2.1 periodicity Flashcards

1
Q

what happens to atomic radius across a period?

A

decreases as proton number increases so electrons pulled closer to nucleus so radius smaller

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2
Q

what happens to melting point across group 3?

A

generally increases from sodium to silicon then generally decreases from silicon to argon

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3
Q

why does melting point increase from sodium to aluminium?

A

they are metals so mp increases across group as metallic bonds get stronger due to increased nuclear charge and delocalised electrons

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4
Q

why is there a big increase in melting point from aluminium to silicon?

A

silicon is macromolecular and has a tetrahedral shape- lots of strong covalent bonds to break

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5
Q

what happens to first ionisation energy across period 3?

A

general increase as you go across as there is increasing attraction between outer shell electrons and nucleus due to proton number increasing

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5
Q

what happens to melting point between phosphorus, sulphur, chlorine and argon?

A

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

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