Inorganic Flashcards
Salt flame test colour
Lithium chloride
Red
Salt flame test colour
Sodium chloride
Yellow
Salt flame test colour
Potassium chloride
Lilac
Salt flame test colour
Barium Chloride
Green
Salt flame test colour
Calcium chloride
Orange red
Salt flame test colour
Strontium chloride
red
Salt flame test colour
Magnesium chloride
no colour
Salt flame test colour
Copper chloride
Blue-green
Salt flame test colour
Zinc chloride
Colourless
G2M reaction with oxygen
Burn in oxygen to form simple metal oxides
2X(s) + O2(g)—> 2XO(s)
G2M reaction with chlorine
Burn in chlorine gas to form solid metal chlorides
X(s) + Cl2(g) —> XCl2(s)
G2M reaction with water
Beryllium= no reaction due to thick oxide layer
Magnesium= slight reaction to cold water
Mg(s) + 2H2O(l) —> Mg(OH)2 (s) + H2 (g)
Reaction soon stops because magnesium hydroxide is almost insoluble in water and forms a barrier
Magnesium will react with steam to form metal hydroxide and hydrogen
Mg(s) + H2O(l)—>MgO(aq) + H2(g)
Other G2M react with cold water with increasing vigour to give metal hydroxide and hydrogen
Ca(s) + 2H2O(l)—>Ca(OH)2 (aq) + H2(g)
Oxides of G2M with water
MgO reacts slightly with water
CaO fizzes to form calcium hydroxide
Solubility of oxides in water increases down a group
Trend in solubility of G2M oxides down a group
Increases
Reaction of oxides of G2M with acids
React with dilute HCl to form chloride salt and water
React with dilute nitric acid to form nitrate salt and water
XO(s) + 2HNO3 (aq)—> X(NO3)2 (aq)
Reaction of G2M hydroxides with HCl and HNO3
React similarly to G2M oxides
X(OH)2 + 2HCl (aq) —> XCl2(aq) + 2H2O
Solubility of G2M hydroxides
Increases down group
Ionic radius increases so metal ions get larger so charge density decreases
Get a lower attraction between OH- and 2+ ions
Ions more easily split apart
Greater conc of OH- ions in water
Solubility of G2M sulfates
Decrease down group
Mg and Ca =soluble
Test for sulfate
Soluble Ba salt
Ba2+(aq) + (SO4)2 2- —> BaSO4 (s) white precip
General formula of G2M carbonates
MCO3
G2M carbonates solubility
Insoluble in water
Thermal decomposition of G2M carbonates
MCO3 (s) —> MO + CO2
Trend in thermal decomposition down G2M carbonates
increase down group, Harder down group= more thermally stable
General formula of G2M nitrates
M(NO3)2
G2M nitrates solubility in water
Soluble
Thermal decomposition of G2M nitrates
2M(NO3)2(s) —> 2MO(s) + 4NO2(g) + O2
Trend in thermal decomposition if G2M nitrates down group
increase down group, Becomes harder=more thermally stable
Thermal stability
Indicator of the ease with which compounds decompose on heating
factors deciding thermal stability of G2M carbonates and nitrates
-charge on metal ion
-size of metal ion
generally what is more stable G2M carbonates/nitrates, or G1M carbonates/nitrates
G1M compounds
effect of charge of metal ion on thermal stability
larger charge on metal ion=smaller ion=less stable
effect of size of metal ion on thermal stability
smaller ion=less stable
polarising power
the extent at which the positive ion can distort neighboring electron cloud
halide ions …. electrons and become ……. molecules. …… ions lose electrons more ……
lose
halogen
larger
easily
trend in reducing agent going down halide group
become better reducing agents as you go down
general half equation formula of oxidation of halides
2X- →X2 + 2e-
list the halides in order of worst to best reducing agent
Cl-
Br-
I-
reaction of halide
Cl- (chloride) salt with conc sulfuric acid H2SO4
white effervesence
which halide reaction involving chloride observes white effervescence
reaction of chloride salt and H2SO4 sulfuric acid
reaction of halide
Cl- (chloride) with indicator paper
orange=acidic
reaction of halide
Cl- (chloride) with conc ammonia
white fumes
Cl- dissolves dilute and conc ammonia
reaction of halide
Cl- (chloride) with lead acetate paper
no change, remains white because Cl- cannot reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)
reaction of halide
Cl- (chloride) with acidified dichromate solution
no change, remains yellow
Cl- cannot reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)
write the equation for sodium chloride salt with sulfuric acid
NaCl + H2SO4 → NaHSO4 + HCl
