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Atomic Structure and Bonding

Define ionisation energy. Use an equation in your answer. The energy required to remove the outermost electron from an atom. Mg(g) → Mg+(g) + e-; H=-744kJ
Element X has successive ionisation energies of 577kJ, 1820kJ, 2740kJ, 11600kJ and 14800kJ. Why is there a progressively large jump in ionisation energy between the third and fourth energies for element X? More energy is required to remove the fourth than the 3rd outermost electron. This suggests the fourth outermost electron is in a shell closer to the nucleus than the shell containing the first three electrons.
The atomic radius, ionisation energy and electronegativity of an element each depend on two opposing influences. What are these? 1. The number of electrons in an atom and the shells occupied by these. The more shells, the further the outermost electron will be from the nucleus of the atom. 2. The positive charge (protons in nucleus). Larger the charge, larger number of protons.
What is the core charge of an atom? Provide an example. The effective positive charge experienced by the valence electrons in the atom. The electrons in the inner shells create a shielding effect on the positive charge on the nucleus. Core charge = no. protons - no. inner shell electrons. E.g. Na: group 1 = +1
Created by: tintins



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