![]() ![]() A detailed explanation of the absence of PH3 hybridization is given by Drago’s rule. Phosphorus will thus have three bond pairs and one lone pair of electrons. The lone pair of electrons is mainly in the ‘s’ orbital and ‘s’ orbital is the lone pair orbital. This acts as a resistance for the orbitals to get hybridized. The detailed analysis of the structure and formation of the phosphine molecule gives an understanding that the electrons in pure ‘p’ orbital will take part in the formation of chemical bonds. The subsequent sections of this page will give a brief overview of the absence of hybridization in Phosphine molecules. In other words, we can simply say that the process of hybridization is not valid in the case of a phosphine molecule. This is because it is a known fact that Phosphine has a well defined orbital structure and electron distribution. It is quite surprising to describe hybridization in Phosphine. Phosphine has a molar mass of 33.99758 g/mol and is highly soluble in water. The melting point of phosphine is -132.8 0 C and its boiling point is -87.7 0 C. Since phosphine is gaseous at room temperature, it's boiling and melting points are comparatively low. The geometry of its structure describes phosphine as a trigonal pyramidal molecule. This indicates that the structure of phosphine should include one phosphorus and three hydrogen atoms bound together. ![]() The molecular formula of Phosphine is PH 3. It is found that the presence of substituted phosphine and diphosphine induces this unpleasant odour. Though phosphine in its purest form does not have any characteristic odour, the technical grade samples of phosphine stink with an unpleasant odour of garlic or rotten fish. However, it is an inflammable and toxic gas. Phosphine does not have any characteristic colour. To stabilize this variation in energy levels of the electrons from two different orbitals, the orbitals that hold the electrons involved in bond formation combine to form a hybrid orbital. This kind of chemical bonding creates an imbalance in the energy levels of the two electrons. Hybridization is a phenomenon that occurs when an atom makes a bond with the other atom with the help of the electrons that are from both ‘s’ and ‘p’ orbitals. The hybrid orbitals are suitable for the pairing of electrons in valence bond theory to form chemical bonds. The new orbitals are thus called hybrid orbitals. These new orbitals are different in shape and energies when compared to the orbitals that are combined to form these orbitals. Orbital Hybridization generally referred to as Hybridization in chemistry, is a concept that narrates the combining of mixing of atomic orbitals to form new orbitals. Orbital Hybridization is one of the most important topics in modern Physical Chemistry. ![]()
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