1. EARTH SCIENCE Prentice Hall EARTH SCIENCE Tarbuck Lutgens 

2. Good Morning From Mrs. Melodi Lowery. My son is having surgery today and I really need to be with him. Please do not waste this day. Please do what the sub asks of you and make me proud. You will have multiple slides to copy the sub will advance the slides at his or her discretion meaning when students that are working are finished. The next slide will be written in Your Starter Notebooks (Remember I have the other notebook). The next slide is your vocabulary you do not have to look them up I have done that for you (Your Welcome). The remaining slides must be done on Loose Leaf Notebook Paper to be turned on Tomorrow. Remember the sub will not go back to catch you up you must keep up. See you, Wednesday.

3. 2 Chapter 2 Vocabulary (Quiz Friday) Copy in Starter Book After Ch 2. Vocabulary 1.Atomic number—The number of Protons & Electrons in an atom 2.Isotope--elements that have the same number of protons but varying numbers of neutrons. 3.Mass number-- the number of neutrons and protons in the nucleus of an atom. 4.Energy Level—the shells that surround an atom 5. Ion—an atom that gains or looses electrons. 6.Group ---the columns on the periodic table, also known as families. 7.Period ---the rows on the periodic table 8.Nonmetal---elements that do not exhibit the properties of a metal 9. Metal –a chemical element that is a good conductor of both electricity and heat 10.Metalloid –an element that exhibits both metal and nonmetal properties

4. Remember: You are to copy all the slides that follow on Loose Leaf Notebook Paper.

5. Chemical Bonding When an atom’s outermost energy level does not contain the maximum number of electrons, the atom is likely to form a chemical bond with one or more other atoms. 3 types of chemical bonds 1. ionic bonds-form ions 2. covalent bonds-form molecules 3. metallic bonds. Ionic bonds form between positive and negative ions. Ex. Salt forms when sodium (Na) reacts with chlorine (Cl) Covalent bonds form when atoms share electrons. Ex. Water forms when Hydrogen(H) reacts with oxygen(O) Metallic bonds form when electrons are shared by metal ions

6. Copy Questions and Answer on your paper! 1. What is an element? 2. What kinds of particles make up atoms? 3. What are isotopes? 4. What are compounds and why do they form?

7. Elements and the Periodic Table 2.1 Matter  Elements are the basic building blocks of minerals.  Over 100 elements are known.

8. Atoms  Smallest particles of matter 2.1 Matter  Have all the characteristics of an element neutrons, which have neutral electrical charges  The nucleus is the central part of an atom and contains protons, which have positive electrical charges

9. Atoms 2.1 Matter  Energy levels, or shells surround the nucleus contain electrons—negatively charged particles  The atomic number is the number of protons in the nucleus of an atom.

10. Model of an Atom

11. Isotopes  Many isotopes are radioactive and emit energy and particles.  Isotopes of an element have the same number of protons but varying numbers of neutrons.  Have different mass numbers: the sum of the neutrons plus protons 2.1 Matter  The mass number is the number of neutrons and protons in the nucleus of an atom.

12. Why Atoms Bond A compound consists of two or more elements that are chemically combined in specific proportions.  When an atom’s outermost energy level does not contain the maximum number of electrons, the atom is likely to form a chemical bond with one or more atoms. 2.1 Matter An ion is an atom that gains or loses electrons.

13. Types of Chemical Bonds 1. Ionic bonds form between positive and negative ions. 2.1 Matter 2. Covalent bonds form when atoms share electrons. 3. Metallic bonds form when metal ions share electrons.

14. Chumbler - Properties of Matter 14 States of Matter Chemistry The Four States of Matter

15. States of Matter The Four States of Matter Four States  Solid  Liquid  Gas  Plasma

16. States of Matter The Four States of Matter Basis of Classification of the Four Types  Based upon particle arrangement  Based upon energy of particles  Based upon distance between particles

17. States of Matter Solids  Particles of solids are tightly packed, vibrating about a fixed position.  Solids have a definite shape and a definite volume.  Solids have an infinite number of free surfaces.

18. States of Matter Solids Particle Movement Examples

19. States of Matter Liquids  Particles of liquids are tightly packed, but are far enough apart to slide over one another.  Liquids have an indefinite shape and a definite volume.  Liquids have one free surface.

20. Chumbler - Properties of Matter 20 States of Matter Liquids Particle Movement Examples

21. States of Matter Gases PParticles of gases are very far apart and move freely. GGases have an indefinite shape and an indefinite volume. GGases have no free surfaces.

22. Gases Particle Movement Examples States of Matter

23. Chumbler - Properties of Matter 23 States of Matter Plasma  A plasma is an ionized gas.  A plasma is a very good conductor of electricity and is affected by magnetic fields.  Plasma, like gases have an indefinite shape and an indefinite volume.

