Formula list form 4
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Chemical formulae, equations, calculations, and reactions are summarized. Molar mass, moles, volume, and molarity calculations are explained for gases, solids, liquids, and solutions. Common cationic and anionic symbols are listed. Formulae for common compounds are provided. Group 1 and 17 elements and their reactions are summarized. Electrochemistry concepts like electrolytes, ionization, and the discharge of ions are condensed. Acid-base reactions and properties are highlighted at a high level. Solubility, preparation, color, and the effect of heating on salts are briefly touched upon.
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Heating effect on Salt
Heating
Effect
CO3
2-
NO3
-
SO4
2-
Cl-
Most Probably
Release CO2
Most Probably
Release NO2
Most Probably
Release SO3
Most Probably
No effect
Heating Effect on Carbonate Salt
Carbonate Salt Equation of The Reaction
Potassium carbonate
Sodium carbonate
Not decomposible
Calcium carbonate
Magnesium carbonate
Aluminium carbonate
Zinc carbonate
Iron (III) carbonate
Lead(II) carbonate
Copper(II) carbonate
CaCO3 ⎯→ CaO + CO2
MgCO3 ⎯→ MgO + CO2
Al2(CO3)3 ⎯→ Al2O3 + 3CO2
ZnCO3 ⎯→ ZnO + CO2
Fe2(CO3)3⎯→ Fe2O3 + 3CO2
PbCO3 ⎯→ PbO + CO2
CuCO3 ⎯→ CuO + CO2
Mercury(II) carbonate
Silver(I) carbonate
2HgCO3 ⎯→ 2Hg + 2CO2 + O2
2Ag2CO3 ⎯→ 4Ag + 2CO2 + O2
Ammonium carbonate (NH4)2CO3 ⎯→ NH3 + CO2 + H2O
Heating Effect on Nitrate Salt
Nitrate Salt Equation of The Reaction
Potassium nitrate
Sodium nitrate
2KNO3 ⎯→ 2KNO2 + O2
2NaNO3 ⎯→ 2NaNO2 + O2
Calcium nitrate
Magnesium nitrate
Aluminium nitrate
Zink nitrate
Iron (III) nitrate
Lead(II) nitrate
Copper(II) nitrate
2Ca(NO3)2 ⎯→ 2CaO + 4NO2 + O2
Mg(NO3)2 ⎯→ 2MgO + 4NO2 + O2
4Al(NO3)3 ⎯→ 2Al2O3 + 12NO2 + 3O2
Zn(NO3)2 ⎯→ 2ZnO + 4NO2 + O2
4Fe(NO3)3⎯→ 2Fe2O3 + 12NO2 + 3O2
Pb(NO3)2 ⎯→ 2PbO + 4NO2 + O2
Cu(NO3)2 ⎯→ 2CuO + 4NO2 + O2
Mercury(II) nitrate
Silver(I) nitrate
Hg(NO3)2 ⎯→ Hg + 2NO2 + O2
2AgNO3 ⎯→ 2Ag + 2NO2 + O2
Ammonium nitrate NH4NO3 ⎯→ N2O + 2H2O
[NOTES: Nitrogen dioxide, NO2 is acidic gas and is brown in colour.]
