In diamond, the carbons are in sp 3 hybrid orbitals, which means they form a framework where each carbon is covalently bonded to four neighbours in a tetrahedral fashion; on the other hand, graphite is composed of sheets of carbons in sp 2 hybrid orbitals, where each carbon is bonded covalently to only three others.
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In diamond, the carbons are in sp 3 hybrid orbitals, which means they form a framework where each carbon is covalently bonded to four neighbours in a tetrahedral fashion; on the other hand, graphite is composed of sheets of carbons in sp 2 hybrid orbitals, where each carbon is bonded covalently to only three others.
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For example, in the Bohr model, an electron has the same energy whether it is in the hybrid orbitals ( also called quantum superpositions ) of the 2s and 2p states where the electron tends to be to the left, which will acquire a lower energy, and other hybrid orbitals where the electron tends to be to the right, which will acquire a higher energy.
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For example, in the Bohr model, an electron has the same energy whether it is in the hybrid orbitals ( also called quantum superpositions ) of the 2s and 2p states where the electron tends to be to the left, which will acquire a lower energy, and other hybrid orbitals where the electron tends to be to the right, which will acquire a higher energy.
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