1. BRN 5H 2 1.What number represents the coefficient? 2.What number represents the subscript? 3.What element is represented by the letter “H”? 4.How many “H’s” do you have? 5H 2 1.What number represents the coefficient? 2.What number represents the subscript? 3.What element is represented by the letter “H”? 4.How many “H’s” do you have?

2. BRN KNO 3 (s) → KNO 2 (aq) + O 2 (g) 1.What compound(s) are the reactants? 2.What compound(s) are the products? 3.What compound is found in the gas state? KNO 3 (s) → KNO 2 (aq) + O 2 (g) 1.What compound(s) are the reactants? 2.What compound(s) are the products? 3.What compound is found in the gas state?

3. Chemical Reactions Notes New section in table of contents

4. Conservation of Mass  Key Concept 1: The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.  KC 2: The mass of the reactants equals the mass of the products. mass reactants = mass products  Key Concept 1: The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.  KC 2: The mass of the reactants equals the mass of the products. mass reactants = mass products

5. Chemical Reactions  KC 3: The process by which one or more substances are rearranged to form different substances is called a chemical reaction  What are some examples of evidence of a chemical reaction?  KC 3: The process by which one or more substances are rearranged to form different substances is called a chemical reaction  What are some examples of evidence of a chemical reaction?

6. Representing Chemical Reactions  Reactants are the starting substances.  Products are the substances formed in the reaction.  This table summarizes the symbols used in chemical equations.  Reactants are the starting substances.  Products are the substances formed in the reaction.  This table summarizes the symbols used in chemical equations.

7. Representing Chemical Reactions  Key Concept 4: A chemical equation is a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction.

9. Balancing Chemical Reactions  KC 5: Subscripts describe the number of atoms present in one molecule (if it is a molecular compound) or in one formula unit (if it is an ionic compound). N 2 (g) + H 2 (g) -------> NH 3 (g)  KC 6: Coefficients are generally used for balancing the chemical equations in accordance with the law of conservation of mass. N 2 (g) + 3 H 2 (g) -------> 2 NH 3 (g)  KC 5: Subscripts describe the number of atoms present in one molecule (if it is a molecular compound) or in one formula unit (if it is an ionic compound). N 2 (g) + H 2 (g) -------> NH 3 (g)  KC 6: Coefficients are generally used for balancing the chemical equations in accordance with the law of conservation of mass. N 2 (g) + 3 H 2 (g) -------> 2 NH 3 (g)

10. Balancing Chemical Reactions  Balancing reactions is like a puzzle, you need to make sure both sides of the equation are equal  Helpful Hints:  Start with either polyatomic ions or carbon containing molecules  Never start with balancing oxygen  Write water as HOH (can be easier to see if OH is present on both sides)  Balancing reactions is like a puzzle, you need to make sure both sides of the equation are equal  Helpful Hints:  Start with either polyatomic ions or carbon containing molecules  Never start with balancing oxygen  Write water as HOH (can be easier to see if OH is present on both sides)

11. Balancing Chemical Reactions  KC 7: H 2 + O 2 → H 2 O

12. Balancing Chemical Reactions  KC 8: Fe + H 2 O → H 2 + Fe 2 O 3

13. Balancing Chemical Reactions  KC 9: Dinitrogen pentoxide gas forms nitrogen gas and oxygen gas.

15. Types of Chemical Reactions  KC 10: There are 4 types of chemical reactions  Synthesis  Combustion  Decomposition  replacement  KC 10: There are 4 types of chemical reactions  Synthesis  Combustion  Decomposition  replacement

16. Don’t forget…  Some molecules are more stable when they are found as diatomic – two of the same element covalently bonded BrINClHOF

17. Bonding

18. Evidence of a Chemical Reaction  KC 11: There are 3 driving forces that are evidence of a chemical reaction:  Evolution of a gas  Production of heat  Production of a solid or pure liquid (water)  KC 11: There are 3 driving forces that are evidence of a chemical reaction:  Evolution of a gas  Production of heat  Production of a solid or pure liquid (water)

19. Types of Chemical Reactions  KC 12: Synthesis – reaction in which 2 or more simpler substances (elements) react to produce a single product (compound)  General Reaction : A + B → AB  KC 12: Synthesis – reaction in which 2 or more simpler substances (elements) react to produce a single product (compound)  General Reaction : A + B → AB  synthesis synthesis  synthesis synthesis

20. Types of Chemical Reactions  KC 13: Combustion – reaction where oxygen combines with a substance (normally contains carbon) and releases energy in the form of heat and light  General Reaction: C x H y +O 2 → H 2 O + CO 2  demo demo  KC 13: Combustion – reaction where oxygen combines with a substance (normally contains carbon) and releases energy in the form of heat and light  General Reaction: C x H y +O 2 → H 2 O + CO 2  demo demo

