Understanding Matter and Mixtures: A Comprehensive Overview

1. MATTER yes no Can it be physically separated? MIXTURE PURE SUBSTANCE yes no yes no Is the composition uniform? Can it be chemically decomposed? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element Colloids Suspensions Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

2. Both elements and compounds have a definite makeup and definite properties. Compounds two or more kinds of atoms that are chemically bonded Mixtures two or more substances that are physically mixed Elements only one kind of atom; atoms are bonded it the element is diatomic or polyatomic two or more kinds of and substance with definite makeup and properties Packard, Jacobs, Marshall, Chemistry Pearson AGS Globe, page (Figure 2.4.1)

3. Matter Flowchart Examples: • graphite • pepper • sugar (sucrose) • paint • soda element hetero. mixture compound hetero. mixture solution homo. mixture Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

4. Pure Substances • Element • composed of identical atoms • EX: copper wire, aluminum foil Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

5. Pure Substances • Compound • composed of 2 or more elements in a fixed ratio • properties differ from those of individual elements • EX: table salt (NaCl) Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

6. Pure Substances Law of Definite Composition • A given compound always contains the same, fixed ratio of elements. Law of Multiple Proportions • Elements can combine in different ratios to form different compounds. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

7. Carbon, C Oxygen, O Carbon monoxide, CO Carbon, C Oxygen, O Oxygen, O Carbon dioxide, CO2 Pure Substances For example… Two different compounds, each has a definite composition. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

8. Mixtures Variable combination of two or more pure substances. Heterogeneous Homogeneous Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

9. Tyndall Effect Mixtures Solution • homogeneous • very small particles • no Tyndall effect • particles don’t settle • EX: rubbing alcohol Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

10. Mixtures Colloid • heterogeneous • medium-sized particles • Tyndall effect • particles don’t settle • EX: milk Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

11. Mixtures Suspension • heterogeneous • large particles • Tyndall effect • particles settle • EX: fresh-squeezed lemonade Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

12. Mixtures Examples: • mayonnaise • muddy water • fog • saltwater • Italian salad dressing colloid suspension colloid solution suspension Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

13. Specific / General Order / Disorder Classification of Matter Materials Homogeneous Heterogeneous Substance Homogeneous mixture Heterogeneous mixture Element Compound Solution Mixture Smoot, Smith, Price, Chemistry A Modern Course, 1990, page 43

14. Classification of Matter MATTER (gas. Liquid, solid, plasma) Separated by PURE SUBSTANCES MIXTURES physical means into Separated by COMPOUNDS ELEMENTS HOMOGENEOUS MIXTURES HETEROGENEOUS MIXTURE chemical means into Kotz & Treichel, Chemistry & Chemical Reactivity, 3rd Edition , 1996, page 31

15. Classification of Matter hetero- geneous mixture no uniform properties? no solution fixed composition? no element chemically decomposable? yes compound http://antoine.frostburg.edu/chem/senese/101/matter/slides/sld003.htm

16. Elements, Compounds, and Mixtures oxygen atoms hydrogen atoms hydrogen atoms (b) a compound (water) (c) a mixture (hydrogen and oxygen) (d) a mixture (hydrogen and oxygen) (a) an element (hydrogen) Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 68

17. Elements, Compounds, and Mixtures oxygen atoms hydrogen atoms hydrogen atoms (b) a compound (water) (c) a mixture (hydrogen and oxygen) (d) a mixture (hydrogen and oxygen) (a) an element (hydrogen) Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 68

18. Mixture vs. Compound Alike Different Different Involve substances Variable Composition Fixed Composition Topic Topic No bonds between components Contain two or more elements Bonds between components Mixture Compound Can be separated by physical means Can be separated into elements Can ONLY be separated by chemical means

19. Compounds vs. Mixtures • Compounds have properties that are uniquely different from the elements from which they are made. • A formula can always be written for a compound • e.g. NaCl  Na + Cl2 • Mixtures retain their individual properties. • e.g. Salt water is salty and wet

