CH1001 Lecture Notes - Lecture 6: Metallic Bonding, Covalent Bond, Electronegativity

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16 Jul 2018
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A formation of ionic bonds between a metal atom and a non-metal atom. Formation of covalent bonds between two non-metal atoms. Metallic bonding - the metal cations are imbedded in a sea of mobile valence electrons. There are three types of interactions within a molecule. In any molecule, these three interactions are balanced to give the molecule its greatest possible stability. This balance is achieved when the electron density is situated between the nuclei of bonded atoms. This shared electron density is called a covalent bond. The attractive energy between nuclei and electrons exceeds the repulsive energy arising from nuclei-nuclei and electron-electron interactions. These concepts are demonstrated below for the simplest stable neutral molecule, molecular hydrogen (h2). Bond length is the separation distance at which the molecule has the maximum energetic advantage over the separated atoms. Bond energy is the energy required to break the bond (kj mol-1). Each different chemical bond has a characteristic bond length and energy.

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