24. States of Matter Plasma Particles The negatively charged electrons (yellow) are freely streaming through the positively charged ions (blue ).

25. States of Matter Microscopic Explanation for Properties of Solids  Solids have a definite shape and a definite volume because the particles are locked into place  Solids are not easily compressible because there is little free space between particles  Solids do not flow easily because the particles cannot move/slide past one another

26. States of Matter Microscopic Explanation for Properties of Liquids  Liquids have an indefinite shape because the particles can slide past one another.  Liquids are not easily compressible and have a definite volume because there is little free space between particles.  Liquids flow easily because the particles can move/slide past one another.

27. Microscopic Explanation for Properties of Gases GGases have an indefinite shape and an indefinite volume because the particles can move past one another. GGases are easily compressible because there is a great deal of free space between particles. GGases flow very easily because the particles randomly move past one another. States of Matter

28. States of Matter Microscopic Explanation for Properties of Plasmas  Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another.  Plasmas are easily compressible because there is a great deal of free space between particles.  Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei).

29. States of Matter The Four States of Matter The Classification and Properties of Matter Depend Upon Microscopic Structure  Particle arrangement  Particle energy  Particle to particle distance

30. Matter MixturesHomogeneous Solution Solvent SolutionColloids Heterogeneous Suspensions Pure Substances ElementMoleculeCompounds

31. End of Monday Notes

32. The Periodic Table

33. Describe how to read the periodic table: Atomic Number The number of protons in an atom identifies the element. The number of protons in an atom is referred to as the atomic number of that element.

34. Describe how to read the periodic table: Atomic Symbol: The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). These symbols are used every where in the world Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element.

35. Describe how to read the periodic table: Atomic Mass: The atomic mass is the average mass of an element in atomic mass units ("amu"). Though individual atoms always have a whole number of amus, the atomic mass on the periodic table is shown as a decimal number because it is an average of all the isotopes of an element.

36. Definition of a Mineral 2.2 Minerals 1. Naturally occurring 2. Solid substance 3. Orderly crystalline structure 4. Definite chemical composition 5. Generally considered inorganic

37. How Minerals Form 2.2 Minerals 1. Crystallization from magma 2. Precipitation 3. Pressure and temperature 4. Hydrothermal solutions

38. Minerals Formed as a Result of Crystallization of Magma

39. Mineral Groups  Can be classified based on their composition 2.2 Minerals 1. Silicates Silicon and oxygen combine to form a structure called the silicon-oxygen tetrahedron. This silicon-oxygen tetrahedron provides the framework of every silicate mineral.

40. The Silicon-Oxygen Tetrahedron

41. Silicon-Oxygen Chains, Sheets, and Three-Dimensional Networks

42. Mineral Groups 2.2 Minerals 2. Carbonates Minerals that contain the elements carbon, oxygen, and one or more other metallic elements 3. Oxides Minerals that contain oxygen and one or more other elements, which are usually metals

43. Mineral Groups 2.2 Minerals 4. Sulfates and Sulfides Minerals that contain the element sulfur 5. Halides Minerals that contain a halogen ion plus one or more other elements 6. Native elements Minerals that exist in relatively pure form

44. Sulfides

45. Native Copper

46. Color 2.3 Properties of Minerals  Small amounts of different elements can give the same mineral different colors.

47. Streak 2.3 Properties of Minerals  Streak is the color of a mineral in its powdered form.

48. Luster 2.3 Properties of Minerals  Luster is used to describe how light is reflected from the surface of a mineral.

49. Pyrite (Fool’s Gold) Displays Metallic Luster.

50. Crystal Form 2.3 Properties of Minerals  Crystal form is the visible expression of a mineral’s internal arrangement of atoms.

51. Quartz Often Exhibits Good Crystal Form.

52. Hardness 2.3 Properties of Minerals  Hardness is a measure of the resistance of a mineral to being scratched.  Mohs scale consists of 10 minerals arranged from 10 (hardest) to 1 (softest).

53. Mohs Scale of Hardness

54. Cleavage 2.3 Properties of Minerals  Cleavage is the tendency of a mineral to cleave, or break, along flat, even surfaces.

55. Mica Has Cleavage in One Direction

56. Fracture 2.3 Properties of Minerals  Minerals that do not show cleavage when broken are said to fracture.  Fracture — the uneven breakage of a mineral

57. Conchoidal Fracture

58. Density 2.3 Properties of Minerals  Density is a property of all matter that is the ratio of an object’s mass to its volume.

59. Distinctive Properties of Minerals 2.3 Properties of Minerals  Some minerals can be recognized by other distinctive properties.