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Matter Physical and Chemical Properties

Matter Physical and Chemical Properties. Matter vs. Energy. The universe is made up of matter and energy. Matter: Has mass and takes up space (volume) Is usually a “thing” Energy: Does not have mass or take up space Energy moves matter!!!!!!

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Matter Physical and Chemical Properties

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  1. MatterPhysical and Chemical Properties

  2. Matter vs. Energy • The universe is made up of matter and energy. • Matter: • Has mass and takes up space (volume) • Is usually a “thing” • Energy: • Does not have mass or take up space • Energy moves matter!!!!!! • ** Energy is the ability to make things move. Light, heat, sound, motion, and electricity are all forms of energy.

  3. Properties of Matter • Property -characteristic that distinguishes one type of matter from another • Chemical • Physical • Specific property – a property that allows for the ID of matter • For 2 separate samples of matter to be the same kind of matter, they have to have all the same specific properties

  4. Extensive/Intensive Intensive – Does not depend on the amount of material Examples: temperature, density, boiling point Extensive – Depends on the amount of material Examples: mass and volume

  5. Physical Properties • Physical property- any property of matter that can be observed or measured without changing the identity of the matter • Examples color shape taste density state/phase malleability D = M V

  6. Volume and Density Volume= length X width X height Density= mass (g) volume (mL or cm3) 1 mL = 1 cm3 Which is more dense?

  7. Physical Properties • States of matter: • Bose-Einstein • Solid • Liquid • Gas • Plasma (Newest State)

  8. States of Matter Solid - fixed shape and volume and particles close together so rigid structure - particles vibrate only – no movement Liquid - fixed volume & takes shape of container - particles farther apart than solid - little order - particles can move around Gas - takes volume and shape of container - particles are far apart - random motion of particles

  9. Physical Properties of Fluids • Viscosity- the resistance of a fluid to flowing. • Viscousmaple syrup (cold especially!) • Not viscouswater

  10. Physical Properties of Solids • Malleable- able to be hammered or pressed out of shape without breaking • This is a property of many metals

  11. Chemical Properties • Chemical property- property of matter that describes a substance based on its ability to change into a new substance • Examples flammability reactivity with vinegar reactivity with oxygen reactivity with water Iron + Oxygen  Iron oxide (rust) 2Fe + 3O2  Fe2O3

  12. Let’s Do It!!! Label your paper 1-5Chemical or Physical Property?Chemical vs. Physical Property video • Paper is white • Boiling point of H2O is 100oC • Zinc reacts with hydrochloric acid and creates hydrogen gas • Nitrogen does not burn • Sulfur smells like rotten eggs Physical Property Physical Property Chemical Property Chemical Property Physical Property

  13. Reference-Comparing Physical and Chemical Properties

  14. Changes in Matter • Matter is constantly changing • There are two types of changes in matter: • Chemical • Physical

  15. Physical Changes • Physical change- a change in shape, size, color, or state a change without a change in chemical composition • Examples tearing paper cutting your hair change in state • Some mixtures can be separated based on their physical properties Physical changes are not indicative of a chemical reaction

  16. Let’s Do It!!! • Get with a partner • Google “Harcourt Mixtures Lab” and click on the link for “The Mixtures Lab” and read the info on the left. • Draw the chart from the lab in your notes. You have 15 minutes • The Mixtures Lab • Online stopwatch

  17. Chemical Changes • Chemical change- a change in which a substance becomes another substance having different properties • A change that is not reversible using ordinary physical means • Changes that usually cause, heat, sound, light, odor, fizzing/foaming, color changes • Examples mixing vinegar & baking soda burning a piece of wood soured milk A chemical analysis is the only 100% way to know a chemical change has occurred.

  18. Chemical Changes • Chemical reaction- the process by which a chemical change occurs • Types of chemical reactions • Synthesis (creating) • Decomposition (separating) • Combustion (burning) • Displacement/Replacement (switching of atoms)

  19. Chemical Changes What does H2 & O2 gas create? • During chemical changes, atoms are rearranged, and chemical bonds are broken and reformed • One or more substances change to produce one or more different substances H2 O2

  20. Let’s Do It!!!!Label your paper 1-5Chemical or Physical Change? • Bending a Paper Clip • Baking a cake • The sublimation of carbon dioxide • Crushing an aluminum can • Vinegar and baking soda combining to create salt and water Physical Change Chemical Change Physical Change Physical Change Chemical Change

  21. Changes are either…. Endothermic– absorbing energy • ex. boiling water • Exothermic- releasing energy ex. burning a candle

  22. Nuclear Changes/Reactions • A new substance is formed by changes in the atoms themselves - not just by rearranging the atoms.

  23. Nuclear Reactions • The TOTAL of mass plus energy is conserved. • Mass + Energy of reactants = Mass + Energy of products • Matter can change into energy and energy can change into matter.

