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Rutherford Atomic Model

 

Introduction

Rutherford Atomic Model - J. J. Thomson's "plum pudding" model was unable to account for several experimental findings related to the atomic structure of elements. British scientist Ernest Rutherford carried out an experiment, and using the results of this experiment, he created Rutherford's Atomic Model and described the atomic structure of the elements.

Experiment:

In an experiment, Rutherford bombarded a thin sheet of gold with -particles and then tracked the paths taken by the particles after they made contact with the foil.

In his experiment, Rutherford fired high-energy beams of -particles at a 100 nm-thick gold sheet coming from a radioactive source. He surrounded the thin gold foil with a fluorescent zinc sulphide screen in order to analyze the deflection the -particles experienced. Rutherford made certain claims that were at odds with Thomson's atomic model.

Observations:

Rutherford's observations lead him to draw the following conclusions:

• Most of the space in an atom is unoccupied since a significant portion of the -particles blasted towards the gold sheet went through the sheet without any deflection.

• Because some of the -particles were somewhat deflected by the gold sheet, the positive charge in an atom is not spread evenly. An atom's positive charge is confined to a relatively tiny volume.

• Only a handful of the -particles had deflection angles that were almost 180 degrees, meaning that very few of the -particles were deflected back. As a result, in relation to the total volume of an atom, the positively charged particles' volume is extremely tiny.

Postulates:

The Rutherford atomic model states:

• An atom's positive charge and the majority of its mass are packed into a very tiny volume. The nucleus of the atom is what he referred to as.

• According to Rutherford's theory, an atom's nucleus is surrounded by electrons that are negatively charged. He also asserted that the electrons that surround the nucleus travel in a circular pattern at extremely high speeds. He gave these elliptical routes the term orbits.

• A powerful electrostatic force of attraction holds the negatively charged electrons and the positively charged mass of particles that makes up the nucleus together.

Defects of Rutherford Atomic Model:

Despite being founded on experimental evidence, the Rutherford atomic model proved unable to account for several phenomena.

• Rutherford's theory was unable to account for an atom's stability. According to Rutherford's assumption, electrons orbit an atom's nucleus in a fixed orbit at a very fast speed. However, Maxwell showed how electromagnetic radiations are produced when charged particles are propelled. Consequently, electromagnetic radiation will be produced when electrons spin around the nucleus.

• The electronic motion will provide energy to the electromagnetic radiation, which will cause the orbits to gradually contract. In the atom's nucleus, the orbits will eventually contract and collapse. Rutherford's model will collapse in 10-8 seconds if Maxwell's explanation is used, according the calculations. As a result, the Rutherford atomic model did not conform to Maxwell's theory and was unable to account for the stability of an atom.

• Rutherford's hypothesis was lacking since it said nothing about how the electrons were arranged in their orbit. This was one of the Rutherford atomic model's biggest flaws.





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