1. H Chem / Chem 2013

2. Notes – Chap 2 Properties of Matter

3. Matter - Anything that takes up space, has mass, and applies inertia. 1)Mass - Measures the amount of matter

4. Matter - Anything that takes up space, has mass, and applies inertia. Weight -The gravitational force of attraction exerted by the earth on a body (SI – Newton) 1) Mass - Measures the amount of matter

5. Matter - Anything that takes up space, has mass, and applies inertia. 2) Volume – The amount of space an object occupies

6. Matter - Anything that takes up space, has mass, and applies inertia. 3) Inertia - It is the resistance to change in motion. Causes a body at rest to stay at rest, and when in motion to continue in motion.

7. Matter - Anything that takes up space, has mass, and applies inertia. 3)Inertia - It is the resistance to change in motion. Causes a body at rest to stay at rest, and when in motion to continue in motion.

8. Energy -The ability to do work. This can be changed from one form to another, but cannot be created or destroyed. Examples - Light, heat, chemical, mechanical, nuclear

10. Types of Matter Atoms -The building blocks of matter. “Atomos” – its name means “uncut”. It is the smallest part of an element which has the properties of that element.

11. Types of Matter Example: HC O FeAu Element -The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

12. Types of Matter Example: HC HydrogenCarbon O Oxygen FeAu IronGold Element -The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

13. Types of Matter Element -The simplest form of matter. It cannot be changed to another form by chemical change, and has only one kind of atom.

14. Types of Matter Substance - Name for matter like elements and compounds because of their uniform and definite composition as well as distinct properties Hydrogen Oxygen Silver Gold NaCl – Table Salt

15. Hydrogen Oxygen Silver Gold

17. Chemical bond – Force of attraction between two atoms Molecule-The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond Types of Matter H 2 – Hydrogen molecule NaCl – Table Salt molecules

18. It includes: H 2 0 NaCl O 2 CO 2 N 2 Molecule-The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond Types of Matter

19. It includes: H 2 0NaCl Water salt O 2 CO 2 oxygen gascarbon dioxide N 2 nitrogen gas Molecule-The smallest particle of a material that can be identified as that material. It is made up of two or more atoms, but they may be the same type of atoms. Held together with a chemical bond Types of Matter

20. H 2 – Hydrogen gas O 2 – Oxygen gas NaCl – Table Salt

21. Chemical formulas – Abbreviated form of elements and compound showing the element symbols and numbers and ratios of atoms Examples- He CO 2 H 2 O NaCl NaHCO 3 Types of Matter

22. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms Examples- He - Helium CO 2 –carbon dioxide H 2 O - water NaCl – sodium chloride (salt) NaHCO 3 – sodium bicarbonate (baking soda) Types of Matter

23. Compound -A substance which cannot be broken into smaller substances by physical changes. It is composed of two or more different elements chemically combined in certain fixed proportions. Example: H 2 0 NaCl C 6 H 12 O 6 C 8 H 24 O 8

24. Compound -A substance which cannot be broken into smaller substances by physical changes. It is composed of two or more different elements chemically combined. Example: H 2 0 - water NaCl – salt C 6 H 12 O 6 – sugar C 8 H 24 O 8 - gasoline

25. Table Salt NaCl- Sodium Chloride

26. Mixtures -Any matter which contains more than one kind of molecule that is not chemically combined and can be separated physically. Not pure substances. The substances retain their individual properties Example:Sand, salad, salted water, air, mixed nuts Types of Matter

27. Solution -A special mixture formed when one kind of material (usually water) fills the space between the particles of another material. Examples: Salt water, coffee, orange juice Types of Matter

28. Solution -A special mixture formed when one kind of material (usually water) fills the space between the particles of another material. Solution are said to be: Homogeneous mixtures – they look the “same” throughout Mixtures that look “different” are called: Heterogeneous mixtures Examples: Salt water, coffee, orange juice Types of Matter

