1 / 44

Unit 1B Matter Properties & Changes

Explore the classification of matter into mixtures, homogeneous and heterogeneous mixtures, pure substances, elements, compounds, and the laws governing their properties and proportions. Learn about separating mixtures and the different states of matter.

yvetter
Download Presentation

Unit 1B Matter Properties & Changes

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Unit 1BMatterProperties & Changes PLC-Unit 1B

  2. Section IClassification of Matter PLC-Unit 1B

  3. PLC-Unit 1B

  4. Mixture • DEF: a combination of two or more substances in which the basic identity of each substance is not changed • can be separated by physical means • retains its own properties • can be classified as heterogeneous or homogeneous PLC-Unit 1B

  5. Heterogeneous Mixture • DEF: a mixture that does not have a uniform composition and in which the individual substances remain distinct • can see individual substances (phases) salad granite banana split PLC-Unit 1B

  6. Homogeneous Mixture • DEF: a mixture that has a uniform composition throughout and always has a single phase • also called a solution Saline solution steel pure air PLC-Unit 1B

  7. Consists of two (2) parts • solute – DEF: the substance that is being dissolved • solvent – DEF: the substance that dissolves the solute • salt water - salt (solute), water (solvent) • Aqueous solution (aq) • DEF: solvent is water • universal solvent PLC-Unit 1B

  8. can be solid, liquid, or gas PLC-Unit 1B

  9. Separating Mixtures • Filtration • DEF: a technique that uses a porous barrier (filter paper) to separate a solid from a liquid • sand and water PLC-Unit 1B

  10. Based on unique physical properties • Magnetism – can separate a sand-iron mixture PLC-Unit 1B

  11. Sieve • DEF: a technique that uses a screen with different pore sizes that separate solids of different sizes • sand and rocks PLC-Unit 1B

  12. Evaporation • DEF: a technique that removes the liquid from a solution, usually to leave a solid • salt and water PLC-Unit 1B

  13. Distillation • DEF: a technique that is based on differences in the boiling points of the substances involved alcohol (bp = 80oC) and water (bp = 100oC) PLC-Unit 1B

  14. Chromatography • DEF: technique that separates the components of a mixture on the basis of the tendency of each to travel or be drawn across the surface of another material • colors in ink PLC-Unit 1B

  15. Pure Substances • DEF: matter with the same fixed composition and properties • two (2) types of Pure Substances • Elements • Compounds PLC-Unit 1B

  16. Elements • DEF: a substance that cannot be broken down into simpler substances • Building block of all matter • composed of one type of atom (EX: copper) • only 92 elements occur naturally on earth PLC-Unit 1B

  17. Organizing the Elements • Periodic Table • DEF: a chart that organizes all known elements into horizontal rows (periods) and vertical columns (groups or families) • Each element has a unique chemical name and symbol • Chemical name (named after) • people (Einsteinium) • countries (Germanium) • states (Californium) • mythological figures (Plutonium) • Latin name (Iron-ferrum [Fe]) PLC-Unit 1B

  18. Symbol • contains 1,2 or 3 letters • 1st letter is capitalized; others are lower case • K (Potassium) • Na (Sodium) • Uun (Ununnilium) PLC-Unit 1B

  19. Compounds • DEF: a chemical combination of two or more elements joined together in a fixed proportion • can be broken down into simpler substances by chemical means • EXAMPLE: water (H2O), salt (NaCl), sugar (C6H12O6) • Has properties that are different from those of its elements PLC-Unit 1B

  20. Formula • DEF: combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element • EXAMPLE: C12H22O11 • 12 atoms carbon • 22 atoms hydrogen • 11 atoms oxygen PLC-Unit 1B

  21. Law of Definite Proportions • DEF: states that, regardless of the amount, a compound is always composed of the same elements in the same proportions by mass • Percent by mass (%) PLC-Unit 1B

