Two atomic orbitals can overlap in two ways depending on their phase relationship. Orbital phases are a direct consequence of the nature of waves like electrons. In graphical representations of orbitals, the orbital phases are represented by plus or minus signs (which have no connection with electric charges) or by incising a lobe. The phase sign itself has no physical meaning except when mixing orbitals to form molecular orbitals.
<h2>Further Explanation
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Molecular orbital diagrams, or OM diagrams, are a qualitative descriptive tool that explains chemical bonds in molecules in terms of general molecular orbital theory and linear combinations of atomic orbitals (LCAO) in particular. The basic principle of these theories is that when atoms are bound to form molecules, a number of atomic orbitals combine to form the same number of molecular orbitals, even though electrons can be redistributed between orbitals. This tool is very suitable for simple diatomic molecules such as dihydrogen, dioxygen, and carbon monoxide but becomes more complex when discussing relatively simple polyatomic molecules, such as methane. OM diagrams can explain why some molecules exist and others don't. They can also predict the strength of bonds, as well as electronic transitions that can occur.
In MO theory molecular orbitals are formed by overlapping atomic orbitals. Because σ bonds have greater overlap than π bonds, σ, and σ * bonds and antibonding orbitals have greater energy separation (separation) from pemisahan and π * orbitals. The energy of atomic orbitals correlates with electronegativity because more electronegative atoms hold their electrons more tightly, reducing their energy. MO modeling only applies if atomic orbitals have comparable energy; When the energy is very different, the bonding mode becomes ionic. The second condition for overlapping atomic orbitals is that they have the same symmetry.
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Grade: College
Subject: Chemistry
keywords: molecular, orbital.
