subshell has to be broken into. Half-full shells are relatively stable so N (with a half-filled p subshell) ii) has a higher IE than O, which has one electron more. Part 3 stands for Valence Shell Electron Pair Repulsion and these electron pair repulsions are responsible for the shapes of molecules and polyatomic ions such as NH4+ Step 1 Calculate the number of outer electrons (or valence) on the central – atom of molecule or ion by taking the number of electrons on the –achieved centre atom and adding one electron for each of the other atoms attached. Note if we are dealing with an ion with a 1+ charge, then we subtract an – electron from the total to account for this charge. For an ion with a -1 charge, we add an electron to the total. For example:
subshell has to be broken into. ii) Half-full shells are relatively stable so N (with a half-filled p subshell) has a higher IE than O, which has one electron more. Part 3 stands for Valence Shell Electron Pair Repulsion and these electron pair repulsions are responsible for the shapes of molecules and polyatomic ions such as NH4+ Step 1 – Calculate the number of outer electrons (or valence) on the central atom of molecule or ion –achieved by taking the number of electrons on the centre atom and adding one electron for each of the other atoms attached. Note – if we are dealing with an ion with a 1+ charge, then we subtract an electron from the total to account for this charge. For an ion with a -1 charge, we add an electron to the total. For example:
InorganicSept2016Final-1.docx