Orbital hybridisation

The hybrid orbitals have an overlapping power of twice the overlapping power of s orbitals. Therefore, 

Hybridization explains the geometry of ammonia (NH3) and water (H2O) and similar compounds. 

Coordination number Orbital configuration Geometry Example 

Hybridisation is not a special effect in which precise participation by, for example, one s and three p orbitals produces four sp hybrid orbitals. Continuous variability is possible. The extent to which hybridisation occurs depends on the energy separation of the initial s and p orbitals. The closer they are energetically, the more complete will be the hybridisation. Hybridisation can also occur with d and f orbitals. Hybridisation is no more than a convenient way of viewing the manner in which the electron orbitals interact during chemical bonding. The shape of various hybrid orbitals is given in Table 2.5. 

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In ethene the situation is rather different here, each carbon atom has one 2s and two 2p orbitals hybridised to form three sp single-pear orbitals which are trigonal planar (shown shaded in each half of Figure 2. JO). The remaining 2p orbital is not hybridised,... 

A covalent bond between two atoms requires two electrons and two orbitals, one for each atom.f The factors determining the properties of the covalent bonds formed by an atom are primarily the number and nature of the orbitals (hybridised bond orbitals) available to the atom, and the number of electrons that it can use in bond formation without losing its electrical neutrality. The opportunities for stabilisation through resonance of covalent bonds among alternative positions are also important. 

A PowerPoint presentation covering molecular orbitals, hybridisation and the bonding continuum can be downloaded from www. brightredbooks.net... 

Figure 2.39 Energy bands from isolated atoms in germanium (Ge). As the spacing between the atoms, r, decreases, first orbital hybridisation occurs and then energy bands develop. These are broad and separated by a narrow energy gap, as expected from the covalent model of bonding...

When a gas interacts with SWCNTs, the adsorbed molecules act as dopants, which possibly influences the SWCNT transport properties. These dopants can shift the Fermi level of SWCNTs or can modify the SWCNT band structure due to the orbital hybridisations between the analytes and the electron cloud of SWCNTs. If the response is assumed to be proportional to the fractional monolayer coverage of molecules adsorbed on the SWCNTs, then the stationary response is given by Equation [10.2] and the response time is given by Equation [10.3] ... 

Fig. 1.11 Results of hybridisation of s and p atomic orbitals. Hybridisation In methane Is sp with four equivalent orbitals in a tetrahedral arrangement...

Zhou and Yildirim proposed that the hydrogen binding in (Mn4Cl)3(btt)8-MOF[ l is not of the expected Kubas type because there is (a) no significant charge transfer from metal to hydrogen, (b) no evidence of any H2- 7 Mn-d orbital hybridisation, (c) no significant H-H... 

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