! Name: STUDENT JOURNAL Week 17 Chemical Reactions

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1 ! Name: Period: STUDENT JOURNAL Week 17 Chemical Reactions Overarching Goal for the Week: Understand that in chemical reactions atoms rearrange to make new substances but matter and mass are neither created nor destroyed in these reactions. Learning Objectives: Define chemical change. Distinguish between physical and chemical change. Identify examples of chemical and physical change. Distinguish among elements, compounds, and molecules. Determine how a chemical reaction satisfies the law of conservation of mass Write a balanced chemical equation. Identify common chemical reactions. Vocabulary Chemical Property Chemical Change Dissolving Law of Conservation of Mass Reactants Products Diatomic molecule Coefficient

2 ! My Mad Minute Graph Day #5 Mad Minute: Question #1 - Are you satisfied with your overall average for this week? Why or why not?! What's Your Average? Day 1 Day Day 3 + Day 4 Total / 3 =

3 ! DAY 1- Monday Kickoff: Pencils down! Wait for Mad Minute Mad Minute Write yes or no. Is the following a physical change? 1. Tearing a piece of paper in half. 2. Melting gold. 3. Iron rusting 4. Wood burning 5. Water boiling Agenda 1. Complete / Look over Compounds Quiz 30 minutes 2. If/When you re done Read Chapter 8;1, define vocab words, and do Day 1 Questions in back 3. Lecture/Notes for the second part of cla Grade and graph your Mad Minute!!!

4 Chemical Properties and Changes Name: Learning Objectives Define chemical change Distinguish between physical and chemical change Identify examples of chemical and physical change Vocabulary Chemical Property Chemical Change Dissolving! Ability to Change In a, the that give a substance its identity, change. Properties of matter help objects. Properties are either or. A chemical property is the ability or inability of a substance to or into one or more substances. Chemical Properties Examples of chemical properties include or. Some substances react. Physical Properties Physical properties can be observed without the. Chemical and Physical Changes Chemical changes change one substance into. Usually chemical changes be easily. Forming New Substances All chemical changes produce substances that are from the starting substances. Examples: A compound is into its. Two elements to form a. Physical Changes A change is a change in which the properties of a substance change but the of the substance. is a process in which substances with one another. Summary:

5 ! Questions /Examples/ Workspace: Guided Practice CCM Chapter 8; Lesson 1 Independent Practice CCM Chapter 8; Lesson 1 Independent Practice Questions Exit Ticket

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8 ! DAY 2 - Tuesday Kickoff & Mad Minute Today we are going to review the last quiz. On your quiz reflection, answer, the questions on how well you think you did and how much you studied. After you have seen your results you ll need to finish the reflection sheet as part of completing this week s journal. Agenda Quiz performance review Review most missed questions Student Questions from Quiz Prepare to turn in Week 16 s journal

9 QUIZ/TEST REFLECTION Iexpectedtoscore (proficiencylevel)onthe quiz/test. ThereasonIexpectedthisscorewasbecause: Iactuallyscored. MyactualscorewasEQUAL/HIGHER/LOWERthanwhatIexpectedbecause: Howdoyoufeelaboutthequiznowthatyouhavehadachancetoreflect?

10 ! DAY 3 - Wednesday Kickoff: Pencils down! Wait for Mad Minute Mad Minute The Law of of Mass states that in a chemical reaction mass of the is always to the mass of the. Matter is neither created nor destroyed, it only changes in. Grade and graph your Mad Minute!!!

11 Chemical Equations Name: Learning Objectives Distinguish among elements, compounds, and molecules. Determine how a chemical reaction satisfies the law of conservation of mass Write a balanced chemical equation. Identify common chemical reactions. Vocabulary Law of conservation of mass reactants products diatomic molecule coefficient Conservation of Mass Chemical equations show that in chemical reactions, atoms, but no atoms are or. The law of of states that the total mass a chemical reaction is to the total mass the reaction. Writing a Chemical Equation are the starting materials in a chemical reaction and are placed on the. are the materials in a chemical reaction and are placed on the. Elements, Compounds, and Molecules Instead of writing long word equations, scientists use and. Symbols represent. Formulas represent. Molecules may be or. Some elements are, that is, they contain atoms. Molecules may also contain two elements, such as hydrogen and oxygen in a water molecule. Balancing a Chemical Equation Atoms are neither nor in a reaction, so both sides of the equation must have the of. Counting Atoms A tells how many of an element are in one molecule. A tells how many,, or units are in a reaction. Using Parentheses with Formulas When counting atoms inside, the subscript all atoms inside. Summary:

12 ! Questions /Examples/ Workspace: Guided Practice CCM Chapter 8; Lesson 2 Independent Practice CCM Chapter 8; Lesson 2 Independent Practice Questions Exit Ticket!!

