Student Journal - Week 17apwscience8.weebly.com/.../1/3/2/9/13294342/student_journal_-_week_17.pdf · STUDENT JOURNAL – Week 17 – Chemical Reactions Overarching Goal for the Week:

!

http://apwscience8.weebly.com

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

!


My Mad Minute Graph

What's Your Average?

Day 1 ___ Day 2 ----- Day 3 ___ + Day 4 ___

Total ___/ 3 = ____

Day #5 Mad Minute: Question #1 - Are you satisfied with your overall average for this week? Why or why not? !

!


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 boil ing _________

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!!!

Learning Objectives

Define chemical change

Distinguish between physical and chemical

change

Identify examples of chemical and physical

change

Vocabulary

Chemical Property

Chemical Change

Dissolving !

Summary:

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.

Chemical Properties and Changes Name: _____________________

!


Questions /Examples/ Workspace: Guided Practice • CCM – Chapter 8; Lesson 1

Independent Practice • CCM – Chapter 8; Lesson 1 • Independent Practice Questions

Exit Ticket

!


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

__________________________________"QUIZ/TEST"REFLECTION"

"I"expected"to"score"______________________________________"(proficiency"level)"on"the"quiz/test.""The"reason"I"expected"this"score"was"because:""___________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________""I"actually"scored"____________________________________________.""My"actual"score"was"EQUAL/HIGHER/LOWER"than"what"I"expected"because:"""""""""How"do"you"feel"about"the"quiz"now"that"you"have"had"a"chance"to"reflect?"

"

!


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 __________.


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

!

Summary:

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.

Chemical Equations Name: ________________________

!


Questions /Examples/ Workspace: Guided Practice • CCM – Chapter 8; Lesson 2

Independent Practice • CCM – Chapter 8; Lesson 2 • Independent Practice Questions

Exit Ticket !

!

!


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?


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: 5P2O3 P = (5 + 2 = ) 10 O = (5 + 3 = ) 15 For example: 4Zn(NO3)2 Zn = (4 + 1 = ) 4 N = (4 + 1 + 2= ) 8 O = (4 + 3 + 2 = ) 24 1. 4K2CO3 K = _____ C = ____ O = ____ 2. 2Sr3(PO4)2 Sr = ____ P = ____ O = ____ 3. 3N4O10 N = _____ O = ____ 4. 2(NH4)3N N = ____ H = ____ 5. 8Cl2O Cl = ____ O = ____ 6. Ca(C2H3O2)2 Ca = ____ C = ____ H = ____ O = _____ 7. 12NaBr Na = ____ Br = ____ 8. 4Al(OH)3 Al = ____ O = ____ H = ____ 9. 3NaHCO3 Na = ____ H = ____ C = ____ O = ____ 10. 5Ga2(Cr2O7)3 Ga = ____ Cr = ____ O = ____ 11. 7C2S2 C = _____ S = _____ 12. 4Fe2O3 Fe = ____ O = _____ 13. 6Ba(MnO4)2 Ba = _____ Mn = _____ O = ______ 14. 3V2O5 V = _____ O = _____ 15. 2KNO3 K = _____ N = _____ O = ______ 16. 9MgSO4 Mg = ____ S = _____ O = ______ 17. 5Al2(SiO3)2 Al = ____ Si = _____ O = ______ 18. 4Au(IO3)3 Au = ____ I = ______ O = ______ (Continued)

Balancing Chemical Equations Worksheet

1. _____ H2 + _____ O2 Æ _____ H2O

2. _____ N2 +_____ H2 Æ_____ NH3

3. _____ S8 + _____ O2 Æ _____ SO3

4. _____ N2 + _____ O2 Æ _____ N2O

5. _____ HgO Æ _____ Hg + _____ O2

6. _____ CO2 + _____ H2O Æ _____ C6H12O6 + _____ O2

7. _____ Zn + _____ HCl Æ _____ ZnCl2 + _____ H2

8. _____ SiCl4 + _____ H2O Æ _____ H4SiO4 + _____ HCl

9. _____ Na + _____ H2O Æ _____ NaOH + _____ H2

10. _____ H3PO4 Æ _____ H4P2O7 + _____ H2O

11. _____ C10H16 + _____ Cl2 Æ _____ C + _____ HCl

12. _____ CO2 + _____ NH3 Æ _____ OC(NH2)2 + _____ H2O

13. _____ Si2H3 + _____ O2 Æ _____ SiO2 + _____ H2O3

14. _____ Al(OH)3 + _____ H2SO4 Æ _____ Al2(SO4)3 + _____ H2O

15. _____ Fe + _____ O2 Æ _____ Fe2O3

16. _____ Fe2(SO4)3 + _____ KOH Æ _____ K2SO4 + _____ Fe(OH)3

17. _____ C7H6O2 + _____ O2 Æ _____ CO2 + _____ H2O

18. _____ H2SO4 + _____ HI Æ _____ H2S + _____ I2 + _____ H2O

19. _____ FeS2 + _____ O2 Æ _____ Fe2O3 + _____ SO2

20. _____ Al + _____ FeO Æ _____ Al2O3 + _____ Fe

21. _____ Fe2O3 + _____ H2 Æ _____ Fe + _____ H2O

22. _____ Na2CO3 + _____ HCl Æ _____ NaCl + _____ H2O + _____ CO2

23. _____ K + _____ Br2 Æ _____ KBr

24. _____ C7H16 + _____ O2 Æ _____ CO2 + _____ H2O

25. _____ P4 + _____ O2 Æ _____ P2O5

!


