Group 17 Elements Flashcards
What do halogens exist as at room temp
Diatomic molecules
Atomic radius _ down the grp because…
Increases
Energy levels are added
Mp and bp _ down the grp due to …
Increase
Van der waals forces increase between molecules as no of electrons increase hence a stronger attractive force harder to break
Volatility _ down the group because…
Ease with which they evaporate decreases
There’s ah increase in vanderwaals between diatomic molecules
Colour intensity _ going down the grp because…
Increases (get darker)
Halogens react with metals by _ and form a _
Gaining an electron
Ionic salt
Halogens are _ agents meaning
Oxidising
They get reduced by accepting an electron
Halogens react with non metals by _
Sharing an electron
What does electronegativity decrease down the grp
Fluorine has a small radius so outer shell receives a lot of nuclear charge since its near and there’s also less shielding so a new electron will be greatly attracted
So fluorine is a better OA than iodine
Displacement:
More reactive ie more electronegative halogen displaces less reactive one from a slide solution
Halogen + H2 gives?
Hydrogen halide gas
Reactivity _ down the grp
Decreases
How can hydrogen halide be decomposed
Insert a hot wire
Thermal stability of hydrogen halides going down
Decreases (F is most stable, I is least)
Hydrogen-halogen bond energy _ down the grp this is due to…
Decreases-easier to break
Overlap of halogen outer she’ll with hydrogen atom gives longer bonds down the group hence reducing the strength (this is why HI is least stable)
Test for presence of halide ions:
Add dil nitric acid and silver nitrate solution
Ppt formed
Results for AgNO3 test
Cl- white
Br-cream
I-yellow
Tests to further distinguish between Cl,Br,I
Dil ammonia:
Cl- dissolves, Br and I- insol
Conc ammonia:
Cl and Br- dissolve, I- insol
NaCl + H2SO4 ->
NAHSO4 (s) + HCl (g) fumes
Sulfuric acid doesn’t further oxidise hcl because
NaBr + H2SO4 ->
NAHSO4 (s) + HBr (g)
Further on H2SO4 reduced to SO2 and HBr oxidised to Br2 gas plus H2O as byproduct
2HBr + H2SO4 -> Br2 + SO2 + 2H2O
NaI + H2SO4 ->
H2SO4 reduced ro various products as it oxidises the HI produced
These include SO2, S, H2S
Iodine is produced as a purple vapour
Ease of hydrogen halide _ down grp
Increases
What is disproportionation
Cl2 when reacted with dil alkali sol
It is a self oxi/red reaction
Depends on temp
Cl2 in cold alkali: 15°C products are nacl+naclo+h20
Cl is reduced and it’s oxidation becomes 0->-1 gains an electron
0.5Cl2 +e- -> Cl-
Also oxidised to form ClO- it’s oxidation state becomes +1 as
0.5Cl2+2OH- ->ClO-+H2O+e-
Cl2 in hot alkali: 70°C products same as for cold but oxi/red nos diff…
3Cl2 + 6NaOH -> 5NaCl +NaClO3 +3H2O
so Cl2 oxi state 0 reduced to +5 and oxidsed to -1
Uses of chlorine
- kills bacteria in water ie the HCl and HClO do so as Cl2 + H20 oxidation to them
- bleach a mixture of nacl and naclo. Oxygen atoms from chlorate ions oxidise dye
- organic compounds such as pvc and halogenated hydrocarbons used as solvents, refrigerants and aerosols