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Introduction to Chemistry

Dive into the world of chemistry by understanding the fundamentals of matter, atoms, compounds, and mixtures. Learn about the properties of elements, compounds, and mixtures through this comprehensive introduction to chemistry.

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Introduction to Chemistry

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  1. Introduction to Chemistry Chapter 7

  2. Chemistry • The study of matter, its structure and the changes it undergoes.

  3. MATTER • Anything that has mass (stuffinside) & takes up space (volume). • It is all around us: trees, houses, soil, water, clouds, sun, us. • All things are made of matter.

  4. Atom • Small particle of matter. • Basic building block of matter.

  5. Atom

  6. Protons- (+) Positive Charge, found in nucleus • Neutrons- NO charge, found in nucleus • Electrons- (-) Negative Charge, found outside the nucleus.

  7. Substance • Matter that always has the composition (makeup). • Aluminum, oxygen, & water. • Has same type of atoms. • 2 types: elements, compounds

  8. ELEMENTS Pure substance that contains only type 1 atom Aluminum foil consists of trillions of aluminum atoms.

  9. Elements • Represented by Chemical Symbols • Ex. O = Oxygen

  10. A pure substance • ONE Capital Letter • Examples: H, Na,Cl

  11. Chemical Symbol = ElementExamples: N, O, C,Ne, Co, Cl, H+, Ca-Elements/Atoms cannot be broken down any more.

  12. H = He = Li = Hydrogen Helium Lithium Elements Responsible for…

  13. Compounds

  14. Made up of 2 or more elements • First letter CAPITALIZED, second letter lowercase, Na, Fe, NaCL (salt), CaCl, • 2 CAPITAL LETTERS

  15. Chemical Formula • A combo of symbols & numbers that represent a compound. • Tells elements, & number of atomsthat combine to make compound.

  16. Chemical Formula Examples Na • NaCl (SALT) - one atom of Na (sodium) + one atom of Cl (chlorine) • H2O (water)- 2atoms of H & one atom of O. • CO2 (Carbon Dioxide)- one atom of C & 2atoms of O. Cl O H H O O C

  17. Chemical Formula = CompoundCompounds can be broken down into elements.

  18. Chemical Bond • Is formed when 2 or more atoms combine. • H2O =2 Hydrogen atoms combine with 1 Oxygen atom. • CO2, C12H22O11, CO

  19. Properties of Compounds • Atoms when combined to make a compound act differently than when they are by themselves. • CO2 (Carbon Dioxide)- gas , but C is a black solid, & O is a gas that helps fuel burn. • NaCl (Salt)- Na is explosive in water, Cl is a poisonous, yellow-green gas. When they combine they make • something we put on our food.

  20. Molecules • Formed when atoms combine. • 2 Hydrogen + 1 Oxygen = Water Molecule (H2O) • 1 Carbon atom + 2 Oxygen atoms = Carbon Dioxide Molecule (CO2)

  21. Circle the ELEMENTS • Box the COMPOUNDS • X the IONS

  22. Ca, F-, CaF2, H

  23. Au, NaCl, H2O , Cl-

  24. Na, Na+, AgCl, MgO

  25. Mixtures • Another form of matter. • Varies in composition. • Physically blended together, not CHEMICALLY COMBINED!

  26. Mixtures • Made of 2 or more substances that are not combined chemically.

  27. Mixtures can be broken down physically. • A filter, by hand, a magnet, dissolving, evaporation.

  28. Heterogeneous Mixture • A mixture that is NOT well mixed. • Can see the different parts of the mixture. • Hoagie, Salad, Taco, Cheeseburger

  29. Homogeneous Mixture • A well-mixed mixture. • Can’t see each part. Evenly mixed. • Suntan lotion, ocean water, lemonade

  30. Solution • A homogeneous mixture where one substance (solute)gets dissolved in another liquid (solvent). • Well-mixed, salt water • Coke, Lemonade, Brass.

  31. Atoms, Mixtures or Compounds? Identification

  32. Atoms, Compound, or Mixture? • A B C X XY X XY Y Y XY X X X X XY XY Y X XY X X X Y X

  33. Compound (A) XY XY XY XY XY

  34. Atoms (Elements) (B) X X X X X X X X X

  35. Mixture (C) Y Y X X X Y X Y

  36. 7-2 Properties of Matter

  37. 2 Properties of Matter • 1. Physical • 2. Chemical

  38. Physical Properties • Can be observed without changing it into a new substance

  39. Examples • Solid, Liquid, Gas, Texture, Color, Freezing, Melting, & Boiling Points

  40. Measuring Matter • Mass • Weight • Volume • Density • Conductivity • Solubility

  41. Mass • The amount of matter (“stuff”) inside in an object. • Holding a basketball vs a bowling ball. • Bowling ball heavier because it has more mass (stuff) inside it.

  42. Weight • Is the measure of the force of gravity on an object. • IT varies by location. • A basketball weighs more on Earth than on the moon. • Earth bigger more pull (Gravity) than moon so bball weighs more • on Earth.

  43. On Earth I weigh12O lbs, on Jupiter I would weigh304lbs, on the moon I would weigh19 lbs. WHY?

  44. Mass • A measure of the amount of matter in an object • CONSTANT

  45. Volume • The amount of space an object takes up. • Ml, L, cm3, • 2 liter bottle of coke, can of coke is 12oz • 355ml.

  46. Volume Length x Width x Height Units = Cubic

  47. Density • Mass per unit volume. (thicker) • Plastic bat vs wooden bat, wooden bat thicker more dense. • Density= Mass/volume

  48. Sink or Float? Density

  49. Water = 1.0 g/cm3

  50. Object > 1.0 = SINK Object < 1.0 = FLOAT

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