1. WEEK OF 9-28-15 through 10-2-15

2. 9-25-15

3. Pre-Test Vs Post Test A pre-test is a test that teachers give students before material has been taught. A post-test is a test that teachers give students after material has been taught.  Why do teachers give pre-tests?  Why do teachers give post-tests?

4.  Classes 1, 2, 6 1. Review notes on “Organization of Matter” for quiz on tomorrow 2. 18.2 Review pg. 584 (1-4), Due Friday, 10-2-15  Classes 4, 5 1. Review notes on “Organization of Matter” for quiz on tomorrow 2. 18.2 Review pg. 584 (1-6), Due Friday, 10-2-15

5. Discuss/Take: **Pre-Assessment on 7th Grade Science SLO –Analyzing and Interpreting Models**

6.  Select the best answer for each question. This is a pre-test. It will not go in the gradebook.  So, do not worry if you do not know the answers. You will take a post-test later after all material has been covered this year to see how much you have learned.  No pressure, no worries!

7.  Family Feud Review Game- Completion

8. Keep in Classwork Section of Binder- Discussion- The chemical formula for simple sugar is C6H12O6. How many atoms of oxygen are in simple sugar?. How many elements makeup simple sugar? What is the process of getting energy from the sun to make simple sugars? Hint- Plants complete this process and also make oxygen in the process.

9. Exit Ticket- Why do scientists represent data in the form of symbols and chemical formulas?

10. 9-29-15

11. Explaining Bonds  Complete the common name and explanations for the following formulas. Use the periodic table. FormulasCommon NamesExplain the Bonds 1. O2Covalent because_______ 2. CO2Covalent because _______ 3. N2Covalent because_______ 4. Fe2O3Ionic because__________ 5. NaClIonic because__________ 6. H2OCovalent because_______ 7. C6H12O6Covalent because_______

12. Organization of Matter

13.  Get your lenovo and log on to www.socrative.com as a student.www.socrative.com  Type your last, first name  Sign in to Room Number 9832ab95  Take the "Organization of Matter Quiz -Part 1 Regular" (Periods 1, 2, 6)  Take the "Organization of Matter Quiz-Part 1 GT" (Periods 4, 5)

14. How can you differentiate between an ionic and covalent bond?

15. 9-30-15

16. Math and Science How are math and science related? Give specific examples?

17. Chemical Equations –Notes

18. 1. Matter is conserved in chemical reactions. 2. When a substance is broken apart or when substances are combined and at least one new substance is formed, a chemical reaction has occurred.

19. CHEMICAL EQUATIONS-NOTES -KEEP IN NOTEBOOK 3. Chemical equations are used to represent a chemical reaction.  It contains the chemical names or the chemical formulas of the substances that are involved in the reaction.  An arrow is used to distinguish between the reactants and the products in the reaction. This arrow ( ) can be translated as “yields” or “makes.”

20. CHEMICAL EQUATIONS-NOTES -KEEP IN NOTEBOOK 4. Reactants are substances broken apart or combined in a chemical reaction and are located on the left side of the arrow. Sketch to learn:

21. CHEMICAL EQUATIONS-NOTES-KEEP IN NOTEBOOK 5. Products are new substances formed in a chemical reaction and are located on the right side of the arrow.

22. CHEMICAL EQUATIONS-NOTES -KEEP IN NOTEBOOK 6. The following chemical equation shows the formation of water (H2O) from oxygen gas (O2 and hydrogen gas (H2). The reactants are oxygen gas (O2) and hydrogen gas (2H2), located on the left side of the arrow. The product, water (2H2O), is on the right side of the arrow. Copy the chart on the next page.

23. ReactantsProducts Hydrogen gas + Oxygen gas Yields/makes Water 2H2+02 2H202

24. 1. Why do scientists use chemical equations?  a. to turn simple reactions into complex processes  b. because equations are used in math and math is like science  c. to represent and understand chemical reactions  to represent substances we cannot see

25. 2. In which part of a chemical equation are you most likely to find the products?  a. to the left of the arrow, at the beginning  b. to the right of the arrow, at the end  c. on both side of the arrow, to be balanced  d. products do not show up in chemical equations

26. 3. If you know that water (H2O) is the only product in a chemical equation, which of the following chemical equations represents the chemical reaction that will occur?  a. 2H2O 2H2 +O2  b. H + Cl HCl  c. 2H2O + O2 2H2O  d. 2N +3H2 2NH3

27. Discussion- What are 2 chemical reactions that occur around you all the time? How do you know these are chemical reactions?