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Formula list form 4
- 1. ONE-SCHOOL.NET Short Notes: Form 4 ChemistryShort Notes: Form 4 Chemistry Chemical Formulae and EquationChemical Formulae and Equation CalculationCalculation SummarySummary × molar volume÷ molar volume × molar mass Avogadro Constant Number of particles Mole of particles Mass of particle (in gram) × Avogadro Constant÷ molar mass Volume of Gas For Solid, liquid or gas mass of subtance number of mole = molar mass Molar mass = RAM/RMM/RFM in gram For gas (only) volume of gas number of mole = molar volme Molar volume = 24dm3 at room temperature Molar volume = 22.4dm3 at s.t.p. For Solution MV number of mole = 1000 M = molarity V = Volume of solution in cm3 For quantity of particle(atom,molecule,ion) 23 quantity of particle number of mole = 6.02 10× http://one-school.net/notes.html 1
- 2. ONE-SCHOOL.NET Chemical Formula Cation (Positive Ions) Ion Symbol Ion Symbol Ion Symbol Potassium K+ Calcium Ca2+ Aluminium Al3+ Sodium Na+ Magnesium Mg2+ Iron (III) Fe3+ Lithium Li+ Zinc Zn2+ Chromium(III) Cr3+ Hydrogen H+ Barium Ba2+ Argentums(I) Ag+ Iron (II) Fe2+ Mercury(I) Hg+ Tin (II) Sn2+ Ammonium NH4 + Lead(II) Pb2+ Copper(II) Cu2+ Manganese(II) Mn2+ Anion (Negative Ions) Ion Symbol Ion Symbol Ion Symbol Oxide O2- Hydroxide OH- Ethanoate CH3COO- Fluoride F- Sulphate SO4 2- Manganate(VII) MnO4 - Chloride Cl- Nitrate NO3 - Dichromate(VI) Cr2O7 2- Bromide Br- Carbonate CO3 2- Phosphate PO4 3- Iodide I- Thiosulphate S2O3 2- Formulae for Certain Molecule Karbon monoxide CO Ammonia NH3 Carbon dioxide CO2 water H2O Nitrogen monoxide NO Hydrogen chloride HCl Nitrogen dioxide NO2 Tetrachloromethane CCl4 Sulphur dioxide SO2 Glucose C6H12O6 Sulphur trioxide SO3 Hydrogen bromide HBr Fluorine F2 Hydrogen iodide HI Bromine Br2 Hydrogen sulphide H2S Chlorine Cl2 Ethanol C2H5OH Iodine I2 Ethanoic Acid CH3COOH http://one-school.net/notes.html 2
- 3. ONE-SCHOOL.NET Periodic Table Reaction of Group 1 Elements 1. Reaction with Oxygen The entire group 1 metal can react with oxygen to form metal oxide. 4Li + O2 ⎯→ 2Li2O 4Na + O2 ⎯→ 2Na2O 4K + O2 ⎯→ 2K2O The metal oxide of group 1 elements can dissolve in water to form alkali (hydroxide) solution Li2O + H2O ⎯→ 2LiOH Na2O + H2O ⎯→ 2NaOH K2O + H2O ⎯→ 2KOH 2. Reaction with halogen (Chlorine) 2Li + Cl2 ⎯→ 2LiCl 2Na + Cl2 ⎯→ 2NaCl 2K + Cl2 ⎯→ 2KCl 3. Reaction with water The entire group 1 metal can react with water to produce alkali (hydroxide) solution and hydrogen gas. 2Li + 2H2O ⎯→ 2LiOH + H2 2Na + 2H2O ⎯→ 2NaOH + H2 2K + 2H2O ⎯→ 2KOH + H2 Reaction of Group 17 Elements 1. React with water Cl2 + H2O ⎯→ HCl + HOCl Br2 + H2O ⎯→ HBr + HOBr I2 + H2O ⎯→ HI + HOI 2. React with Sodium Hydroxide Cl2 + 2NaOH ⎯→ NaCl + NaOCl + H2O Br2 + 2NaOH ⎯→ NaBr + NaOBr + H2O I2 + 2NaOH ⎯→ NaI + NaOI + H2O 3. React with Iron 3Cl2 + 2Fe ⎯→ 2FeCl3 3Br2 + 2Fe ⎯→ 2FeBr3 3I2 + 2Fe ⎯→ 2FeI3 Preparation of Chlorine Gas 2KMnO4 + 16HCl ⎯→ 2KCl + 2MnCl2 + 5Cl2 + 8H2O http://one-school.net/notes.html 3
