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Classification of Matter

Learn about classification of matter, composition of matter, states of matter, phase changes, physical and chemical properties, and more in this comprehensive overview.

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Classification of Matter

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  1. MATTER Classification of Matter I. Composition of Matter Matter Flowchart Pure Substances Mixtures

  2. MIXTURE PURE SUBSTANCE yes no yes no Is the composition uniform? Can it be decomposed by chemical means? A. Matter Flowchart MATTER yes no Can it be separated by physical means? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

  3. B. Pure Substances • Element • matter composed of identical atoms • EX: copper

  4. Periodic Table of Elements

  5. B. Pure Substances • Compound/ Molecule • matter composed of 2 or more elements in a fixed ratio • properties differ from those of individual elements • chemically combined • EX: salt (NaCl) or water (H2O)

  6. Chemical Formulas • Shows how many atoms of each element are in the substance. Example: C16H10N2O2 is a blue dye. • The number of atoms of each element is written after the element’s symbol as a subscript. • If only one atom is present, no subscript is needed.

  7. Chemical Formulas • You try. C12H22O11 How many atoms of each element are in this formula? C is for carbon. H is for hydrogen. O is for oxygen.

  8. C. Mixtures • Variable combination of 2 or more pure substances. • Homogeneous Mixture (Solution) • even distribution of components • very small particles • particles never settle • EX: saline solution

  9. C. Mixtures • Heterogeneous Mixture • uneven distribution of components • Can physically separate • Colloids and Suspensions • EX: granite

  10. C. Mixtures • Colloid • medium-sized particles • Tyndall effect - particles scatter light (looks cloudy) • particles never settle • EX: milk

  11. C. Mixtures • Suspension • large particles • particles scatter light • particles will settle (needs to be shaken) • EX: fresh-squeezed lemonade

  12. Law of Conservation of Mass and Energy • Mass cannot be created nor destroyed • Energy cannot be created nor destroyed; it can be transformed or transferred to other forms of energy.

  13. MATTER Solids, Liquids, & Gases I. States of Matter Kinetic Molecular Theory Four States of Matter Thermal Expansion

  14. A. Kinetic Molecular Theory • KMT • Tiny, constantly moving particles make up all matter. • The kinetic energy (motion) of these particles increases as temperature increases.

  15. B. Four States of Matter • Solids • low KE - particles vibrate but can’t move around • definite shape & volume • crystalline - repeating geometric pattern • amorphous - no pattern (e.g. glass, wax)

  16. B. Four States of Matter • Liquids • higher KE - particles can move around but are still close together • indefinite shape • definite volume

  17. B. Four States of Matter • Gases • high KE - particles can separate and move throughout container • indefinite shape & volume

  18. B. Four States of Matter • Plasma • very high KE - particles collide with enough energy to break into charged particles (+/-) • gas-like, indefiniteshape & volume • stars, fluorescentlight bulbs, TV tubes

  19. C. Thermal Expansion • Most matter expands when heated & contracts when cooled. •  Temp causes  KE. Particles collide with more force & spread out. • EX: thermostats (bimetallic strip)

  20. MATTER Solids, Liquids, & Gases II. Changes in State Phase Changes Heating Curves

  21. A. Phase Changes • Melting • solid to liquid • Freezing • liquid to solid melting point = freezing point

  22. A. Phase Changes • Vaporization (boiling) • liquid to gas at the boiling point • Evaporation • liquid to gas below the boiling point • Condensation • gas to liquid

  23. A. Phase Changes • Sublimation • solid to gas • EX: dry ice, freeze drying, iodine

  24. A. Phase Changes

  25. B. Heating Curves • Kinetic Energy • motion of particles • related to temperature • Potential Energy • space between particles • related to phase changes

  26. Gas - KE  • Boiling - PE  • Liquid - KE  • Melting - PE  • Solid - KE  B. Heating Curves

  27. B. Heating Curves • Heat of Fusion • energy required to change from solid to liquid • some attractive forces are broken

  28. B. Heating Curves • Heat of Vaporization • energy required to change from liquid to gas • all attractive forces are broken • EX: steam burns, sweating, and… the drinking bird • HEATING CURVE

  29. MATTER Classification of Matter II. Describing Matter Physical Property Physical Change Chemical Change Chemical Property

  30. A. Physical Property • A characteristic of a substance that can be observed without changing its identity. • can be used to separate mixtures • EX: magnetism, density

  31. B. Physical Change • A change in the form of a substance without changing its identity. • properties remain the same • reversible • can be used to separate mixtures • EX: dissolving, grinding

  32. C. Chemical Change • A change in the identity of a substance. • properties change • irreversible • Signs: color change, formation of a gas/solid, release of light/heat • EX: burning, rusting

  33. D. Chemical Property • A characteristic that indicates whether a substance can undergo a specific chemical change. • EX: flammability, reactivity

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