29. Solution -A special mixture formed when one kind of material (usually water) fills the space between the particles of another material. Examples: Salt water, coffee, orange juice Solution are said to be: Homogeneous mixtures – they look the “same” throughout Mixtures that look “different” are called: Heterogeneous mixtures Types of Matter

30. Solution are said to be: Homogeneous mixtures – they look the “same” throughout Mixtures that look “different” are called: Heterogeneous mixtures Types of Matter

31. Solutions Solutions consist of one or more solutes and a solvent. Solute – the dissolved substance in a solution. Salt in salt water is a solute Solvent – The dissolving agent in a solution. Water dissolving salt in salt water is an example

32. Aqueous – Solutions which are actually water based Colloid – The type of mixture which contains small particles suspended in a solution Solutions

33. Aqueous – Solutions which are actually water based Colloid – The type of mixture which contains small particles suspended in a solution – Tyndall effect : The scattering of light indicating small solid particles Solutions

34. Suspension - A type of heterogeneous mixture where the solid particles are large enough to settle out or can be separated by filtration. The process that separates solids from a liquid

35. Solutions Separation of solutes from homogeneous mixtures can be accomplished by distillation. The process where a liquid is boiled to produce a vapor that is condensed to a liquid.

36. Solutions Separation of solutes from homogeneous mixtures can be accomplished by distillation. The process where a liquid is boiled to produce a vapor that is condensed to a liquid.

38. States of Matter (4) Determined by the amount of energy in their moving particles.

39. States of Matter (4) 1) Solids -State of matter which maintains a constant volume and shape. Normally has a crystalline structure. Example:Ice, Rocks and Minerals

40. Solids

41. States of Matter (4) 2) Liquids – State of matter which takes the shape of its container and has a relatively constant volume. Example:Water, Mercury

43. States of Matter (4) 3) Gases -State of matter with no constant shape and whose volume varies with temperature and pressure. Vapor – Gaseous state of a substance that is generally a liquid or solid at room temperature. Ex: Water vapor Example:Air, Oxygen, Water vapor

44. Water vapor (steam)

45. States of Matter (4) 4) Plasma -State of matter similar to gas, made up of electrical particles at extremely high temperatures. It is found in the sun and stars.

49. Changes of State Melting - solid to liquid (ice to water) Fusion (freezing) - liquid to solid (water to ice) Evaporation -liquid to gas (water to steam/water vapor) Condensation - gas to liquid(water vapor to water) Sublimation -solid to gas(ice to water vapor)

51. Changes of Matter Physical Change - When a substance is changed to a new form, but its molecules are the same as before, and it can be changed back physically. Includes density, melting, boiling, texture, color, flexibility Examples:When substances are bent, smashed, ripped, melted, frozen, etc. Ripping a piece of paper, melting ice.

53. Special Properties of Matter Density – The amount of matter (mass) in a given volume. It is how much something weighs versus how much space it takes up Measured in grams per milliliter (g/mL) or grams per cubic centimeter (g/cm 3 ). Examples:Water has a density of 1 g/mL wood is.7 g/mL iron is 7.8 g/mL.

54. Special Properties of Matter Measured in grams per milliliter (g/mL) or grams per cubic centimeter (g/cm 3 ). Examples:Water has a density of 1 g/mL wood is.7 g/mL iron is 7.8 g/mL.

55. Changes of Matter Chemical Change - When a substance is changed to a new form, but its molecules are different from before, and can’t be changed back. Describes its ability to change. Flammability, ability to react Examples:When substances are burned or chemically react. Burning paper, iron rusting, fireworks exploding.

58. Chemical Changes Chemical properties – The ability of a substance to undergo chemical change Chemical reaction – When one or more substances change into two or more substances – Reactant : Substance present at the beginning of a reaction – Product: Substance produced in the reaction ReactantsProducts

59. Chemical changes Evidence of chemical change: 1) Transfer of energy (warm or cold) 2) Change in color 3) Production of a gas 4)Formation of a precipitate (solid from a liquid mixture)

60. Law of Conservation of Mass During a chemical reaction, the mass of the products is always equal to the mass of the reactants. Mass is neither created nor destroyed, only changed to a different form.