1 3 Compounds Page 61 Science 10/Kennedy/2016

2 Introduction Page 61 Millions of different chemical compounds exist as a result of different combination of elements. A systematic way of naming these compounds has been developed by the International Union of Pure and Applied Chemistry (IUPAC). Science 10/Kennedy/2016

3 International Union of Pure and Applied ChemistryPage 61 International Union of Pure and Applied Chemistry IUPAC International Union of Pure and Applied Chemistry Science 10/Kennedy/2016

4 Introduction Page 61 Millions of different chemical compounds exist as a result of different combination of elements. A systematic way of naming these compounds has been developed by the International Union of Pure and Applied Chemistry (IUPAC). Compounds contain more than one kind of element chemically bonded together. Alloys: metal-metal Science 10/Kennedy/2016

5 Alloys Alloys are combinations of metals: e.g., steelAlloys have properties such as higher melting point, hardness. Gold is a very soft metal; too soft to use as jewelry in its pure form. It is combined with copper and silver to make it harder. The purity of gold is given in units of karats: Pure gold 24 k 25% copper 18 k Science 10/Kennedy/2016

6 Introduction Page 61 Millions of different chemical compounds exist as a result of different combination of elements. A systematic way of naming these compounds has been developed by the International Union of Pure and Applied Chemistry (IUPAC). Compounds contain more than one kind of element chemically bonded together. Alloys: metal-metal Ionic: metal-nonmetal Molecular: nonmetal-nonmetal Science 10/Kennedy/2016

7 Atoms are bonded together using valence electrons.Page 61 Atoms are bonded together using valence electrons. Science 10/Kennedy/2016

8 Page 61 Compounds form when two or more atoms bond together. Bonds occur when valence electrons between two atoms form a pair. Electrons can form a pair by transferring sharing Ionic compounds Molecular compounds Science 10/Kennedy/2016

9 3.1 Binary Ionic CompoundsPage 61  Notes: Ionic compounds combine a metal with a nonmetal. Binary ionic compounds contain one type of metal ion and one type of non-metal ion. metal-nonmetal Properties: empirical Solids at SATP Conduct electricity if dissolves in water Theoretical: A metal atom losses an electron to a nonmetal atom. Thus positive and negative ion are produced. This forms a network of ions where the overall charge is balanced. Science 10/Kennedy/2016

10 All the ions are interconnected with each otherTheoretical: Page 61 A metal atom losses an electron to a nonmetal atom. Thus positive and negative ion are produced. This forms a network of ions where the overall charge is balanced. + _ All the ions are interconnected with each other Single units of ionic compounds do not exist by themselves Science 10/Kennedy/2016

11 Page 62 Nomenclature Science 10/Kennedy/2016

12 An analogy between words and compounds:Nomenclature Page 62 An analogy between words and compounds: The elements of the periodic table are like letters of the alphabet. The elements are put together to form compounds like letters are put together to form words. There are scientific rules for putting elements together just as there are spelling rules for putting letters together. There are rules for how compounds may react just as there are grammatical rules for how words interact Science 10/Kennedy/2016

13 e.g., sodium chloride Page 62 Nomenclature Notes: Cation name/space/anion name e.g., sodium chloride Science 10/Kennedy/2016

14 NaCl MgCl2 SrBr2 sodium chloride magnesium chloride strontium bromidePage 63 Cation name/space/anion name 2. Name the following binary ionic substances. IUPAC Name Formula a. NaCl b. MgCl2 c. SrBr2 sodium chloride magnesium chloride strontium bromide p. 63 #1, 2 Do Science 10/Kennedy/2016

15 Always use the lowest possible numbersPage 63 Ionic substances All the atoms are interconnected with each other + _ 1:1 Ratio 2:1 Ratio Ca2+ Cl- e.g., NaCl Always use the lowest possible numbers Na2Cl2 CaCl2 Na4Cl4 Science 10/Kennedy/2016