OS of sulfur remains at +6
not a redox reaction
reaction of halide
Br- (Bromide) salt with conc sulfuric acid H2SO4
yellow/orange effervescence
reaction of halide
Br- (Bromide) salt with indictor paper
red=acidic
reaction of halide
Br- (Bromide) salt with conc ammonia
white fumes, Br- dissolves CONC ammonia not dilute ammonia
reaction of halide
Br- (Bromide) salt with conc ammonia
white fumes, Br- dissolves CONC ammonia not dilute ammonia
reaction of halide
Br- (Bromide) salt with lead acetate paper
no change (white)
Br- is not a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)
reaction of halide
Br- (Bromide) salt with acidified dichromate solution
yellow to white
Br- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)
write 2 reactions, starting with sodium bromide with H2SO4 and then the redox. and the changes in OS of both bromine and sulfur
NaBR + H2SO4→NaHSO4 + HBr
2HBr + H2SO4→SO2 +2H2O + Br2
Bromine = -1→0
sulfur= +6→+4
reaction of halide
I- (iodide) salt with conc sulfuric acid H2SO4
brown/black/red effervescence
reaction of halide
I- (iodide) with indicator paper
red=acidic
reaction of halide
I- (iodide) with concentrated ammonia
no reaction
reaction of halide
I- (iodide) with lead acetate paper
white→brown
I- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)
reaction of halide
I- (iodide) with acidified dichromate
yellow → white
I- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)
write the 3 reactions iodide has to reduce the sulfur. initially start with NaI and H2SO4
NaI + H2SO4→ NaHSO4 + HI
2HI + H2SO4→SO2 + 2H2O + I2
6HI + SO2→H2S + 2H2O + 3I2
change in OS of sulfur when reacted with each halide salt
Cl- doesn’t reduce H2SO4
Br- reduces H2SO4 to SO2 (+6→+4)
I- reduces H2SO4 to SO2 and then to H2S (+6→+4→-2)
describe the test for halide ions
add sample to a test tube, add 3 drops dilute nitric acid, add 3 drops silver nitrate (get rid of carbonates) let mixture stand, should see an initial colour change.
Cl-=white
Br-=cream
I-=yellow
to help distinguish between these colours add ammonia
Cl-= dissolves dilute and conc
Br-=dissolves conc
I-=no reaction
testing for halogens
reaction of chlorine with bromide
cream
testing for halogens
reaction of chlorine with iodide
yellow/gold
testing for halogens
reaction of chlorine with hexane
colourless
testing for halogens
reaction of bromine with chloride
no change
testing for halogens
reaction of bromine with iodide
red
testing for halogens
reaction of bromine with hexane
orange
testing for halogens
reaction of iodine with chloride
no change
testing for halogens
reaction of iodine with bromide
no change
testing for halogens
reaction of iodine with hexane
brown with a purple layer
disproportionation definition
same element/species is reduced and oxidised at the same time
chlorine reaction with cold and dilute NaOH produces
sodium chlorate NaClO
sodium chloride
water
balanced equation of chlorine with cold and dilute NaOH
Cl2 (aq) + 2NaOH (aq) → NaClO (aq) + NaCl (aq) + H2O(l)
what is the change in oxidation state of chlorine in the reaction with cold and dilute NaOH
Cl2 (aq) + 2NaOH (aq) → NaClO (aq) + NaCl (aq) + H2O(l)
0 in Cl2
+1 in NaClO
-1 in NaCl
which product of chlorine with cold and dilute NaOH is an oxidising agent
sodium chlorate (i)
chlorine reaction with hot and dilute NaOH equation
3Cl2(g) + 6NaOH(aq)→ NaClO3(aq) + 5NaCl(aq) + 3H2O (l)
what are the products from the reaction of chlorine with hot and dilute NaOH
sodium chlorate (v)
sodium chloride
water
what reaction is this:
3Cl2(g) + 6NaOH(aq)→ NaClO3(aq) + 5NaCl(aq) + 3H2O (l)
reaction of chlorine with hot and dilute NaOH to produce sodium chlorate (v) and sodium chloride and water
write the equation of the reaction between chlorine and sunlight/water
2Cl2(g) + 2H2O(l)→4HCl(aq)+O2(g)
what reaction is this:
2Cl2(g) + 2H2O(l)→4HCl(aq)+O2(g)
reaction between chlorine and sunlight/water
ionic equation for reaction of chlorine (chloric acid) with water
HClO(aq)+H2O(l) ⇌ H+(aq) + ClO- (aq)
what happens during the reaction of chlorine (chloric acid) and water
chloric acid dissociates H+ and ClO-
what product of chlorin (chloric acid) with water is a strong reducing ion
ClO (kills algae and bacteria)
