Skip to main content

ALKALI METALS

 ALKALI METAL 

Alkali Metal are  lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr)

1.Physical state of alkali metal
  •  One electron in outermost shell & General formula ns¹. 
  •  Francium is radioactive element. 
  • All are silvery white. 
  • Light soft, malleable and ductile metals with metallic lustre. 
  •  Alkali metals are paramagnetic, diamagnetic and colourless in form of ions.
2.Atomic size of alkali metal 

  • Biggest in their respective period (except noble gas element) 
  • Size increases from Li to Fr due to addition of an extra shell.  Li < Na < K < Rb < Cs < Fr
3. Softness of alkali metal 
  • Alkali metals are soft because of-
 (i) Large atomic size
 (ii) BCC crystal structure (HCP in Li)

 (iii) Loose packing (68% packing efficiency) 

(iv) Weak metallic bond 

  • Cs is the softest metal in s-block

4. Melting point and boiling point of alkali metal 
  • Weak interatomic bonds are due to their large atomic radii and presence of only one valence electron hence melting point and boiling point are low. 
  • Decreasing order of melting point and boiling point of alkali metal  is Li > Na > K > Rb > Cs 
  • With the increase in the size of metal atom, the repulsion of the non-bonding electrons increases and therefore melting point and boiling point decreases from Li to Cs.
5. Electro positive character or Metallic character of alkali metal 
   Electropositive ∝ 1/ Ionisation potential
Due to their larger size electron can easily be removed to form M+ ion. Electro positive property increases from Li to Cs. 
6. Flame test  of alkali metal 
Alkali metals and their salts gives characteristic colour to bunsen flame. The flame energy causes an excitation of the outer most electron which on dropping back to ground state emits absorbed energy as visible light.
Example :
 Li-Crimson red 
Na-Golden yellow 
K-Violet 
Rb-Red violet 
Cs-Blue

7. Reaction of alkali metal with NH3

  •  2Li + NH3   ⟶ Li2NH (Lithimide) 
2Na + 2NH3  ⟶ 2NaNH2 + H2 ↑ (Sodamide) 

  •  Solubility in liquid ammonia 
 (i) All the alkali metals dissolves in NH3 (liq.) and produces blue solution. 
(ii) This blue solution conducts electricity and possesses strong reducing power, due to the presence of ammoniated electrons. 
Na(s) + (x+y) NH3 ⟶[Na(NH3 ) x ] + + [e(NH3 ) y ] – ammoniated electron 
(iii) This dilute solution is paramagnetic in nature

 8. Photo electric effect of alkali metal 

  • Atomic size of K, Rb and Cs is quite large, so their ionisation potential is very low.
  • Due to very low ionisation potential their valence shell electrons gets excited even by absorbing visible light. That's why Cs is used in photo cells.
9. Standard oxidation potential of alkali metal 

  • All the alkali metals have high +ve values of standard oxidation potential (tendency of releasing electrons in water or self ionic solutions).
  • So these are good reducing agent, having upper most positions in the electro chemical series. 
  • Li has highest standerd oxidation potential (+3.05 eV) due to its high hydration energy. Such that it converts into. Li+ ion by loosing one electron.
10. Hydration energy ( Heat of Hydration ) of alkali metal 

  • Alkali metals salts are generally soluble in water due to hydration of cations by water molecules.
  • Smaller the cation, greater is the degree of its hydration. 

11. Reducing property of alkali metal 

  • Since alkali metals have high standard oxidation potential, so these are strongest reductants. 
  • Reducing property increases down the group in gaseous or molten state

 Li+ < Na+ < K+ < Rb+ < Cs+ 

  • But in aqueous solution order is -

 Li+ > K+ ~ Rb+ > Cs+ > Na+

12. Reaction of alkali metal with air 

  • Alkali metals gets turnish in air due to the formation of oxide at their surface hence they are kept in kerosene or paraffin oil. 
  • These elements reacts with moist air to form carbonates 
4Na + O2 ⟶ 2Na2O 
Na2O + H2O ⟶ 2NaOH (moist) 
2NaOH + CO2 ⟶ Na2 CO3 + H2 O (in air) 
In dry air only Li gives nitride and oxide both while other elements gives only oxides.
13. Reaction of alkali metal with Oxygen 
  • Oxide ion [O2-] : 
Li forms only Li2 O (Lithium oxide). 
  • Peroxide [O2] -² : 
Na reacts with O2 to form peroxide (Na2O2 ). 
  • Super oxide [O2 ‐] :
 K, Rb and Cs forms MO2 type oxides (super oxides) in excess of O2 . So super oxides are paramagnetic and coloured. 

 Their stability order is – Normaloxide > Peroxide > Superoxide 

14. Reaction of alkali metal with water 

  • Alkali metals react vigorously with water forming hydroxides with the liberation of H2 . 

2M + 2H2O ⟶ 2MOH + H2 

  •  Reactivity with water increases from Li to Cs. 

Li ⟶ least reactive towards water 

Na ⟶ reacts vigorously

K ⟶ reacts producing a flame

Rb, Cs⟶ reacts explosively. 

  • These metals also reacts with alcohol gives alkoxide and H2 . 

2Li + 2C2 H5 OH ⟶ 2C2H5O-Li+ + H2 

  •  Monoxides gives strongly alkaline solution with water 

M2 O + H2 O ⟶ 2MOH

15. Reaction of alkali metals with Halides 

  •  Alkali metals reacts directly with halogen to form MX 

(M – alkalimetal, X – Halide ion)

  • Ionic properties of MX increases from LiCl to CsCl 
  • LiCl is covalent in nature (due to polarisation of Cl– ion by small Li+ ion). hence it hydrolyses with water while rest are ionic so do not hydrolyse. 
  • K, Rb and Cs halides reacts with more halogens to gives polyhalides. 

