1. Physical Science Unit 3: Periodic Table and Bonding Day One Classifying Matter

2. UNIT 3 PERIODIC TABLE and BONDING

3. Take Notes in Notebook http://www.gpb.org/chemistry- physics/chemistry/202 http://www.gpb.org/chemistry- physics/chemistry/202 Do worksheet on this page together

4. Types of Matter Element - _______________ substance _______________ kind of _______________ − represented by ______________ or ______________ letter symbol − example: ______________ (___) Compound -______________ or more ______________ ______________ combined − represented by ______________ ______________ − example: ______________ (____) − H 2 O ______________ into _____________ _________ and ______________ _________. − ______________ in same ______________ Mixture - ______________ or more substances ______________ ______________ do not ______________ in same ______________ heterogeneous mixture - not _________ homogeneous mixture (solution) - _________ alloy - _________ of two or more _________ Pure ______________ are ______________.

5. Take Notes in Notebook http://www.gpb.org/chemistry- physics/chemistry/202 http://www.gpb.org/chemistry- physics/chemistry/202 Do worksheet on this page together

7. Solvents and Solutes Solvents and solutes can be any state of matter. A solution is another name for homogeneous mixtures that are stable. In salt water, for instance, the salt stays dissolved. – A solution cannot be separated by filtration. Figure 15.6 A solution cannot be separated by filtration. The small size of the solute particles allows them to pass through filter paper.

8. Suspensions Suspensions are heterogeneous because at least two substances can be clearly identified. – Unlike solutions, suspensions can be separated by filtration. Figure 15.14 A suspension is a heterogeneous mixture. Suspended particles can be removed by filtration. Comparing And Contrasting How does the filtration of a suspension compare with the filtration of a solution?

12. Worksheet: Classifying Matter

13. Physical Science Unit 3: Periodic Table and Bonding Day Two Classifying Matter and Intro to PT

14. Take Notes http://www.gpb.org/chemistry-physics/chemistry/203 Separating Mixtures The components of a mixture may be separated based on the physical properties of: __________________ __________________ (An instrument that uses this property to separate mixtures when tiny solid particles are dissolved in a liquid is called a __________________.) Some techniques used to separate the components of a mixture are: __________________ -- used to separate liquids and solids __________________ -- used to separate solutions

15. Review WS (from GPB 202) Classify each of the following as an element (E), compound (C), homogeneous mixture/solution (S), or heterogeneous mixture (HE). chocolate chip cookie _____ oxygen gas _____ salt water _____ taco _____ gold _____ carbon dioxide _____ water _____ kool aid _____ table salt _____ muddy water _____ potassium _____ brass _____ graphite _____ glass _____ air _____

16. Worksheet: Classifying Matter

17. Periodic Table

18. Periodic Table (Flash)

19. Physical Science Unit 3: Periodic Table and Bonding Day Three PT Cheat Sheet and Notes

20.  1 2 3 4 5 6 7 6 7

21.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

22.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

23.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 B Si As Ge SbTe PoAt metalsnonmetals

24.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 B Si As Ge SbTe PoAt metalsnonmetals Hg Br

25.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 B Si As Ge SbTe PoAt metalsnonmetals Hg Br H He NOF Cl Ne Ar Kr Xe Rn

26.  12345671234567 6767 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 B Si As Ge SbTe PoAt metalsnonmetals Hg Br H He NOF Cl Ne Ar Kr Xe Rn Alkali Metals Alkaline earth Metals Transition Metals HalogensNoble Gases Lanthanides Actinides

27. Periodic Table Definitions Period – horizontal row on P.T. There are 7 of them. Is equal to number of energy levels Group – Also called family. Vertical column on the P.T. There are 18 of them. Last number for 1, 2, 13-18 indicated number of valence electrons.

28. Periodic Table Definitions Metals – Good conductors of heat and electricity. Located on the left of the zigzag line on P.T. Nonmetals – Poor conductors of heat and electricity. Often brittle. Located on the right of the zigzag line on the P.T. Metalloids – Properties are inbetween metals and nonmetals. Good semi-conductors of electricity. Located along the zigzag line.

29. Periodic Table Groups Alkali metals – Group 1 metals. VERY reactive. Only found as compounds in nature. Alkaline earth metals – Group 2 metals. Reactive; only found as compounds in nature. Not as reactive as group 1. Transition metals – Metals in Groups 3-12. Lots of variation in properties. Generally don’t talk about these.

30. Periodic Table Groups Halogens – Group 17 nonmetals. Means “Salt former”. Very reactive. Noble gases – Group 18. Inert (means “unreactive”). Do not form compounds. Lanthanides and Actinides – placed under P.T. to keep P.T. short.

