Greetings,
In my last post, the first of this "Energy and Matter" series, I discussed the ground state concept for the hypothetical existence of elements on the Periodic Table. A discussion on the Hybrid Orbital Theory of Covalent Bonding naturally follows.
The Hybrid Orbital Theory goes like this: When non-metal ground state atoms approach each other the opposing forces of electron clouds induce a purturbation energy. For elements forming two or more bonds, such as carbon and sulfur, energized atomic orbitals "mix" resulting in hybrid atomic orbitals. The hybrid atomic orbitals are thought to form sigma bonds with atomic orbitals of adjacent atoms. A sigma bond is an "end-to-end" overlap of atomic orbitals. The formation of double and triple bonds involve a "side-to-side" overlap of unhybridized orbitals; pi bonds.
There is a naming system for describing the combination of hybrid and nonhybrid atomic orbitals utilized in the formation of covalent bonds between nonmetal atoms: The "mixed" atomic orbitals are listed starting with s, then p and finally d orbital(s) (e.g. Six-sp3d2 hybrid orbitals for a sulfur atom). Here is an important rule to remember: The number of original ground-state orbitals used equals the number of hybrid orbitals produced. For example, a combination of 1 s-orbital and 3 p-orbitals yields 4-sp3 hybrid atomic orbitals.
Yet another important point, is the satisfaction of certain spatial requirements upon the formation of hybrid atomic orbitals. In the case of a carbon atom forming four single bonds (such as for methane, CH4), four identical sp3 hybrid orbitals naturally arrange themselves in a minimum-energy tetrahedral formation, as required according to the VSEPR theory. The tetrahedral geometry cannot be attained by ground-state s and p(3) atomic orbitals. The following diagram depicts the theory visually.
That's all for this post. As always, thank you for reading!
A Publication of http://ExcellenceInLearning.biz
In my last post, the first of this "Energy and Matter" series, I discussed the ground state concept for the hypothetical existence of elements on the Periodic Table. A discussion on the Hybrid Orbital Theory of Covalent Bonding naturally follows.
The Hybrid Orbital Theory goes like this: When non-metal ground state atoms approach each other the opposing forces of electron clouds induce a purturbation energy. For elements forming two or more bonds, such as carbon and sulfur, energized atomic orbitals "mix" resulting in hybrid atomic orbitals. The hybrid atomic orbitals are thought to form sigma bonds with atomic orbitals of adjacent atoms. A sigma bond is an "end-to-end" overlap of atomic orbitals. The formation of double and triple bonds involve a "side-to-side" overlap of unhybridized orbitals; pi bonds.
There is a naming system for describing the combination of hybrid and nonhybrid atomic orbitals utilized in the formation of covalent bonds between nonmetal atoms: The "mixed" atomic orbitals are listed starting with s, then p and finally d orbital(s) (e.g. Six-sp3d2 hybrid orbitals for a sulfur atom). Here is an important rule to remember: The number of original ground-state orbitals used equals the number of hybrid orbitals produced. For example, a combination of 1 s-orbital and 3 p-orbitals yields 4-sp3 hybrid atomic orbitals.
Yet another important point, is the satisfaction of certain spatial requirements upon the formation of hybrid atomic orbitals. In the case of a carbon atom forming four single bonds (such as for methane, CH4), four identical sp3 hybrid orbitals naturally arrange themselves in a minimum-energy tetrahedral formation, as required according to the VSEPR theory. The tetrahedral geometry cannot be attained by ground-state s and p(3) atomic orbitals. The following diagram depicts the theory visually.
That's all for this post. As always, thank you for reading!
A Publication of http://ExcellenceInLearning.biz