A Timeline on Atomic Structure

In 400 BC, Atomism of Democritus insists that all problems are composed of small, non-destructive units he calls Atom.

1803 John Dalton suggests that elements are composed of the same atoms of the same mass and compounds are bonded from atoms of different elements.

In 1873, James Clerk Maxwell proposed the theory of electromagnetism and tied light to electromagnetic waves.

In 1879, Sir William Crooks experimented with a cathode ray tube to confirm the study of early scientists by clearly demonstrating that the cathode lines are negatively charged.

Marie Sklodowska Curie studied the collapse of uranium and thorium in 1898, discovered Radium and Pol and developed the term radiation.

In 1900 Max Planck proposed a quantitative idea to explain how shiny lighting objects shine.

In 1900 Frederic Sodie proposed the term "isotope" to explain unintentional destruction of radioactive elements.

In 1903, Hanaka Nagaoka proposed an atomic model called Saturn model to describe the structure of atoms.

In 1914, H. G. J. Mosley discovered that the number of protons in the element determines its atomic number.

In 1922 Niels Bohr proposed an atomic structure theory that the atom's external orbit can contain more electrons than the internal orbit.

Welcome to atomic structure timeline. This site is investigating the discovery related to the atomic structure of electrons, protons, neutrons and so on. Since many scientists have been spending decades researching topics, the date used for the event is published. Please check the link for more detailed material. The most important thing is to have fun. The found cathode ray goes straight from the cathode, causes the glass to emit fluorescence, applies a negative charge to the collided object, is deflected by the electric field and the magnet to generate a negative charge, rotates the rotation path, Indicates that there is.

The atomic structure is an abundant subject, experimental research is done in various ways, among which optical, x-ray and radio frequency (rf) spectroscopy are particularly important. The atomic spectrum is affected by external magnetic field (Zeeman effect) and electric field (Stark effect). Coupling of nuclear atoms with degrees of freedom of atoms leads to small effects such as electrical and magnetic hyperfine structure and isotope drift, but only in this detail, the atomic structure has atomic mass A (or equivalently neutron Number N). ) The internal trapping parallel to the electron capture mechanism and nuclear gamma collapse of nuclear beta decay is another kind of atom-nuclear interaction.

Regular physical chemical substances are composed of atoms. An atom is defined by its atomic number Z. Neutral atoms have Z electrons whose negative charges are matched by equal positive charges on small, large cores. Depending on the nuclear electrostatic attraction, each of the electronic structures of the atoms, the electrostatic repulsion between the electrons is suitable for small scale quantum motion law material, and ultimately is characterized by quantum physics. Known as Pauli's principle, it limits the extent to which a set of electrons is compressed. The atoms may be present in a number of states and each state has atomic energy E and angular momentum J. a constant degree of freedom of the ground state and although they do not have clear boundaries, , But the interaction with other atoms, if they have one atom. Effective diameter about 0.04 to 0.28 nm