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Classifying Matter

Matter. Elements. Compounds. Mixtures. Classifying Matter. Scientists classify matter according to make-up. Elements. Simplest pure substance – fixed composition. Pure substance is made of only one material. Same throughout. Referred to as homogeneous matter .

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Classifying Matter

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  1. Matter Elements Compounds Mixtures Classifying Matter • Scientists classify matter according to make-up.

  2. Elements • Simplest pure substance – fixed composition. • Pure substance is made of only one material. Same throughout. Referred to as homogeneous matter. • Are made of alike atoms, which are the basic building blocks of matter. • Represented by chemical symbols - H, O, Al, Cu, Au. • 118 elements organized in the periodic table in squares called an element key.

  3. Element Key Atomic Number Symbol Element Name Atomic Mass I.D’s the element represents elements mass of element (amu’s)

  4. Calcium Tin Uranium Magnesium Phosphorus Iron iodine Silver Helium Mercury Nickel Silicon Sulfur Copper Chromium Aluminum Bromine Hydrogen Zinc Potassium Elements/Symbols • Oxygen • Lead • Lithium • Gold • Fluorine • Neon • Nitrogen • Sodium • Carbon • Chlorine

  5. Compounds • Two or more elements chemically combined. • Represented by chemical formulas. • Examples: H2O, CO2, NaCl, C12H22O11 • Molecules are the smallest natural unit of a compound or diatomic element. A molecule is made up of two or more atoms chemically combined.

  6. Chemical Formulas • Combination of chemical symbols that represents compounds. • Sometimes represents a molecule of an element. Example: O2, N2, Cl2 called diatomic elements – two atoms of the same element. • Subscripts are the # of atoms of an element - H2O • Coefficients are the # placed in front of chemical formula. Represents # of molecules of a compound - 4 H2O

  7. Identifying Substances Element Symbol Atom Compound Formula Molecule Element Formula Molecule

  8. Counting Atoms Ca=1 C=1 O=3 Mg=1 O=2 H=2 H=9 P=3 O=12 C=14 N=6 H=10 O=12

  9. Calculating Formula Mass • Formula mass of a compound is the sum of the atomic weights of all atoms in a chemical formula. • Examples:AtomsAtomic MassTotals • H2O 2 of H 2 x 1.0 2.0 • 1 of O 1 x 16.0 16.0 • 18.0 amu • C12H22O1112 of C 12 x 12.0 144.0 • 22 of H 22 x 1.0 22.0 • 11 of O 11 x 16.0 176.0 • 342.0 amu

  10. Mixtures • Two or more substances mixed together but not chemically combined. • Has unlike parts and a composition that varies from sample to sample. • Properties: • Sub. in a mixture keep their separate identities. • Sub. can be present in any amount. • Sub. can be separated out by physical means.

  11. Mixtures

  12. The least-mixed. Doesn’t appear to be the same throughout. Particles large enough to be seen. Examples: sand, dirt, concrete, suspensions, etc. Heterogeneous Mixtures

  13. Well-mixed. Same throughout a given sample. Examples: air, soda, toothpaste, lotions, etc. Homogeneous Mixtures

  14. Solutions • A homogeneous mixture. • One substance dissolves in another. Solutions remain constantly & uniformly mixed. • Examples: lemonade, soda, ocean water, antifreeze, metal alloys (steel, brass), etc.

  15. Colloids • A homogeneous mixture. • Mixed together but not dissolved. • Appears cloudy. Scatters light. • Examples: milk, cool whip, toothpaste, lotions, fog, paint, etc.

  16. Composition of Matter

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