20. Diatomic Elements, 1 and 7 H2 O2 F2 N2 Cl2 Br2 F2

21. Products made from Sulfur SULFURIC ACID 88% Superphosphates Ammonium phosphate Ammonium sulfate Mixed fertilizers CARBONDISULFIDE 3% GROUND & DEFINED 3% Magazines and printing papers Writing and fine papers Wrapping and bag papers Sanitary and tissue papers Absorbent papers Containers and boxes Newsprint Pulp for rayon and film Autos Appliances Tin and other containers Galvanized products PULP 3% IRON & STEEL 1% OTHER INDUSTRIES 6% Rayon Cellophane Carbon Tetrachloride Ruber processing chemicals OTHER 3% CHEMICAL 17% TITANIUM AND OTHER PIGMENTS 5% RAYON & FILM 3% PETROLEUM 2% NONACID 12% Explosives Nonferrous metals Synthetic rubber Storage batteries Textile finishing Tire cords Viscose textiles Acetate textiles Blended fabrics Cellophane Photographic film Insecticides Fungicides Rubber vulcanizing Soil sulfur Synthetic detergents Feed additives Anti-knock gasoline Synthetic resins Protective coating Dyestuffs Oil well acidizing Petroleum catalysts Specialty steels Magnessium Leather processing Photography Dyestuffs Bleaching Soybean extraction Aluminum reduction Paper sizing Water treatment Pharmaceuticals Insecticides Antifreeze Paints and enamels Linoleum and coated fabrics Paper Printing inks Aviation Gasoline Lubricants Other Refinery products

22. Sulfur • Rhombic sulfur • “Brimstone” (when molten) • Polyatomic (S8) • Forms SO2 Amorphous sulfur • (without shape) The sudden cooling of m-sulfur produces amorphous sulfur.

23. Amorphous (Glass) Crystalline

24. The Haber Process

25. Matter Physically separable Substance Definite composition (homogeneous) Mixture of Substances Variable composition Chemically separable Element (Examples: iron, sulfur, carbon, hydrogen, oxygen, silver) Compound (Examples: water. iron (II) sulfide, methane, Aluminum silicate) Homogeneous mixture Uniform throughout, also called a solution (Examples: air, tap water, gold alloy) Heterogeneous mixture Nonuniform distinct phases (Examples: soup, concrete, granite)

26. The Organization of Matter MATTER HOMOGENEOUS MIXTURES HETEROGENEOUS MIXTURE Physical methods PURE SUBSTANCES ELEMENTS COMPOUNDS Chemical methods Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 41

27. Top TenElements in the Universe • Percent • Element (by atoms) • Hydrogen 73.9 • Helium 24.0 • Oxygen 1.1 • Carbon 0.46 • Neon 0.13 • Iron 0.11 • Nitrogen 0.097 • Silicon 0.065 • Magnesium 0.058 • Sulfur 0.044 A typical spiral galaxy (Milky Way is a spiral galaxy) Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 26

28. The Composition of Air Nitrogen Helium Oxygen Air Neon Water vapor Carbon dioxide Argon Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 34

29. Chart Examining Some Components of Air Nitrogen consists of molecules consisting of two atoms of nitrogen: Oxygen consists of molecules consisting of two atoms of oxygen: Water consists of molecules consisting of two hydrogen atoms and one oxygen atom: Argon consists of individual argon atoms: Carbon dioxide consists of molecules consisting of two oxygen atoms and one carbon atom: Neon consists of individual neon atoms: Helium consists of individual helium atoms: N2 O2 H2O Ar CO2 Ne He Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 35

30. Reviewing ConceptsClassifying Matter • Why does every sample of a given substance have the same properties? • Explain why the composition of an element is fixed. • Describe the composition of a compound. • Why can the properties of a mixture vary? • On what basis can mixtures be classified as solutions, suspensions, or colloids?