Chem Formula List

8/6/2019 Chem Formula List

1/12

Short Notes: Form 4 ChemistryChemical Formulae and Equation

CalculationFor Solid, liquid orgas

number of mole =

mass of subtance

molar mass

For gas (only)

volume of gasnumber of mole =

molar volme

Molar mass = RAM/RMM/RFM in gram

For Solution

MV

Molar volume = 24dm3 at room temperature

Molar volume = 22.4dm3 at s.t.p.

For quantity of particle(atom,molecule,ion)

quantity of particlenumber of mole =

M = molarity

V = Volume of solution in cm3

1000number of mole =23

6.0210

Summary

molar mass Avogadro Constant

Mass of particleMole ofNumber of(in gram)particlesparticles

molar massAvogadro Constant

molar volume molar volume

Volume ofGas

1


2/12

Chemical Formula

Cation (Positive Ions)

Ion SymbolIonSymbolIon SymbolPotassium K+ CalciumCa2+ Aluminium Al3+

Sodium Na+ MagnesiumMg2+ Iron (III) Fe3+

Lithium Li+ Zinc Zn2+ Chromium(III) Cr3+

HydrogenH+ BariumBa2+

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 SymbolIonSymbolIon Symbol

Oxide O2- HydroxideOH- EthanoateCH3COO-

FluorideF-Sulphate SO42-Manganate(VII) MnO4-

Chloride Cl-NitrateNO3-Dichromate(VI)Cr2O72-

Bromide Br-Carbonate CO32- Phosphate PO43-

Iodide I-Thiosulphate S2O32-

Formulae for Certain Molecule

Karbon monoxide COAmmoniaNH3Carbon dioxide CO2 waterH2O

Nitrogen monoxideNO Hydrogen chlorideHClNitrogen dioxideNO2TetrachloromethaneCCl4Sulphur dioxideSO2 GlucoseC6H12O6Sulphur trioxide SO3 Hydrogen bromide HBrFluorineF2Hydrogen iodideHIBromine Br2 Hydrogen sulphide H2S

Chlorine Cl2Ethanol C2H5OHIodine I2 Ethanoic AcidCH3COOH

2


3/12

Periodic TableReaction of Group 1 Elements

1. Reaction with Oxygen

The entire group 1 metal can react with oxygen to form metal oxide.4Li + O2 2Li 2O

4Na + O2 2Na 2O

4K + O2 2K 2O

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 waterThe entire group 1 metal can react with water to produce alkali (hydroxide) solution and hydrogen gas.

2Li + 2H2O 2LiOH + H 2

2Na + 2H2O 2NaOH + H 2

2K + 2H2O 2KOH + H

2

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 +H2OBr2 + 2NaOH NaBr + NaOBr +H2OI2 + 2NaOH NaI + NaOI + H2O

3. React with Iron

3Cl2 + 2Fe 2FeCl 3

3Br2 + 2Fe 2FeBr 3

3I2 + 2Fe 2FeI 3

Preparation of Chlorine Gas

2KMnO4 + 16HCl 2KCl + 2MnCl 2 + 5Cl2 + 8H2O

3


4/12

Electrochemistry

Electrolyte

Ionisation of ElectrolyteIonisation of Molten Compound

PbBr2 Pb2+ + Br-

NaCl Na + + Cl-

Al2O3 2Al3+ + 3O2-

Ionisation of Aqueous Solution

NaCl Na + + Cl-HCl H + + Cl- CuSO4 Cu2+ + SO42-

H2

O H

+

+ OH

-

H2

O H

+

+ OH

-

H2

O H

+

+ OH

-

Discharge of Positive Ion

Na+ + e NaObservation: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 AgObservation:Silver deposit is formed.

2H+ + 2e H 2Observation:Gas bubble is formed. A pop sound is produced

when a lighted splinter is placed near the mouth of

the test tube.

