Textbook Question
Draw a molecular orbital energy diagram for ClF. (Assume that the sp orbitals are lower in energy than the p orbitals.) What is the bond order in ClF?
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Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
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Tro 6th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblem 99
Tro 6th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblem 99Chapter 11, Problem 99
Can you provide the formulas of the compounds or ions that bromine forms with one to five fluorine atoms, assign a hybridization to each, and describe their electron and molecular geometry?
Verified step by step guidance1
Identify the possible compounds or ions that bromine can form with one to five fluorine atoms: BrF, BrF_2^-, BrF_3, BrF_4^-, and BrF_5.
For each compound or ion, determine the number of electron domains around the central bromine atom, which includes both bonding pairs and lone pairs.
Assign the hybridization based on the number of electron domains: sp^3d for 5 domains, sp^3d^2 for 6 domains, etc.
Determine the electron geometry using the VSEPR theory: linear, trigonal bipyramidal, octahedral, etc., based on the number of electron domains.
Describe the molecular geometry by considering the arrangement of atoms, ignoring lone pairs: linear, T-shaped, see-saw, square planar, etc.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bromine and Fluorine Compounds
Bromine (Br) can form several compounds with fluorine (F) by sharing electrons, resulting in various bromine fluorides. The most common compounds include BrF, BrF2, BrF3, BrF4, and BrF5, each differing in the number of fluorine atoms bonded to bromine. Understanding these compounds requires knowledge of their molecular formulas and the nature of the bonds formed.
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Noble Gas Compounds
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. For bromine compounds with fluorine, the hybridization can vary: BrF has sp3 hybridization, BrF2 is sp3d, BrF3 is sp3d2, BrF4 is sp3d3, and BrF5 is sp3d3. This hybridization determines the geometry and bond angles of the molecules.
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00:51Hybridization
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which is influenced by the number of bonding pairs and lone pairs of electrons. For example, BrF has a linear geometry, BrF2 is bent, BrF3 has a T-shaped geometry, BrF4 is square planar, and BrF5 adopts a trigonal bipyramidal shape. Understanding these geometries helps predict the physical and chemical properties of the compounds.
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Related Practice
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Water does not easily remove grease from dishes or hands because grease is nonpolar and water is polar. The addition of soap to water, however, allows the grease to dissolve. Study the structure of sodium stearate (a soap) and describe how it works.
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Textbook Question
Draw the structure of a molecule with the formula C4H6Cl2 that has a dipole moment of 0.
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Textbook Question
Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and space-filling models of these vitamins and determine whether each one is fat soluble (mostly nonpolar) or water soluble (mostly polar). (c) niacin (vitamin B3)
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Textbook Question
The compound C3H4 has two double bonds. Describe its bonding and geometry, using a valence bond approach.
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Textbook Question
Draw the structures of two compounds that have the composition CH3NO2 and have all three H atoms bonded to the C. Predict which compound has the larger ONO bond angle.
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