1. Electron configuration directly influences the properties of the elements. The modern periodic table classifies the elements according to their atomic numbers, and thus also by their electron configurations. The configuration of the outermost electrons (valence electrons) directly affects the properties of the atoms of the representative elements. 2. The size of an atom, indicated by atomic radius, varies periodically with the arrangement of the elements in the periodic table. It decreases as we move across a period and increases as we move down a group. 3. Metals form giant metallic structures. They have high melting points, high boiling points, high density and high conductivity. 4. Metalloids and diamond form giant molecular structures. They have very high melting points, very high boiling points, high density but poor conductivity. 5. Non-metals (except diamond) form simple molecular structures. They have low melting points; low boiling points, low density and they are non-conductors. 6. From left to right across the periodic table, elements change from reactive metals, through less reactive metals, metalloids, less reactive non-metals to reactive non-metals. (On the extreme right are the noble gases)
Posted on: Fri, 13 Sep 2013 07:52:38 +0000