Textbook Question
Suggest a plausible structure for the silicate anion in the mineral thortveitite, Sc2Si2O7.
Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 22, Problem 22.92
Draw the electron-dot structure for CO, CO2, and CO32–, and predict which substance will have the strongest carbon–oxygen bond.
Verified step by step guidance1
Identify the total number of valence electrons for each molecule or ion. For CO, carbon has 4 valence electrons and oxygen has 6, totaling 10 electrons. For CO_2, carbon has 4 and each oxygen has 6, totaling 16 electrons. For CO_3^{2-}, carbon has 4, each oxygen has 6, and the 2- charge adds 2 more electrons, totaling 24 electrons.
Draw the Lewis structure for CO by placing carbon and oxygen next to each other. Use a triple bond between carbon and oxygen to satisfy the octet rule, and place any remaining electrons as lone pairs on the oxygen atom.
Draw the Lewis structure for CO_2 by placing carbon in the center with double bonds to each oxygen. Ensure each atom satisfies the octet rule, with carbon having 8 electrons and each oxygen having 8 electrons.
Draw the Lewis structure for CO_3^{2-} by placing carbon in the center with single bonds to each oxygen. Distribute the remaining electrons to satisfy the octet rule for each oxygen. Use resonance structures to show the delocalization of electrons, indicating that the double bond can be with any of the three oxygens.
Compare the bond orders: CO has a triple bond (bond order of 3), CO_2 has double bonds (bond order of 2), and CO_3^{2-} has resonance structures with an average bond order of 1.33. The strongest bond is the one with the highest bond order, which is the triple bond in CO.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron-Dot Structures
Electron-dot structures, also known as Lewis structures, represent the valence electrons of atoms within a molecule. They illustrate how electrons are shared or transferred between atoms, helping to visualize bonding and lone pairs. For CO, CO2, and CO3^2–, drawing these structures reveals the arrangement of electrons and the types of bonds formed, which are crucial for understanding molecular geometry and reactivity.
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Lewis Dot Structures: Ions
Bond Order
Bond order is a concept that indicates the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding and antibonding electrons divided by two. Higher bond orders generally correlate with stronger bonds; thus, analyzing the bond order in CO, CO2, and CO3^2– will help predict which carbon-oxygen bond is the strongest based on the number of shared electron pairs.
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Resonance Structures
Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In molecules like CO3^2–, resonance indicates that the actual structure is a hybrid of these forms, affecting bond lengths and strengths. Understanding resonance is essential for predicting the stability and reactivity of the molecule, as it influences the effective bond order and the strength of the carbon-oxygen bonds.
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Related Practice
Textbook Question
Compare and contrast the properties of ammonia and phosphine.
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Arrange the following oxides in order of increasing basic character: Al2O3, Cs2O, K2O, N2O5.
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Describe the structure of diborane (B2H6) and explain why the bridging B–H bonds are longer than the terminal B–H bonds.
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Textbook Question
Which of the following elements (X) will form a covalent hydride with the formula XH3 that is a gas at room temperature? (LO 22.4)
(a) Al (b) As (c) Ba (d) Se
Textbook Question
Give an example of an ionic carbide. What is the oxidation state of carbon in this substance?