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IQ 1

IQ 1. Define “ Matter ” 2. What 2 major groups is matter divided into? 3. Give an example of a heterogeneous and homogeneous mixture. Unit 2: Matter and Density. Chapter 2, 3-4. I. Matter. NOTE: Matter = anything that: a) has mass , and b) takes up space

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IQ 1

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  1. IQ 1 • Define “Matter” 2. What 2 major groups is matter divided into? 3. Give an example of a heterogeneous and homogeneous mixture.

  2. Unit 2: Matter and Density Chapter 2, 3-4

  3. I. Matter NOTE:Matter= anything that: a) has mass, and b) takes up space NOTE: Mass= a measure of the amount of “stuff” (or material) the object contains (don’t confuse this with weight, a measure of gravity) NOTE: Volume= a measure of the space occupied by the object

  4. A. Describing Matter 1. Properties used to describe matter can be classified as: a. Extensive– depends on the amount of matter in the sample • Mass, volume, calories are examples b. Intensive – depends on the type of matter, not the amount present - Hardness, Density, Boiling Point

  5. B. Properties are… 1. Words that describematter (adjectives) 2. Physical Properties- a property that can be observed and measured without 3. changing the material’s composition. - Examples- color, hardness, m.p., b.p. 4. Chemical Properties- a property that can only be observed by changing the composition of the material. - Examples- ability to burn, decompose, ferment, react with, etc.

  6. C. States of matter 1. Solid- matter that can not flow (definite shape) and has definite volume. 2. Liquid- definite volume but takes the shape of its container (flows). 3. Gas- a substance without definite volume or shape and can flow. a. Vapor- a substance that is currently a gas, but normally is a liquid or solid at room temperature. (Which is correct: “water gas”, or “water vapor”?)

  7. 4. 4th state:Plasma - formed at high temperatures; ionized phase of matter as found in the suns

  8. States of Matter Result of aTemperature Increase? Definite Volume? Definite Shape? Will it Compress? Small Expans. Solid YES YES NO Small Expans. Liquid NO NO YES Large Expans. Gas NO NO YES

  9. Three Main Phases – page 41

  10. Condense Freeze Evaporate Melt Gas Liquid Solid

  11. Copper Phases - Solid

  12. Copper Phases - Liquid

  13. Copper Phases – Vapor (gas)

  14. D. Physical vs. Chemical Change 1. Physical change will change the visible appearance, without changing the composition of the material. • Boil, melt, cut, bend, split, crack • Is boiled water still water? 2. Can be reversible, or irreversible. 3. Chemical change - a change where a new form of matter is formed. • Rust, burn, decompose, ferment

  15. E. Mixtures 1. Mixtures are a physical blend of at least two substances; have variable composition. They can be either: a. Heterogeneous – the mixture is not uniform in composition • Chocolate chip cookie, gravel, soil. b. Homogeneous - same composition throughout; called “solutions” • Kool-aid, air, salt water 2. Every part keeps it’s own properties.

  16. 3. Solutions are homogeneous mixtures 4. Mixed molecule by molecule, thus too smallto see the different parts 5. Can occur between any state of matter: gas in gas; liquid in gas; gas in liquid; solid in liquid; solid in solid (alloys), etc. 6. Thus, based on the distribution of their components, mixtures are called homogeneous or heterogeneous.

  17. F. Phase 1. The term “phase” is used to describe any part of a sample with uniform composition of properties. 2. A homogeneous mixture consists of a single phase 3. A heterogeneous mixture consists of two or more phases. 4. Note Figure 2.6, page 45

  18. 2.2 When olive oil is mixed with vinegar, they form a heterogeneous mixture with two distinct phases. Olive oil and vinegar are homogeneous mixtures. Fig. 2.6 pg. 45

  19. G. Separating Mixtures 1. Some can be separated easily by physical means: rocks and marbles, iron filings and sulfur (use magnet) 2. Differences in physical properties can be used to separate mixtures. 3. Filtration - separates a solid from the liquid in a heterogeneous mixture (by size) – (Fig. 2.7, page 46)

  20. 2.2 Separating Mixtures A colander is used to separate pasta from the water in which it was cooked. This process is a type of filtration. Figure 2.7, page 46

  21. 2.2 Separating Mixtures During a distillation, a liquid is boiled to produce a vapor that is then condensed into a liquid. Figure 2.8, page 47

  22. Distillation:takes advantage of different boiling points. NaCl boils at 1415 oC

  23. Separation by Physical Means magnet

  24. Separation of a Mixture Components of dyes such as ink may be separated bypaper chromatography.

  25. II. Substances NOTE: Substances are either: a) elements, or b) compounds

  26. A. Substances: element or compound 1. Elements- simplest kind of matter a. cannot be broken down any simpler and still have properties of that element! b. all one kind of atom. 2. Compoundsare substances that can be broken down only by chemical methods a. when broken down, the pieces have completely different properties than the original compound. b. made of two or more atoms, chemically combined (not just a physical blend!)

  27. Made of one kind of material Made of more than one kind of material Made by a chemical change Made by a physical change Definite composition Variable composition B. Compound vs. Mixture Compound Mixture

  28. Element Compound Mixture Which is it?

  29. C. Elements vs. Compounds 1. Compounds canbe broken down into simpler substances by chemical means, but elements cannot. 2. A “chemical change” is a change that produces matter with a different composition than the original matter.

