CTEVT Chemistry Note : Inorganic Chemistry(II) : Carbon, Ammonia and Phosphorus.

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CHAPTER- 3  : CARBON AND IT’S OXIDES

Symbol          :   C

Atomic number   :   6

Atomic weight   :   12

Electronic configuration : 1s22s22p2

Valency         :   4
Allotropes of carbon: [ Allotropy]:

The two or more forms of same element having similar chemical properties but different physical properties are called allotropes and the phenomenon is called allotropy.

    1.Crystalline form: –

  • Diamond
  • Graphite
  • Fullerene

     2.Amorphous form: –

  • Coal
  • Charcoal
  • Coke
  • Lamp black
  • Gas carbon.
Compound of carbon: Carbon monoxide (CO) :
Laboratory preparation of carbonmonoxide gas :

Carbon monoxide gas can be prepared in lab by heating formic acid or oxalic acid with conc. H2SO4.

   

Lab preparation of carnon CO gas

Procedure: Small amount of oxalic acid crystal is taken in a round- bottomed flask and all the apparatus are fitted as shown in figure. When conc. H2SO4 is poured in the flask through thistle funnel and heated then a mixture of CO and CO2 gas is formed. The mixture of gas is passed through a bottle containing NaOH solution where the CO2 gas is absorbed by NaOH.

     

The pure CO gas is then collected in a gas jar by downward displacement of water.

Chemical Properties of carbon monoxide :

 1. Combustibility (Reaction with oxygen) : It burns in air to form carbon dioxide.

           

 2. Action with chlorine: Carbon monoxide reacts with chlorine in presence of sunlight to produce phosgene ( carbonyl chloride) which is a poisonous gas.

     

 3. Action with NaOH ( caustic soda) : When carbon monoxide is heated with sodium hydroxide then sodium formate is formed.

     

 4. Action with nickel: When Ni is heated with CO, nickel tetracarbonyl is formed.

   

 5. Action with iron: When Fe is heated with CO, iron pentacarbonyl is formed.

   

 6. Action with haemoglobin:

Q) Why carbon monoxide gas is extremely poisonous( toxic) ?

Carbon monoxide combines with haemoglobin to form carboxy haemoglobin. This makes haemoglobin unable to carry oxygen from lungs to the different parts of the body and causes suffocation and even death. Thus CO gas is highly toxic.

  CHAPTER- 4  : NITROGEN  (AMMONIA)

Symbol        : N

Atomic Number : 7

Atomic Weight : 14

Electronic configuration : 1s22s22p3
Laboratory preparation of ammonia gas:

Ammonia gas is prepared in laboratory by heating a mixture of ammonium chloride and slaked lime.

    

Procedure : A mixture of ammonium chloride and slaked lime in the ratio of 1:3 is taken in a hard glass test tube and all the apparatus are fitted as shown in figure. When the mixture is heated, ammonia gas is produced which is passed through a tower packed with quick lime (CaO) to remove moisture( i.e. to make dry).

     

The dry ammonia gas is then collected in a gas jar by downward displacement of air.

Chemical Properties of ammonia :

 1. Basic nature:

  i) It dissolves in water to give NH4OH, which is basic in nature.

  ii) It reacts with acid to give salt.

  iii) As a Lewis base: Due to presence of lone pair of electrons on the nitrogen atom, ammonia acts as a Lewis base, i.e. it donates lone pair of electrons to the electron deficient molecules.

 2. Action with metals:

 a) When ammonia reacts with molten sodium or potassium gives amide and hydrogen.

  b) Lithium and magnesium give nitride instead of amide with ammonia.

 3. Reaction with Nessler’s reagent: When ammonia gas is passed to Nessler’s reagent, a brown ppt. of Millon’s base is formed.

Uses of Ammonia :
  1. For the manufacture of nitrogenous fertilizers such as urea.
  2. For the manufacture of nitric acid.
  3. Liquid ammonia is used as a coolant.

CHAPTER : 5 -PHOSPHORUS

Symbol        : P

Atomic number : 15

Atomic weight : 31

Electronic configuration : 1s22s22p63s23p3
Chemical properties of (white) phosphorus :

 1. Action with air (O2) : Phosphorescence : Phosphorus is highly reactive and it burns(oxidize) in air giving yellow-green flame forming phosphorus pentoxide and trioxide. This phenomenon is called phosphorescence.

     

{ Thus phosphorus is stored in water to prevent phosphorescence}

 2. Action with chlorine : Phosphorus forms trichloride and pentachloride with chlorine.

   

 3. Action with caustic alkali (i.e. Caustic soda or caustic potash) :

When phosphorus is boiled with aqueous solution of caustic soda(NaOH) or caustic potash(KOH), phosphine gas is formed.

   Uses of phosphorus:
  1. It is used as a poison for killing rats.
  2. Used to prepare phosphine gas.
  3. Used for making match stick.
  4. Used in the manufacture of phosphate fertilizer.

    ⇐ See previous chapters 

    See next chapters ⇒

    REFERENCES :

  • Mitra, L.A. , a Text Book of Inorganic Chemistry, Ghos and Company, 61th edition, Calcutta, 1996. 
  • Madan, R.D., Modern Inorganic Chemistry, S. Chand and Company Ltd.
  • https://www.mayoclinic.org/diseases-conditions/carbon-monoxide/symptoms-causes/syc-20370642
  • https://en.wikipedia.org/wiki/Carbon_monoxide
  • https://pubchem.ncbi.nlm.nih.gov/compound/Ammonia