1 / 23

Atomic Theory

Explore the historical development of atomic theories from Greek philosophers to modern scientists. Learn about the key contributors and their groundbreaking experiments, including Dalton's atomic theory, Rutherford's gold foil experiment, and the development of the Bohr model. Understand concepts such as isotopes and ions in the study of atomic structure.

ginol
Download Presentation

Atomic Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Atomic Theory Chemistry

  2. Early Atomic Theories • - first theory of elements was by Greek philosopher Plato (440BC) • his student Aristotle carried out his work (384-322BC) • emphasized the five elements that all matter is made of: • 1 • 2 • 3 • 4 • 5

  3. Indivisible particles • the less popular theory was by the philosopher Democritus(470-370BC) • all matter was divisible up to a certain point • you eventually get down to a particle that is indivisible • the Greek word translates to “not cuttable” or atomos • Aristotle’s idea was followed for several centuries

  4. John Dalton • first atomic theory 1803-1810, with the criteria: • Elements are composed small, indivisible particles called atoms • Atoms of the same element have the same size and weight • Atoms of different elements have different size and weight • Atoms cannot be created nor destroyed • Compounds are formed by the addition of two or more different elements in simple whole number ratios • In chemical reactions, atoms are combined, separated, or generally rearranged

  5. Dalton’s Theory of Compounds Law of Definite Proportions: compounds are defined by their unique ratio of elements Law of Multiple Proportions: elements may combine in multiple ratios to make different compounds Give two (or more) compounds involving the following elements. Do not use any other elements. a) Hydrogen and Oxygen b) Nitrogen and Oxygen c) Carbon and Oxygen

  6. Antoine Lavoisier (late 1700s) • Early experiments in quantitative chemistry • Oxygen theory of combustion (opposes phlogiston theory) • Age 28 marries Marie-Anne Paulze (13 years old) • Favor to his boss • Expert on language, translates other chemist works • Lab tech, writes all reports, technical drawings • Executed during French revolution • Wife rescued his works

  7. Joseph Priestly (1700s) • Highly religious Christian scientist, known as a founder of the Unitarians • Experimented and observed several different gases or “ airs“, notably: • Isolated and discovered pure, elemental oxygen • Found its connection with respiration, and its function in blood • Unfortunately connected many ideas to phlogiston theory

  8. Michael Faraday (mid 1800s) • discovers electric charge, which has two types: • positive and negative • similar charges repel; opposite charges attract • charges can be transferred • such charged particles are called ions • this means “wanderer”

  9. Svante Arrhenius • found that when exposed to a charge, ions moved towards electrodes: • due to their attraction, the ions are labeled: • Cation = positive ion • Anion = negative ion

  10. J.J. Thomson (1897) • used a Crook’s tube, which is a simple vacuum tune and ran an electric current through it • a visible ray shot from the negative side to the positive side • since it was a vacuum tube, there would be nothing to transfer this, so it must be a particle • since it came from electricity, henamed it the electron • later experiment used a magnet to bend the ray, proving that it has a negative charge

  11. Cathode Ray Tube

  12. Robert Millikan(1908) • Oil drop experiment proved that there is a fundamental charge • all charges come in multiples of a certain number: • e = 1.6 x 10-19 C

  13. Model of the atom • Dalton’s atomic theory no longer works since atoms aredivisible into subatomic particles • Thomson proposes the plum pudding model

  14. Ernest Rutherford (1907) • used the α-particle discovered by Henri Becquerel to prove Thomson’s model • this was his famous gold foil experiment • actually performed by Hans Geiger and Ernest Marsden, based on Rutherford’s theories

  15. Ernest Rutherford (1907) • Major conclusions: • The nucleus is very small and dense, with a positive charge. • Most of the atom is empty space

  16. James Chadwick(1932) • also used alpha particles shot at a beryllium foil • a piece of paraffin wax caught the radiation, and hydrogen atoms were displaced • his particle did not have a charge and was as heavy as hydrogen • this was the neutron

  17. The Bohr Model • chemist G.N. Lewis remarked that the atom was like a seed, composed of a kernel and shell • the name nucleus was adopted, Greek for kernel • Neils Bohr proposed that the atom worked like planets • nucleus was heavy like the Sun • electrons surrounded the nucleus, in circular orbits • this model proved to be wrong, but is still used for simplicity

  18. Atomic structure

  19. Isotopes • Meaning “same place” • Refers to location on periodic table • Elements have same protons, but different neutrons • Usually expressed as a mass numbers • the sum of protons plus neutronsEx Carbon-14 is used in dating artifacts and very old samples. How many neutrons does carbon 14 have?

  20. Ions • Caused by an imbalance of electrons • More electrons means a negativecharge

  21. Complete the table

More Related