This later became known as the plum pudding model.

This is because the alpha particles are heavy and the charge in the "plum pudding model" is widely spread.

The data generated from the gold foil experiment demonstrated that the plum pudding model of the atom was incorrect.

This paper presents the classical "plum pudding model" from which the Thomson Problem is posed.

The popular theory of atomic structure at the time of Rutherford's experiment was the "plum pudding model".

Thomson also proposed the plum pudding model, which was later confirmed as scientifically incorrect by Rutherford.

The plum pudding model predicted that the alpha particles should come out of the foil with their trajectories being at most slightly bent.

J. J. Thomson proposes the plum pudding model for the atom.

Thomson imagined the atom as being made up of these corpuscles orbiting in a sea of positive charge; this was his plum pudding model.

This disproved the plum pudding model of the atom, and led to the Rutherford model (also called the planetary model).

The plum pudding model of J.J. Thomson also had rings of orbiting electrons.

In his plum pudding model, Thomson stated that an atom consisted of negative electrons randomly scattered within a sphere of positive charge.

If Thomson's Plum Pudding model was to be accurate, the big alpha particles should have passed through the gold foil with only a few minor deflections.

The nucleus was discovered in 1911, as a result of Ernest Rutherford's efforts to test Thomson's "plum pudding model" of the atom.

The physicist J. J. Thomson posed the problem in 1904 after creating his so-called plum pudding model of the atom.

He proposes the Rutherford model of the atom and demonstrates that J. J. Thomson's plum pudding model is incorrect.

Ernest Rutherford's gold foil experiment disproved the plum pudding model of the atom which suggested that the mass and positive charge of the atom are almost uniformly distributed.

Rutherford used alpha particles emitted by radium bromide to infer that J. J. Thomson's Plum pudding model of the atom was fundamentally flawed.

In 1903 Thomson had suggested that the atom was a sphere of uniform positive electrification, with electrons scattered through it like plums in a pudding, the plum pudding model.

Thomson created the plum pudding model, which stated that an atom was like plum pudding: the dried fruit (electrons) were stuck in a mass of pudding (protons).

Unlike the plum pudding model, the positive charge in Nagaoka's "Saturnian Model" was concentrated into a central core, pulling the electrons into circular orbits reminiscent of Saturn's rings.

The plum pudding model was the prevailing theory on the structure of the atom until it was disproved by Ernest Rutherford in his analysis of the gold foil experiment, published in 1911.

In the plum pudding model, proposed by J. J. Thomson in 1904, the atom is composed of electrons surrounded by a 'cloud' of positive charge to balance the electrons' negative charge.

Rutherford directed the famous Geiger-Marsden experiment in 1909 which suggested, upon Rutherford's 1911 analysis, that the so-called "plum pudding model" of J. J. Thomson of the atom was incorrect.

Under the prevailing plum pudding model, the alpha particles should all have been deflected by, at most, a few degrees; measuring the pattern of scattered particles was expected to provide information about the distribution of charge within the atom.