Very Short Question and Answers - Comparison of Atomic Models

J.J. Thomson proposed the Plum Pudding Model in 1898.

The Nuclear Model describes the atom as having a dense, positively charged nucleus with electrons orbiting around it.

Electrons move in fixed orbits, also known as energy levels, around the nucleus.

Thomson's model describes the atom as a sphere of positive charge with electrons embedded within it.

Thomson's Model did not account for experimental observations, such as those from Rutherford's scattering experiment.

Rutherford's experiment revealed that an atom has a dense nucleus and that most of the atom is empty space.

Bohr's Model explained the stability of atoms and quantized energy levels of electrons.

Electrons are randomly distributed within a positively charged sphere.

Rutherford's Model could not explain why electrons do not spiral into the nucleus.

Bohr’s Model restricts electrons to specific, quantized orbits or shells around the nucleus.

Thomson's Model was the first to introduce the concept of electrons in the atom.

Rutherford introduced the concept of a dense nucleus and that most of the atom is empty space.

Bohr introduced the concept of energy levels and electron transitions between them.

It explained the overall neutrality of atoms.

Electrons were believed to orbit the nucleus, but not in any specific energy levels.

It provided an explanation for stable electron orbits and atom stability.

Bohr's Model failed to explain the spectra of atoms with more than one electron.

All models agree that atomic structure includes a nucleus surrounded by electrons.

The term refers to Thomson's model where electrons (plums) are embedded in a positive 'pudding' shape.

Bohr’s Model is associated with the concept of quantized energy levels.