- 4. ONE-SCHOOL.NET Electrochemistry Electrolyte Ionisation of Electrolyte Ionisation of Molten Compound PbBr2 ⎯→ Pb2+ + Br- NaCl ⎯→ Na+ + Cl- Al2O3 ⎯→ 2Al3+ + 3O2- Ionisation of Aqueous Solution NaCl ⎯→ Na+ + Cl- H2O ⎯→ H+ + OH- HCl ⎯→ H+ + Cl- H2O ⎯→ H+ + OH- CuSO4 ⎯→ Cu2+ + SO4 2- H2O ⎯→ H+ + OH- Discharge of Positive Ion Discharge of Negative Ion Na+ + e ⎯→ Na Observation: Grey deposit is formed. Al3+ + 3e ⎯→ Al Observation: Grey deposit is formed. Pb2+ + 2e ⎯→ Pb Observation: Grey deposit is formed. Cu2+ + 2e ⎯→ Cu Observation: Brown deposit is formed. Ag+ + e ⎯→ Ag Observation: Silver deposit is formed. 2H+ + 2e ⎯→ H2 Observation: Gas bubble is formed. A ‘pop’ sound is produced when a lighted splinter is placed near the mouth of the test tube. 2Cl- ⎯→ Cl2 + 2e Observation: Bubbles of pungent yellowish green gas are produced. The gas turns moist litmus paper to red and then bleaches it. 2Br- ⎯→ Br2 + 2e Observation: Molten electrolyte: Brown colour gas is produced. Aqueous solution: Light brown solution is formed. 2I- ⎯→ I2 + 2e Observation: Molten electrolyte: Brown colour gas is produced. Aqueous solution: Light brown solution is formed. The solution turns blue when a few drops of starch solution is added in. 4OH- ⎯→ O2 + 2H2O + 4e Observation: Gas bubble is formed. Gas produces light up a wooden splinter. http://one-school.net/notes.html 4
- 5. ONE-SCHOOL.NET Acid and Base Ionisation of Acid Hydrochloric Acid HCl ⎯→ H+ + Cl- HCl + H2O ⎯→ H3O+ + Cl- Nitric Acid HNO3 ⎯→ H+ + NO3 - HNO3 + H2O ⎯→ H3O+ + NO3 - Sulphuric Acid H2SO4 ⎯→ H+ + SO4 2- H2SO4 + 2H2O ⎯→ 2H3O+ + SO4 2- Ethanoic Acid CH3COOH ⎯→ H+ + CH3COO- CH3COOH + H2O ⎯→ H3O+ + CH3COO- Chemical Properties of Acid Acid + Reactive Metal ⎯→ Salt + H2 Example: 2HCl + Zn ⎯→ ZnCl2 + H2 6HNO3 + 2Fe ⎯→ 2Fe(NO3)3 + 3H2 H2SO4 + Pb⎯→ PbSO4 + H2 6CH3COOH + 2Al ⎯→ 2Al(CH3COO)3 + 3H2 Acid + Metal Oxide⎯→ Salt + H2O Example: 2HCl + ZnO ⎯→ ZnCl2 + H2O 2HNO3 + MgO ⎯→ Mg(NO3)2 + H2O H2SO4 + CuO ⎯→ CuSO4 + H2O 2CH3COOH + Na2O ⎯→ 2CH3COO- Na+ + H2O Acid + Metal Hydroxide⎯→ Salt + H2O Example: 2HCl + Ca(OH)2 ⎯→ CaCl2 + 2H2O HNO3 + NaOH⎯→ NaNO3 + H2O H2SO4 + 2NH4OH ⎯→ (NH4)2SO4 + 2H2O or H2SO4 + 2NH3 ⎯→ (NH4)2SO4 CH3COOH + KOH ⎯→ CH3COO- K+ + H2O Acid + Metal Carbonate ⎯→ Salt + CO2 + H2O Example: 2HCl + ZnCO3 ⎯→ ZnCl2 + CO2 + H2O 2HNO3 + CaCO3 ⎯→ Ca(NO3)2 + CO2 + H2O H2SO4 + Na2CO3 ⎯→ Na2SO4 + CO2 + H2O 2CH3COOH + MgCO3 ⎯→ Mg(CH3COO)2 + CO2 + H2O http://one-school.net/notes.html 5
