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Angular functions: 'shapes'
The mathematical functions for atomic orbitals may be described as a product of two factors: the radial wavefunction defines the behavior of the electron as a function of distance from the nucleus (see below); the angular wavefunction shows how it varies with the direction in space. Angular wavefunctions do not lay on n and are characteristic features of s, p, d,...orbitals.
Fig. 1. The shapes of s, p and d orbitals. Shading shows negative values of the wavefunction
NOBEL GASES With their closed-shell electron design the noble gas elements of group 18 were long regarded as chemically inert. However, in 1962 Bartlett pinpoint that the ioniza
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The cell diagram of a mercury cell can be written Zn(s) | ZnO (s) NaOH (aq) HgO (s) HgO (I) (a) Write the electrode reactions and cell reaction with electron number z = 2.
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