Discharge of Negative Ion

2Cl- Cl 2 + 2eObservation:Bubbles of pungent yellowish green gas are

produced. The gas turns moist litmus paper to red

and then bleaches it.

2Br- Br 2 + 2eObservation:Molten electrolyte:

Brown colour gas is produced.

Aqueous solution:

Light brown solution is formed.

2I- I 2 + 2eObservation: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- O 2 + 2H2O + 4eObservation:Gas bubble is formed. Gas produces light up awooden splinter.

4


5/12

Acid and BaseIonisation of Acid

Hydrochloric AcidSulphuric Acid

HCl H

+ + Cl- H2SO4 H

+ + SO42-HCl + H2O H 3O

+ + Cl- H2SO4 + 2H2O 2H 3O+ + SO42-

Nitric Acid

HNO3 H + + NO3-Ethanoic Acid

HNO3 + H2O H 3O+ + NO3- CH3COOH H+ + CH3COO

-

CH3COOH + H2O H 3O+ + CH3COO

-

Chemical Properties of Acid

Acid + Reactive Metal Salt + H2Example:

2HCl + Zn ZnCl 2 + H26HNO3 + 2Fe 2Fe(NO 3)3 + 3H2H2SO4 + Pb PbSO 4 + H26CH3COOH + 2Al 2Al(CH 3COO)3 + 3H2

Acid + Metal Oxide

Salt + H2OExample:

2HCl + ZnO ZnCl 2 + H2O

2HNO3 + MgO Mg(NO 3)2 + H2O

H2SO4 + CuO CuSO 4 + H2O

2CH3COOH + Na2O 2CH 3COO-Na++ H2O

Acid + Metal Hydroxide Salt + H2OExample:

2HCl + Ca(OH)2 CaCl

2 + 2H2OHNO3 + NaOH NaNO 3 + H2O

H2SO4 + 2NH4OH (NH 4)2SO4 + 2H2O or H2SO4 + 2NH3 (NH 4)2SO4CH3COOH + KOH CH 3COO

-K+ + H2O

Acid + Metal Carbonate Salt + CO2 + H2OExample:

2HCl + ZnCO3 ZnCl 2 + CO2 + H2O

2HNO3 + CaCO3 Ca(NO 3)2 + CO2 + H2O

H2SO4 + Na2CO3 Na

2SO4 + CO2 + H2O2CH3COOH + MgCO3 Mg(CH 3COO)2 + CO2 + H2O

5


6/12

SaltSolubility of Salt

Salt Solubility

Salt of potassium, sodium and ammoniumAll are solublein waterSalt of nitrateAll aresolublein waterSalt of sulphateMostlysolublein water except:

(Pb) Lead sulphate(Ba) Barium sulphate(Ca) Calcium sulphate

Salt of chlorideMostlysoluble in water except:(Pb) Lead chloride(Ag) silver chloride(Hg) mercury chloride

Salt of carbonateMostly insolublein water except:

Potassium carbonateSodium carbonate

Ammonium carbonate

Oxide and HydroxideSolubilityOxideMostly insolublein water except: K2O and Na2O.HydroxideMostly insolublein 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 + H 2O

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 ZnSO 4 + H2

H2SO4 + ZnO ZnSO 4 + H2O

H2SO4 + ZnCO3 ZnSO 4 + H2O + CO2


7/12

Preparation of Insoluble Salt

Ionic PrecipitationInsoluble 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)

Colour of Salt

Salt or metal oxideSalt of:

Sodium, Calcium, Magnesium, Aluminium, zinc,Lead, ammonium

Chloride, sulphate, nitrate, carbonate

Salt of Copper(II).-Copper(II) Carbonate

Copper(II) sulphate, Copper(II) nitrate, Copper(II)

chloride

Copper(II) oxide

Salt of Iron (II)Iron(II) sulphate; Iron(II) nitrate; Iron(ID chloride

Salt of Iron (III).

