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=Chapter 1 Some Basic Concepts Of Chemistry

=Chapter 2 Structure Of Atom

=Chapter 3 Classification of Elements And Periodicity In Properties of Elements

=Chapter 4 Chemical Bonding And Molecular Structure

=Chapter 5 States of Matter

=Chapter 6 Thermodynamics

=Chapter 11 The p- Block Element

=Chapter 7 Equilibrium

=Chapter 8 Redox Reactions

=Chapter 10 The s- Block Element

=Chapter 12 Organic chemistry : Some Basic Principles and Techniques

=Chapter 13 Hydrocarbon

=Chapter 14 Environmental Chemistry


Chapter 10 The s- Block Element

S Block Elements Properties
in PDF Free Downloal For CBSE Notes

  Groups (1 & 2) belong to the s-block of the Periodic Table.
  Group 1 consists of : lithium, sodium, potassium, rubidium, caesium and francium and collectively known as the alkali metals.
➣   Group 2 include : beryllium, magnesium,calcium, strontium, barium and radium. Except Beryllium they are known as alkalinev

Physical properties-

a) Large atomic radii: The atomic radii of alkali metals are the largest in their respective periods. These increase as we travel down the group.

b) Large ionic radii: The ionic radii increase as we move down the group due to the addition of a new energy shell with each succeeding element.

c) Low ionization enthalpy: The ionization enthalpies  decrease as we move down the group.The ionization enthalpies of the alkali metals are the lowest due to loosely held s- electron.

d) Hydration enthalpy: It decreases with the increase in ionic radii.The hydration enthalpy of Li ion is the maximum and the hydration enthalpy of Cs ion is the minimum.

e) Oxidation  state:  The  alkali  metals  exhibit  oxidation  state  of  +1  in  their compounds and are strongly electropositive in character. The electropositive character increases from Li to Cs.

f) Metallic character: The metallic character increases down the group.

g) Melting point and boiling point:: The m p and b p  of alkali metals are very low and decrease with increase in atomic number.

h) Nature of bonds formed: These metals form ionic bonds. The ionic character increases as we down the group.

i) Flame colouration: All the alkali metals impart a charactersistic colour to the flame.                             

j) Photoelectric effect: Alkali metals (except Li) exhibits photoelectric effect.

Chemical features of alkali metals:

a) Reducing character: As the ionization enthalpies of the alkali metals decrease
down the  group their reducing character or reactivity in the gaseous state increases down the group. i.e., Li < Na < K < Rb < Cs .

b) Reaction with dihydrogen: Alkali metals react with dry hydrogen at about 673 K to form crystalline hydrides which are ionic in nature and have high melting points.Alkali metals react with dry hydrogen

c) Oxides  and  hydroxides:  Alkali  metals  when  burnt  in  air  form  different
compounds, for example the alkali metals on reaction with limited quantity of oxygen form normal oxides ( M2O) M= Li, Na, K, Rb, Cs

d) Reaction with halogens: The members of the family combine with halogen to form corresponding halides which are ionic crystalline solids.
Reactivity of alkali metls with particular halogen increases from Li to Cs.

e) Reaction with water: Alkali metals react with water and other compounds containing acidic hydrogen atoms such as hydrogen halides, acetylene etc. to liberate hydrogen gas.

f) Solubility in liquid ammonia: All alkali metals dissolve in liquid ammonia giving deep blue solutions which are conducting in nature.

g) Reaction with sulphur and phosphorus: Alkali metals react with sulphur and phosphorus on heating to form sulphides and phosphides respectively

Diagonal relationship between Li and Al

Li resembles Mg mainly due to similarity in sizes of their atoms and ions.

The main points of similarity are:

i)  Both are quite hard.
ii)  Both LiOH and Mg(OH)2 are weak bases.
iii) Carbonates of both on heating decompose to produce oxides and carbondioxide.
iv) Both react with nitrogen to give ionic nitrides.
v)  Nitrates of both decompose on heating to give oxides.
vi) Both Li and Mg do not form solid bicarbonates.
vii Because of covalent character LiCl and MgCl2 are soluble in ethanol.
viii) The hydroxides, bicarbonates and fluorides of both Li and Mg are sparingly soluble in water.

Biological importance of  Na and K

i) Sodium ions participate in the transmission of nerve signals.
ii) Sodium ions also regulate flow of water across the cell membranes and in transport of sugars and amino acids into the cells.
ii) Potassium ions are the most abundant cations within cell fluids, where they activate many enzymes, participate in oxidation of glucose to produce ATP.
iv) Potassium ions in combination with sodium  ions are responsible for transmission of nerve signals.
v) The functional features of nerve cells depend upon the sodium potassium ion gradient that is established in the cell.

