Skip to main content

Structure of atom( part 1)

             Atom 


      Atom is a Greek word which means indivisible  they believed that matter can be broken  down  into very  small indivisible particles .

1. In other words we can say atoms are fundamental building blocks of matters.

2.  Matter composed of three subatomic particles the proton ,the neutron and therefore the electrons. 
        

1. In other words we can say atoms are fundamental building blocks of matters.

2.  Matter composed of three subatomic particles the proton ,the neutron and therefore the electrons. 

          Atomic  theories.

The atomic theory given
 by  maharishi kanad . an ancient indian scientist and philosopher propounded a theory of atom.He explain the creation and existence of the universe.

1 .  He explain his atomic theory of matter in his book vaisheshika Sutra also called kanad Sutra . 

2 .  According to kanad  everything can be subdivided .

3 .  That subdivision leads to creation of parmanu (atom) which are the smallest entities .

4 .   Parmanu (atom) is not visible to the naked eye .

5 .  Atom are indestructible, indivisible and it cannot be further divided.

6 . Earth ,fire ,water ,air those are made up of parmanu , but sky ,time ,space are not the combination of parmanu (atom) .

7 . Parmanu (atom) have two State
a. State of motion 
b. Absolute rest
 
8. He explain nityam mandalam (in Sanskrit  गोलाकार ) that means a atom has a spherical shape .

According to dalton's atomic theory :-

• the discovery of atomic theory is attributed to jhon Dalton English chemist, physicist, and meteorologist.

1. All matter made up of  extremely small particles called atom.

2. It is indivisible.

3. It is indestructible.

4.  Two or more diffrent kinds of atom form a compound.

5.  A chemical reaction is a rearrangement of atoms .

6 . He explain the formation of different kinds of molecules by the combination of different atoms .

7.  Understand the origin and nature of electromagnetic radiation absorbed or emitted by atoms .

           Discovery of  electron 


     Electron was discover by j.j Thomson in 1897 time .
J.J Thomson  began experimenting with cathode ray tubes  .
A cathode ray tube is made of glass containing two thin pieces of metal ,called electrodes, are vaccum- sealed  glass tubes that have had most of the air removed  At one end of the tube, a high voltage is placed between two electrodes causing  a stream of particles to flow from the cathode ( the negative charged electrode)   to the  anode ( the positive charged electrode)  because the particle beam . The flow of current from cathode to anode the ray can be detected by painting a material known as phosphorus onto the far end of the tube beyond the anode . The phosphorus spark ,or emit light when impacted by the cathode ray .
Thomson also placed two magnets on both side of the tube, and observed that this magnetic field also deflected the cathode ray with this information and Thomson's

 mass of an electron .
                  Mass/charge ×charge                                                            =mass 
Charge on the electron  ÷ 
     
   

Thomson model  of atom (plum pudding theory ):- 




The plum pudding model given by j.j Thomson . It is a historical scientific model of the atom.
According to this model, the atom is a spehre who surrounded by a volume of  positive charge  like blue berries stuck into a muffins.or a plum pudding  and negatively charged electrons are embedded in it to balance the positive charge . The  electrons are like plum or blue berries in a pudding or muffins. 
However this model was discarded when Rutherford performed the famous alpha particles scattering experiment. This model was simillar to our solar system . With electrons revolving around a positively  charged,dense nucleus.  


  Rutherford's nuclear model of atom

Rutherford  and his student (hans Geiger  and Ernest Marsden )
Conducted his famous  Alpha-  particles scattering experiment in which a stream  of high energy Alpha particles was directed at a thin  foil of gold . The gold foil had a circular fluorescent zinc sulphide screen around it whenever Alpha - particles is the a particles struck the  screen, a tiny flash of light was produced at that point.
Rutherford tested  Thomson's hypoth-esis by devising his gold foil .

•  the gold foil was selected so as to obtain an extremely thin layer. The thickness of the gold foil was about 1000 atoms .

• doubly - charged  He (helium) ions are known as alpha particles, rapidly moving Alpha- particles possess a great deal of energy as, they have a mass of about 4amu .

--->> the hypothesis was that Alpha-particles would be deflected by the sub- atomic particles in the gold atoms .