Iron(III) sulphate; Iron(III) nitrate; Iron(III)

chloride

Lead Iodide

Lead Chloride

(ionic equation)

Solid

White

Green

Blue

Black

Green

Brown

Yellow

White

Aqueous solution

Colourless

Insoluble

Blue

Insoluble

Green

Brown

Insoluble

Insoluble

Zink oxide

Lead(II) oxide-

Magnesium oxide, Aluminium oxide

Potassium oxide, Sodium oxide, Calcium oxide

Yellow when it is hot and

white when it is cold.

Brown when it is hot and

yellow when it is cold.

White

White

Insoluble

Insoluble

Insoluble

Colourless

6


8/12

Heating effect on Salt

HeatingEffect

CO32- NO3- SO42- Cl-

Most Probably Most ProbablyMost ProbablyMost ProbablyRelease CO2 Release NO2 Release SO3 No effect

Heating Effect on Carbonate SaltCarbonate Salt Equation of The Reaction

Potassium carbonate Not decomposibleSodium carbonate

CaCO3 CaO + CO 2Calcium carbonate

Magnesium carbonate

Aluminium carbonate

Zinc carbonate

Iron (III) carbonate

Lead(II) carbonate

Copper(II) carbonate

Mercury(II) carbonate

Silver(I) carbonate

Ammonium carbonate

MgCO3 MgO + CO

2

Al2(CO3)3 Al 2O3 + 3CO2

ZnCO3 ZnO + CO 2Fe2(CO3)3 Fe 2O3 + 3CO2PbCO3 PbO + CO 2CuCO3 CuO + CO 2

2HgCO3 2Hg + 2CO 2 + O22Ag2CO3 4Ag + 2CO 2 + O2

(NH4)2CO3 NH 3 + CO2 + H2O

Heating Effect on Nitrate SaltNitrate SaltPotassium nitrate

Sodium nitrate

Calcium nitrate

Magnesium nitrateAluminium nitrate

Zink nitrate

Iron (III) nitrate

Lead(II) nitrate

Copper(II) nitrate

Mercury(II) nitrate

Silver(I) nitrate

Ammonium nitrate

Equation of The Reaction

2KNO3 2KNO 2 + O22NaNO3 2NaNO 2 + O2

2Ca(NO3)2 2CaO + 4NO 2 + O2

Mg(NO3)2 2MgO + 4NO 2 + O2

4Al(NO3)3 2Al 2O3 + 12NO2 + 3O2

Zn(NO3)2 2ZnO + 4NO 2 + O2

4Fe(NO3)3 2Fe 2O3 + 12NO2 + 3O2

Pb(NO3)2 2PbO + 4NO 2 + O2

Cu(NO3)2 2CuO + 4NO 2 + O2

Hg(NO3)2 Hg + 2NO 2 + O2

2AgNO3 2Ag + 2NO 2 + O2

NH4NO3 N 2O + 2H2O

[NOTES: Nitrogen dioxide, NO2 is acidic gas and is brown in colour.]

7


9/12

Heating effect on sulphate saltMost 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)

sulphateZnSO4 ZnO + SO 3CuSO4 CuO + SO 32Fe2(SO4)3 Fe 2O3 + SO2 + SO3

Ammonium sulphate

(NH4)2SO4 2NH 3 + H2SO4

The heating effect on chloride saltsAll chloride salts are not decomposable by heat

except ammonium chloride.

Example:

NH4Cl NH 3 + HCl

Identification of GasesGassesOxygen

Hydrogen

Carbon Dioxide

Chlorine

Ammonia

Sulphur Dioxide

Nitrogen Dioxide

Qualitativeanalysis

CharacteristicsRekindle glowing splinter.

Explode with a pop sound when brought close to a lighted splinter.

Turns lime water chalky.

Bleach moist litmus paper.

Pungent smell.

Turn moist red litmus paper to blue.

Produces white fume when reacts with concentrated hydrochloric Acid.

