NEET Chemistry – d & f-Block Elements- Study Notes

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About this unit

General introduction, electronic configuration, characteristics of transition metals, general trends in properties of the first row transition metals- metallic character, ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds, alloy formation. Preparation and properties of K2Cr2O7 and KMnO4.Lanthanoids- electronic configuration, oxidation states, chemical reactivity, and lanthanoid contraction and its consequences.Actinoids: Electronic configuration, oxidation states and comparison with lanthanoids

d- AND f-BLOCK ELEMENTS

TRANSITION ELEMENTS

Elements where the last orbitals filled are the d orbitals known as transition elements. They have been placed in the middle of the periodic table between electropositive s-block and electronegative p-block elements.

GENERAL ELECTRONIC CONFIGURATION

Transition metals have the electronic configuration (n-1)d1-10ns0-2. When electrons fill orbitals, ns-orbital is filled first than (n-1)d-orbital.When losing during oxidation, ns electrons are lost first than (n-1)d electrons.

 

Zn ,Cd, Hg ,the end members of first three series have their general electronic configuration (n-1)d10ns2. These do not show properties of transition elements to any appreciable extent and are called non-typical transition elements.

CLASSIFICATION

Transition elements consist of the following four series

ELECTRONIC CONFIGURATION OF TRANSITION ELEMENTS

PHYSICAL PROPERTIES OF TRANSITION ELEMENTS

METALLIC CHARACTER

Transition metals can lose valence electrons and form cations
They have simple hcp, ccp and bcc lattices characteristic of true metals. Except Hg, they are solids at room temperature and are dense ( in general, in case of osmium 22.6g/), lustrous, malleable, ductile thermal and electrical conductors. There is gradual decrease in electropositive character from left to right.

MELTING AND BOILING POINT

Due to strong metallic bond, they have high mpts and bpts. The mpts of these elements rise to a maximum and then fall with the increase in atomic number the manganese and technetium show abnormal values as shown by graph)

IONISATION ENERGY

The ionisation energy increases with the increase in the atomic number but not in regular manner. The ionisation energies of 5d elements are higher than those of 4 d and 3d elements due to greater effective nuclear charge which in turn is due to poor shielding of nucleus by 4f electrons.
Formation of requires and formation requires.
Hence Ni (II) compounds are thermodynamically more stable than Pt (II) Compounds.
Formation ofrequires and formation of requires
Hence Pt (IV) compounds are relatively more stable than nickel (IV) compounds.
Thus  is well known where as the corresponding nickel compound is not known. (Ionisation energy graph is sketched here for ready reference)

ELECTRODE POTENTIAL

() () is governed by three factors
  • Heat of sublimation
  • Heat of ionisation
  • Heat of hydration
For the 3d transition metals the values are
V   Cr   Mn  Fe  Co  Ni  Cu
-1.18  -0.91 -1.18 -0.44 -0.28 -0.25 0.35 (Volts)
The irregular trend is due to variation in ionization energies and sublimation energies. Except copper 3d elements are good reducing agents but weaker than s-block elements.

OXIDATION STATES

In different types of compounds , transition metals exhibit different oxidation states. The highest oxidation state is exhibited in fluorides and oxides. In lower oxidation state the compounds formed are ionic and in higher oxidation state they are covalent in nature.
Osmium exhibit +8 O.S. (highest)often but Ru exhibit +8 oxidation state rarely. Transition metals also show oxidation states +1 and zero.
Fe3+ is more stable than Fe2+. Hence Fe2+ act as reducing agent Cr3+ is more stable than Cr2+. Hence Cr2+ act as reducing. Mn2+ is more stable than Mn3+ Hence Mn3+ act as oxidising agent

ATOMIC AND IONIC RADII

The values for atomic radii and ionic radii are in between the values for s and p-block elements. In 3d transition series the ionic radii forion decreases upto the middle of the period then becomes almost constant. Due to lanthanide contraction the second and third member of each group have atomic radii close to each other (Zr.160pm, Hf 159pm)

DENSITY

d-block elements have high density because of their small atomic sizes and strong metallic bonding.
Density      Sc Ti V Cr Mn Fe  Co Ni Cu Zn
g/ml         3.0 4.54 6.10 7.19 7.40 7.87 8.70 8.90 8.92   7 .13

ATOMIC VOLUME

Atomic volume decreases along the period due to decrease in size.

