Basics of Chemical Bonding - 2

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Published on February 24, 2009

Author: youmarks

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Chemical Bonding Part 2

Chemical Bonding Part II copyrights © youmarks.com

Polar Bonds Ionic and covalent bonds are two ideal types. Many bonds share characteristics of both ionic and covalent bonding. They are called polar covalent bonds and they tend to occur between atoms of moderately different electronegativities. In polar covalent bonds the electrons belong predominantly to one type of atom while they are still partially shared by the other type, as illustrated in the pictures of the valence electron densities. copyrights © youmarks.com

Ionic and covalent bonds are two ideal types.

Many bonds share characteristics of both ionic and covalent bonding. They are called polar covalent bonds and they tend to occur between atoms of moderately different electronegativities.

In polar covalent bonds the electrons belong predominantly to one type of atom while they are still partially shared by the other type, as illustrated in the pictures of the valence electron densities.

Polar Bonds copyrights © youmarks.com

Metallic Bonding Electron SEA Model for METALS Metals are formed from elements on the left hand side of the periodic table. Having generally low electronegativity they tend to lose their valence electrons easily. When we have a macroscopic collection of the same or similar type of metallic atoms, the valence electrons are detached from the atoms but not held by any of the other atoms. In other words, these valence electrons are free from any particular atom and are only held collectively by the entire assemblage of atoms. In a metal the ion cores are held more or less at fixed places in an ordered, or crystal, lattice. The valence electrons are free to move about under applied stimulation, such as electric fields or heat. copyrights © youmarks.com

Electron SEA Model for METALS

Metals are formed from elements on the left hand side

of the periodic table. Having generally low electronegativity

they tend to lose their valence electrons easily.

When we have a macroscopic collection of the same

or similar type of metallic atoms, the valence electrons

are detached from the atoms but not held by any of

the other atoms. In other words, these valence electrons

are free from any particular atom and are only

held collectively by the entire assemblage of atoms.

In a metal the ion cores are held more or less at fixed

places in an ordered, or crystal, lattice. The valence

electrons are free to move about under applied stimulation,

such as electric fields or heat.

Metallic Bonding copyrights © youmarks.com

Metallic Bonding copyrights © youmarks.com

Intra-molecular Forces In addition to covalent, polar, ionic and metallic bonding there are intermolecular forces which contribute to the stability of things. These include dipole-dipole forces, hydrogen bonding and London dispersion forces. copyrights © youmarks.com

In addition to covalent, polar, ionic and metallic bonding there are intermolecular forces which contribute to the stability of things. These include dipole-dipole forces, hydrogen bonding and London dispersion forces.

Intra-molecular Forces copyrights © youmarks.com

Intra-molecular Forces copyrights © youmarks.com

Intra-molecular Forces copyrights © youmarks.com

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