16 NaBr Na2O K3N Mg3P2 Page 63 Cl- Ca2+ + CaCl2 Cl-Two to one ratio for neutral compound Needed to balance charge 3. Determine the formula for each of the following binary ionic substances. Name Formula a. sodium bromide b. sodium oxide c. potassium nitride f. magnesium phosphide Na+ Br- NaBr Na+ Na+ O2- Na2O K+ K+ K+ N3- K3N Mg2+ P3- Mg3P2 Science 10/Kennedy/2016

17 Mg2+ P3- Mg3P2 + Page 63 Superscripts are different than subscriptsSuperscripts – the charge on each ion Mg2+ P3- + Mg3P2 Subscripts – how many ions are in the compound p. 63 #3 Do Science 10/Kennedy/2016

18 Metal name(roman numeral)Page 62  Notes: Multivalent Ions metals Multivalent ions: Some atoms have the possibility of forming more than one type of ion charge. This will affect the properties and therefore the name of the substance. Only positive ions Fe2+ Iron(II) Fe3+ Iron(III) Metal name(roman numeral) Science 10/Kennedy/2016

19 The total charge must = zeroPage 63 The total charge must = zero 4. Determine the formula for each of the following binary ionic substances. Name Formula a. iron(II) bromide b. iron(III) bromide h. gold(I) oxide i. gold(III) oxide Fe2+ Br- FeBr2 Fe3+ Br- FeBr3 Au+ O2- Au2O Au3+ O2- Au2O3 p. 63 #4 Do Science 10/Kennedy/2016

20 Metal name(roman numeral) nonmetal namePage 63 Stock Nomenclature for multivalent ions Metal name(roman numeral) nonmetal name Space No space 5. Determine the name for each of the following binary ionic substances. Formula Name c. Nb2O3 d. Nb2O5 niobium(III) oxide niobium(V) oxide First consider negative charge on nonmetal ion Science 10/Kennedy/2016

21 Some elements may form differently charged ions.Page 62 Stock Nomenclature for Multivalent Ions Some elements may form differently charged ions. This will affect their formula and properties. Consider negative charge on nonmetal ion Determine the total negative charge The total positive charge is equal to the total negative charge Determine the charge on each positive ion p. 63 #5 Do Science 10/Kennedy/2016

22 Latin: Ferric and FerrousClassical Nomenclature Latin: Ferric and Ferrous Fe3+ Fe2+ Latin: cupric and cuprous Cu2+ Cu+ Science 10/Kennedy/2016

23 sulfate SO42- ammonium NH4+ Page 62 Polyatomic ions Notes: Polyatomic ions Groups of atoms may form an ion and form ionic bonds with other ions. sulfate SO42- ammonium NH4+ Science 10/Kennedy/2016

24 Page 274 Science 10/Kennedy/2016

25 Memorize Common Polyatomic Ionshydroxide OH- sulfate SO42- acetate CH3COO- nitrate NO3- phosphate PO43- ammonium NH4+ No Quiz Science 10/Kennedy/2016

26 Metal name(roman numeral) nonmetal namePage 64 Metal name(roman numeral) nonmetal name 6. Determine the name for each of the following polyatomic substances. Name Formula a. Na2CO3 b. NaNO2 g. Al(OH)3 i. Fe2(SO4)3 sodium carbonate sodium nitrite aluminium hydroxide iron(III) sulfate p. 64 #6 Do Science 10/Kennedy/2016

27 There are many more polyatomic ions than what are in our chartPage 64 7. Determine the formula for each of the following polyatomic substances. Name Formula a. sodium cyanide c. calcium hydroxide e. iron(II) carbonate f. iron(III) carbonate h. aluminium persulfide NaCN Ca(OH)2 FeCO3 Fe2(CO3)3 Al2(S2)3 There are many more polyatomic ions than what are in our chart e.g., persulfide S22- p. 64 #7 Do Science 10/Kennedy/2016

28 Does not dissolve (or very little)Page 62 Solubility aqueous Solubility is if a substance dissolves in water  Notes: dissolves A substance may be highly soluble or low soluble when placed into water Does not dissolve (or very little) ionic NaCl(s) Dissociates when it dissolves Separates into ions molecular Does not dissociates when it dissolves C12H22O11(s) Science 10/Kennedy/2016

