Q. 94.7( 11 Votes )

# Using Rutherford

Answer :

According to Rutherford’s model of an atom, for dynamic stability of an atom the electronic forces on the electron must account for the centripetal forces acting on it, thus, Where, me is the mass of the electron,

vn is the velocity of the electron in the nth shell

rn is the radius of the orbit

Fe is the electrostatic force between revolving electron and nucleus

Fc is the centripetal force required by the electron to move in circular orbits of radius r

By coulomb’s law we can write,  For a hydrogen atom Z=1, The kinetic energy (K) is, The Electrostatic potential energy (U) is, (The negative sign in U signifies that the electrostatic force is in the –r direction.) Thus, the total energy E of the electron in a hydrogen atom is,  The total energy being negative signifies that the electron is bound to the nucleus.

OR

Suppose m be the mass of an electron and vn be its speed in the nth orbit of radius rn. From Rutherford model, the centripetal force for revolution is produced by electrostatic attraction between electron and nucleus.

For dynamic stability of an atom the electronic forces on the electron must account for the centripetal forces acting on it, thus, Where, me is the mass of the electron, vn is the velocity of the electron in the nth shell and rn is the radius of the orbit

By coulomb’s law we can write,  For a hydrogen atom Z=1, Bohr’s model of atom postulates that the values of angular momentum of the electron should be the integral multiples of h/2 , so, where n is an integer, rn is the radius of nth possible orbit and vn is the

speed of moving electron in the nth orbit.

Using the above relation and equation (a) we get,  no

The Expression of Bohr’s radius can be obtained by substituting n=1, Substituting the values of all the constants,

We get the value Bohr’s radius as, a0 = 5.29 × 10-11 m

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Using Rutherford Physics - Board Papers