1 / 50

Properties of Matter

Chapter 2. Properties of Matter. Matter. anything that has mass and volume Mass : measure of the amount of matter an object contains Volume : measure of space occupied by the object. Matter. Every sample of matter is Pure Substance Element or Compound Mixture

stesha
Download Presentation

Properties of Matter

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. Chapter 2 Properties of Matter

  2. Matter • anything that has mass and volume • Mass: measure of the amount of matter an object contains • Volume: measure of space occupied by the object

  3. Matter • Every sample of matter is • Pure Substance • Element or Compound • Mixture • Homogeneous or Heterogeneous

  4. Matter

  5. Elements • A substance that cannot be broken down into simpler substances by chemical means • Elements are made up of one type of atom • Atom: smallest unit of matter that keeps its chemical properties

  6. Elements • Elements are represented by an element symbol

  7. Molecules • Smallest unit of a substance that behaves like the substance • Chemically bonded together

  8. Compounds • A substance made up of atoms of different elements. • Contains 2 or more elements • Chemically combined • Definite proportions • Elements combine in the same proportions • Ex: water, H2O hydrogen peroxide, H2O2

  9. Chemical Formula • Represent compounds • C12H22O11 table sugar • 3 molecules of table sugar (3C12H22O11) are equivalent to • 36 Carbons • 66 Hydrogens • 22 Oxygens

  10. Pure substances and Mixtures • All matter is either a pure substance or a mixture • Pure substance • Compound or Element • Mixture • Heterogeneous or Homogenous

  11. Pure substance • Element or Compound • Matter that has fixed composition and definite properties • Table Salt (NaCl – sodium chloride)

  12. Mixtures • Physical blend of 2 or more compounds • Heterogeneous: composition is not uniform throughout (2 or more phases) • Homogeneous: composition is uniform throughout (1phase) • aka: solution • Phase: any part of a sample with uniform composition

  13. Properties of Matter • Extensive: depends on amount of matter • Ex: volume, mass • Intensive: depends on type of matter • Ex: density, m.p., hardness

  14. Properties of Matter • Physical property:can be observed or measured without changing substance’s composition • Color, mass, etc. • Chemical property: ability of substance to undergo a specific chemical change • Flammability, reactivity, etc. • Gold vs. Copper

  15. Density • is a physical property • = Mass per Volume • Grams/cubic centimeter (g/cm3) • Grams/ milliliter (g/ml)

  16. Classification of Matter

  17. END of DAY 1

  18. Physical Changes • Some properties of a material change, but the composition of the material does not change • Reversible: Boil, freeze, melt, condense • Irreversible: Break, split, grind, cut, crush

  19. Physical Changes • Affects one or more physical properties – does not change the identity • Composition of substance remains unchanged • Reversible: melt, freeze, sublime, etc • Irreversible: cut, crack, chip, etc

  20. Chemical Changes • A complete new substance is formed • Reversible/Irreversible • Burn, rot, rust, decompose, ferment, explode, corrode, grow

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

  22. Separating Mixtures • Physical means: rocks and marbles, iron filings and sulfur (use magnet) • Differences in physical properties can be used to separate mixtures. • Magnetic, temperature, etc. • Filtration - separates a solid from the liquid in a heterogeneous mixture (by size) • Distillation – liquid boiled to produce a vapor that is condensed into a liquid

  23. Separation of a Mixture Distillation:takes advantage of different boiling points. NaCl boils at 1415 oC

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

  25. States of Matter • Solid: def shape, def volume • Liquid: indef shape, def volume • Gas: indef shape, indef volume • Easily compressed • Vapor: the gaseous state of a substance that is generally a liquid

  26. Three Main Phases – page 41

  27. States of Matter Result of aTemperatureIncrease? 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

  28. Condense Freeze Evaporate Melt Gas Liquid Solid

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

  30. Elements vs. Compounds • Compounds can be broken down into simpler substances by chemical means, but elements cannot. • A “chemical change” is a change that produces matter with a different composition than the original matter.

  31. 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 Compound vs. Mixture Compound Mixture

  32. Element Compound Mixture Which is it?

  33. Volume is: • A measure of the space occupied by the object

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

  35. Properties are… • Words that describe matter (adjectives) • Physical Properties- a property that can be observed and measured without changing the material’s composition. • Examples- color, hardness, m.p., b.p. • 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.

  36. States of matter • Solid- matter that can not flow (definite shape) and has definite volume. • Liquid- definite volume but takes the shape of its container (flows). • Gas- a substance without definite volume or shape and can flow. • 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”?)

  37. 4th state: Plasma - formed at high temperatures; ionized phase of matter as found in the sun

  38. Copper Phases - Solid

  39. Copper Phases - Liquid

  40. Copper Phases – Vapor (gas)

  41. Physical vs. Chemical Change • 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? • Can be reversible, or irreversible • Chemical change - a change where a new form of matter is formed. • Rust, burn, decompose, ferment

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

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

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

  45. Section 2.3Elements and Compounds • OBJECTIVES: • Explain the differences between an element and a compound.

  46. Section 2.3Elements and Compounds • OBJECTIVES: • Distinguish between a substance and a mixture.

  47. Section 2.3Elements and Compounds • OBJECTIVES: • Identify the chemical symbols of elements, and name elements given their symbols.

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

  49. Symbols & Formulas • Currently, there are 117 elements • Elements have a 1 or two letter symbol, and compounds have a formula. • An element’s first letter always capitalized; if there is a second letter, it is written lowercase: B, Ba, C, Ca, H, He • Start learning the elements names and symbols listed in Table B.7 on page R53 • Some names come from Latin or other languages; note Table 2.2, page 52

  50. Section 2.4Chemical Reactions • OBJECTIVES: • Describe what happens during a chemical change.

More Related