Textbook Question
Write the Lewis structure for each molecule. d. CH4
Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 10, Problem 55a,b,c
Write the Lewis structure for each molecule. a. PH3 b. SCl2 c. HI
Verified step by step guidance1
Determine the total number of valence electrons in the molecule. Phosphorus (P) has 5 valence electrons, and each hydrogen (H) has 1 valence electron. Since there are three hydrogen atoms, the total number of valence electrons is 5 + 3(1) = 8.
Place the least electronegative atom in the center. In PH_3, phosphorus is less electronegative than hydrogen, so phosphorus will be the central atom.
Connect each hydrogen atom to the central phosphorus atom with a single bond. Each P-H bond will use 2 valence electrons, so 3 bonds will use 6 electrons.
Distribute the remaining valence electrons to satisfy the octet rule for the central atom. After forming the bonds, 2 electrons remain, which will be placed as a lone pair on the phosphorus atom.
Verify that all atoms have a complete valence shell. Hydrogen atoms are satisfied with 2 electrons each, and phosphorus has 8 electrons around it (6 from bonds and 2 from the lone pair).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules.
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Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's reactivity and stability. For example, phosphorus (P) has five valence electrons, which play a key role in forming bonds in molecules like PH3.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom. In the case of PH3, the geometry is trigonal pyramidal due to the presence of one lone pair on phosphorus, affecting the molecule's shape and properties.
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Related Practice
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Write the Lewis structure for each molecule. b. SiH4
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Write the Lewis structure for each molecule. a. SF2
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Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of MgO. (ΔHsub for magnesium is 137 kJ/mol; IE1 and IE2 for magnesium are 738 kJ/mol and 1450 kJ/mol, respectively; EA1 and EA2 for O are −141 kJ/mol and 744 kJ/mol, respectively.)
Textbook Question
Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of LiBr. (ΔHsub for lithium is 138 kJ>mol.)