3.2 group 2 + halogens Flashcards
going down group 2 atomic radius:
increases
going down group 2 first ionisation energy:
decreases
going down group 2 melting point:
decreases
would group 2 be reducing or oxidising agents?
reducing agents as another element will be reudced when they recieve the 2 electrons
group 2 reaction with oxygen
group 2 reaction with acids
group 2 reaction with water
down the group, solubility of hydroxides of group 2 elements:
increases
use of Mg(OH)₂
sold as indigestion remedy
use of Ca(OH)₂
limewater
treat agriculture to treat acidic soil
use of CaCO₃
indigestion remedy
group 2 oxide reaction with water
properties of the halogens
- diatomic molecules
- instantaneous dipole-induced dipole
down the group the boiling point of halogens: + why
increases because more electrons = stronger forces = more energy needed
down the group the electronegativity of halogens: + why
decreases because shielding increases so electrons less attracted so electronegativty decreases
what colour do the halogens go in water?
chlorine = pale green
bromine = orange-brown
iodine = brown
how to tell the difference between bromine and iodine solutions
add cyclohexane and iodine = deep violet
disproportionation reaction
when the same element is both oxidised and reduced
chlorine reaction with water + oxidation states
Cl = 0 in Cl
chlorine reaction with water + oxidation states
Cl = 0 in Cl₂
+1 in HClO
-1 in HCl
use of Chloric(I) acid
used as bleach or to kill bacteria due to oxidising properties
chlorine reaction with water in presence of sunlight
sodium chlorate reaction with water
chlorine reaction wtih diulte aq NaOH