21. Types of Chemical Reactions  KC 14: Decomposition – Reaction in which a single compound breaks down into 2 or more elements or new compounds  General Reaction: AB → A + B  demo - 3:00 demo - 3:00  KC 14: Decomposition – Reaction in which a single compound breaks down into 2 or more elements or new compounds  General Reaction: AB → A + B  demo - 3:00 demo - 3:00

22. Types of Chemical Reactions 1.__________NH 3 + ___H 2 SO 4  ___(NH 4 ) 2 SO 4 2._________C 5 H 9 O + ___O 2  ___CO 2 + _H 2 O 3.__________H 2 + ___O 2  ___H 2 O 4.__________NH 4 OH  ___NH 3 + ___H 2 O 5.__________CO + ___O 2  ___CO 2 1.__________NH 3 + ___H 2 SO 4  ___(NH 4 ) 2 SO 4 2._________C 5 H 9 O + ___O 2  ___CO 2 + _H 2 O 3.__________H 2 + ___O 2  ___H 2 O 4.__________NH 4 OH  ___NH 3 + ___H 2 O 5.__________CO + ___O 2  ___CO 2 KC 15: Correctly identify and balanceeach type of rxn S = synthesis D = decomposition C = combustion

23. Closure – Exit Pass 1.This type of reaction always forms products of carbon dioxide and water a.Synthesis b.Decomposition c.Combustion 2.What type of reaction has the general format AB → A + B a.Synthesis b.Decomposition c.Combustion 1.This type of reaction always forms products of carbon dioxide and water a.Synthesis b.Decomposition c.Combustion 2.What type of reaction has the general format AB → A + B a.Synthesis b.Decomposition c.Combustion

25. Types of Chemical Reactions  KC 16: Single Replacement – Reaction in which the atoms of one element replace the atoms of another element in a compound  General Reaction: A + BX → AX + B  Other Information: A metal will not always replace a metal in a compound dissolved in water because of differing reactivities  KC 16: Single Replacement – Reaction in which the atoms of one element replace the atoms of another element in a compound  General Reaction: A + BX → AX + B  Other Information: A metal will not always replace a metal in a compound dissolved in water because of differing reactivities

26. Single Replacement Reactions  Elements will not always replace each other in a single replacement reaction  The activity series tells us if the replacement will occur  Elements replace lower elements in the chart, but not the other way around  Elements will not always replace each other in a single replacement reaction  The activity series tells us if the replacement will occur  Elements replace lower elements in the chart, but not the other way around

27. Single Replacement  Zn(II) (s) + AgNO 3 (aq) →  Cl 2 (g) + HBr(aq) →  Na(s) + CaO(aq) →  Zn(II) (s) + AgNO 3 (aq) →  Cl 2 (g) + HBr(aq) →  Na(s) + CaO(aq) →

29. Fe(III) + PbSO 4 → 1.See if the reaction will occur using reactivity series 2.Identify the charges of the elements 3.Do single replacement to predict the products (*same charges switch)) 4.Balance the reaction using coefficients

30. Single Replacement Practice  I 2 + HCl 2 →  Zn(II) + Cu 2 SO 4 →  AlCl 3 + Mg →  Cu(I) + Ag 2 SO 4 →  LiNO 3 + Ag →  Fe(II) + PbSO 4 →  I 2 + HCl 2 →  Zn(II) + Cu 2 SO 4 →  AlCl 3 + Mg →  Cu(I) + Ag 2 SO 4 →  LiNO 3 + Ag →  Fe(II) + PbSO 4 →

31. Types of Chemical Reactions  KC 17: Double Replacement – reaction in which the ions exchange between 2 compounds. All double replacement reactions produce either water, a precipitate, or a gas  General Reaction: AX + BY → AY + BX  KC 17: Double Replacement – reaction in which the ions exchange between 2 compounds. All double replacement reactions produce either water, a precipitate, or a gas  General Reaction: AX + BY → AY + BX

32. Types of Chemical Reactions  KC 18: The solid produced during a chemical reaction is called a precipitate.  Precipitation comes from the clouds – “precipitates out”  KC 18: The solid produced during a chemical reaction is called a precipitate.  Precipitation comes from the clouds – “precipitates out”

34. KC 19: Write a balanced chemical equation for each double-replacement reactions BaCl 2 (aq) + K 2 CO 3 (aq) (a precipitate of barium carbonate is formed) FeS (s) + HCl (aq)(Hydrogen sulfide gas is formed) Writing Reactions