Group 2 elements: Alkaline earth metals

a) Atomic radii : The atomic radii of alkaline earth metals are fairly large thoughsmaller than the corresponding alkali metals and they increase down the group. This is because on moving down the group, atomic radii increase primarily due to the addition of an extra shell of electrons in each succeeding element.
(b) Ionic radii: the atoms of these elements form divalent ions which show the same trend of increase in their size down the group.
c)  Ionization enthalpy:  The  alkaline  earth  metals  have  fairly  low  Ionizations enthalpies though greater than those of the corresponding elements of group 1 and this value decreases down the group.

(d)  Hydration  enthalpy:  the  Hydration  enthalpies  of  alkaline  earth  metal  ion decrease as the size of the metal ion increases down the Group
Be2>+ >Mg2+ >Ca2+ >Sr2+ >Ba2+               
e) Oxidation State: All the members of the family exhibit +2 oxidation state in their compounded and the form divalent cations (M2+)
f) Electro negativity : The electro negativity values of alkaline earth metals are quite close to those of alkali metals, though slightly more.
(g) Metallic Character :  Alkaline earth metals have stronger metallic bonds as compared to the alkali metals present in the same period.
(h) Melting and boiling point : The melting and Boiling points of these metals are higher than those of alkali metals present in the same period.
(i) Colouration to the flame : With the exceptio9n of beryllium and magnesium, the rest of the elements impart characters in colour to the same flame. For example,

Be  Mg  Ca  Sr   Ba    Ra
Brick Red    Crimson Grassy   Green  Crimson

J) Complex formation: Generally the members do not form complexes. However, smaller ions ( Be & Mg Ions) form complexes with the  electron donor species
k) Formation of  organo-metallic compounds:  Both  beryllium and  magnesium form a number of organo-metallic compounds containing M-C bond with certain organic compounds. For example, magnesium reacts with alkyl halide in the presence of dry ether to give Grignard reagent.

l)  Reducing character: Alkaline earth metals are weak reducing agent than the corresponding alkali metals which have lower ionization enthalpies and comparatively bigger atomic sizes.

m) Reaction with oxygen: With the exception of Ba and Ra which form peroxides ( MO2) rest of the metals form normal oxides (MO) on heating with excess of oxygen.

n) Reaction with  halogens: The  members of the  family combine directly with halogen at appropriate temperature to form corresponding halides.

o) Reaction with water: The members of this group are less reactive towards water as compared to the corresponding alkali metals because these are less electropositive in nature.

p) Reaction  with  hydrogen:  The  members  except  Be combine  with  hydrogen directly upon heating to form metal hydrides.

Uses of some important compounds:-
Caustic soda:

It is used: in soap, paper, textile, petroleum industry

Sodium carbonate

It is used:

a)  in glass and soap industry
in paper making and textile manufacturing c)  in paint and dye stuffs
d) in metal refining
e)  in  production of sodium compounds such as  borax,  caustic  soda,  sodium phosphate etc.

Quick lime:

It is used:

a).  in the preparation of cement, glass and calcium carbide.
b).  In the purification of sugar
c).  In softening of hard water 
d). As a flux in the extraction of metal

Lime stone:

It is used

a) as building material
b) in the manufacture of quick lime
c) in Solvay process to prepare Na2CO3 as it is a source of CO2
in metallurgy for the extraction of iron
e) in toothpaste and certain cosmetics


It is an important building material. It is used in concrete and reinforced concrete, in plastering and in the construction of bridges, dams and buildings.

 Plaster of paris:

It is used
in making moulds for pottery and ceramics etc.
in surgical bandages for setting broken bones of the body
c) for making statues, models, decorative materials and black board chalk.

Biological importance of  Ca and Mg

i)  Magnesium ions are concentrated in animal cells and Calcium ions are concentrated in body fluids, outside the cell.
ii) All enzymes that utilize ATP in phosphate transfer require magnesium ion as cofactor.
iii) In green plants magnesium is present in chlorophyll.
iv) Calcium and magnesium ions are also essential for the transmission of impulses along nerve fibres.
v) Calcium ions are important in blood clotting and are required to trigger the contraction of muscles.
vi) Calcium ions also regulate the beating of the heart.

S Block Elements Properties

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S Block Elements Properties in PDF Free Downloal For CBSE Notes
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