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23. In chemistry, orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory.
In the molecule CH4 the central atom C has 4 valence electrons where the C atom is forming 4 sigma bonds with H atoms and therefore the stearic number of C is 4 which imply that the hybridization of the molecule is sp3 where the geometry and the shape is tetrahedral.
24. The ammonia molecule has a trigonal pyramidal shape with the three hydrogen atoms and an unshared pair of electrons attached to the nitrogen atom. It has an experimental bond angle of 106. 70.
The VSEPR theory assumes that each atom in a molecule will achieve a geometry that minimizes the repulsion between electrons in the valence shell of that atom. ... Repulsion between these pairs of electrons can be minimized by arranging them so that they point in opposite directions.
the ammonia molecule has a trigonal pyramidal shape as predicted by the valence shell electron pair repulsion theory (VSEPR) theory with an experimentally determined bond angle of 106.7°. the central nitrogen atom has 5 outer electrons with an additional electron from each hydrogen atom.
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Key Points. The bonds in a methane (CH4) molecule are formed by four separate but equivalent orbitals; a single 2s and three 2p orbitals of the carbon hybridize into four sp3 orbitals. In the ammonia molecule (NH3), 2s and 2p orbitals create four sp3hybrid orbitals, one of which is occupied by a lone pair of electrons.
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the ammonia molecule has a trigonal pyramidal shape as predicted by the valence shell electron pair repulsion theory (VSEPR) theory with an experimentally determined bond angle of 106.7°. the central nitrogen atom has 5 outer electrons with an additional electron from each hydrogen atom.
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