28. Why do scientists write chemical equations?

29. 10-1-15

30. Parts of a Chemical Equation  Label and define the parts of the chemical equation below. Identify all elements, the reactants, the products, coefficients, subscripts, and yield.  N2 + 3H2 2NH3

31.  Chemical Equations

32. 1. Law of Conservation of Matter states that the amount of matter does not change during a chemical reaction, only that the atoms are rearranged to form new substances. Another interpretation of this law is that matter can neither be created nor destroyed, but can be changed in form.

33. 2. Because matter is neither created nor destroyed, the total mass of the material(s) before the reaction is the same as the total mass of material(s) after the reaction.  A balanced chemical equation has the same number of each kind of atom on the reactant side as on the product side.

34. 3. To determine whether a chemical equation is balanced, two numbers are considered: the subscript and the coefficient.  A coefficient is the number that comes before the chemical formula and indicates the number of particles that participate in the reaction. THE COEFFICIENT IS THE LARGE NUMBER IN FRONT OF THE ELEMENT!  The subscript is the number written below and behind the symbol for the element and tells the number of atoms in the element. THE SUBSCRIPT IS THE SMALL NUMBER BEHIND THE ELEMENT!!

35. 3. SKETCH TO LEARN:

36. 4. In order to determine whether an equation is balanced, one must  Multiply the number in front of the chemical formula in the equation (coefficient) by the number written below the symbol for the element(s) (subscript) in the formula. If no coefficient is written, it is understood to be one. For instance, for “2H2O” there are 4 hydrogen atoms and 2 oxygen atoms. If no subscript is written, it is understood to be 1.  Determine if the number of each kind of atom on the left side of the arrow is equal to the number of each kind of atom on the right side of the arrow.

37. 5. For example, in the chemical equation for the reaction of water (liquid) breaking into hydrogen (gas) and oxygen (gas) as represented by the balanced chemical equation: 2H2O 2H2 + O2  There are four hydrogen atoms on the reactant side (coefficient of 2 x subscript 2) and four hydrogen atoms on the product side (coefficient 2 x subscript 2).  There are two oxygen atoms on the reactant side (coefficient 2 x (understood) subscript 1) and two oxygen atoms on the product side ((understood coefficient 1 x subscript 2).

38. 5. For example, in the chemical equation for the reaction of water (liquid) breaking into hydrogen (gas) and oxygen (gas) as represented by the balanced chemical equation: 2H2O 2H2 + O2  There are the same number of hydrogen atoms (4) and oxygen atoms (2) on both sides of the equation; therefore, the equation is balanced.  Since there are the same number of each kind of atom on both sides of the arrow and atoms represent kinds of matter, the amount of matter is the same on both sides of the equation, which supports the law of conservation of matter. *YOU CAN MULTIPLY A COEFFIENT BY A SUBSCRIPT IF THEY ARE NOT SEPARATED BY AN ADDITION SIGN OR ARROW. *YOU CANNOT MULTIPLY ACROSS AN ARROW OR ADDITION SIGN *REMEMBER YOUR UNDERSTOOD OR INVISIBLE 1

39. 1.Balancing Chemical Equations 6:21 *Watch First* https://youtu.be/4jISjQvdyhs

40. 2. Video Analysis-Balancing Chemical Equations 3:25 *Watch Second* https://youtu.be/Q4WWiAm3nPM 3. Balancing Chemical Equations Worksheet (Textbook Reference-pgs. 581, 582, 583

41. Apply pg. 583 (1-2)

42. How is the law of conservation of energy related to balanced equations?

43. 10-2-15

44. Mystery Substances What information would you gather to differentiate a glass of vinegar from a glass of rubbing alcohol? Glass of VinegarGlass of Rubbing Alcohol 11 22

45. Physical and Chemical Properties-Notes

46. 1. Physical and chemical properties can be used to classify and identify substances. 2. Physical properties can be observed without changing the composition of the substance.

