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...Periodicity trends in the periodic table atomic radius angstroms melting point kelvin unknown decreases across a period as nuclear charge increases but shielding effects metallic bonded and macromolecular substances tend to have high points for both this remain approximately constant resulting electrons being drawn closer nucleus is due fact that bonds require lot of energy break down group valence become increasingly distant from majority non metals simple molecular structure also leads increase despite low only weak intermolecular forces must be overcome order melt them increasing strength these determined by size molecule electronegativity pauling scale ionisation kilojoules mole measure tendency an atom attract bonding pair first generally left right electron moving towards top increased becomes harder remove p orbitals are slightly easier than those s same greater force attraction level paired orbital can lead repulsion again making felt factors lower expected energies c compound ...