Classification of Matter Ordinary solid salt is a compound but not a molecule. It is built from interpenetrating lattices of sodium and chloride ions that extend indefinitely. This well-known molecule is a compound because it contains more than one element. A molecule but not a compound Ozone, O3, is not a compound because it contains only a single element.

MATTER yes no MIXTURE PURE SUBSTANCE yes no yes no Homogeneous Mixture Can it be physically separated? MIXTURE PURE SUBSTANCE yes Is the composition uniform? no yes Can it be chemically decomposed? no Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element Colloids Suspensions

Elements Compounds Mixtures Both elements and compounds have a definite makeup and definite properties. Elements only one kind of atom; atoms are bonded it the element is diatomic or polyatomic Compounds two or more kinds of atoms that are bonded Mixtures two or more substances that are physically mixed substance with definite makeup and properties two or more kinds of compounds

Matter Flowchart Examples: graphite pepper element sugar (sucrose) paint soda element heterogeneous mixture compound heterogeneous mixture Graphite image: geology.about.com/.../bl/images/blgraphite.htm solution homogeneous mixture

Pure Substances Element composed of identical atoms EX: copper wire, aluminum foil http://www.friedlandindustries.com/images/new/NonferrousMetalsCopper.jpg

Pure Substances Compound composed of 2 or more elements in a fixed ratio properties differ from those of individual elements EX: table salt (NaCl)

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.

Two different compounds, each has a definite composition. Pure Substances For example… Carbon, C Oxygen, O Carbon monoxide, CO Carbon, C Oxygen, O Oxygen, O Carbon dioxide, CO2 Two different compounds, each has a definite composition.

Mixtures Variable combination of two or more pure substances. Heterogeneous Homogeneous

Mixtures Solution homogeneous very small particles no Tyndall effect particles don’t settle EX: rubbing alcohol

Mixtures Colloid heterogeneous medium-sized particles Tyndall effect particles don’t settle EX: milk

Mixtures Suspension heterogeneous large particles Tyndall effect particles settle EX: fresh-squeezed lemonade

Mixtures Examples: colloid suspension colloid solution suspension mayonnaise muddy water fog saltwater Italian salad dressing colloid suspension colloid solution suspension

Classification of Matter Specific / General Materials Homogeneous Heterogeneous Substance Homogeneous mixture Heterogeneous mixture Element Compound Solution Mixture Order / Disorder

Classification of Matter (gas. Liquid, solid, plasma) Separated by PURE SUBSTANCES MIXTURES physical means into Separated by COMPOUNDS ELEMENTS HOMOGENEOUS MIXTURES HETEROGENEOUS MIXTURE chemical means into

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

Elements, Compounds, and Mixtures oxygen atoms hydrogen atoms hydrogen atoms “Elements, Compounds, and Mixtures”   Description: This slide shows the molecular composition of an element, a compound, and two mixtures. Basic Concepts All samples of a substance have the same molecular composition and intensive properties and are homogeneous. Elements and compounds are substances; mixtures are not. The elements making up a compound combine in fixed ratios. Mixtures can be separated by physical methods. Mixtures that have a uniform composition throughout are homogeneous; those that have parts with different compositions are heterogeneous. Teaching Suggestions Use this transparency to help students visualize the molecular composition of elements, compounds, and mixtures and to review the definitions of these terms. Make sure students understand the difference between the terms matter and substance. Remind students that elements and compounds are always homogeneous, while mixtures can be either homogeneous or heterogeneous. Questions: Which of the bottles pictured above contain(s) matter? Which contain(s) a single substance? Explain your answers. How many elements are present in each molecule of water shown in bottle (b)? What is the relative number of atoms of each element in a water molecule? As you know, ice is frozen water. In other words, ice and water are the same substance, in different phases. What would you expect the ratio of hydrogen atoms to oxygen atoms to be in a molecule of ice? Explain your reasoning. Bottle (c) and bottle (d) both contain mixtures. How are these mixtures similar? How are they different? Suppose you find an unlabeled bottle containing a clear liquid. Can you tell by looking at it whether the material is a compound or a mixture? Explain your answer. How can you prove that a sample of sea water is a mixture? Classify the following items as elements, compounds or mixtures; rice pudding, copper, carbon dioxide, air, milk, magnesium chloride, granite, mercury, and maple syrup. A chocolate-chip cookie with more chips in one part of the cookie than another can be used to demonstrate a heterogeneous mixture. Name two other materials that can be classified as heterogeneous mixtures. Explain your reasoning. (a) an element (hydrogen) (b) a compound (water) (c) a mixture (hydrogen and oxygen) (d) a mixture (hydrogen and oxygen)

