2.1 periodicity Flashcards
what happens to atomic radius across a period?
decreases as proton number increases so electrons pulled closer to nucleus so radius smaller
what happens to melting point across group 3?
generally increases from sodium to silicon then generally decreases from silicon to argon
why does melting point increase from sodium to aluminium?
they are metals so mp increases across group as metallic bonds get stronger due to increased nuclear charge and delocalised electrons
why is there a big increase in melting point from aluminium to silicon?
silicon is macromolecular and has a tetrahedral shape- lots of strong covalent bonds to break
what happens to first ionisation energy across period 3?
general increase as you go across as there is increasing attraction between outer shell electrons and nucleus due to proton number increasing
what happens to melting point between phosphorus, sulphur, chlorine and argon?
phosphorus, sulphur and chlorine are all molecular substances. their melting points depend on vdw forces- weak so easily overcome. more atoms in molecule means more vdw. sulphur is biggest so has highest mp. argon very low as it is monoatomic so very weak vdw