- 6. ONE-SCHOOL.NET Salt Solubility of Salt Salt Solubility Salt of potassium, sodium and ammonium All are soluble in water Salt of nitrate All are soluble in water Salt of sulphate Mostly soluble in water except: (Pb) Lead sulphate (Ba) Barium sulphate (Ca) Calcium sulphate Salt of chloride Mostly soluble in water except: (Pb) Lead chloride (Ag) silver chloride (Hg) mercury chloride Salt of carbonate Mostly insoluble in water except: Potassium carbonate Sodium carbonate Ammonium carbonate Oxide and Hydroxide Solubility Oxide Mostly insoluble in water except: K2O and Na2O. Hydroxide Mostly insoluble in water except: NH4OH, KOH and NaOH Preparation of Salt Preparation of Soluble Salt Salt of Potassium, Sodium and Ammonium Acid + Alkali ⎯→ Salt + Water Example: Preparation of Sodium Chloride (NaCl) HCl + NaOH ⎯→ NaCl + H2O Salt of non-Potassium, Sodium and Ammonium Acid + Reactive metal ⎯→ Salt + Hydrogen Gas Acid + Metal Oxide ⎯→ Salt + Water Acid + Metal Carbonate ⎯→ Salt + Water + Carbon Dioxide Example: Preparation of Zinc Sulphate (ZnSO4) H2SO4 + Zn ⎯→ ZnSO4 + H2 H2SO4 + ZnO ⎯→ ZnSO4 + H2O H2SO4 + ZnCO3 ⎯→ ZnSO4 + H2O + CO2 http://one-school.net/notes.html 6
- 7. ONE-SCHOOL.NET Preparation of Insoluble Salt Ionic Precipitation Insoluble salts can be made by double decomposition. This involves mixing a solution that contains its positive ions with another solution that contains its negative ions. Example: Preparation of Silver Nitrate AgNO3 (aq) + NaCl (aq) ⎯→ AgCl (s) + NaNO3 (aq) Ag+ (aq) + C1- (aq) ⎯→ AgCl (s) (ionic equation) Colour of Salt Salt or metal oxide Solid Aqueous solution Salt of: Sodium, Calcium, Magnesium, Aluminium, zinc, Lead, ammonium Chloride, sulphate, nitrate, carbonate White Colourless Salt of Copper(II).- Copper(II) Carbonate Green Insoluble Copper(II) sulphate, Copper(II) nitrate, Copper(II) chloride Blue Blue Copper(II) oxide Black Insoluble Salt of Iron (II) Iron(II) sulphate; Iron(II) nitrate; Iron(ID chloride Green Green Salt of Iron (III). Iron(III) sulphate; Iron(III) nitrate; Iron(III) chloride Brown Brown Lead Iodide Yellow Insoluble Lead Chloride White Insoluble Zink oxide Yellow when it is hot and white when it is cold. Insoluble Lead(II) oxide- Brown when it is hot and yellow when it is cold. Insoluble Magnesium oxide, Aluminium oxide White Insoluble Potassium oxide, Sodium oxide, Calcium oxide White Colourless http://one-school.net/notes.html 7
- 8. ONE-SCHOOL.NET Heating effect on Salt Heating Effect CO3 2- NO3 - SO4 2- Cl- Most Probably Release CO2 Most Probably Release NO2 Most Probably Release SO3 Most Probably No effect Heating Effect on Carbonate Salt Carbonate Salt Equation of The Reaction Potassium carbonate Sodium carbonate Not decomposible Calcium carbonate Magnesium carbonate Aluminium carbonate Zinc carbonate Iron (III) carbonate Lead(II) carbonate