KI + I2 ⟶KI3 ⟶

K+   + I3-

 CsBr + Br2 ⟶CsBr3⟶Cs+ + Br3 –

16. Carbonates of alkali metals 

  • All the alkali metals forms M2CO3 type carbonates. 
  • Except Li2CO3 , all the carbonates are stable towards heat 

Li2CO3     ⟶ (heat)  Li2O + CO2 

  •  Thermal stability of carbonates ∝1/ф(Ionic potential) Order of stability is – 

Cs2CO3 > Rb2CO3 > K2CO3 > Na2CO3 > Li2CO3  

17.  Nitrates of alkali metal 

  • Alkali metals forms MNO3 type nitrates (M – alkali metal) 
  • Stability increases from LiNO3 to CsNO3 . LiNO3 decompoes into Lithium oxide & NO2 on heating. 

4LiNO3 ⟶(heat + oxide) 2Li2 O + 4NO2 + O2 

  • Other nitrates, on heating to give nitrite and oxygen.

MNO3⟶ (heat) 2MNO2 + O2

18. Nitrides of alkali metals

 Only Li reacts directly with N2 to form nitride which gives NH3 on reacting with water. 

6Li + N2 ⟶2Li3N 

 Li3N + 3H2O ⟶ 3LiOH + NH3 ↑

  19. Formation of amalgam with alkali metals 

  • Alkali metals gives amalgam with Hg. 
  • These metals reacts with other metals to give mixed metals (alloys)

20. Sulphates for alkali metals 
  • Alkali metals forms M2SO4 type sulphates.
  • All alkali metal sulphates are ionic. Ionic properties increases from Li to Cs. 
Li2SO4 < Na2SO4 < K2SO4 < Rb2SO4 < Cs2SO4 
  • Li2SO4 Least soluble in water. 
  • These sulphates on burning with C forms sulphides 
M2SO4 + 4C  →M2S + 4CO 
  • Except lithium, sulphates of IA group reacts with sulphates of trivalent metals like Fe+3, Cr+3, Al+3 etc. gives double salts called alum.
21. Reaction of alkali metals with acids
  • Reacts vigaorously with acids 
2M + H2SO4 ⟶ M2SO4 +H2 ↑
Labels:

Comments

Post a Comment

Popular posts from this blog

PERIODIC TABLE

 Modern Periodic table Modern Periodic Law :  The recent work has established that the fundamental property of an atom is atomic number and not atomic weight. Therefore, atomic number is taken as the basis of the classification of the elements. The modern periodic law was given by Moseley, it may be stated as : ''The properties of elements are periodic functions of their atomic number". Modern periodic table is also called long form of the periodic table or Bohr’s table. In this table, the elements are arranged in order of their increasing atomic number. It consists of 4 blocks (s, p, d and f), 18 groups numbered from 1 to 18 and 7 periods numbered from 1 to 7. Short tricks to learn periodic table  Blocks : The periodic table is divided into four main blocks (s, p, d and f) depending upon the subshell to which the valence electron enters into.  (1) Elements of group 1 and 2 constitute s-Block.   (2) Elements of group 13, 14, 15, 16, 17, 18 constitut...
Post a Comment
Read more

COMPOUNDS OF ALKALI METALS

 COMPOUNDS OF ALKALI METALS  1. Sodium (Na) , Natrium  Extraction of sodium  : Down's Process  By Electrolysis of fused NaCl + CaCl 2 + NaF  At cathode (Iron Vessel) : Na+ +e– ⟶  Na(s)  At Anode (Graphite) : 2Cl–   →    Cl 2 + 2e–  (i) (CaCl 2 + NaF) is used to lower Melting point (8000 C) of NaCl to about 6000 C.  (ii) Aqueous sodium chloride cannot be used for preparing sodium by electrolysis. Because instead of metallic sodium, hydrogen gas will be liberated at cathode. Properties sodium , Natrium (i) sodium is a crystalline soft metal.  (ii) Highly reactive, so kept in kerosene.  (iii) Na dissolves in liquid NH3 to give blue solution.  Uses of sodium , natrium  (i) In the preparation of sodium amalgam (used as reducing agent)  (ii) In sodium vapour lamp, which emits monochromatic yellow light.  (iii) As heat transfer medium in nuclear reactors. 2. Sodium chloride NaCl Occ...
Post a Comment
Read more

Chemistry 101: A Beginner's Guide to Understanding the World Around Us

Chemistry 101: A Beginner's Guide to Understanding the World Around Us Chemistry  What is Chemistry ? Chemistry is the study of matter and its properties, composition, and interactions with other substances. It is a fundamental science that encompasses a wide range of topics, from the behavior of atoms and molecules to the reactions that occur in living organisms. Chemistry is the foundation of modern technology and plays a critical role in fields such as medicine, engineering, and materials science. At its core, chemistry is concerned with understanding the structure and behavior of matter at the atomic and molecular level. Chemists study the properties of elements, the structure of molecules, and the forces that govern chemical reactions. They also investigate the behavior of matter under different conditions, such as temperature, pressure, and concentration. One of the key aspects of chemistry is the concept of the chemical bond, which is the force that holds atoms together in m...
1 comment
Read more