The Rutherford model of the atom is a model of the atom devised by the British physicist Ernest Rutherford. Rutherford’s new model for the atom is based on the experimental results obtained from the Geiger-Marsden experiments (also called the Rutherford gold foil experiment). The Geiger–Marsden experiments were performed between 1908 and 1913 by Hans Geiger (of Geiger counter fame) and Ernest Marsden (a 20-year-old student who had not yet earned his bachelor’s degree) under the direction of Ernest Rutherford.
Rutherford’s idea was to direct energetic alpha particles at a thin metal foil and measure how an alpha particle beam is scattered when it strikes a thin metal foil. A narrow collimated beam of alpha particles was aimed at a gold foil of approximately 1 μm thickness (about 10,000 atoms thick). Alpha particles are energetic nuclei of helium (usually about 6 MeV). Alpha particles, which are about 7300 times more massive than electrons, have a positive charge of +2e. Because of their relatively much greater mass, alpha particles are not significantly deflected from their paths by the electrons in the metal’s atoms.
According to Thomson’s model, if an alpha particle were to collide with a plum-pudding atom, it would just fly straight through, its path deflected by at most a fraction of a degree. But in the experiment, Geiger and Marsden saw that most of the particles were scattered through rather small angles, but this was a big surprise. A small fraction of them is scattered through very large angles, approaching 180° (i.e., they recoiled backward).
In Rutherford’s words:
“It is almost as incredible as if you had fired a fifteen-inch shell at a sheet of tissue paper, and it came back and hit you.”
Rutherford assumed that to deflect the alpha particle backward, and there must be a very large force. This force could be provided as an only result of a collision with a massive target or from an interaction with an electric or magnetic field of great strength. Previous experiments showed that the deflections had to be electrical or perhaps magnetic in origin.
As a result, Rutherford abandoned the Thomson model. Geiger-Marsden experiments were a landmark series of experiments. Scientists discovered that every atom contains a nucleus (whose diameter is of the order of 10-14m.). Its positive charge and most of its mass is concentrated in a small region called an atomic nucleus. In Rutherford’s atom, the diameter of its sphere (about 10-10 m) of influence is determined by its electrons. In other words, the nucleus occupies only about 10-12 of the total volume of the atom or less (the nuclear atom is largely empty space), but it contains all the positive charge and at least 99.95% of the total mass of the atom.
Based on these results, Ernest Rutherford proposed a new model of the atom. He postulated that the positive charge in an atom is concentrated in a small region (in comparison to the rest of the atom) called a nucleus at the center of the atom with electrons existing in orbits around it. Furthermore, the nucleus is responsible for most of the mass of the atom.
Failure of Rutherford Model
It must be noted that the Rutherford model of the atom was not the first model which proposed a nuclear structure. The idea of a nuclear structure was previously proposed in 1903 by a Japanese physicist Hantaro Nagaoka, who rejected Thomson’s model because opposite charges are impenetrable. His model was known as the Saturnian model of the atom. According to this model, the atom consists of a massive positive center surrounded by many orbiting electrons in the manner of Saturn and its rings.
Nagaoka’s planetary model had two predictions:
- a very massive atomic center (in analogy to a very massive planet)
- electrons revolving around the nucleus, bound by electrostatic forces
Ernest Rutherford successfully confirmed both predictions in 1911. However, other details of the model were incorrect. Notwithstanding the Rutherford model of the atom was very close to the modern concept of the atom, it was based on classical physics. But neither classical physics nor the Rutherford model can explain the following problem. Why the negatively charged electrons are prevented from falling into the positively charged nucleus? Forces between static electrically charged particles are governed by the Coulomb’s law:
Rutherford suggested that perhaps the electrons revolve in orbits about the nucleus. In classical mechanics, a condition for the dynamic stability of such systems of rotating particles is that only forces of attraction act between its components.
Classical physics also states that any accelerating electric charge (oscillating or revolving) emits electromagnetic radiation. As a result, an electron orbiting inside an atom should be continually losing energy, and it should spiral into the nucleus within a fraction of a second. Physicists calculated that the electron should lose all of its energy and spiral down into the proton in only about 0.000000000001 seconds, which means that every atom should not exist longer than a mere 10-12 seconds.
The solution to the problem of the stability of the electrons in an atom was provided by young Danish physicist Niels Bohr working with Ernest Rutherford at the University of Manchester in 1913. His model adopted Planck’s quantum hypothesis, and he proposed a model in which the electrons of an atom were assumed to orbit the nucleus but could only do so in a finite set of orbits. He postulated that an atom emits or absorbs energy only in discrete quanta corresponding to the absorption or radiation of a photon.