Textbook Question
Using the shorthand notation of Figure 22.9, draw the structure of the silicate anion in:
(a) K4SiO4 (b) Ag10Si4O13
What is the relationship between the charge on the anion and the number of terminal O atoms?
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 22, Problem 22.93
What is the hybridization and geometry around carbon atoms in graphene? Explain why graphene is an excellent conductor of electricity.
Verified step by step guidance1
Graphene is a single layer of carbon atoms arranged in a two-dimensional honeycomb lattice. Each carbon atom in graphene is bonded to three other carbon atoms.
To determine the hybridization of the carbon atoms in graphene, consider the number of sigma bonds and lone pairs around each carbon. In graphene, each carbon forms three sigma bonds with neighboring carbon atoms.
The hybridization of a carbon atom with three sigma bonds and no lone pairs is \( sp^2 \). This hybridization involves the mixing of one \( s \) orbital and two \( p \) orbitals, resulting in three \( sp^2 \) hybrid orbitals.
The geometry around each carbon atom in graphene is trigonal planar, with bond angles of approximately 120 degrees. This planar structure allows for the overlap of \( p \) orbitals, forming a delocalized \( \pi \) bond system across the entire graphene sheet.
Graphene is an excellent conductor of electricity because the delocalized \( \pi \) electrons can move freely across the entire sheet, allowing for efficient charge transport. This delocalization is a result of the \( sp^2 \) hybridization and the planar geometry of the carbon atoms.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the process by which atomic orbitals mix to form new hybrid orbitals, which can explain the bonding properties of atoms in molecules. In graphene, carbon atoms undergo sp2 hybridization, where one s orbital and two p orbitals combine to create three equivalent sp2 hybrid orbitals. This arrangement allows for the formation of strong sigma bonds with neighboring carbon atoms, resulting in a planar structure.
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00:51
Hybridization
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. In graphene, the sp2 hybridization leads to a trigonal planar geometry around each carbon atom, with bond angles of approximately 120 degrees. This planar structure contributes to the stability and unique properties of graphene, including its high strength and flexibility.
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01:33Molecular Geometry with Two Electron Groups
Electrical Conductivity
Electrical conductivity in materials is the ability to conduct electric current, which in graphene is attributed to its delocalized π electrons. The planar structure of graphene allows these π electrons to move freely across the lattice, facilitating the flow of electricity. This property, combined with its high electron mobility, makes graphene an excellent conductor, surpassing many traditional conductive materials.
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Related Practice
Textbook Question
Draw the electron-dot structure for CO, CO2, and CO32–, and predict which substance will have the strongest carbon–oxygen bond.
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Textbook Question
An important physiological reaction of nitric oxide (NO) is its interaction with the superoxide ion (O2–) to form the peroxynitrite ion (ONOO–).
a. Write electron-dot structures for NO, O2–, and ONOO–, and predict the O–N–O bond angle in ONOO–.
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Textbook Question
GeCl4 reacts with Cl- to give GeCl62-, but CCl4 does not react with excess Cl-. Explain.
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Textbook Question
The following pictures represent various silicate anions. Write the formula and charge of each anion.
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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
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