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Chapter 3

Chapter 3. MATTER. Section 3.1 The Particulate Nature of Matter. Objective: Learn about the composition of matter. Matter. Matter is anything that: a) has mass, and b) takes up space

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Chapter 3

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  1. Chapter 3 MATTER

  2. Section 3.1 The Particulate Nature of Matter • Objective: • Learn about the composition of matter

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

  4. States of Matter • Objective: • To define the 3 states of matter

  5. 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”?)

  6. States of Matter Result of aTemperatureIncrease? Definite Volume? Definite Shape? Will it Compress? Small Expands. Solid YES YES NO Small Expands. Liquid NO NO YES Large Expands. Gas NO NO YES

  7. Three Main Phases Solids – molecule are locked into fixed positions….little movement to move Liquids – molecules can slide past one another Gas – a free to move randomly about

  8. Copper Phases - Solid

  9. Copper Phases - Liquid

  10. Copper Phases – Vapor (gas)

  11. Condense Freeze Evaporate Melt Gas Liquid Solid

  12. 4th state:Plasma - formed at high temperatures; ionized phase of matter as found in the sun

  13. Ever heard of a Bose-Einstein Condensate??? http://www.pbs.org/wgbh/nova/physics/ultracold-atoms.html

  14. Section 3.2Physical/Chemical Properties and Changes • Objective: • To distinguish between physical and chemical properties • To distinguish between physical and chemical changes

  15. Properties are… • Words that describe matter (adjectives) • Physical Properties- a property that can be observed and measured without changing the material’s composition. • Describes individual characteristics • Examples- color, hardness, m.p., b.p. • Chemical Properties- a property that can only be observed by changing the composition of the material. • Describes social characteristics • Examples- ability to burn, decompose, ferment, react with, etc.

  16. 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

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

  18. Section 3.5Separation of Mixtures • Objective: • Learn 2 methods of separating a mixture

  19. Separation of a Mixture • Objective: • Learn 2 methods of separating mixtures

  20. Separating Mixtures- (talk more about mixtures is tomorrow) • Some mixtures can be separated easily by physical means: rocks and marbles, iron filings and sulfur (use magnet) • Differences in physical properties can be used to separate mixtures. • Filtration - separates a solid from the liquid in a heterogeneous mixture (by size) – Figure 2.7, page 46

  21. Filtration separates a liquid from a solid.

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

  23. Another view of Distillation

  24. Separation of a sand-saltwater mixture To separate sand-saltwater mixture: first use filtration to separate sand from saltwater then use distillation to separate salt and water

  25. Section 3.3Elements and Compounds • Objective: • The difference between a element & compound

  26. What about atoms? • All matter is made up of tiny particles called ATOMS • Although objects look quite continuous and uniform, they are really particulate in nature • Atoms are not all alike • About 100 different types of atoms make up all the different types of matter • Think of the alphabet (atoms) and words (matter)

  27. Element, Compound or Molecule • Elements simplest kind of matter • cannot be broken down any simpler and still have properties of that element! • all one kind of atom. • Compoundsare 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 moredifferent atoms, chemically combined (not just a physical blend!) • Molecules are substances that can be broken down only by chemical methods • made of two or more atoms, chemically combined (not just a physical blend!)

  28. I am not clear on what a molecule is. If water is a molecule, is it also a compound because the hydrogen and oxygen have been chemically combined? If so, how do you determine whether a substance is a compound or a molecule? • A molecule is what you get when any atoms join together. • A compound is what you get when atoms of two or more different elements join together. • All compounds are molecules, but not all molecules are compounds. • Water is a molecule because it is made from atoms that have been chemically combined. It is also a compound because the atoms that make water are not all the same - some are oxygen and some are hydrogen. • Oxygen in the atmosphere is a molecule because it is made from two atoms of oxygen. It is not a compound because it is made from atoms of only one element - oxygen. This type of molecule is called a diatomic molecule, a molecule made from two atoms of the same type.

  29. Elements vs Compounds • Currently, there are 117elements • 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 • Some names come from Latin or other languages

  30. Compounds vs Elements • Compounds can be broken down into simpler substances by chemical means, but elementscannot. • Compounds always contain atoms of different elements…..Always in the same composition • Ex.Water is always found as 2 hydrogen atoms combined with 1 oxygen atom

  31. Section 3.4Mixtures vs Pure substance • Objective: • To distinguish between mixtures and pure substances

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

  33. 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.

  34. Alloy – mixture of metals Twenty-four-karat gold is an element Eighteen-karat gold is an alloy. Fourteen-karat gold is an alloy.*An alloy is a mixture or metallic solid solution composed of two or more elements

  35. Tie together some of the information What is the difference then between a mixture and a compound????

  36. 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

  37. Pure Substances • Pure substances – always have same composition • Either elements or compounds • Ex pure water is a pure substance – it only contains H2O molecules • Tap water is a mixture – it contains H2O and other minerals such as calcium and magnesium

  38. Classification of Matter

  39. Which is it?

  40. Element

  41. Which is it?

  42. Compound/molecule

  43. Which is it?

  44. Mixture

  45. Which is it?

  46. Molecule. CANNOT be a compound. WHY????

  47. Chapter 3 The End

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