Classically, an electron can be in any orbit around the nucleus of an atom. Then what determines the typical atomic size? Why is an atom not, say, thousand times bigger than its typical size ? The question had greatly puzzled Bohr before he arrived at his famous model of the atom that you have learnt in the text. To simulate what he might well have done before his discovery, let us play as follows with the basic constants of nature and see if we can get a quantity with the dimensions of length that is roughly equal to the known size of an atom `(-10^(-10)m)`
Construct a quantity with the dimensions of length from the fundamental constants` e, m_(e)` and c. Determine its numerical value.

Explanation

Orbital radius of electron in `n^(th)` orbit from Bohr formula
`r_(n)=(n^(2)h^(2) epsi_(0))/(pi me^(2))`
for first orbit n=1,
`r_(1)=(h^(2)epsi_(0))/(pi me^(2))`
`=((6.625xx10^(-34))^(2)xx8.85xx10^(-12))/(3.14x9.1xx10^(-31)xx(1.6xx10^(-19))^(2))`
`=0.53xx10^(-10)m`
`:.r_(1)=0.53Å` which is the order of the dimension of the atom.