Physics

4.2 - Developing the Model of the Atom

7 min

Early ideas about atoms

The plum pudding model

Alpha scattering experiment

Bohr, protons and neutrons

note 1 of 3

The plum pudding model

In 1897, J. J. Thomson discovered the electron - a tiny, negatively charged particle.
This showed atoms are not indivisible spheres, but contain smaller charged parts.
Thomson proposed the plum pudding model:
- The atom is a ball of positive charge.
- Tiny negative electrons are embedded inside it.

A pale green ball holding eight small pink electrons, each marked with a minus sign, labelled ball of positive charge and negative electron.

note 2 of 3

Rutherford's alpha scattering and the nuclear model

In 1909, Ernest Rutherford (with Hans Geiger and Ernest Marsden) fired positively charged alpha particles at a thin sheet of gold foil.
If the plum pudding model had been correct, the alpha particles should have passed straight through or been deflected only slightly.

Observations and conclusions

Most particles passed straight through - The atom is mostly empty space.
A small number were deflected through large angles - The atom's mass and positive charge are concentrated in a tiny central nucleus.
A few bounced almost straight back - The nucleus is very dense and positively charged, repelling the positive alpha particles.

This led to the nuclear model: a tiny, dense, positively charged nucleus at the centre, surrounded by electrons.

A box source fires a beam of alpha particles at gold foil inside a ring-shaped screen, labelled circular fluorescent screen, thin gold foil, most particles are undeflected, and small number deflected through large angles.

note 3 of 3

Bohr's energy levels

Rutherford's model had electrons in a "cloud" around the nucleus, but electrons in this arrangement would spiral inwards, causing the atom to collapse.
Niels Bohr adapted the model:
- Electrons orbit the nucleus only at fixed distances, called energy levels or shells.
- Electrons can exist in these allowed shells, but not in between them.
Bohr's theoretical calculations matched experimental observations.

A grey nucleus ringed by two circles, two pink electrons on the inner one and eight on the outer, labelled nucleus, electron, and energy levels or shells.

key terms

TermDefinition

ElectronA tiny, negatively charged particle found in atoms.

Plum pudding modelAn early model of the atom as a ball of positive charge with negative electrons embedded in it.

Nuclear modelA model of the atom with a tiny, dense, positively charged nucleus at the centre, surrounded by electrons.

Energy levelA fixed distance from the nucleus where electrons can orbit. It is also called a shell.

end of notes

Key points to remember

The plum pudding model

In 1897, J. J. Thomson discovered the electron - a tiny, negatively charged particle.

This showed atoms are not indivisible spheres, but contain smaller charged parts.

Thomson proposed the plum pudding model:

The atom is a ball of positive charge.
Tiny negative electrons are embedded inside it.

Rutherford's alpha scattering and the nuclear model

In 1909, Ernest Rutherford (with Hans Geiger and Ernest Marsden) fired positively charged alpha particles at a thin sheet of gold foil.

If the plum pudding model had been correct, the alpha particles should have passed straight through or been deflected only slightly.

Observations and conclusions

Most particles passed straight through - The atom is mostly empty space.

A small number were deflected through large angles - The atom's mass and positive charge are concentrated in a tiny central nucleus.

A few bounced almost straight back - The nucleus is very dense and positively charged, repelling the positive alpha particles.

This led to the nuclear model: a tiny, dense, positively charged nucleus at the centre, surrounded by electrons.

Bohr's energy levels

Rutherford's model had electrons in a "cloud" around the nucleus, but electrons in this arrangement would spiral inwards, causing the atom to collapse.

Niels Bohr adapted the model:

Electrons orbit the nucleus only at fixed distances, called energy levels or shells.
Electrons can exist in these allowed shells, but not in between them.

Bohr's theoretical calculations matched experimental observations.