History of the atom. Atoms (created by the Big Bang) are the smallest unit that makes up matter.

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History of Atomic Structure

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Presentation transcript:

History of the atom

Atoms (created by the Big Bang) are the smallest unit that makes up matter

Atoms All life, whether in the form of trees, whales, mushrooms, bacteria or amoebas, consists of cells. Similarly, all matter, whether in the form of aspirin, gold, vitamins, air or rocks, consists of atoms. Regardless of size, atoms are made up of the same basic units.

History of the atom : Democritus Democritus (b. c. 460 BC; d. c. 370 BC) postulated the existence of invisible atoms, characterized only by quantitative properties: size, shape, and motion. Imagine these atoms as indivisible spheres, the smallest pieces of an element that still behave like the entire chunk of matter.

Aristotle  emphasized that nature consisted of four elements: air, earth, fire, and water. He thought these are bearers of fundamental properties, dryness and heat being associated with fire, heat and moisture with air, moisture and cold with water, and cold and dryness with earth.  He did not believe in discontinuous or separate atoms but felt that matter was continuous

John Dalton Dalton ( ) Theorized that all matter is made up of tiny particles called atoms. No other smaller particles exist and the atom is indivisible (same as Democritus) Atoms of the same element are identical Atoms of different elements are different

Atoms cannot be made or destroyed All atoms of the same element are identical Different elements have different types of atoms

J. J. Thomson J.J. Thomson ( ) Played with cathode ray tubes and found that the atom was divisible! He discovered that atoms consisted of both + and – charges. “Plum Pudding” model or “Watermelon” model of the atom:

J. J. Thomson Later on he discovered a positively charged particle (proton) and adapted his model:

Cathode ray tube

Ernest Rutherford ( ) Performed the “gold foil experiment”, in which he discovered that the atom is made up of mostly empty space. Most of the mass of an atom is concentrated in a tiny nucleus that has a positive charge. Electrons orbit the nucleus like planets in the solar system

Gold foil experiment

Niels Bohr (1885 – 1962)  Discovered that electrons exist around the nucleus in specific energy levels or electron shells.  Different levels have different sizes and capacities.  They are numbered 1 – 7, with level 1 closest to the nucleus.  Electrons prefer to be close to the nucleus, but some levels fill up fast, and some may only fill partially.  The maximum number of electrons that a given shell can hold can be calculated:

Niels Bohr

The Bohr-Rutherford Model of the Atom

 An element is defined by the number of protons it contains.  To remain electrically neutral, it must contain the same number of protons and electrons.  The number of neutrons can vary in an element.  Because electrons are so small, nearly all the mass of an atom is contained in it’s nucleus.  The nucleus is very small and dense compared to the whole atom

Using a Periodic Table Tells you the number of protons and electrons

Drawing: Carbon Atom Rutherford-Bohr Model

Drawing: Carbon Atom Simplified atomic model

James Chadwick (1891 – 1974) Discovered the neutron = a particle equal in size to the proton, but with no charge. The neutron is found in the nucleus with the protons.

The Bohr-Rutherford Model