REACTIVITY

d-block elements are less reactive due to high ionisation energies. Some are almost inert and known as noble metals, e.g. Au, Pt, Ru, Rh, Os, Ir etc.

COMPLEX FORMATION

They are well known to form a large number of complex compounds mainly due to
  • Small atomic size and higher nuclear charge
  • Presence of partly filled or vacant orbitals
    eg.

COLOURED IONS

The colour exhibited by transition metal ions is due to the presence of unpaired electrons in d-orbitals which permits the d-d excitation of electrons.
Colour of a complex depends on the metal, its oxidation state and its ligands. e.g.
[ Cu(H2O)4 ]2+ is Pale blue
[ Cu(NH3)4 ]2+ is Dark blue
CuSO4.5H2O is blue in colour and anhydrous CuSO4 is colourless.

 

In absence of ligands  all d orbitals are degenerate (same energy) and the possibility of d-d excitation is no more.
In presence of ligand have higher energy, d-d transition take place by absorption of light, hence the colour.

MAGNETIC PROPERTIES

  • Paramagnetic – This is due to the presence of unpaired electrons in d-orbitals. Paramagnetic character increases with the number of unpaired electrons.
  • Diamagnetic – Diamagnetic substances are repelled by an applied magnetic field.
  • Ferromagnetism – In this case permanent magnetic moment is acquired by substance e.g. Fe. Magnetic moment is given by  B.M. where n = number of unpaired electrons and B.M. = Bohr magneton (unit of magnetic moment)

CATALYTIC PROPERTIES

The transition metals and their compounds behave as catalyst due to-
  • The presence of partly filled d-orbitals and exhibiting various oxidation states.
  • Their formation of intermediate complex with reactants and thus lowering the energy of activation
  • Their rough surface area provides active sites for adsorption of reactant molecules. eg.
Iron in the preparation of NH3 (Habers process)
Finely divided nickel for hydrogenation
Pt or V2O5  in the preparation of H2SO4 (Contact process)
Pt in the preparation of nitric acid (Ostwald’s process)

FORMATION OF ALLOYS

d block elements have a strong tendency to form alloys since their atomic sizes are very similar and in the crystal lattice one metal can be readily replaced by another. Alloys so formed are hard, have high m.pts. The metals Mo, W, Cr, Ni, and V are used for the production of stainless steel and alloy steel.
Amalgam is an alloy formed by mercury with other metals. Iron and platinum do not form any alloy with mercury.

INTERSTITIAL COMPOUNDS

The empty space present in a crystal lattice is known as interstitial place. The non metal atoms due to their small size (eg H, B, N, C etc.) when occupy such place the resulting compound is known interstitial compound. Such compounds are hard and rigid e.g. cast iron and steel.

NON STOICHIOMETRIC COMPOUNDS

The compounds not having the elements in the exact ratio as shown by the molecular formula are known as non stoichiometric compounds e.g., etc. In FeO the Fe:O is approx. 0.94:1 and not exactly 1:1.

IRON 

OCCURRENCE

Being reactive in nature it does not occur in free state.
Ores of Iron-
  • Haematite
  • Magnetite
  • Limonite or hydrated ferric oxide
  • Iron pyrites
  • Siderite
  • Copper pyrites

EXTRACTION

It is extracted from haematite in a blast furnace by reduction with carbon and carbon monoxide. The steps involved are-
  • Concentration – The crushed ore is agitated with water and then concentrated by electromagnetic method.
  • Roasting or Calcination – To remove volatile substances and organic matter.
                          