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15 ! DAY 4 - Thursday Kickoff: Pencils down! Wait for Mad Minute Mad Minute 1. What are the reactants? 2. What are the products? 3. How many carbon atoms are on the reactant side? 4. How many carbon atoms are on the product side? 5. This reaction produces how many water molecules? Grade and graph your Mad Minute!!!

16 NAME: BLOCK: DATE: CHEMISTRY: COUNTING ATOMS IN COMPOUNDS WORKSHEET #7.0.1 INSTRUCTIONS: Write the quantity of atoms of each element opposite the formula of the compound for the quantity of formula units and molecules shown: For example: 5P 2 O 3 P = (5 2 = ) 10 O = (5 3 = ) 15 For example: 4Zn(NO 3 ) 2 Zn = (4 1 = ) 4 N = (4 1 2= ) 8 O = (4 3 2 = ) K 2 CO 3 K = C = O = 2. 2Sr 3 (PO 4 ) 2 Sr = P = O = 3. 3N 4 O 10 N = O = 4. 2(NH 4 ) 3 N N = H = 5. 8Cl 2 O Cl = O = 6. Ca(C 2 H 3 O 2 ) 2 Ca = C = H = O = 7. 12NaBr Na = Br = 8. 4Al(OH) 3 Al = O = H = 9. 3NaHCO 3 Na = H = C = O = 10. 5Ga 2 (Cr 2 O 7 ) 3 Ga = Cr = O = 11. 7C 2 S 2 C = S = 12. 4Fe 2 O 3 Fe = O = 13. 6Ba(MnO 4 ) 2 Ba = Mn = O = 14. 3V 2 O 5 V = O = 15. 2KNO 3 K = N = O = 16. 9MgSO 4 Mg = S = O = 17. 5Al 2 (SiO 3 ) 2 Al = Si = O = 18. 4Au(IO 3 ) 3 Au = I = O = (Continued)

17 Balancing Chemical Equations Worksheet 1. H 2 + O 2 H 2 O 2. N 2 + H 2 NH 3 3. S 8 + O 2 SO 3 4. N 2 + O 2 N 2 O 5. HgO Hg + O 2 6. CO 2 + H 2 O C 6 H 12 O 6 + O 2 7. Zn + HCl ZnCl 2 + H 2 8. SiCl 4 + H 2 O H 4 SiO 4 + HCl 9. Na + H 2 O NaOH + H H 3 PO 4 H 4 P 2 O 7 + H 2 O 11. C 10 H 16 + Cl 2 C + HCl 12. CO 2 + NH 3 OC(NH 2 ) 2 + H 2 O 13. Si 2 H 3 + O 2 SiO 2 + H 2 O Al(OH) 3 + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 O 15. Fe + O 2 Fe 2 O Fe 2 (SO 4 ) 3 + KOH K 2 SO 4 + Fe(OH) C 7 H 6 O 2 + O 2 CO 2 + H 2 O 18. H 2 SO 4 + HI H 2 S + I 2 + H 2 O 19. FeS 2 + O 2 Fe 2 O 3 + SO Al + FeO Al 2 O 3 + Fe 21. Fe 2 O 3 + H 2 Fe + H 2 O 22. Na 2 CO 3 + HCl NaCl + H 2 O + CO K + Br 2 KBr 24. C 7 H 16 + O 2 CO 2 + H 2 O 25. P 4 + O 2 P 2 O 5

18 ! Questions /Examples/ Workspace: Guided & Independent Practice Balancing Equations Exit Ticket H2O + CO2! C6H12O6 + O2 When the equation above is balanced how many water (H 2O) molecules are present on the reactant side and how many oxygen molecules are present on the product side?