Questions /Examples/ Workspace: Guided & Independent Practice • Balancing Equations

Exit Ticket

H2O + CO2 ! C6H12O6 + O2

When the equation above is balanced how many water (H2O) molecules are present on the reactant side and how many oxygen molecules are present on the product side?

!


DAY 5 - Friday Kickoff &Mad Minute Review Kickoff and Mad Minutes for the week. They must be CORRECT for you to get ful l 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!

!


Independent Practice Questions

Chapter 8; Lesson 1

!

!


Chapter 8; Lesson 2

!

- 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: 5P2O3 P = (5 + 2 = ) 10 O = (5 + 3 = ) 15 For example: 4Zn(NO3)2 Zn = (4 + 1 = ) 4 N = (4 + 1 + 2= ) 8 O = (4 + 3 + 2 = ) 24 19. 8SnCl4 Sn = ____ Cl = _____ 20. 6Cu2SeO4 Cu = ____ Se = _____ O = ______ 21. 3AsBr3 As = _____ Br = _____ 22. 2H2SO4 H = _____ S = _____ O = _____ 23. SBr2 S = _____ Br = _____ 24. 4Ca(OH)2 Ca = _____ O = _____ H = _____ 25. 5Mg3(PO4)2 Mg = _____ P = _____ O = _____ 26. 12H 2O H = _____ O = _____ 27. 5N2O4 N = _____ O = _____ 28. 3ClF Cl = _____ F = _____ 29. 7P2O5 P = _____ O = _____ 30. 2KrCl6 Kr = _____ Cl = _____ 31. 5Al(C2H3O2)2 Al = _____ C = _____ H = _____ O = _____ 32. 3(NH4)2Cr2O7 N = _____ H = _____ Cr = _____ O = _____ 33. 5Fe3(PO4)2 Fe = _____ P = _____ O = _____ 34. 2NH4NO3 N = _____ H = _____ O = _____ 35. 5BaC4H4O6 Ba = _____ C = _____ H = _____ O = _____ 36. 4Cu(HSO3)2 Cu = ______ H = _____ S = _____ O = _____ 37. 9Au(NO2)2 Au = _____ N = _____ O = _____ 38. 3K2ZnO2 K = _____ Zn = _____ O = ______ 39. 3Sr(MnO4)2 Sr = _____ Mn = _____ O = _____ 40. 4Al2(CO3)3 Al = _____ C = _____ O = _____

26. Dicarbon dihydride + Oxygen Æ Carbon dioxide + Water

27. Potassium oxide + Water Æ Potassium hydroxide

28. Hydrogen peroxide Æ Water + Oxygen

29. Aluminum + Oxygen Æ Aluminum oxide

30. Sodium peroxide + Water Æ Sodium hydroxide + oxygen

31. Silicon dioxide + Hydrogen fluoride Æ Silicon tetrafluoride + Water

32. Carbon + water Æ Carbon monoxide + Hydrogen

33. Potassium chlorate Æ Potassium chloride + Oxygen

34. Potassium chlorate Æ Potassium perchlorate + Potassium chloride

35. Aluminum sulfate + Calcium hydroxide Æ Aluminum hydroxide + Calcium sulfate

36. Tetraphosphorus decoxide + Water Æ Hydrogen phosphate

37. Iron III chloride + Ammonium hydroxide Æ Iron III hydroxide + Ammonium chloride

38. Antimony + Oxygen Æ Tetrantimony Hexoxide

39. Tricarbon octahydride + Oxygen Æ Carbon dioxide + water

40. Dinitrogen pentoxide + Water Æ Hydrogen nitrate

41. Nitrogen trihydride + Nitrogen monoxide Æ Nitrogen + Water

42. Aluminum + Hydrogen chloride Æ Aluminum chloride + Hydrogen

43. Phosphorus pentachloride + water Æ Hydrogen chloride + Hydrogen phosphate

44. Magnesium + Nitrogen Æ Magnesium nitride

45. Iron + Water Æ Iron III oxide + Hydrogen

46. Sodium hydroxide + Chlorine Æ Sodium chloride + Sodium hypochlorite + water

47. Lithium oxide + Water Æ Lithium hydroxide

48. Ammonium nitrate Æ Dinitrogen monoxide + water

49. Lead II nitrate Æ Lead II oxide + Nitrogen dioxide + Oxygen

50. Calcium chlorate Æ Calcium chloride + Oxygen

Student Journal - Week 17apwscience8.weebly.com/.../1/3/2/9/13294342/student_journal_-_week_17.pdf · STUDENT JOURNAL – Week 17 – Chemical Reactions Overarching Goal for the Week:

Documents