nitride ion (N³⁻) gains three electrons, bringing its valence count to eight.
Understanding valence electrons enables us to visualize the interaction possibilities and predict chemical reactions.

Electron Configuration

The electron configuration of an atom describes how its electrons are distributed in different atomic orbitals. This configuration helps us understand the atom's characteristics and chemical behavior.

• Electrons are arranged into shells and subshells (s, p, d, f) based on their energy levels.
• Each shell follows a specific order based on increasing energy levels, usually noted as 1s, 2s, 2p, 3s, and so on.
• The number of valence electrons stems from the electron configuration, impacting how Lewis symbols are drawn.

For example, the electron configuration for potassium is \\( 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^1 \), showing that the single valence electron is in the 4s subshell. For arsenic, the configuration \\( 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^{10} \, 4s^2 \, 4p^3 \) places the five valence electrons in the 4s and 4p subshells.
This electron arrangement explains why some atoms are more likely to form certain types of bonds.

Periodic Table Groups

The periodic table is organized into vertical columns known as groups or families, each possessing specific chemical properties determined by their electron configuration. These groups are essential for predicting chemical behavior and properties, including the number of valence electrons.

• Elements in the same group have the same number of valence electrons.
• This similarity leads to comparable chemical properties among group elements.
• Groups are numbered from 1 to 18, sometimes using old notations like IA, IIA, etc.

For instance, potassium (K) belongs to group 1 (alkali metals), sharing a single valence electron trended feature with its group members. Arsenic (As) is part of group 15, meaning it carries five valence electrons, akin to all pnictogens. Tin (Sn), in group 14, has four valence electrons initially, following the carbon group pattern, although its ion form adjusts due to electron loss. Analyzing groups helps in swiftly referencing the basic behavior and potential interactions of elements, bringing a better context to their Lewis symbols representation.