29 Soluble – dissolves in water aqueousPage 62 Soluble – dissolves in water aqueous Breaks apart into ions as it dissolves dissociates Science 10/Kennedy/2016

30 All the ions are interconnected with each otherIonic substances + _ All the ions are interconnected with each other Molecular substances The atoms join to form molecules that are not connected with other molecules Science 10/Kennedy/2016

31 Dissociate – individual ions are formedIonic substances Molecular substances + - Sugar Salt Dissociate – individual ions are formed Science 10/Kennedy/2016

32 Both dissolve Ionic substances Molecular substances Salt solutionSugar solution - + + - - + - - + + + - Dissociate – individual ions are formed Science 10/Kennedy/2016

33 Compounds that include group I ions or NH4+ are generally solubleUsing Solubility Table Only works for ionic substances Page 274 aq s Science 10/Kennedy/2016

34 Use solubility table aq aq s Page 648. Use your solubility table to determine the solubility for each of the following. Formula Solubility (s or aq) a. Na2CO3 c FeSO4 f. Al(OH)3 aq aq s aq s p. 64 #8 Do Not all substances are in the solubility table Compounds that include group I ions are always soluble Science 10/Kennedy/2016

35 Use solubility table aq aq aq Page 6510. Use your solubility table to determine the solubility for each of the following. Name Solubility (s or aq) a. sodium carbonate b. ammonium carbonate f. Sodium hypochlorite aq aq aq p. 64 #8, 9 Do p. 65 # Do Science 10/Kennedy/2016

36 Ionic Nomenclature Quiz: Provide the name or formula for the followingIonic Nomenclature Quiz: Provide the name or formula for the following. (1 mark each) Science 10/Kennedy/2016

37 Ionic Nomenclature Quiz: Provide the name or formula for the followingIonic Nomenclature Quiz: Provide the name or formula for the following. (1 mark each) 0.5 marks off for each minor mistake Name Formula 1. magnesium bromide 2. nickel(II) hydroxide 3. sodium carbonate 4. gold(III) borate 5. ZnCl2 6. (NH4)2SO4 7. Fe(OH)3 8. V(Cr2O7)2 Ni(OH)2 MgBr2 Na2CO3 Au2(B03)3 zinc chloride ammonium sulfate iron(III) hydroxide vanadium(IV) dichromate 10 Name Solubility (s or aq) 9. Lithium carbonate 10. calcium hydroxide Use your solubility table to determine the solubility for each of the following. aq s Science 10/Kennedy/2016

38 3.2 Molecular Compounds Empricial Page 66 Notes: Molecular compounds are combinations of nonmetals Properties: Empricial They may be solid, liquid, or gas They do not conduct electricity if they dissolve in water Theoretical: Nonmetals may combine by sharing electrons Science 10/Kennedy/2016

39 All the ions are interconnected with each otherIonic substances + _ All the ions are interconnected with each other Molecular substances The atoms join to form molecules that are not connected with other molecules Science 10/Kennedy/2016

40 O H Molecular Compounds Page 66Atoms join to form individual molecules that are not connected with other molecules H O Science 10/Kennedy/2016

41 O H Ionic Substances Page 66All the atoms are interconnected with each other Molecular Substances The atoms join to form molecules that are not connected with other molecules H O Science 10/Kennedy/2016

42 H O C Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Science 10/Kennedy/2016

43 Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Science 10/Kennedy/2016

44 Nomenclature Ionic Compounds Metal, nonmetal Balance chargesMolecular Compounds Page 66 Nonmetal, nonmetal Use prefix system Science 10/Kennedy/2016

45 3.2 Molecular Compounds Ozone O3(g) Sulfur S8(s) Phosphorus P4(s)Page 66  Notes: Molecular compounds are combinations of nonmetals Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements: O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) Molecular elements contain only one type of atom: Monoatomic atoms can exist on their own e.g., Ar, Ni, Cr Science 10/Kennedy/2016

46 Memorize Some elements tend to come together as groups. Ozone O3(g)Page 66 Some elements tend to come together as groups. Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2(g) Memorize Science 10/Kennedy/2016

