Core - Chemistry

Chapter 9

Chemical Bonding: Basic Concepts

9.1 : Types of Chemical Bonds

9.1 : Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and ...

9.2 : Lewis Symbols and the Octet Rule

9.2 : Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

9.3 : Ionic Bonding and Electron Transfer

9.3 : Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

9.4 : The Born-Haber Cycle

9.4 : The Born-Haber Cycle

Lattice Energy An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

9.5 : Trends in Lattice Energy: Ion Size and Charge

9.5 : Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

9.6 : Covalent Bonding and Lewis Structures

9.6 : Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

9.7 : Electronegativity

9.7 : Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity. Electronegativity values of ...

9.8 : Bond Polarity, Dipole Moment, and Percent Ionic Character

9.8 : Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity The absolute value of the difference in electronegativity (ΔEN) of two bonded atoms provides a rough measure of the polarity to be ...

9.9 : Lewis Structures of Molecular Compounds and Polyatomic Ions

9.9 : Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined: Determine the ...

9.10 : Resonance

9.10 : Resonance

The Lewis structure of a nitrite anion (NO2−) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

9.11 : Formal Charges

9.11 : Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

9.12 : Exceptions to the Octet Rule

9.12 : Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories: ...

9.13 : Bond Energies and Bond Lengths

9.13 : Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

9.14 : Bonding in Metals

9.14 : Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the ...

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