Elements, Compounds, and Mixtures oxygen atoms hydrogen atoms hydrogen atoms “Elements, Compounds, and Mixtures”   Description: This slide shows the molecular composition of an element, a compound, and two mixtures. Basic Concepts All samples of a substance have the same molecular composition and intensive properties and are homogeneous. Elements and compounds are substances; mixtures are not. The elements making up a compound combine in fixed ratios. Mixtures can be separated by physical methods. Mixtures that have a uniform composition throughout are homogeneous; those that have parts with different compositions are heterogeneous. Teaching Suggestions Use this transparency to help students visualize the molecular composition of elements, compounds, and mixtures and to review the definitions of these terms. Make sure students understand the difference between the terms matter and substance. Remind students that elements and compounds are always homogeneous, while mixtures can be either homogeneous or heterogeneous. Questions: Which of the bottles pictured above contain(s) matter? Which contain(s) a single substance? Explain your answers. How many elements are present in each molecule of water shown in bottle (b)? What is the relative number of atoms of each element in a water molecule? As you know, ice is frozen water. In other words, ice and water are the same substance, in different phases. What would you expect the ratio of hydrogen atoms to oxygen atoms to be in a molecule of ice? Explain your reasoning. Bottle (c) and bottle (d) both contain mixtures. How are these mixtures similar? How are they different? Suppose you find an unlabeled bottle containing a clear liquid. Can you tell by looking at it whether the material is a compound or a mixture? Explain your answer. How can you prove that a sample of sea water is a mixture? Classify the following items as elements, compounds or mixtures; rice pudding, copper, carbon dioxide, air, milk, magnesium chloride, granite, mercury, and maple syrup. A chocolate-chip cookie with more chips in one part of the cookie than another can be used to demonstrate a heterogeneous mixture. Name two other materials that can be classified as heterogeneous mixtures. Explain your reasoning. (a) an element (hydrogen) (b) a compound (water) (c) a mixture (hydrogen and oxygen) (d) a mixture (hydrogen and oxygen)

Mixture vs. Compound Different Alike Different Topic Topic Mixture Involve substances Variable Composition Fixed Composition Topic Topic No bonds between components Contain two or more elements Bonds between components Mixture Compound Compounds have different properties than the elements they are made from. In a mixture, the mixture retains the properties of the materials it is made from. A chemical formula can always be written for a compound. Can be separated by physical means Can be separated into elements Can ONLY be separated by chemical means

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

Diatomic Elements, 1 and 7 H2 N2 O2 F2 Cl2 Br2 I2

Products made from Sulfur SULFURIC ACID 88% Superphosphates Ammonium phosphate Ammonium sulfate Mixed fertilizers CARBON DISULFIDE 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 PULP 3% Autos Appliances Tin and other containers Galvanized products IRON & STEEL 1% OTHER INDUSTRIES 6% Rayon Cellophane Carbon Tetrachloride Ruber processing chemicals Link to slide of Frasch process Sulfur is used in making sulfur dioxide, carbon disulfide, sulfuric acid, and other sulfur compounds. Several million tons are used annually in the manufacture of sulfuric acid. Matches, fireworks, and black gunpowder all contain either sulfur or sulfur compounds. Sulfur is also used in the preparation of certain dyes, medicines, and fungicides. It is also used in the vulcanization of rubber. Modern Chemistry, Metcalfe. Williams, and Catska (1966) pg. 499 OTHER 3% CHEMICAL 17% TITANIUM AND OTHER PIGMENTS 5% RAYON & FILM 3% NONACID 12% PETROLEUM 2% Explosives Nonferrous metals Synthetic rubber Storage batteries Textile finishing Insecticides Fungicides Rubber vulcanizing Soil sulfur Tire cords Viscose textiles Acetate Blended fabrics Cellophane Photographic film 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

Amorphous Crystalline (Glass) Crystalline - a pattern to the manner in which the atoms are bonded together. crystalline lattice structure Amorphous - 'without shape'; no regular pattern exists as to how the atoms are bonded together

Heterogeneous mixture                                                                                                                                                        Matter Physically separable Substance Definite composition (homogeneous) Mixture of Substances Variable composition Basis for separation: different components, different properties. Strategy: devise a process that discriminates between components with different properties. high density / low density reactive / inert volatile / nonvolatile soluble / insoluble polar / nonpolar magnetic . nonmagnetic 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)

The Organization of Matter HOMOGENEOUS MIXTURES HETEROGENEOUS MIXTURE Physical methods PURE SUBSTANCES ELEMENTS COMPOUNDS Chemical methods

Top Ten Elements 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)

The Composition of Air Air Nitrogen Helium Oxygen Neon Water vapor Carbon dioxide Argon

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

Reviewing Concepts Classifying 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? Every sample of a given substance has the same properties because a substance has a fixed, uniform composition. An element has a fixed composition because it contains only one type of atom. A compound always contains two or more elements joined in a fixed proportion. The properties of a mixture can vary because the composition of a mixture is not fixed. Based on the size of its largest particles, a mixture can be classified as a solution, a suspension, or a colloid.