19 ! DAY 5 - Friday Kickoff &Mad Minute Review Kickoff and Mad Minutes for the week. They must be CORRECT for you to get full credit when your journals are checked. Guided Practice & Independent Practice Review/Reteach Work on unfinished work. ASK QUESTIONS ALL ANSWERS MUST BE CORRECT FOR THINGS WE ADDRESS DIRECTLY IN CLASS. Weekend Checklist What do you need to complete? What are you having trouble with that needs extra attention? WORK HARD! NO EXCUSES! COME IN ON MONDAY WITH QUESTIONS AND ANSWERS!

20 ! Independent Practice Questions Chapter 8; Lesson 1!

21 ! Chapter 8; Lesson 2!

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24 - 2 - INSTRUCTIONS: Write the quantity of atoms of each element opposite the formula of the compound for the quantity of formula units and molecules shown: For example: 5P 2 O 3 P = (5 2 = ) 10 O = (5 3 = ) 15 For example: 4Zn(NO 3 ) 2 Zn = (4 1 = ) 4 N = (4 1 2= ) 8 O = (4 3 2 = ) SnCl 4 Sn = Cl = 20. 6Cu 2 SeO 4 Cu = Se = O = 21. 3AsBr 3 As = Br = 22. 2H 2 SO 4 H = S = O = 23. SBr 2 S = Br = 24. 4Ca(OH) 2 Ca = O = H = 25. 5Mg 3 (PO 4 ) 2 Mg = P = O = H 2 O H = O = 27. 5N 2 O 4 N = O = 28. 3ClF Cl = F = 29. 7P 2 O 5 P = O = 30. 2KrCl 6 Kr = Cl = 31. 5Al(C 2 H 3 O 2 ) 2 Al = C = H = O = 32. 3(NH 4 ) 2 Cr 2 O 7 N = H = Cr = O = 33. 5Fe 3 (PO 4 ) 2 Fe = P = O = 34. 2NH 4 NO 3 N = H = O = 35. 5BaC 4 H 4 O 6 Ba = C = H = O = 36. 4Cu(HSO 3 ) 2 Cu = H = S = O = 37. 9Au(NO 2 ) 2 Au = N = O = 38. 3K 2 ZnO 2 K = Zn = O = 39. 3Sr(MnO 4 ) 2 Sr = Mn = O = 40. 4Al 2 (CO 3 ) 3 Al = C = O =

25 26. Dicarbon dihydride + Oxygen Carbon dioxide + Water 27. Potassium oxide + Water Potassium hydroxide 28. Hydrogen peroxide Water + Oxygen 29. Aluminum + Oxygen Aluminum oxide 30. Sodium peroxide + Water Sodium hydroxide + oxygen 31. Silicon dioxide + Hydrogen fluoride Silicon tetrafluoride + Water 32. Carbon + water Carbon monoxide + Hydrogen 33. Potassium chlorate Potassium chloride + Oxygen 34. Potassium chlorate Potassium perchlorate + Potassium chloride 35. Aluminum sulfate + Calcium hydroxide Aluminum hydroxide + Calcium sulfate 36. Tetraphosphorus decoxide + Water Hydrogen phosphate 37. Iron III chloride + Ammonium hydroxide Iron III hydroxide + Ammonium chloride 38. Antimony + Oxygen Tetrantimony Hexoxide 39. Tricarbon octahydride + Oxygen Carbon dioxide + water 40. Dinitrogen pentoxide + Water Hydrogen nitrate 41. Nitrogen trihydride + Nitrogen monoxide Nitrogen + Water 42. Aluminum + Hydrogen chloride Aluminum chloride + Hydrogen 43. Phosphorus pentachloride + water Hydrogen chloride + Hydrogen phosphate 44. Magnesium + Nitrogen Magnesium nitride 45. Iron + Water Iron III oxide + Hydrogen 46. Sodium hydroxide + Chlorine Sodium chloride + Sodium hypochlorite + water 47. Lithium oxide + Water Lithium hydroxide 48. Ammonium nitrate Dinitrogen monoxide + water 49. Lead II nitrate Lead II oxide + Nitrogen dioxide + Oxygen 50. Calcium chlorate Calcium chloride + Oxygen