Pungent smell.

Bleach the purple colour of potassium manganate(VII).

Turn moist blue litmus paper to red.

Pungent smell.Brown in colour.

Turn moist blue litmus paper to red.

Identification of Anions (Negative ions)

Diluted HCl or BaCl(aq) or Ba(NO 3)2 AgNO3 follow by Brown Ring Testdiluted HNO3 or (aq) follow by diluted diluted HNO3. ( + FeSO4 (aq ) +diluted H2SO4 HCl/HNO3 concentratedH2SO4

CO32-Carbon Dioxide isreleased.

White precipitate is

formed. It is soluble indiluted HCl/HNO3

White precipitate isformed. It is soluble in

diluted HNO3

-


SO42- - formed. It is NOT solublein diluted HCl/HNO3

- -


Cl--

NO3- -

-

-

formed. It is NOT

soluble in dilutedHNO3

-

-

Formation of Brown

Ring

8


10/12

Idendification of cation

NaOH(ak)NH3(ak) HCl or NaClH2SO4orNa2SO4

Na2CO3 KI

Na+

Ca2+White

precipitate.

White White

precipitate isprecipitate is

produced. produced.

WhiteWhite White

Mg2+precipitate is precipitate is precipitate isproduced. produced.produced.

White

Al3+

Zn2+

Pb2+

precipitate isproduced.

Dissolve in

excess NaOH

solution.

White


Dissolve in

excess NaOH

solution.

White


Dissolve in

excess NaOH

solution.

White

precipitate is

produced.

White


Dissolve in

excess NH3solution.

White

Whiteprecipitate isprecipitate is produced.

produced. Dissolve in hot

water

White

precipitate is

produced.

White

precipitate is

produced.

Yellow

White White precipitate isprecipitate is precipitate is produced.

produced. produced.Dissolve in hotwater

Dirty green Dirty green Green

Fe2+precipitate is precipitate is precipitate isproduced. produced.produced.

Red brown

Fe3+precipitate isproduced.

Red brownBrown

precipitate is precipitate is

produced. produced.

A red brown

solution formed.

Blue precipitate

Cu2+Blue precipitate

is produced.

is produced.

Dissolve in

excess NH3solution and

form a blue

solution.

White

Blue precipitate precipitate form

is produced. in brown

solution

NH4+

= No changes is observed

109


11/12

Distibguish Iron(II) and Iron(III)

Reagent

Solution of potassium hecxacianoferate(II)

Solution of potassium hecxacianoferate(III)

Solution of potassium Thiocyanate(II)

Observation Ion presents

Light blue precipitate Fe2+

Dark Blue precipitate Fe3+

Dark blue precipitateFe2+

Greenish brown solution Fe3+

Pinkish solution Fe2+

Blood red solutionFe3+

Manufactured Substances in Industry

Contact Process (Making Sulphuric Acid)

Stage 1: Formation of SO2Combustion of Sulphur

S (s) + O2 (g) SO 2(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) 2SO 2(g) + 2H2O(ce)

Stage 2: Formation of SO3

2SO2(g) + O2(g) 2SO 3(g)

Catalyst: vanadium(V)oxide Temperature: 450CPressure: 2-3 atmospheres

Stage 3 Formation of oleum H2S2O7

SO3(g) + H2SO4(aq) H

2S2O7(l)

Stage 4:Formation of Sulphuric acid

H2S207(1) + H2O (1) 2H2SO4(aq)

11


12/12

Haber Process (Making Ammonia)

Sources of the raw material

Hydrogen1. Reaction between steam and heated cokeH2O + C CO + H

2

2. Reaction between steam and natural gas.

2H2O + CH4 CO 2 + 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) 2NH

3(g); H = -92 kJ mo1-1

Catalyst: IronPromoter: Aluminium oxideTemperature: 450 CPressure: 200-1000 atm

12

Chem Formula List

Documents

Transcript of Chem Formula List