47 Paint solvent, gas line antifreeze, lantern fuel lighter fluid butane Compounds at Home Common Name Chemical Name Use muriatic acid hydrochloric acid Cleaning cement nail polish remover acetone Nail polish remover Wood alcohol methanol Paint solvent, gas line antifreeze, lantern fuel lighter fluid butane lighters propane BBQ fuel hydrogen peroxide Hydrogen peroxide H2O2 disinfectant for wounds (3 %) Hair bleach (6 %) Rocket fuel (> 70 %) Baking soda Sodium bicarbonate Cleaning, baking, putting out fires, absorbing odours vinegar Acetic acid Cooking, cleaning 99.98 % % Science 10/Kennedy/2016

48 Memorized Compounds Science 10/Kennedy/2016

49 Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Memorized Compounds Water H2O(l) or HOH(l) Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Ethanol C2H5OH(l) or CH3CH2OH(l) Methanol CH3OH(l) Ammonia NH3(g) Hydrogen sulfide H2S(g) Sucrose C12H22O11(s) Glucose C6H12O6(s) Science 10/Kennedy/2016

50 Compound Quiz: Provide the name or symbol for the following elementsCompound Quiz: Provide the name or symbol for the following elements. (1 mark each) Science 10/Kennedy/2016

51 10 CH4(g) C12H22O11(s) NH3(g) O3(g) CH3OH(l) Propane Ethanol HOHCompound Quiz: Provide the name or symbol for the following compounds. (1 mark each) CH4(g) C12H22O11(s) NH3(g) O3(g) CH3OH(l) Propane Ethanol HOH Glucose H2O2(l) Methane Sucrose Ammonia Ozone Methanol C3H8(g) C2H5OH(l) or CH3CH2OH(l) water C6H12O6(s) Hydrogen peroxide 10 Science 10/Kennedy/2016

52 3.2 Molecular Compounds Page 66 Notes: Molecular compounds are combinations of nonmetals Nomenclature: The number of atoms present must be indicated using a prefix Science 10/Kennedy/2016

53 The number of atoms in a molecule must be indicated using a prefix:Page 66 Nomenclature: The number of atoms in a molecule must be indicated using a prefix: 1 – mono 4 – tetra 7 – hepta 10 – deca 2 – di 5 – penta 8 – octa 3 – tri 6 – hexa 9 – nona The first element is usually the one more to the left on the periodic table. The second element gets an “ide” ending to its name The prefix “mono” only gets used on the second atom Science 10/Kennedy/2016

54 Double vowels that sound the same - drop the first one If there are two vowels in a row that sound the same once the prefix is added (they "conflict"), the extra vowel on the end of the prefix is removed. Page 67 3. Name each compound. IUPAC Name Formula c. N2O d. P2O5 Double vowels that sound the same - drop the first one dinitrogen monoxide diphosophorus pentoxide The “a” is dropped 2. Provide the formula for each molecular compound Name formula a. nitrogen dioxide b. dinitrogen dioxide NO2 N2O2 p. 67 #1 - 3 Do Science 10/Kennedy/2016

55 3.3 Acids & Bases H+ Page 68 Acids Properties (empirical) Notes: Acids Properties (empirical) Turns blue litmus paper red Acids are s, l or g as pure compounds at SATP but act as an acid only when dissolved in water Conducts electricity as an aqueous solution Sour tasting Theoretically, acids release a hydrogen ion while in solution H+ Science 10/Kennedy/2016

56 3.3 Acids & Bases Page 68 Bases Empirically Tastes bitter Notes: Bases Empirically Tastes bitter Feels slippery Turns red litmus paper blue Conducts electricity as an aqueous solution Theoretically Bases release a hydroxide ion (OH-) while in solution Science 10/Kennedy/2016

57 3.3 Acids & Bases OH- H+ Page 68The strength of an acid or base is measured on the pH scale. pH means power of the hydrogen OH- H+ Neutral Acidic Basic (alkaline) 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH may be measured using a pH meter or dyes that change colour such as as indicators of pH paper Science 10/Kennedy/2016

