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Understanding Chemistry: Matter, Mixtures, and Atomic Theory Explained

Chemistry is the study of matter's composition, structure, properties, and changes. Matter, anything with mass that occupies space, can be categorized into elements and mixtures. Elements consist of atoms, the smallest units maintaining their properties. Mixtures can be separated physically, unlike compounds, which have fixed compositions. This text explores key concepts such as the laws of definite proportions, conservation of mass, and atomic theory, including the discovery of the electron and models of the atom, to provide a comprehensive understanding of how matter functions.

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Understanding Chemistry: Matter, Mixtures, and Atomic Theory Explained

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Presentation Transcript

  1. What is Chemistry? • The study of the composition, structure, and properties of matter, and the changes matter undergoes.

  2. What is Matter? • Anything that has mass and occupies space.

  3. How Can We Study Matter When There is So Much of It? • All of matter is made up of just a few “kinds” of matter. • People once believed that everything was made up of air, earth, fire and water. • Each “kind” of matter has a smallest possible piece that has all the properties of that “kind” of matter.

  4. How Can We Study Matter When There is So Much of It? • Today, we call those “kinds” of matter elements. • The smallest piece of an element that has the properties of that element is an atom.

  5. Matter can be . . . • A mixture • A kind of matter that can be separated into two or more other kinds of matter by physical processes. • A substance • A kind of matter that can not be separated into other kinds of matter by physical processes.

  6. Separation of a Homogeneous Mixture

  7. Separation of a Heterogeneous Mixture

  8. When a Mixture is Separated . . . • There is no change in the chemical identity of any of its components (substances). • We take advantage of differences in physical properties to achieve the separation.

  9. Example of a Physical Change

  10. Example of a Chemical Change

  11. Mixtures vs. Compounds • A mixture can have a variable composition but a compound has a fixed composition. • Example: H2O is 11.19% H, 88.81% O • When a mixture is formed, the individual substances retain their properties, but when a compound is formed, the elements lose their properties.

  12. Law of Definite Proportions Law of Multiple Proportions Law of Conservation of Mass Evidence for the Atomic Theory

  13. Definite / Multiple Proportions

  14. Conservation of Mass

  15. Discovery of the Electron

  16. Charge of the Electron

  17. Plum Pudding Atom

  18. A Test of the “Plum-Pudding Hypothesis”

  19. Nuclear Model of the Atom

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