31. GPB http://www.gpb.org/chemistry- physics/chemistry/402 http://www.gpb.org/chemistry- physics/chemistry/402

32. Valence Electron An electron in the outermost energy level

33. Octet Rule Atoms gain, lose or share valence electrons so that there are EIGHT valence electrons

34. Energy Level Areas where electrons exist. Higher energy levels are far from nucleus. Can be 7 or more. 123

35. IONS Ions are atoms that have gained or lost electrons, and thus have a CHARGE!

36. Metal IONS Metals tend to LOSE electrons and form a positive charged ION, called a CATION. – Cations are positive charged ions.

37. Nonmetal IONS Nonmetals tend to GAIN electrons and form a NEGATIVE charged ION, called an ANION. – Anions are negative charged ions.

38. Physical Science Unit 3: Periodic Table and Bonding Day Four Intro to PT and Bohr Models

39. Valence Electron An electron in the outermost energy level

40. Octet Rule Atoms gain, lose or share valence electrons so that there are EIGHT valence electrons

41. Energy Level Areas where electrons exist. Higher energy levels are far from nucleus. Can be 7 or more. 123

42. IONS Ions are atoms that have gained or lost electrons, and thus have a CHARGE!

43. Metal IONS Metals tend to LOSE electrons and form a positive charged ION, called a CATION. – Cations are positive charged ions.

44. Nonmetal IONS Nonmetals tend to GAIN electrons and form a NEGATIVE charged ION, called an ANION. – Anions are negative charged ions.

45. GPB http://www.gpb.org/chemistry- physics/chemistry/402 http://www.gpb.org/chemistry- physics/chemistry/402

46. Glencoe WS: The Periodic Table

47. Physical Science Unit 3: Periodic Table and Bonding Day Five Intro to Bonding

48. Chemical Bond Definitions Chemical bond – Force that holds atoms together in a compound

49. Chemical Bond Definitions Ionic bond – forms when valence electrons are transferred from a metal to a nonmetal. Properties of ionic bonds: – High melting and boiling points (most are solids at room temperature) – Hard (not easily crushed) – Conduct electricity as liquid or dissolved in water Na + ClNa + Cl + ¯

50. Chemical Bond Definitions Covalent Bond – Electrons are shared between two nonmetals, forming a molecule. Properties of Covalent Bonds: – Lower (than ionic) melting and boiling points (can be solid, liquid or gas at room temp) – Can be brittle (easy to crush) – Do not conduct electricity (except acids DO)

51. Chemical Bond Definitions Metallic Bond – occurs in metals. Valence electrons are shared by ALL atoms, forming a “sea of electrons”. Properties of metallic bonds – Good conductors of electricity when in solid form – Typically high melting and boiling points (most are solid at room temp. Mercury is the exception.) – Luster (shiny) – Malleable (shapeable and form into thin sheets) – Ductile (can be drawn into wires)

52. Writing Ionic Formula Chemical formula – tells what elements and how many make up a compound.

53. GPB http://www.gpb.org/chemistry- physics/chemistry/501 http://www.gpb.org/chemistry- physics/chemistry/501

54. Physical Science Unit 3: Periodic Table and Bonding Day 7 Intro to Bonding

55. Chemical Bond Definitions Chemical bond – Force that holds atoms together in a compound

56. Chemical Bond Definitions Ionic bond – forms when valence electrons are transferred from a metal to a nonmetal. Properties of ionic bonds: – High melting and boiling points (most are solids at room temperature) – Hard (not easily crushed) – Conduct electricity as liquid or dissolved in water Na + ClNa + Cl + ¯

57. Chemical Bond Definitions Covalent Bond – Electrons are shared between two nonmetals, forming a molecule. Properties of Covalent Bonds: – Lower (than ionic) melting and boiling points (can be solid, liquid or gas at room temp) – Can be brittle (easy to crush) – Do not conduct electricity (except acids DO)

58. Chemical Bond Definitions Metallic Bond – occurs in metals. Valence electrons are shared by ALL atoms, forming a “sea of electrons”. Properties of metallic bonds – Good conductors of electricity when in solid form – Typically high melting and boiling points (most are solid at room temp. Mercury is the exception.) – Luster (shiny) – Malleable (shapeable and form into thin sheets) – Ductile (can be drawn into wires)

59. Writing Ionic Formula Chemical formula – tells what elements and how many make up a compound.

60. GPB http://www.gpb.org/chemistry- physics/chemistry/501 http://www.gpb.org/chemistry- physics/chemistry/501

61. Physical Science Unit 3: Periodic Table and Bonding Day Nine Writing Ionic Formulae

62. GPB http://www.gpb.org/chemistry- physics/chemistry/601 http://www.gpb.org/chemistry- physics/chemistry/601

63. Day 10 Binary Ionic Compounds

65. Day 11 Tertiary Ionic Compounds (Polyatomic Ions)

67. Day 12 Binary Covalent Compounds