Lesson 5: Corpuscles to Chemical Atomic Theory (The Development of Atomic Theory)
2 likes•3,050 views
The document covers key historical figures in chemistry, including Robert Boyle, Antoine Lavoisier, John Dalton, Joseph Gay-Lussac, Amedeo Avogadro, and Dmitri Mendeleev, detailing their contributions to the understanding of elements, compounds, and atomic theory. Specific fundamental laws such as the conservation of mass, definite proportions, and multiple proportions are highlighted. It concludes with Mendeleev's development of the periodic table, which organized elements by atomic weight and predicted the existence of undiscovered elements.
Lesson 5: Corpuscles to Chemical Atomic Theory (The Development of Atomic Theory)
- 1. LESSON 5:
- 2. • He recognized elements as the simplest substances that constitute mixtures, and that elements are those that cannot be decomposed into other substances via chemical reactions. • He emphasized the need to observe and test the presence of corpuscles in alchemical experiments. ROBERT BOYLE
- 3. ROBERT BOYLE • Had the idea of: Corpuscles “certain primitive and simple, or perfectly unmingled bodies” that were indivisible and whole.
- 4. Antoine Lavoisier • Father of Modern Chemistry • He opposed the Phlogiston Theory (a superseded scientific theory that postulated that a fire-like element called phlogiston is contained within combustible bodies and released during combustion)
- 5. Antoine Lavoisier Defined CHEMICAL ELEMENT (substance that cannot be broken down into simpler components.) Defined COMPOUND (a substance composed of these elements.) Made an initial list of 33 elements, and created a systematic way of naming elements and the compounds they created. He also wrote the first Chemistry textbook.
- 6. JOHN DALTON • His Chemical Atomic Theory merged the concepts of the atom and element
- 7. • Gases, and all chemically inseparable elements, are made of atoms. • The atoms of an element are identical in their masses. • Atoms of different elements have different masses. • Atoms combine in small, whole number ratios. Chemical atomic theory
- 8. •Antoine Lavoisier’s Law of Conservation of Mass •Joseph Proust’s Law of Definite Proportions •John Dalton’s Law of Multiple Proportions 3 Fundamental laws
- 9. Antoine Lavoisier’s Law of Conservation of Mass mass is neither created nor destroyed during an ordinary chemical reaction or physical reaction. 3 Fundamental laws
- 10. • Antoine Lavoisier’s Law of Conservation of Mass 3 Fundamental laws
- 11. •Joseph Proust’s Law of Definite Proportions chemical compound contains the same elements in exactly the same proportions by mass regardless of the sample of the source of the compound. 3 Fundamental laws
- 12. • Joseph Proust’s Law of Definite Proportions 3 Fundamental laws
- 13. •John Dalton’s Law of Multiple Proportions if two or more different compounds are composed of the same two elements, then the ratios of the masses of the second element, combined with a certain mass of the first element is always a ratio of small whole numbers 3 Fundamental laws
- 14. • John Dalton’s Law of Multiple Proportions 3 Fundamental laws
- 15. • that elements were made of the same atoms and had properties unique to the element, while chemical compounds were made of different combined or compounded atoms, and exhibited different sets of properties. • that one could compute the weights of elements (and their atoms) by looking at comparable amounts of the compounds they formed. • that one could compute atomic weights compared to a reference. Dalton’s Chemical Atomic Theory
- 16. Joseph Gay-Lussac He determined that oxygen gas was made of 2 atoms of oxygen and took the form of a molecule instead of an atom. This offered the possibility that an element wasn’t necessarily made up of one atom, thus distinguishing the atom from the molecule.
- 17. Amedeo Avogadro He figured out a reliable way of weighing atoms and molecules. (MOLE) He determined that equivalent volumes of two gases under similar conditions contained equal numbers of particles, and that differences in their masses was a result of a difference in their molecular mass.
- 18. He published a periodic table of elements that ordered elements according to their atomic weights. He noted patterns in their properties that enabled him to predict the discovery of other elements. His table became the basis of the modern Periodic Table. Dmitri Mendeleev