Textbook Question
Consider the lattice energies of the following Group 2A compounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol; CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol. (a) What is the oxidation number of H in these compounds?
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Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 76
Draw the Lewis structure for NO+ . Is the nitrogen–oxygen bond in NO+ longer, shorter, or the same length as thenitrogen–oxygen bond in NO? Explain.Draw the Lewis structure for NO+ .
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Identify the total number of valence electrons for NO^+. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6 valence electrons, and the positive charge indicates the loss of one electron, so the total is 5 + 6 - 1 = 10 electrons.
Place the nitrogen and oxygen atoms next to each other, as they will form a bond. Start by drawing a single bond between N and O, which uses 2 electrons, leaving 8 electrons to distribute.
Distribute the remaining electrons to satisfy the octet rule, starting with the more electronegative atom, oxygen. Place 6 electrons (3 lone pairs) on oxygen, and 2 electrons (1 lone pair) on nitrogen.
Check if the octet rule is satisfied for both atoms. Nitrogen has 5 electrons (1 lone pair and 2 from the bond), and oxygen has 8 electrons (3 lone pairs and 2 from the bond). To satisfy the octet for nitrogen, form a double bond by moving one lone pair from oxygen to form a second bond with nitrogen.
Compare the bond order of NO^+ and NO. NO^+ has a bond order of 3 (triple bond), while NO has a bond order of 2. A higher bond order typically indicates a shorter bond length, so the N-O bond in NO^+ is shorter than in NO.
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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 predicting molecular geometry, bond lengths, and the overall reactivity of the molecule.
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Lewis Dot Structures: Ions
Bond Length
Bond length is the distance between the nuclei of two bonded atoms. It is influenced by the type of bond (single, double, or triple) and the atoms involved. Generally, as the number of shared electron pairs increases, the bond length decreases, leading to shorter and stronger bonds. This concept is crucial for comparing bond lengths in different molecules.
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Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. It helps in determining the most stable Lewis structure by minimizing formal charges across the molecule. In the case of NO+ and NO, analyzing formal charges can provide insight into the stability and bond characteristics of the nitrogen-oxygen bond.
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Related Practice
Textbook Question
Consider the lattice energies of the following Group 2A compounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol; CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol. (c) Consider BeH2. Does it require 3205 kJ of energy to break one mole of the solid into its ions, or does breaking up one mole of solid into its ions release 3205 kJ of energy?
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