  22. Percent by Mass A 78.0 g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound? 15.9% PLC-Unit 1B

  23. Percent by Mass What is the percent by mass of carbon in glucose (C6H12O6)? (mass of compound) 40.0% PLC-Unit 1B

  24. Law of Multiple Proportions • DEF: states that when different compounds are formed by the combination of the same elements, they combine in small-whole number ratios PLC-Unit 1B

  25. Section IIProperties and Changes of Matter PLC-Unit 1B

  26. Physical Properties • DEF: characteristics of a sample of matter that can be observed or measured without any change in its identity • EXAMPLE: color, electrical conductivity, boiling point, melting point, density, state of matter (solid, liquid, or gas) PLC-Unit 1B

  27. States of Matter • DEF: physical forms of matter • Four (4) states of matter • Solid • Liquid • Gas • Plasma • state of matter is based upon: • particle arrangement • energy of particles • distance between particles PLC-Unit 1B

  28. SOLID • DEF: a form of matter that has a definite shape and definite volume • particles vibrate in place PLC-Unit 1B

  29. LIQUID • DEF: a form of matter that has a definite volume but takes the shape of its container • particles vibrate in place are able to slip past each other which allows liquid to flow PLC-Unit 1B

  30. GAS • DEF: a form of matter that has no definite shape and no definite volume; takes the shape of its container • Particles are far apart and constantly moving • Gas vs. Vapor • Gas – a substance that is naturally in the gaseous state at room temperature • EXAMPLE: Helium PLC-Unit 1B

  31. Vapor – the gaseous state of a substance that is a solid or liquid at room temperature • EXAMPLE: Steam PLC-Unit 1B

  32. PLASMA • DEF: a form of matter that does not have a definite shape or volume and whose particles have broken apart • composed of electrons and positively charged ions • conducts an electric current (gases do not) • affected by electric and magnetic fields which is used to contain plasma (gases are not) PLC-Unit 1B

  33. Artificial plasma – created by passing electric current through gases • EXAMPLE: fluorescent lights, plasma TV PLC-Unit 1B

  34. STATES OF MATTER SOLID LIQUID GAS PLASMA Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles PLC-Unit 1B

  35. Chemical Properties • DEF: a property that can be observed only when there is a change in the composition of a substance • Describes the ability or inability of a substance to react with other substances or to decompose • EXAMPLE: ability to rust, unreactive, flammable PLC-Unit 1B

  36. Physical Change • DEF: a change in matter that does not involve a change in the identity of the substance • same substance remains after change • EXAMPLE: change of state, dissolving PLC-Unit 1B

  37. Melting is an example of a reversible change. For example, when chocolate is warmed until it melts, the melted chocolate can be changed back into solid chocolate by cooling. PLC-Unit 1B

  38. Chemical Change • DEF: the change of one or more substances into other substances • also called a chemical reaction • evidence of a chemical change • precipitate • gas formation • color change • energy change • Odor PLC-Unit 1B

  39. Law of Conservation of Mass (LOCOM) • DEF: matter is neither created nor destroyed during a chemical reaction • Massreactant = Massproduct PLC-Unit 1B

  40. Law of Conservation of Mass From a laboratory process a student collected 10.0 g hydrogen and 79.4 of oxygen. How much water was originally involved? Massreactant = Massproduct Masswater = Masshydrogen + Massoxygen Masswater = 10.0 g + 79.4 g 89.4 g PLC-Unit 1B

  41. Law of Conservation of Mass A 10.0-g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide. How many grams of oxygen reacted? Massreactant = Massproduct Massmagnesium + Massoxygen = MassMgO 10.0 g + Massoxygen = 16.6 g 6.6 g PLC-Unit 1B

  42. Energy • DEF: capacity to do work • all physical and chemical changes require energy • can be exothermic or endothermic PLC-Unit 1B

  43. Exothermic • DEF: chemical reaction that gives off heat energy • EXAMPLE: burning wood in a fireplace PLC-Unit 1B

  44. Endothermic • DEF: chemical reaction that absorbs heat energy • EXAMPLE: photosynthesis • absorbs light energy from sun and produces sugars from carbon dioxide and water PLC-Unit 1B

More Related