  30. D. Chemical Change 1. A change in which one or more substances are converted into different substances. 2. Heat and light are often evidence of a chemical change.

  31. E. Properties of Compounds 1. Quite different properties than their component elements. 2. Due to a CHEMICAL CHANGE, the resulting compound has new and different properties: a. Table sugar – carbon, hydrogen, oxygen b. Sodium chloride – sodium, chlorine c. Water – hydrogen, oxygen

  32. Colloids Suspensions F. Classification of Matter Matter Flowchart MATTER yes no Can it be physically separated? MIXTURE PURE SUBSTANCE yes no yes no Is the composition uniform? Can it be chemically decomposed? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

  33. G. Symbols & Formulas 1. Currently, there are 118 elements 2. Elements have a 1 or two letter symbol, and compounds have a formula. 3. An element’s first letter always capitalized; if there is a second letter, it is written lowercase: B, Ba, C, Ca, H, He 4. Start learning the elements names and symbols listed in Table B.7 on page R53 5. Some names come from Latin or other languages; note Table 2.2, page 52

  34. Elements named after Latin (old). a. Sodium _____ _______________________ • Gold _____ _______________________ c. Silver _____ _______________________ d. Potassium _____ _______________________ e. Lead _____ _______________________ f. Antimony _____ _______________________ g. Iron _____ _______________________ h. Tungsten _____ _______________________ i. Tin _____ _______________________ j. Copper _____ _______________________ k. Mercury _____ _______________________ Na Natrium Au Aurum Ag Argentium K Kalium Pb Plumbum Sb Stibinite Fe Ferrum W Wolfram Stannum Sn Cuprum Cu Hydrogyrum Hg

  35. Ag Nitrogen Oxygen Mg Helium F Zn H Carbon Mercury Element Quiz #1 Silver N O Magnesium He Fluorine Zinc Hydrogen C Hg

  36. Element quiz 1 • Ag • Nitrogen • Oxygen • Mg • Helium • F • Zn • H • Carbon • Mercury

  37. Zn Strontium Manganese Se Argon Fe Au Be Silicon Lead Element Quiz #2 Zinc Sr Mn Selenium Ar Iron Gold Beryllium Si Pb

  38. Sr Boron Bromine P Iodine F Cu Ba U Calcium Element Quiz #2 Strontium B Br Phosphorus I Fluorine Copper Barium Uranium Ca

  39. H. Extensive vs. Intensive intensive extensive extensive intensive intensive • Examples: 1. boiling point 2. volume 3. mass 4. density 5. conductivity

  40. I . Physical vs. Chemical Properties physical chemical physical physical chemical • Examples: 1. melting point 2. flammable 3. density 4. magnetic 5. tarnishes in air

  41. J. Physical vs. Chemical Change chemical physical chemical physical physical • Examples: 1. rusting iron 2. dissolving in water 3. burning a log 4. melting ice 5. grinding spices

  42. Basic Vinaigrette Recipe • 1 shallot finely minced • 1 tsp. dijon mustard (weak emulsifiers) • ¾ tsp. mayonnaise (contains lectithin- emulsifier) • 7 tsp. vinegar (basalmic or other acid) • ¼ cup olive oil • ½ tsp. honey (optional) • Salt and pepper • Fresh herbs can be added if desired • Mix shallot, honey, vinegar, dijon, and mayo until smooth. Slowly drizzle in ¼ cup of light or regular olive oil (other neutral flavored oils will work fine, but avoid extra virgin olive oil as the flavor can be overpowering. Season with salt and pepper to taste.

  43. K. Chemical Changes 1. The ability of a substance to undergo a specific chemical change is called a chemical property. a. iron plus oxygen forms rust, so the ability to rust is a chemical property of iron. 2. During a chemical change (also called chemical reaction), the composition of matter always changes.

  44. L. Chemical Reactions are… 1. When one or more substances are changed into new substances. 2. Reactants- the stuff you start with 3. Products- what you make 4. The products will have NEW PROPERTIES different from the reactants you started with 5. Arrow points from the reactants tothe new products

  45. M. Recognizing Chemical Changes 1. Energy is absorbed or released (temperature changes hotter or colder) 2. Color changes 3. Gas production (bubbling, fizzing, or odor change; smoke) 4. formation of aprecipitate- a solid that separates from solution (won’t dissolve) 5. Irreversibility- not easily reversed NOTE: But, there are examples of these that are not chemical – boiling water bubbles, etc.

  46. N. Conservation of Mass 1. During any chemical reaction, the mass of the products is always equal to the mass of the reactants. 2. All of the mass can be accounted for: a. Burning of wood results in products that appear to have less mass as ashes; where is the rest? 3. Law of Conservation of Mass

  47. - Page 55 43.43 g Original mass = 43.43 g Final mass reactants = product

  48. End of Chapter 2 Matter and Change Start of Section 3.4 Density

  49. II. DENSITY A. Density is an intensiveproperty of matter. 1. does NOT depend on quantity of matter. 2. temperature B. Contrast with extensive 1. depends on quantity of matter. 2. mass and volume. Brick Styrofoam

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