  • Smelting – Roasted or calcinated ore is mixed with limestone and coke and fed into blast furnace. Reactions taking place in the blast furnace.
Lower region 
Middle region
Upper region

 

The gases leaving the furnace contain CO and used to heat incoming air blast.The two layers in the blast furnace are-
Upper layer – Molten Iron – It is poured out in moulds and known as PIG IRON or CAST IRON.It contains 3-5% carbon and varying amounts of Mn, Si, P and S which make the iron hard and brittle.
Lower layer – Molten CaSiO3 (slag)

WROUGHT IRON

It is obtained by heating cast iron with haematite. The impurities are oxidised.
It contains carbon 0.2-0.5% and traces of P and Si. It is pure form of Iron and soft , malleable, ductile. It is used to make magnets in electric cranes and dynamos, railway carriage couplings being corrosion resistant.

STEEL

It contains carbon 0.1-1.5% and manufactured by following methods.
  • Bessemer process – Molten pig iron is heated in large pear shaped furnace lined with silica bricks at 1873K when impurities such as Mn, Si, C burn off. When all carbon is completely burn off the requisite amount of carbon is added.
Bessemer converter is lined with lime (CaO) or magnesia (MgO) when pig iron contains high percentage of phosphorous.
  • Open hearth process – The cast iron, scrap iron , haematite ore and lime are mixed together and melted in open hearth furnace lined with or calcined dolomite (MgO. CaO) depending upon the nature of impurities.
  • Electric furnace process – It is combination of Bessemer and open hearth process.

 

TYPES OF STEEL
  • Soft steel – contains carbon 0.25%
  • Mild steel – contains carbon 0.25-0.5%
  • Hard steel – contains carbon 0.5-1.5%
  • Alloy steel – contains varying percentage of Ni, Cr, Mn, Co,W, V e.g. stainless steel is an alloy of Fe, Cr and Ni.

 

HEAT TREATMENT OF STEEL
The hardness of steel depends on its carbon content and heat treatment.
  • Quenching – It involves the heating of steel to red hot (1123K) and cooling it by plunging into cold water or oil.  It makes the steel hard and brittle.
  • Annealing – The steel is heated well below red heat and then cooled slowly. The steel becomes soft.
  • Tempering – In this process the quenched steel is reheated to 504 to 574K and allowed to cool slowly. The brittleness disappears and hardness is retained.
  • Nitriding – It involves the heating of steel in an atmosphere of ammonia when surface is coated with iron nitride. The steel becomes hard.
  • Case hardening -The steel is heated in charcoal and then quenched.The steel becomes hard.

 

ALLOYS OF STEEL
The important alloy steels are-
Name
Composition
Uses and Properties
Tungsten steel
Fe 94%, W 5%, C 1%
It is very hard, resistant to water and used for making Rock drills and Safeties
Stainless steel
Fe 73% Cr 18%, Ni 8%, C  1%
It is resistant to corrosion. Used for making cutlery
Manganese steel
Fe 86%, Mn 13%, C  1%
It is hard, used for manufacturing high speed cutting tools
Invar
Fe 64%, Ni 36%
It has small coefficient of expansion, used in watches, meter scales and pendulum rods
Permalloy
Fe 21%, Ni 78%, C  1%
It is strongly magnetised by electric current and lose magnetism when current is let off, used for manufacturing electromagnets and ocean cable.
Nickel steel
Fe 96-98%, Ni 2-4%
Resistant to corrosion, hard and elastic wire, used for making cables, gears and drive shafts.

SOME CHEMICAL PROPERTIES OF IRON

  • Red hot iron burns in O2 giving sparks
  • When steam is passed over red hot iron, hydrogen is liberated and magnetic oxide of iron (ferroso ferric oxide) is formed
  • Action of dil. H2SO4
  • Hot and conc. H2SO4
  • Action of dil. HNO3
        

PASSIVITY

The inertness exhibited by metals under conditions when chemical activity is to be expected is called passivity. Iron becomes passive with conc. HNO3, Chromic acid, conc. H2SO4 and KMnO4 etc. It is due to the formation of a thin layer of oxide at the surface of iron.

