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Chemistry 101: Matter, States of Matter, and Chemical Changes

Learn about matter, its states, physical and chemical changes, and properties. Understand elements, compounds, and mixtures, as well as separation methods.

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Chemistry 101: Matter, States of Matter, and Chemical Changes

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  1. Chemistry 101 Chapter 3 Matter

  2. Matter Matter: has mass and takes space.

  3. States of Matter

  4. Changes Chemical change (chemical reaction): substance(s) are used up (disappear) → others form burning or cooking the egg Physical change: identities of the substances do not change. (change of state) evaporation of water or melting

  5. Physical Changes move faster Kinetic energy ↑ T ↑ Boiling is a physical change.

  6. Physical Changes Composition of the substance is not affected. Change of states

  7. Water Chemical Changes (reactions) Electrolysis Decomposition

  8. Chemical and physical Changes Think about it: Classify each of the following as a physical or chemical change. • Bleaching clothes • Burning of wood • Dissolving of sugar in water • Melting a popsicle on a warm summer day • Baking soda (sodium carbonate) forming CO2(g) • Iron metal melting

  9. Physical and Chemical Properties Physical Properties: a directly observable characteristic of a substance exhibited as long as no chemical change occurs. Color, Odor, Volume, State, Density, Melting and boiling point. Chemical Properties:Ability to chemical changes. (forming a new substance(s)) Burning wood – rusting of the steel

  10. Matter Anything that occupies space and mass Physically Separable into Pure substances Fixed composition, con not be more purified Mixtures A combination of two or more pure substance Element Cannot be subdivided by chemical or physical means Compounds Elements united In fixed ratios Heterogeneous matter Nonuniform composition Homogeneous matter Uniform Composition throughout Combine Chemically To form

  11. Monatomic Diatomic Polyatomic Ar He N2 O2 S8 Elements Element: is a substance consists of identical atoms. Cannot be divided by chemical & physical methods. Carbon, Hydrogen, Oxygen 116 elements – 88 in nature

  12. Compounds Compound: is a pure substance made up of two or more elements in a fixed ratio by mass. H2O (Water): 2 Hydrogen & 1 Oxygen CO2: 1 Carbon & 2 Oxygen 20 million compounds By Chemical Methods Compounds Elements

  13. Elements & Compounds The character of each element is lost when forming a compound. Oxygen (gas) H2O (liquid) Hydrogen (gas)

  14. Elements & Compounds Sodium (Na) NaCl Chlorine (Cl)

  15. 2 H or = 2 : 1 1 O 1 C or = 1 : 1 1 O Compounds Formula Identifies each element Ratios H2O CO

  16. NaCl, salt Compound & molecule • Molecule: • the smallest unit of a compound that retains the characteristics of that compound. H2O, CO2 • atoms of one element bonded into a unit. • Buckyballs, C60 oxygen, O2 ozone, O3 Buckyball, C60 Ethanol, C2H6O compound --- --- molecule compound molecule

  17. Pure substance & Mixture Pure substance: same composition Elements - Compounds Water Mixture: different composition Different water samples (impurities). • salad dressing Coffee

  18. Mixtures Mixture:is a combination of two or more pure substances. Homogeneous (solutions): uniform and throughout Air, Salt in water Heterogeneous: nonuniform Soup, Milk, Blood, sand in water

  19. Different Physical Property Technique Boiling point Distillation State of matter (solid/liquid/gas) Filtration Adherence to a surface Chromatography Volatility Evaporation Separation of Mixtures Physical Methods Mixture Two or more pure substances

  20. Separation of Mixtures Distillation Filtration Decantation

  21. Distillation Separation by using the differences in boiling points. (Physical change) Salt & Water

  22. Distillation Heater Distillation Tower

  23. Filtration For Heterogeneous mixtures. Separation by using the differences in size of particles.

  24. Salt, Sand and Water

  25. Matter Homogeneous mixtures Heterogeneous mixtures Physical Methods Pure substances Elements Compounds Chemical Methods Separation

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