Copper(II) carbonate CaCO3 ⎯→ CaO + CO2 MgCO3 ⎯→ MgO + CO2 Al2(CO3)3 ⎯→ Al2O3 + 3CO2 ZnCO3 ⎯→ ZnO + CO2 Fe2(CO3)3⎯→ Fe2O3 + 3CO2 PbCO3 ⎯→ PbO + CO2 CuCO3 ⎯→ CuO + CO2 Mercury(II) carbonate Silver(I) carbonate 2HgCO3 ⎯→ 2Hg + 2CO2 + O2 2Ag2CO3 ⎯→ 4Ag + 2CO2 + O2 Ammonium carbonate (NH4)2CO3 ⎯→ NH3 + CO2 + H2O Heating Effect on Nitrate Salt Nitrate Salt Equation of The Reaction Potassium nitrate Sodium nitrate 2KNO3 ⎯→ 2KNO2 + O2 2NaNO3 ⎯→ 2NaNO2 + O2 Calcium nitrate Magnesium nitrate Aluminium nitrate Zink nitrate Iron (III) nitrate Lead(II) nitrate Copper(II) nitrate 2Ca(NO3)2 ⎯→ 2CaO + 4NO2 + O2 Mg(NO3)2 ⎯→ 2MgO + 4NO2 + O2 4Al(NO3)3 ⎯→ 2Al2O3 + 12NO2 + 3O2 Zn(NO3)2 ⎯→ 2ZnO + 4NO2 + O2 4Fe(NO3)3⎯→ 2Fe2O3 + 12NO2 + 3O2 Pb(NO3)2 ⎯→ 2PbO + 4NO2 + O2 Cu(NO3)2 ⎯→ 2CuO + 4NO2 + O2 Mercury(II) nitrate Silver(I) nitrate Hg(NO3)2 ⎯→ Hg + 2NO2 + O2 2AgNO3 ⎯→ 2Ag + 2NO2 + O2 Ammonium nitrate NH4NO3 ⎯→ N2O + 2H2O [NOTES: Nitrogen dioxide, NO2 is acidic gas and is brown in colour.] http://one-school.net/notes.html 8
- 9. ONE-SCHOOL.NET Heating effect on sulphate salt The heating effect on chloride salts Most sulphate salts do not decompose by heat. Only certain sulphate salts are decomposed by heat when heated strongly. Zinc sulphate, Copper (II) sulphate, Iron (III) sulphate ZnSO4 ⎯→ ZnO + SO3 CuSO4 ⎯→ CuO + SO3 2Fe2(SO4)3⎯→ Fe2O3 + SO2 + SO3 Ammonium sulphate (NH4)2SO4 ⎯⎯→ 2NH3 + H2SO4 All chloride salts are not decomposable by heat except ammonium chloride. Example: NH4Cl ⎯→ NH3 + HCl Identification of Gases Gasses Characteristics Oxygen Rekindle glowing splinter. Hydrogen Explode with a ‘pop’ sound when brought close to a lighted splinter. Carbon Dioxide Turns lime water chalky. Chlorine Bleach moist litmus paper. Ammonia Pungent smell. Turn moist red litmus paper to blue. Produces white fume when reacts with concentrated hydrochloric Acid. Sulphur Dioxide Pungent smell. Bleach the purple colour of potassium manganate(VII). Turn moist blue litmus paper to red. Nitrogen Dioxide Pungent smell. Brown in colour. Turn moist blue litmus paper to red. Qualitative analysis Identification of Anions (Negative ions) Diluted HCl or diluted HNO3 or diluted H2SO4 BaCl (aq) or Ba(NO3)2 (aq) follow by diluted HCl/HNO3 AgNO3 follow by diluted HNO3. Brown Ring Test ( + FeSO4 (aq ) + concentratedH2SO4 CO3 2- Carbon Dioxide is released. White precipitate is formed. It is soluble in diluted HCl/HNO3 White precipitate is formed. It is soluble in diluted HNO3 - SO4 2- - White precipitate is formed. It is NOT soluble in diluted HCl/HNO3 - - Cl- - - White precipitate is formed. It is NOT soluble in diluted HNO3 - NO3 - - - - Formation of Brown Ring http://one-school.net/notes.html 9