COMPOUNDS OF IRON

FERRIC CHLORIDE

PREPARATION
  • By passing dry chlorine over heated iron, anhydrous ferric chloride is obtained
  • By the action of hydrochloric acid on ferric hydroxide or ferric oxide

 

PROPERTIES
  • It is soluble in water, alcohol and ether.  is yellow. Its aqueous solution is acidic. Sublimes  at 300ºC, covalent and dissociates above 973K first into and e.g.
  • Action of heat
  • Oxidising nature of FeCl3 is shown by following reactions
      

 

STRUCTURE

 

USES
Used in medicine as ASTRINGENT and ANTISEPTIC. Its concentrated solution is used for etching copper and silver.

FERROUS SULPHATE (GREEN VITRIOL)

PREPARATION
  • Manufacture – From iron pyrites by oxidation by air

 

PROPERTIES
  • Hydrated is green and anhydrous is colourless.
  • Action of heat
  • Its aqueous solution is acidic due to cationic hydrolysis
  • Reducing nature – It is strong reducing is nature.
  • Addition compound with NO which is dark brown

 

USES
As mordant in dyeing, insecticide and in the preparation of Mohr’s salt.

FERROUS AMMONIUM SULPHATE (MOHR’S SALT)

PREPARATION
By mixing saturated solutions of and cooling.

 

PROPERTIES
It is light green crystalline compound and does not effloresce.

FERRIC OXIDE

In nature it occurs as haematite.
Used in Bosch process as catalyst and polishing powder by jewellers and as red pigment.

IRON SULPHIDE FeS

By heating iron filings with dil. H2SO4
,        
The reaction is carried out in Kipp’s apparatus. FeSO4 is obtained as by product H2S. Finds an extensive application in analytical chemistry. It has smell of rotten eggs.

COPPER

OCCURRENCE

It occurs in nature in large quantities in Michigan (USA).
Important ores are
  • Copper glance
  • Copper pyrites
  • Malachite
  • Cuprite  (Ruby copper)
  • Azurite

PREPARATION

EXTRACTION
It is mainly extracted from copper pyrites.

 

CONCENTRATION
The ore is concentrated by froth floatation process.

 

ROASTING
The concentrated ore is strongly heated by hot blast of air on the hearth of reverberatory furnace. The following changes take place

 

SMELTING
The roasted ore is mixed with sand and heated in blast furnace.
The mixture of copper and iron sulphides melt together to form “matte”.

 

BESSEMERISATION
The molten matte mixed with little sand is poured into Bessemer converter. The following changes take place
The copper thus produced is called ‘blister copper’ and contains 2.0% impurities of Ag, Au, Ni, Zn, Pb, Sn, As, S etc.

 

REFINING
It is carried out by either of the following methods
  • By polling – The melt is stirred vigorously with green poles of wood and oxides are reduced by hydrocarbons emanating from wood.
  • Electrolytic refining of copper – Slabs of impure copper are made anode and thin sheets of pure copper as the cathode. Acidic copper sulphate is used as electrolyte.
The impurities like Zn, Fe, Ni,Co remain in solution being more electropositive in nature and Ag, Au, Pt, (less electropositive) collect below the anode in the form of anode mud or slime 99.99% pure copper is obtained. Anode mud provides about 25% of U.S. Silver production and 13% of U.S. gold production.

PROPERTIES OF COPPER

In aqueous solution it has two oxidation states +1 (cuprous) and +2 (cupric). Cu (I) salts tend to be white and insoluble in water while many salts of Cu (II) are water soluble however Cu(OH)2 is insoluble. CuS is one of the least soluble compounds.
  • Cu (I) disproportionates easily in aqueous solution.
  • Action of – It is attacked by first forming copper (I) oxide (Red) and then copper (II) oxide CuO (Black).
  • It forms a green layer of basic carbonate in presence of and moisture.
  • Not attacked by dilute acids e.g. HCl and but dissolves in these acids in presence of air.