 Rutherford  drew the following conc-lusions   :- 


1.  Most of the space in the atom is       empty as most of the Alpha-             particles  passed through the foil undeflected. 

2.  A few positively charged Alpha-particles were deflected. 
The deflection due to the enormous repulsive force .

3.  The positive charge has to be concentrated in a very small volume that repelled and deflected the positively charged Alpha-particles. 

4.  Rutherford showed the volume occupied bt the nucleus negligibly small as compared to the total volume of the atom . 

Atomic number and mass number :-

  Atomic number :- atomic no. Is defined as the total no. Of protons or electrons in an nucleus of each atom of the element.

It is represented by the latter Z
Example : - carbon  atomic no. Is 6 and it has 6 no. Of protons. 

Mass number :-  an elements mass no. Is the total number of the protons and the number of neutrons .(the small role of mass from electrons ) .it is represented by the latter A 

Example :- carbon atom no. 
Of protons =6  , no. Of neutrons = 6
                         
                       Mass =  12 



         Isotopes and  isobars 


Isotopes :- those elements that have the same atomic number but different mass number are referred to as isotopes. 

Example :- considering of hydrogen (H) atom  99.985% of hydrogen atoms contain only  one proton .

 This isotope called protium ( H1) .
 Rest of percentage of hydrogen atom contains two isotopes
1 proton and 1 neutron called deuterium .(D2)
And other one possessing 1 proton and 2 neutron  called  tritium .(T3)

Isobars :- the atoms having the  same mass number . But a different atomic number. 


Example :-  atomic no. Of Argon (Ar) is 18  and mass number is 40 , the atomic number is Potassium (k) is 19 and the mass number is simillarly  40
And also calcium is 20 and the mass number is 40 .
So Ar, K Ca are the same mass number But different atomic number so they isobars . 

      Thank you :)
          

Comments

Post a Comment

Popular posts from this blog

Heisenberg's Uncertainty Principle

Introduction Werner   Heisenberg   a German physicist  in 1927 stated uncertainty principle which is the consequence of dual behaviour of matter and radiation. It states that it is impossible to determine simulataneously, the exact position and exact momentum( or velocity) of an electron. Heisenberg's Uncertainty Principle states that there is inherent uncertainty in the act of measuring a variable of a particle. Commonly applied to the position and momentum of a particle, the principle states that the more precisely the position is known the more uncertain.  the momentum is and vice versa. This is contrary to classical Newtonian physics which holds all   variables of particles to be   measurable to an arbitrary uncertainty given good enough equipment. The Heisenberg Uncertainty Principle is a fundamental theory in quantum mechanics that defines why a scientist cannot measure multiple quantum variables simultaneously. Until the dawn of quantum me...
Post a Comment
Read more

CARBON AND ITS COMPOUNDS (PART-2)

  Homologous Series:   Series of organic compounds having the same functional group and chemical properties and successive members differ by a CH 2   unit or 14 mass units are known as Homologous series. Homologous series of Alkanes, Alkenes and Alkynes Characteristic of Homologous Series The successive members in homologous series differ by CH 2  unit or 14 mass unit. Members of given homologous series have the same functional group. All the members of homologous series shows similar chemical properties. Functional Group:   An atom or group of atoms present in a molecule which largely determines its chemical properties are called Functional Group. Nomenclature of Organic Compounds:   It is difficult to remember millions of compounds by their individual common name. Thus, to systematize the nomenclature of organic compounds IUPAC (International Union of Pure and Applied Chemistry) has given certain rule which is as follows: 1. Identify the Number of Carbon ...
13 comments
Read more

CARBON AND ITS COMPOUNDS

CARBON :- Carbon is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Carbon makes up only about 0.025 percent of Earth’s crust. Bonding in Carbon:   The Covalent bond, Electron dot structure, Physical properties of organic compounds, Allotropes of Carbon . Covalent Bond:   The atomic number of carbon is 6. Its electronic configuration is 2, 4. It requires, 4 electrons to achieve the inert gas electronic configuration. But carbon cannot form an ionic bond.                                                     It could gain four electrons forming C 4-  cation. But it would be difficult for the nucleus with six protons to hold on to ten electrons. It could lose four electrons forming C 4+ ...
42 comments
Read more