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INTRODUCTION

INTRODUCTION. Matter And Measurement. Physical Separation. Chemical Separation. Classification of Matter. M A T T E R. Anything that occupies space (has volume) and has mass. S B S T A N C E. PURE. H 2 O. NaCl. C 12 H 22 O 11. CO 2. examples. O 2. Al.

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INTRODUCTION

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  1. INTRODUCTION Matter And Measurement

  2. Physical Separation Chemical Separation Classification of Matter

  3. M A T T E R Anything that occupies space (has volume) and has mass

  4. S B S T A N C E PURE H2O NaCl C12H22O11 CO2 examples O2 Al Matter that has a uniform and definite composition Substances have distinctive characteristic (identifying) physical & chemical properties Elements & compounds are substances

  5. E L E M E N T O2 Na H2 examples Al Cu A substance that can not be broken down to simpler substances by chemical means Most elements are composed of individual atoms (some elements are composed of groups of identical atoms).

  6. C O M P O U N D C12H22O11 examples CO2 H2O A substance composed of two or more elements A compound can be broken down (decomposed) by chemical means In compounds, elements are chemically bonded

  7. M I X T U R E Heterogeneous Mixture Homogeneous Mixture A mixture which is uniform and has a single phase (single state); also called a solution A mixture which is NOT uniform and usually has more than one phase example example Sand & Water Sand & Salt Sand alone Salt & Water A physical blend of two or more substances

  8. Comparison of Mixture & Compound MIXTURE (Example  Saltwater) COMPOUND (Example  Water) • Physical blend of substances • Physical properties of mixture are the same properties of its components • Components combine in any ratio • Separation is by physical process • Chemical combination (bonding) of 2 or more elements • Physical properties of compound are unique & different from properties of its elements • Components (elements) combine in a definite ratio • Separation (decomposition) is a chemical process

  9. Mixture Compound H2 (g) and O2 (g) Hydrogen Gas + Oxygen Gas H2O (g) Water Vapor (steam)

  10. Properties of Matter Extensive properties depend on the amount of matter that is present. Volume Mass Energy Content (think Calories!) Intensive properties do not depend on the amount of matter present. Melting point Boiling point Density

  11. Classification of Matter

  12. Classification of Matter

  13. Classification of Matter

  14. Classification of Matter

  15. Substances can be altered by Physical Changes or Chemical Changes Examples PHYSICAL changes CHEMICAL changes • Will alter a substance withoutchanging its composition • Are frequently reversible • Properties or characteristics do not change • Will alter a substance by changing its composition • Are not frequently reversible • New substances formed have new properties or characteristics

  16. Examples PHYSICAL changes CHEMICAL changes • Dissolving • Evaporating • Freezing Sodium + chlorine  NaCl silver metal gas salty taste, white, H2O soluble explosive in water “green” color non flammable toxic toxic non toxic

  17. When a chemical reaction occurs, one or more substances is changed into new substances Chemical Change In every chemical reaction, one or more of the following can be observed

  18. Indicators of a Chemical Reaction Many chemical reaction are NOT reversible

  19. Classify each process as being a physicalchangeonly OR a process that also involves a chemical change (chemical reaction)

  20. Boiling Decomposing Dissolving Grinding

  21. Melting Evaporating Tarnishing Baking

  22. Rusting Growing Fermenting Subliming

  23. Condensing Rotting Freezing Digesting

  24. Three Phases States of Matter

  25. Phase Differences Solid – definite volume and shape; particles packed in fixed positions. Liquid – definite volume but indefinite shape; particles close together but not in fixed positions Gas – neither definite volume nor definite shape; particles are at great distances from one another Plasma – high temperature, ionized phase of matter as found on the sun.

  26. Separation of a Mixture The components of dyes such as ink may be separated by paper chromatography. The components of dyes such as ink may be separated by paper chromatography.

  27. Separation of a Mixture Distillation

  28. Separation of a CompoundThe Electrolysis of water Compounds must be separated by chemical means. With the application of electricity, water can be separated into its elements Reactant  Products Water  Hydrogen + Oxygen H2O  H2 + O2

  29. Organization of Matter Matter Mixtures: a) Homogeneous(Solutions) b) Heterogeneous Pure Substances Elements Compounds Atoms Nucleus Electrons Protons Neutrons

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