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Ch.9 - Molecular Geometry and Bonding Theories
All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 49a,b
Chapter 9, Problem 49a,b

Consider the molecule BF3. (a) What is the electron configuration of an isolated B atom? (b) What is the electron configuration of an isolated F atom?

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To determine the electron configuration of an isolated B (Boron) atom, first identify its atomic number, which is 5. This means a neutral Boron atom has 5 electrons.
Write the electron configuration for Boron by filling the orbitals in order of increasing energy: 1s, 2s, 2p. The configuration is: 1s22s22p1.
Next, consider the isolated F (Fluorine) atom. Its atomic number is 9, indicating it has 9 electrons.
Write the electron configuration for Fluorine by filling the orbitals in order of increasing energy: 1s, 2s, 2p. The configuration is: 1s22s22p5.
These configurations show how electrons are distributed in the atomic orbitals of Boron and Fluorine, which is essential for understanding their chemical behavior and bonding in molecules like BF3.

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Key Concepts

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

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. For example, the electron configuration of a neutral boron (B) atom, which has 5 electrons, is 1s² 2s² 2p¹, while fluorine (F), with 9 electrons, has the configuration 1s² 2s² 2p⁵.
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Atomic Structure

The atomic structure refers to the arrangement of protons, neutrons, and electrons within an atom. The nucleus contains protons and neutrons, while electrons orbit the nucleus in defined energy levels. Understanding atomic structure is essential for determining electron configurations, as it helps explain how electrons fill available orbitals based on energy levels and the principles of quantum mechanics.
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Periodic Table Trends

The periodic table organizes elements based on their atomic number and electron configurations, revealing trends in properties such as electronegativity, ionization energy, and atomic radius. Elements in the same group often exhibit similar electron configurations in their outer shells, which influences their chemical behavior. For instance, boron and fluorine are in different groups, leading to distinct electron configurations and reactivity patterns.
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Related Practice
Textbook Question

Draw sketches illustrating the overlap between the following orbitals on two atoms: (b) the 2pz orbital on each atom (assume both atoms are on the z-axis) (c) the 2s orbital on one atom and the 2pz orbital on the other atom.

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Textbook Question

For each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.

Textbook Question
How would you expect the extent of overlap of the bondingatomic orbitals to vary in the series IF, ICl, IBr, and I2?Explain your answer.
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Textbook Question

Consider the molecule BF3. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF3?

Textbook Question

Consider the SCl2 molecule. (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2?

Textbook Question

Consider the SCl2 molecule.(d) What valence orbitals, if any, remain unhybridized on the S atom in SCl2?