  24. Einstein’s Equation • E = mc2 • Einstein is saying that matter and energy are different forms of the same thing! • c =(3.00 x 1010 cm/sec)2

  25. How much energy can be obtained by completely converting 1.00g of matter into energy? • E = mc2 • E = (1.00g) (3.00 x 1010 cm/sec)2 (after adjusting units) • E = 21,500,000,000,000calories

  26. This means…… • SMALL amounts of matter convert to LARGE amounts of energy

  27. Reaction Laws • Law of Conservation of Energy– in chemical and physical reactions, energy is conserved(not created or destroyed) • Law of Conservation of Mass – in chemical and physical reactions, mass is conserved (not created or destroyed)

  28. Law of Conservation of Mass Chemical Equation H + O H2O Reactants  Products Mass of Reactants = Mass of Products Example: H + O H2O 5.0g + 5.0g = ? 10.0g

  29. ReviewChemical vs. Physical Changes video 7 min • Number your paper from 1-5 and answer the following questions • Which of these is a metric unit? • A. pounds • B. cups • C. liters • D. inches

  30. Review • C • 2. Which of these is the symbol for the metric unit micro? • A. M • B. m • C. ρ • D. μ

  31. Review • D • 3. Which of these is a physical property? • A. density • B. reaction to water • C. combustibility

  32. Review • A • 4. Which of the following is a chemical property? • A. reaction to acid • B. odor • C. temperature • D. color

  33. Review • A • 5. If 59 g of NaCl is produced in a creaction, how much Cl was combined with 23 g of Na? Na + Cl NaCl • A. 36 • B. 36 g • C. 79 g • D. 23 g

  34. Review • B

  35. Composition of Matter • All matter has a composition, what it’s made of • Different kinds of composition are: • Pure substances- matter with a fixed composition that can’t be separated physically • Element • Compound • Mixture- can be separated physically • Solutions • Colloids • Mechanical mixture

  36. Classification is based on physical and chemical properties-Reference Matter Mixture Pure substance Element Compound Homogeneous (Solution) Heterogeneous Metal Metalloid Nonmetal

  37. Pure Substances • Element- made up of one kind of atom and can’t be broken down intosimpler substancesby physical or chemical means • 90 occur naturally on Earth 29 were synthesized (made) by scientists • C, N, O, Na, H, Au (gold), etc.

  38. Elements • Metal- properties: luster, reflects heat and light, good conductors of heat and electricity, malleable, ductile, all are solids except mercury (liquid) • Nonmetal-properties: poor conductors of heat and electricity, brittle, not malleable or ductile, are solids, liquids and gases • Metalloid- has some properties of metals and some properties of nonmetals

  39. Pure Substances • Compound- composed of two or more different elements • The atoms are chemically combined so that the elements take on new identities and lose their original properties Examples: H2O, CO2,CO, NO2,

  40. Mixtures • Mixtures- two or more substances that do not combine chemically, but remain the same individual substances; • Can be separated by physical means • Two types: • Heterogeneous • Homogeneous Based on the prefixes “hetero” and “homo,” what do you think are characteristics of these two types of mixtures?

  41. Heterogeneous Mixtures • “Hetero” = different • Consists of visibly different substances or phases (solid, liquid, gas) • Mechanical mixture- visibly not wholly one • Example: Notice the visibly different substances in these mechanical mixtures Pizza Trail Mix

  42. Heterogeneous Mixtures • Suspension- special type of heterogeneous mixture of larger particles that eventually settle

  43. Heterogeneous Mixtures • Colloids-heterogeneous mixture with particles that never settle • Milk and paint • Foggy appearance because its particles are large enough to scatter light, unlike a solution

  44. Homogeneous Mixtures • “Homo” = same • Same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas) • Commonly referred to as solutions • Example: Notice the uniform appearance Salt Water

  45. Homogeneous Mixtures • Solution- a mixture of two or more substances that is identical throughout • Can be physically separated • Composed of solutes and solvents Salt water is considered a solution. How can it be physically separated? the substance in the smallest amount and the one that dissolves in the solvent the substance in the larger amount that dissolves the solute Iced Tea Mix (solute) Water (solvent) Iced Tea (solution) Colloids (milk, fog, jello) are considered solutions

  46. ReviewSeparating Mixtures video 8min • Number your paper from 1-5 and answer the following questions • Which of these is a metric unit? • A. centiliters • B. cups • C. pounds • D. inches

  47. Review • A • 2. Which of these is a chemical property? • A. density • B. reaction with water • C. color • D. length

  48. Review • B • 3. Which of these is a pure substance? • A. pizza • B. tap water • C. aluminum

  49. Review • C • 4. Which of the following is a homogenous mixture? • A. air • B. trail mix • C. soil • D. air with dust particles

  50. Review • A Liquefy and then distill to separate • 5. Which of these is a compound? • A. • B. • C. • D. A B C D

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