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Structure of an Atom

Dalton's Atomic Theory and Laws of Chemical Combination-Group A

Dividing Matter

Matter cannot be divided infinite number of times.


For example, if we keep chopping a log of wood into smaller and smaller pieces, then we will reach a point when the wood will not be divisible any further. Minute particles of wood will remain and these will not be visible to the naked eye. This is true for all forms of matter.The same was believed by the early Indian and Greek philosophers. In India, around 500 BC, an Indian philosopher named Maharishi Kanad called matter as padarth and these smallest particles (atoms) as ‘parmanu’. The word ‘atom’ is derived from the Greek word ‘atomos’ which means ‘indivisible’. It was the Greek philosopher Democritus who coined the term. However, for these ancient thinkers, the idea of the minute indivisible particle was a purely philosophical consideration. 



By the end of the eighteenth century, scientists had begun to distinguish between elements and compounds. Two French chemists named Antoine Lavoisier and Joseph Proust observed that elements combine in definite proportions to form compounds. On the basis of this observation, each of them proposed an important law of chemical combination. The laws proposed by them helped Dalton formulate his atomic theory.

Dalton’s Atomic Theory 

In the early nineteenth century, an English chemist named John Dalton proposed a theory about atoms. Known as ‘Dalton’s atomic theory’, it proved to be one of the most important theories of science. The various laws of chemical combination also supported Dalton’s theory. Dalton asserted that ‘atoms are the smallest particles of matter, which cannot be divided further’. He published his atomic theory in 1808 in his book A New System of Chemical Philosophy. The postulates of Dalton’s atomic theory are as follows:

  • All matter is made up of very tiny particles. These particles are called atoms.
  • An atom cannot be divided further, i.e., atoms are indivisible.
  • Atoms can be neither created nor destroyed in a chemical reaction.
  • All atoms of an element are identical in all respects, e.g. in terms of mass, chemical   properties, etc.
  • Atoms of different elements have different masses and chemical properties.
  • Atoms of different elements combine in small whole-number ratios to form compounds .
  • In a given compound, the relative numbers and types of atoms are constant.


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