COMPOUNDS OF COPPER

COPPER SULPHATE (BLUE VITRIOL OR NILA THOTHA)

PREPARATION
  • By dissolving Cu (II) oxide or carbonate in dilute.
  • From scrap copper
PROPERTIES
  • Blue crystalline compound.
  • Action of heat
  • Action of NH4OH
     
Tetrammine copper sulphate is known as SCHWITZER’S REAGENT. It is used to dissolve cellulose in the manufacture of artificial silk.
  • Action of KI
(It does not react with KCl, KBr or KF)
  • Action of potassium ferrocyanide
  • Action of KCN
  • Structure of
Four with cation and fifth with anion.

 

USES
In electroplating, as mordant in dyeing.
Bordeaux mixture (Mixture of
It is used as fungicide. In the preparation of Fehling solution and electric batteries.

CUPROUS CHLORIDE – COPPER (I) CHLORIDE 

PREPARATION
  • It can be prepared from Cu alone or in combination with by action of concentrated hydrochloric acid.
  • By passing in a solution of
          

 

PROPERTIES
  • It is a white solid, almost insoluble in water.
  • Action of conc. HCl – It dissolves forming soluble complex.
or
On dilution white precipitate again appears.
  • Action of ammonia – It dissolves forming soluble complex
  • Action of acetylene – Red precipitate of cuprous acetylide is obtained.          
  • With carbon monoxide it forms addition product.
  • With air – In air it is slowly oxidised to green basic cupric chloride.
  • With NaOH
  • With H2S
USES
In gas analysis for absorbing and CO. In combination with as catalyst for synthetic rubber.

CUPRIC CHLORIDE COPPER (II) CHLORIDE

PREPARATION
  • Form copper, cupric oxide or copper carbonate by the action of conc. HCl.
  • Anhydrous cupric chloride is prepared by burning copper in current of chlorine

 

PROPERTIES
  • Hydrated
  • Anhydrous
  • Aqueous dilute solution is blue due to complex
  • Concentrated solution is green due to complex
  • With Ammonia – First a precipitate which dissolves in excess of.
 
  • Action of heat
  • Hydrated salt on heating gives

 

STRUCTURE

CUPROUS OXIDE (RED OXIDE OF COPPER)  

PREPARATION
When Fehling solution is reduced by glucose or aldehyde.

 

PROPERTIES
Red colour, insoluble in water. It forms stable complexes.

 

USES
In making ruby red glass and enamel.In manufacturing anti rust paints.

CUPRIC OXIDE (BLACK OXIDE OF COPPER)

PREPARATION
By heating malachite which is native copper carbonate.
PROPERTIES
Black powder reduced to metallic copper by.

 

USES
In the manufacture of glass.It gives green colour to glazes and glass.

SILVER (Ag)

OCCURRENCE

It is found in nature and in combined state.
Principal ores are –
  • Argentite (silver glance)
  • Horn silver AgCl,
  • Pyrargyrite (ruby silver)
In small quantities in lead ,copper and zinc ores.

EXTRACTION

MAC ARTHER FOREST’S CYANIDE PROCESS
  • Concentration – Ore is concentrated by froth floatation process.
  • Treatment with NaCN – The powdered ore is treated with NaCN solution (0.7%) and air is bubbled through the mixture.
(a) 
(b) 
(c) 
Reversible reaction is prevented by oxidation of by air.
  • Precipitation of silver – It is done with zinc.
  • Refining
    Electrolytic method
Anode – impure silver
Cathode – pure silver
Electrolyte –

 

SILVER FROM ARGENTIFEROUS LEAD (DESILVERISATION OF LEAD)
Lead, extracted from galena (PbS) contains small amount of silver and is called argentiferous lead. Silver is recovered from it by-
  • Parke’s process – Molten argentiferous lead is shaken with zinc when whole of silver passes into zinc. On cooling Ag- Zn alloy solidifies and being lighter floats over molten lead. It is separated, melted and distilled. Zinc distills over and silver is left behind. Success of the method depends upon the fact that-
(a) Silver is more soluble in molten zinc and
(b) Molten Zn and lead are immiscible
  • Pattison’s process – (When silver is less than 1.0%).The lead-silver mixture containing 2.6%. Silver melts at lower temperature than pure lead. When molten argentiferous lead is allowed to cool pure lead solidifies first and removed. The silver content of the mixture is allowed to raise to 2.6%.The silver is then recovered by cupellation.

