Inorganic Flashcards by millie west

Salt flame test colour
Lithium chloride

Red

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Salt flame test colour
Sodium chloride

Yellow

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Salt flame test colour
Potassium chloride

Lilac

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Salt flame test colour
Barium Chloride

Green

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Salt flame test colour
Calcium chloride

Orange red

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Salt flame test colour
Strontium chloride

red

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Salt flame test colour
Magnesium chloride

no colour

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Salt flame test colour
Copper chloride

Blue-green

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Salt flame test colour
Zinc chloride

Colourless

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G2M reaction with oxygen

Burn in oxygen to form simple metal oxides
2X(s) + O2(g)—> 2XO(s)

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G2M reaction with chlorine

Burn in chlorine gas to form solid metal chlorides
X(s) + Cl2(g) —> XCl2(s)

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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)

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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

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Trend in solubility of G2M oxides down a group

Increases

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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)

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Reaction of G2M hydroxides with HCl and HNO3

React similarly to G2M oxides
X(OH)2 + 2HCl (aq) —> XCl2(aq) + 2H2O

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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

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Solubility of G2M sulfates

Decrease down group
Mg and Ca =soluble

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Test for sulfate

Soluble Ba salt
Ba2+(aq) + (SO4)2 2- —> BaSO4 (s) white precip

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General formula of G2M carbonates

MCO3

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G2M carbonates solubility

Insoluble in water

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Thermal decomposition of G2M carbonates

MCO3 (s) —> MO + CO2

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Trend in thermal decomposition down G2M carbonates

increase down group, Harder down group= more thermally stable

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General formula of G2M nitrates

M(NO3)2

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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)