Ch.1 - Structure and Bonding

Wade9th EditionOrganic ChemistryISBN: 9780135213728Not the one you use?Change textbook

Wade 9th Edition

Ch.1 - Structure and Bonding

Problem 1b

Chapter 1, Problem 1b

Write the electronic configurations of the third-row elements shown in the partial periodic table in Figure 1-6.

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Identify the third-row elements in the periodic table. These elements are sodium (Na), magnesium (Mg), aluminum (Al), silicon (Si), phosphorus (P), sulfur (S), chlorine (Cl), and argon (Ar).

Understand that the electronic configuration is a representation of the distribution of electrons in an atom's orbitals. The third-row elements fill the 3s and 3p orbitals.

Start with sodium (Na), which has an atomic number of 11. Its electronic configuration is written by filling the 1s, 2s, 2p, and then the 3s orbitals:

{1s}^{2} {2s}^{2} {2p}^{6} {3s}^{1}

Continue with magnesium (Mg), which has an atomic number of 12. Its electronic configuration is:

{1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2}

Proceed with the remaining elements (Al, Si, P, S, Cl, Ar) by adding electrons to the 3p orbitals, following the order of increasing atomic number and ensuring that the Pauli exclusion principle and Hund's rule are observed.

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Key Concepts

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

Electronic Configuration

Electronic configuration refers to the distribution of electrons in an atom's orbitals. It is typically represented using the notation that indicates the energy levels, sublevels, and the number of electrons in each sublevel, such as 1s² 2s² 2p⁶. Understanding electronic configurations helps predict an element's chemical properties and behavior.

Periodic Table Structure

The periodic table is organized into rows called periods and columns called groups. Each period corresponds to the filling of a principal energy level with electrons. The third row, or period, includes elements where the 3s and 3p orbitals are being filled. Recognizing this structure is crucial for determining the electronic configurations of elements in a specific period.

Aufbau Principle

The Aufbau principle is a guideline for determining the electron configuration of an atom. It states that electrons fill orbitals starting from the lowest energy level to higher ones. This principle, along with Hund's rule and the Pauli exclusion principle, helps in predicting the order in which atomic orbitals are filled, which is essential for writing accurate electronic configurations.

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Related Practice

Textbook Question

For each of the following compounds,1. Give the hybridization and approximate bond angles around each atom except hydrogen.2. Draw a three-dimensional diagram, including any lone pairs of electrons.d. (CH3)3N e. [CH3NH3]+f. CH3COOH

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Textbook Question

Nitrogen has relatively stable isotopes (half-life greater than 1 second) of mass numbers 13, 14, 15, 16, and 17. All except ¹⁴N and ¹⁵N are radioactive.) Calculate how many protons and neutrons are in each of these isotopes of nitrogen.

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Textbook Question

Use electronegativities to predict the direction of the dipole moments of the following bonds.

(f) N—Cl

(g) N—O

(h) N—S

(i) N—B

(j) B—Cl

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Textbook Question

Use your molecular models to make ethane, and compare the model with the preceding structures.

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