35. BaCl 2 (aq) + K 2 CO 3 (aq)

36. FeS (s) + HCl (aq)

37. Predicting Reactions Practice 1.Barium chloride + sodium sulfate → precipitate of barium sulfate is formed

38. Predicting Practice  Silver (I) nitrate + calcium sulfide → precipitate of silver sulfide is formed

39. Practice  Potassium carbonate + hydrochloric acid (HCl) → a precipitate of hydrogen carbonate is formed

40. Practice  Sodium sulfate + barium nitrate → a precipitate of barium sulfate is formed

42. Solubility  KC 20: Solubility is the maximum quantity of a substance that may be dissolved in another  Solubility…  Depends on temperature  Of most solids increases as temperature increases  Of gases decreases as temperature increases  KC 20: Solubility is the maximum quantity of a substance that may be dissolved in another  Solubility…  Depends on temperature  Of most solids increases as temperature increases  Of gases decreases as temperature increases

44. White Solid Water + universal indicator Water (at room temperature) HClMethanolIodine Temp of solubility in water Baking Soda Green Slightly soluble Produces gas Insoluble --------- - 50 C Sugar Yellow- orange Soluble----------Insoluble Turns blue 20 C Benzoic Acid PinkInsoluble----------Soluble --------- - 100 C FlourOrangeInsoluble----------Insoluble Turns blue insoluble Sodium Chloride Orangesoluble---------- Slightly soluble --------- - 20 C

45. Soluble and Insoluble Salts KC 21: Ionic compounds that  dissolve in water are soluble salts  do not dissolve in water are insoluble salts KC 21: Ionic compounds that  dissolve in water are soluble salts  do not dissolve in water are insoluble salts

47. Using Solubility Rules  Ba(NO 3 ) 2 (aq) + Li 2 SO 4 (aq) →  What does this actually look like?  Ba(NO 3 ) 2 (aq) + Li 2 SO 4 (aq) →  What does this actually look like?

48. Equations for Forming Solids A full equation shows the formulas of the compounds. Pb(NO 3 ) 2 (aq) + 2NaCl(aq) PbCl 2 (s) + 2NaNO 3 (aq) An ionic equation shows the ions of the compounds. Pb 2+ ( aq ) + 2NO 3 − (aq) + 2Na + (aq) + 2Cl − ( aq ) PbCl 2 ( s ) + 2Na + (aq) + 2NO 3 − (aq) A full equation shows the formulas of the compounds. Pb(NO 3 ) 2 (aq) + 2NaCl(aq) PbCl 2 (s) + 2NaNO 3 (aq) An ionic equation shows the ions of the compounds. Pb 2+ ( aq ) + 2NO 3 − (aq) + 2Na + (aq) + 2Cl − ( aq ) PbCl 2 ( s ) + 2Na + (aq) + 2NO 3 − (aq)

49. Equations for Forming Solids  Key Concept 22: A net ionic equation shows only the ions that form a solid or water or gas. Pb 2+ (aq) + 2Cl − (aq) → PbCl 2 (s)  The ions that do not form the solid are called spectator ions 2NO 3 − (aq) + 2Na + (aq) → 2Na + (aq) + 2NO 3 − (aq)  Key Concept 22: A net ionic equation shows only the ions that form a solid or water or gas. Pb 2+ (aq) + 2Cl − (aq) → PbCl 2 (s)  The ions that do not form the solid are called spectator ions 2NO 3 − (aq) + 2Na + (aq) → 2Na + (aq) + 2NO 3 − (aq) Pb 2+ (aq) + 2NO 3 − (aq) + 2Na + (aq) + 2Cl − (aq) → PbCl 2 (s) + 2Na + (aq) + 2NO 3 − (aq)

50. Predicting Reactions  KC 23: Write the full and net ionic equation for the following reaction – calcium carbonate + potassium phosphate

51. Predicting Reactions  KC 24: Write the full and net ionic equation for the reaction when calcium chloride reacts with cobalt (II) sulfate

52. Predicting Reactions  KC 25: Write the full and net ionic equation when lithium sulfide reacts with calcium nitrate

53. Summary  video video  video video

54. Closure – Exit Pass 1.What is not always an indication that a chemical reaction has occurred? a.Evolution of a gas b.Production of water c.Color change d.Production of heat 2.What is the reaction type that follows this general pattern – AX + BY → AY + BX a.Single replacement b.Double replacement 1.What is not always an indication that a chemical reaction has occurred? a.Evolution of a gas b.Production of water c.Color change d.Production of heat 2.What is the reaction type that follows this general pattern – AX + BY → AY + BX a.Single replacement b.Double replacement