periodic table ! Flashcards
down group - atomic radius !
atomic radius increases : number of electron shells increases
down group - metallic character !
metallic character increases : becomes easier to lose valence electrons as atomic radius increases -> electrons are further away from nucleus -> not as strongly attached to nucleus
down group - ionisation energy !
ionisation energy decreases : size of atom increases -> electrons are further away from nucleus -> not as strongly attached to nucleus -> easier to lose electrons
across period - atomic radius !
atomic radius decreases : increase in number of protons -> nucleur charge increases -> electrons are more strongly attached to nucleus
across period - metallic character !
metallic character decreases : atomic radius decreases -> nuclear charge increases -> electrons are more strongly attached to nucleus -> harder to lose electrons
across period - ionisation energy !
ionisation energy increases : atomic radius decreases -> nuclear charge increases -> electrons are more strongly attached to nucleus -> harder to lose electrons
across period - oxide nature !
oxide nature : basic (metal ) -> amphoteric (transition metal) -> acidic (non-metal) -> neutral (non-metal)
group 1 - PHYSICAL properties !
shiny & silvery solids
soft : easily cut apart
low density
low melting boiling point
group 1 - CHEMICAL properties !
highly reactive
react vigoursly with water : produces alkaline metal hydroxide & hydrogen
strong reducing agents
group 1 PHYSICAL trends - down group !
density increases : atomic radius increases -> number of electron shells increases -> ionsiation energy decreases -> easier to lose electrons
melting & boiling point decreases : valence electrons are further away from positive metal ions -> electrostatic F.O.A between. metal ions & sea of delocalised electrons becomes weaker -> less energy to overcome F.O.A -> easier to lose electrons
group 1 CHEMICAL trends - down group !
chemical
- reactivity increases : atomic radius increases -> number of electron shells increases -> valence electrons are further away from positively charged nucleus -> easier to lose valence electrons -> more reactive
group VII (halogens) PHYSICAL properties !
diatomic non-metals
toxic elements
poor conductors of heat & electricity
low melting & boiling points
group VII CHEMICAL properties !
very reactive non-metals
strong oxidising agents
group VII PHYSICAL trends - down group !
melting point increases : size of element increases -> intermolecular F.O.A between molecules increases -> more energy required to overcome F.O.A -> harder to lose electrons -> mpt increases
colour darkens : pale yellow -> black
group VII CHEMICAL trends - down group !
reactivity decreases : atomic radius increases -> electron shells increases -> electrons are further away from positively charged nucleus -> harder to gain electrons (halogens are reactive non-metals -> only need to gain 1 valence electron to achieve stable noble gas configuration)
