CHM135H1 Lecture 7: 26/09/16 CHM135H1 F LEC0101 Lecture Notes
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CHM135H1 Full Course Notes
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Chm135h1 f - lecture 7 - chapter 5 (5), chapter 8. No need to know other exceptions (e. g. niobium, palladium) Half-filled orbital is stable, as electrons are further apart in this configuration compared to 4s2 3d4. Filled and half-filled orbitals have lower energy state, so half-filled s and d is more stable than filled s but partially-filled d. Butane is bigger than methane (size) - increases london dispersion forces (also induced-dipole induced-dipole force, and is one type of the van der waals forces) Not because butane is heavier than methane (mass) - gravity is not relevant in such a small molecule. Butane has larger electron cloud, increasing opportunities for interactions; protons of one molecule temporarily attracts electrons of another molecule. As first electron cloud moves towards other molecule, repels electron cloud of second molecule. Going down the halogens, the melting and boiling points increase; due to increasing london dispersion forces, increasing attraction between molecules.
