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In class assignment

In class assignment Draw in your notes the two pie charts in figure 2-3, page 39, of your textbook. Read pages 41 -42 in your textbook. Record in your notes the following terms and their definitions as found in your textbook. Chemical formula pure substance mixture

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In class assignment

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  1. In class assignment Draw in your notes the two pie charts in figure 2-3, page 39, of your textbook. Read pages 41 -42 in your textbook. Record in your notes the following terms and their definitions as found in your textbook. Chemical formula pure substance mixture heterogeneous mixture homogeneous mixture immiscible miscible

  2. Chemical Formulas - The chemical symbol and the numbers indicating the atoms contained in a molecule

  3. Pure Substance – matter with a fixed composition and definite properties • Can be an element or a compound • Cannot be broken down by physical actions such as boiling or melting • Ex: Hydrogen, Helium, Carbon, Gold, Silver, Oxygen, Nitrogen, Argon, Calcium, PotassiumEx of compounds: Methane, carbon monoxide, carbon dioxide, pure water and table salt (sodium chloride).

  4. Mixture – a combination of more than one pure substance • Can be broken down by physical actions • Ex: sand and sugar

  5. Ex: Is grape juice a mixture or pure substance? In chemistry grape juice is not a pure substance. It is a mixture of many pure substances like water, sugars, and acids. It can be separated.

  6. Mixture Classification - how thoroughly the substances mix 1. Homogeneous - all parts are the same ex: salt with water brass – mix of copper and zinc 2. Heterogeneous – not all parts are the same ex: sand and water

  7. Miscible vs. Immiscible Pertains to liquid mixtures miscible – 2 or more liquids that dissolve into each other immiscible – liquids that do not dissolve

  8. Chemical formulas show how many atoms of each element are in the basic unit of a substance. • Number of atoms is written as a subscript • Ex: C6H12O6 • means: 6 atoms of C (carbon) • 12 atoms of H (hydrogen) • 6 atoms of O (oxygen) • No subscript means 1 atom present • Ex: H2O not H2O1

  9. Number in front shows the number of molecules. • Ex: 2 AgNO3 (silver nitrate) • 2 molecules of silver nitrate • 2 atoms of Ag (silver) • 2 atoms of N (nitrogen) • 6 atoms of O (oxygen)

  10. Sometimes groups of atoms act as a single atom and they are put in parentheses with a subscript. All elements in the parentheses should be multiplied by that subscript. Fe(OH)3 (iron) 1 atom of Fe 3 atoms of O 3atoms of H

  11. Ex 1: C16H10N2O2 (indigo dye) 1 molecule of indigo 16 atoms of C 10 atoms of H 2 atoms of N 2 atoms of O

  12. Ex 2: 3 C12H22O11 (table sugar) 3 molecules of sugar 36 atoms of C 66 atoms of H 33 atoms of O

  13. Homework: Review pages 38 – 44 Complete problems 1 and 2 on page 43 Complete problems 1-8 on page 44

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