58 There are three ways of determining the name of an acid:Page 69 Acid Nomenclature: There are three ways of determining the name of an acid: i. Memorization ii. IUPAC System iii. Classical System Science 10/Kennedy/2016

59 i. Memorize Common Acids:Page 69 i. Memorize Common Acids: HCl(aq) H2SO4(aq) HNO3(aq) HF(aq) H3PO4(aq) Hydrogen ion combined with a non-metal CH3COOH(aq) Organic acids contain carbon and a COOH HCl(g)  HCl(aq) Acids will always be aqueous p. 70 #1, 2 Do Science 10/Kennedy/2016

60 ii. IUPAC System for AcidsPage 69 ii. IUPAC System for Acids Give ionic name Place “aqueous” in front 3. Name the hydrogen compound using the ionic system and then modify the name using the IUPAC system for acids. Ionic Name IUPAC Acid name Formula a. HNO2 hydrogen nitrite aqueous hydrogen nitrite p. 70 #3 Do Science 10/Kennedy/2016

61 iii. Classical Acid NomenclaturePage 69 iii. Classical Acid Nomenclature Name the hydrogen compound using the ionic system and then modify the name as shown in the chart below. Rule Ionic Name Acid Name 1. hydrogen ________ ide hydro ______ ic acid 2. hydrogen ________ ite ______ ous acid 3. hydrogen ________ ate ______ ic acid Acid names containing sulfur must add “ur” to the acid name. phosphorus must add “or” to the acid name. Science 10/Kennedy/2016

62 Page 247 Science 10/Kennedy/2016

63 Page 71 hydrogen thiosulfate thiosulfuric acid hydrogen sulfideRule Ionic Name Acid Name 1. hydrogen ________ ide hydro ______ ic acid 2. hydrogen ________ ite ______ ous acid 3. hydrogen ________ ate ______ ic acid Acid names containing sulfur must add “ur” to the acid name. phosphorus must add “or” to the acid name. 4. Complete the chart. Ionic Name Classical Acid Name Formula a. H2S2O3(aq) b. H2S(aq) c. chloric acid hydrogen thiosulfate thiosulfuric acid hydrogen sulfide hydrosulfuric acid hydrogen chlorate HClO3 p. 71 #4 Do Science 10/Kennedy/2016

64 H+ OH- neutral acidic basic 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Page 68The strength of an acid or base is measured using the pH scale pH = power of the hydrogen H+ OH- neutral acidic basic pH may be measured using: a pH meter dyes that change colour such as indicators or pH paper Science 10/Kennedy/2016

65 Nomenclature Quiz: Provide the name or formula for the followingNomenclature Quiz: Provide the name or formula for the following. (1 mark each) Name Formula 1. diphosophorus pentoxide 2. nickel(II) hydroxide 3. glucose 4. gold(III) tetraborate 5. N2O7 6. H2SO3(aq) Ni(OH)2 P2O5 C6H12O6 Au2(B4O7)3 dinitrogen heptaoxide sulfurous acid 6 aqueous hydrogen sulfite Science 10/Kennedy/2016

66 Nomenclature Quiz: Provide the name or formula for the followingNomenclature Quiz: Provide the name or formula for the following. (1 mark each) Name Formula 1. triphosophorus heptoxide 2. nickel(II) nitrite 3. sucrose 4. gold(III) thiosulfate 5. N2Cl7 6. H2SO3(aq) Ni(NO2)2 P3O7 C12H22O11 Au2(S2O3)3 dinitrogen heptachloride sulfurous acid 6 aqueous hydrogen sulfite Science 10/Kennedy/2016

67 Empirical Classification of Compoundsionic molecular Solids at SATP s, l, or g at SATP Conducts electricity when dissolved in water Do not conduct electricity when dissolved in water p. 71 #5, 6 Do Science 10/Kennedy/2016

68 Plastics, Polymers, and AlloysPolymers are long molecules made from small molecules, such as silk, spider webs and sap from rubber trees. The molecule repeats itself to form a long chain. Natural polymers: silk, spider webs and sap from rubber trees. Artificial polymers: plastics, polyethylene, polystyrene. Science 10/Kennedy/2016