47. 3. Physical properties of metals include:  Luster—Having a shiny surface or reflecting light brightly  Conductors—Heat and electricity move through them easily  Malleable—Ability to be hammered into different shapes  Ductile—Ability to be drawn into a wire  High density—Heavy for their size

48. 4. Physical properties of nonmetals include:  Dull—Not shiny  Nonconductors—Heat and electricity do not move through them easily  Brittle—Break or shatter easily (solids)

49. 5. Physical properties can be observed and measured without changing the kind of matter being studied.  The following physical properties can be used to help identify a substance: melting point, boiling point, conductivity, density, color, hardness, and magnetism.

50. 6. Melting Point  The temperature at which a solid can change to a liquid  Unchanging under constant conditions  Example: Ice melts to form liquid water at 0° C (32° F).

51. 7. Boiling Point  The temperature at which a liquid changes from a liquid to a gas.  Boiling begins when bubbles form, grow larger, rise to the surface, and burst.  As long as the substance is boiling the temperature of the liquid remains constant (at the boiling point).  Boiling point is unchanging under constant conditions for a given substance.  Example: The boiling point for pure water at sea level is 100° C (212 F).

52. 8. Density  The relationship between the mass of a material and its volume  Substances that are more dense contain more matter in a given volume.  The density of a substance is unchanging no matter how large or small the sample of the substance.  Example:  Lead is a very heavy, dense metal. The density of lead is much greater than the density of the very light metal, aluminum.  Generally, metals have a heavier density than nonmetals. * Marble Vs Christmas Ornament

53. 8. Density is a physical property that can be measured and calculated. Density  Density is the mass of a substance per unit of volume. Density of a substance changes with phase changes due to the difference in the particle arrangement in solids, liquids and gasses. The volume and density of a particular substance is dependent upon its phase or state of matter.  Bowling Ball Vs Basketball

54. 8. Density is calculated using the formula: density = mass/volume  Volume is measured in milliliters (mL) and can be calculated using basic mathematical computations or the liquid displacement method.  Mass is measured in grams.  The composition of a substance does not change when one measures mass and volume. Density, therefore, is a physical property.

55. 8. Example: If the mass of an object is 20 grams and the volume of the same object is 10 mL, what is the density of the object?  D=20g/10mL  D= 2 g/mL

56. 9. Conductivity  The ability to act as an electrical conductor or an electrical insulator is based on the solid’s ability to complete an electric circuit, i.e., conduct electricity.  Materials with high conductivity are called electrical conductors because they allow current to flow easily.  Materials with low conductivity are called electrical insulators (nonconductors) because they do not allow current to flow.  Example: Most metals are electrical conductors while nonmetals are electrical insulators.

57. 10. Color  Color can be used to help identify a substance, along with other properties.  By itself, color is not a significant identifier of a substance.  Absence of color is also a physical property.

58. 11. Hardness  The relative resistance of a metal or other material to denting, scratching, or bending.

59. 12. Magnetism  The property of reacting to the forces exerted by magnets  Example: materials that are attracted to magnets are considered to be magnetic. Magnetic materials are mostly metals.

60. 13. Chemical properties Chemical properties can be recognized only when substances react or do not react chemically with one another, that is, when they undergo a change in composition.  Chemical properties cannot be observed without changing the composition of the substance, changing it into a new substance.

61. 14. Chemical properties  The following chemical property can be used to help identify a substance:  Ability to burn: The ability to burn involves a substance reacting quickly with oxygen to produce light and heat. This process is called burning

62. 15. Chemical properties  The following chemical property can be used to help identify a substance:  Ability to rust: The ability of a substance to rust is a chemical property that involves a substance reacting slowly with oxygen. The process is called rusting.

63.  Video Analysis-Physical Vs Chemical Properties 6:25  https://youtu.be/Z5L2NOMEWT0 https://youtu.be/Z5L2NOMEWT0

64. 1. What 2 quantities must be known to calculate the density of a sample of matter? a. color and mass b.mass and volume c. length and mass d. volume and texture

65. 2. Which of these is a physical property of matter? a. ability to rust b. ability to react with oxygen c. melting point d. ability to burn

66. 3. Which of these is a chemical property of matter? a. ability to burn b. freezing point c. boiling point d. density

67. 4. Identify the unknown substance. Properties recorded: colorless, has a strong and sour odor, and boils over 100 degrees Celsius. Based on the chart below and information recorded, which liquid do you have? Boiling Points of Selected Liquids a. alcohol c. vinegar b. pure water d. olive oil LiquidsBoiling Points (Degrees Celsius) Alcohol79 Pure Water100 Vinegar139 Olive Oil300

68. How do physical and chemical properties differ?