- 10. ONE-SCHOOL.NET Idendification of cation NaOH(ak) NH3(ak) HCl or NaCl H2SO4 or Na2SO4 Na2CO3 KI Na+ Ca2+ White precipitate. White precipitate is produced. White precipitate is produced. Mg2+ White precipitate is produced. White precipitate is produced. White precipitate is produced. Al3+ White precipitate is produced. Dissolve in excess NaOH solution. White precipitate is produced. . White precipitate is produced. Zn2+ White precipitate is produced. Dissolve in excess NaOH solution. White precipitate is produced. Dissolve in excess NH3 solution. White precipitate is produced. Pb2+ White precipitate is produced. Dissolve in excess NaOH solution. White precipitate is produced. White precipitate is produced. Dissolve in hot water White precipitate is produced. White precipitate is produced. Yellow precipitate is produced. Dissolve in hot water Fe2+ Dirty green precipitate is produced. Dirty green precipitate is produced. Green precipitate is produced. Fe3+ Red brown precipitate is produced. Red brown precipitate is produced. Brown precipitate is produced. A red brown solution formed. Cu2+ Blue precipitate is produced. Blue precipitate is produced. Dissolve in excess NH3 solution and form a blue solution. Blue precipitate is produced. White precipitate form in brown solution NH4 + = No changes is observed http://one-school.net/notes.html 10
- 11. ONE-SCHOOL.NET Distibguish Iron(II) and Iron(III) Reagent Observation Ion presents Light blue precipitate Fe2+ Solution of potassium hecxacianoferate(II) Dark Blue precipitate Fe3+ Dark blue precipitate Fe2+ Solution of potassium hecxacianoferate(III) Greenish brown solution Fe3+ Pinkish solution Fe2+ Solution of potassium Thiocyanate(II) Blood red solution Fe3+ Manufactured Substances in Industry Contact Process (Making Sulphuric Acid) Stage 1: Formation of SO2 Combustion of Sulphur S (s) + O2 (g) ⎯⎯→ SO2 (g) or Heating of metal sulphide such as lead(II) sulphide 2PbS(s) + 3O2(g) ⎯⎯→ 2PbO(s) + 2SO2(g) or Combustion of hiydrogen sulphide 2H2S(g) + 3O2(g) ⎯⎯→ 2SO2(g) + 2H2O(ce) Stage 2: Formation of SO3 2SO2 (g) + O2 (g) ⎯⎯→ 2SO3 (g) Catalyst: vanadium(V) oxide Temperature: 450°C Pressure: 2-3 atmospheres Stage 3 Formation of oleum H2S2O7 SO3(g) + H2SO4(aq) ⎯⎯→ H2S2O7(l) Stage 4:Formation of Sulphuric acid H2S207 (1) + H2O (1) ⎯⎯→ 2H2SO4(aq) http://one-school.net/notes.html 11
- 12. ONE-SCHOOL.NET Haber Process (Making Ammonia) Sources of the raw material Hydrogen 1. Reaction between steam and heated coke H2O + C ⎯→ CO + H2 2. Reaction between steam and natural gas. 2H2O + CH4 ⎯→ CO2 + 4H2 Nitrogen From distillation of liquid air. The reaction 1. Ammonia is made by the Haber process from nitrogen and hydrogen: N2(g) + 3H2(g) ⎯→ 2NH3(g); ΔH = -92 kJ mo1-1 Catalyst: Iron Promoter: Aluminium oxide Temperature: 450 °C Pressure: 200-1000 atm http://one-school.net/notes.html 12