PROPERTIES

  • It is a noble metal not attacked by atmospheric oxygen. The surface is tarnished due to formation of  Ag2S due to H2S present in air.
  • Dissolves in dilute and concentrated nitric acid
  • Dissolves in alkali cyanide   
  • Dissolves in conc. sulphuric acid (not in dil. sulphuric acid)

USES

For making ornaments (80%Ag+20%Cu), electroplating, preparation of mirrors.
Fineness of Silver – It is the amount of silver present in 1000 parts of silver alloy. 925 fine silver means an alloy of 92.5% silver and 7.5%copper.

COMPOUNDS OF SILVER

SILVER NITRATE OR LUNAR CAUSTIC

PREPARATION
By the action of dilute nitric acid on silver.

 

PROPERTIES
  • It is colourless crystalline solid, soluble in water. It leaves black deposit when rubbed on the skin due to formation of finely divided silver.
  • Action of heat
  • Tollen’s reagent – The ammoniacal silver nitrate solution is known as Tollen’s reagent.
  • Reaction with aqueous solution of certain compounds
USES
For silvering mirror ,electroplating, in medicines, for the preparation of silver halides used in photography. Particularly AgBr which is most sensitive to light.

GOLD (Au)

OCCURRENCE

It occurs free as Reef gold, Vein gold or auriferous quartz. Some improtant ores are
  • Claverite ,
  • Sylvanite
  • Auriferous pyrites. These are sulphide ores of Cu, Ag, lead which contain gold.

EXTRACTION

By cyanide or Mac Arther Forest cyanide process

 

CONCENTRATION
Sulphides and tellurides are concentrated by froth floatation process.

 

ROASTING
The concentrated ore is roasted to remove oxidisable impurities of Te, As and S.
Formation of complex- NaCN solution is sprayed over the crushed ore and the gold with air, forming complex ion in solution.

 

The gold is then recovered as a solid by reduction.

 

PARTING
Removal of impurities of Ag and Cu from gold is known as parting.Impure gold is boiled with conc.  when Ag and Cu dissolve and Au remains unaffected.

 

PURIFICATION
By electrolytic method using gold chloride 2.5-6.0% and conc. HCl.·

 

Plattner chlorine extraction process (From auriferous pyrites)
The moistened auriferous pyrites is saturated with chlorine, leached with water then treated with which precipitates gold.
Auriferous pyrites (moistened)
Impurities of Ag and Cu are removed by parting (as above).

PROPERTIES

  • Pure gold is soft, hardened by Ag or Cu.
Fineness of gold – It is expressed in terms of carats. Pure gold is 24 carats. 22 carats mean it contains 22 parts by weight of gold and 2 parts by weight of other metals generally copper.
  • It is very inert and not attacked by oxygen, water and acids.
  • It is attacked by aqua regia
  • It is attacked by chlorine.
  • Auric chloride forms red crystals. Soluble in water and decomposed on heating.

ZINC (Zn)

OCCURRENCE

It is not found free in nature.The principal ores are –
  • Zinc blende (sphalerite) ZnS
  • Zincite or Red zinc oxide ZnO
  • Franklinite
  • Calamine or Zinc spar  
  • Willemite

PREPARATION

EXTRACTION
It is extracted by reduction process from ZnS (Zinc blende).

 

CONCENTRATION
The ore is concentrated by froth flotation process.

 

ROASTING
The concentrated Zinc blende is roasted in a current of air.
(is utilised for the manufacturing of H2SO4)
If calamine ore is used, it is calcined.