69 Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Water H2O(l) or HOH(l) Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Ethanol C2H5OH(l) or CH3CH2OH(l) Methanol CH3OH(l) Ammonia NH3(g) Hydrogen sulfide H2S(g) Sucrose C12H22O11(s) Glucose C6H12O6(s) Hydrochloric acid HCl(aq) Sulfuric acid H2SO4(aq) Acetic acid CH3COOH(aq) Nitric acid HNO3(aq) Phosphoric acid H3PO4(aq) Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2 (g) Science 10/Kennedy/2016

70 4 Chemical Change Page 77 Science 10/Kennedy/2016

71 Kinetic molecular theoryIntroduction Page 77 Chemistry is the study of change. The change may be physical or chemical.  Notes: 4.1 Chemical Reactions Chemical reactions may be defined theoretically or empirically: KMT Kinetic molecular theory Theoretical: A chemical reaction occurs when atoms rearrange themselves into new molecules Particles are in constant and random motion Particles must collide with a minimum speed/energy and orientation. Science 10/Kennedy/2016

72 Reactants Products 4.1 Chemical Reactions Page 77Chemical reactions are changes that may be defined theoretically or empirically: Reactants Products Chemicals you start with Chemicals you end up with Science 10/Kennedy/2016

73 The yeast produces carbon dioxide to make the bread risePhysics Phun Useful Reactions Laundry detergent: The oxygen in hydrogen peroxide and sodium hypochlorite takes the colour away from stains Baking: The yeast produces carbon dioxide to make the bread rise Swimming pool: Chlorine in the water kills bacteria and micro-organisms Swimming pool: Chlorine in the water kills bacteria and micro-organisms Science 10/Kennedy/2016

74 Exothermic: heat is given off (surrounding temp increases)4.1 Chemical Reactions Page 77  Notes: Empirical: reaction Exothermic: heat is given off (surrounding temp increases) Endothermic: heat is absorbed (surrounding temp decreases) Evidence of a chemical change: colour change odor change gas produced state change energy change (the substance changes temperature) Science 10/Kennedy/2016

75 Chemical changes always involve energy changes Page 77 Chemical changes always involve energy changes An energy change may show up as a temperature change or light given off. Exothermic: heat is given off (surrounding temp goes up) Endothermic: heat is absorbed (surrounding temp goes down) Science 10/Kennedy/2016

76 KMT Page 77  Notes: Mass is conserved in all chemical reactionsTheoretical A chemical reaction occurs when atoms rearrange themselves into new molecules. Particles must collide with a minimum speed/energy and orientation to react. KMT A reaction is written as follows: Reactants Products Science 10/Kennedy/2016

77 Reactants Products Chemical Reactions Page 77 Chemicals you start withChemicals you end up with Product 1 Product 2 + Reactant 1 Reactant 2 Science 10/Kennedy/2016

78 Methane and oxygen react to form water and carbon dioxidePage 77 Methane and oxygen react to form water and carbon dioxide CH O > H2O CO2 C H O + 2 H 1 C 3 O 4 H 1 C 2 O The number of atoms on each side do not add up!!!??? They must add up!! Science 10/Kennedy/2016

79 Mass is conserved CH4 + O2 ----> H2O + CO2 Page 7510 g of reactants 10 g of products Mass is conserved Science 10/Kennedy/2016

80 Law of Conservation of MassPage 78 Law of Conservation of Mass For mass to be conserved the number of atoms in the reactants must be the same as the number of each type of atoms in the products The number of atoms don’t add properly. It must be balanced. CH O > H2O CO2 2 2 C H O + O H O Science 10/Kennedy/2016

81 H2O 2H2O One water molecule Two hydrogen atoms O H One oxygen atomTwo water molecules 2H2O H O Four hydrogen atoms H O Coefficient Two oxygen atoms subscript Science 10/Kennedy/2016

82 Law of Conservation of MassPage 78 Law of Conservation of Mass It must be balanced. CH O > H2O CO2 2 2 One molecule of methane reacts with 2 molecules of oxygen to produce 2 molecules of water and 1 molecule of carbon dioxide Science 10/Kennedy/2016

83 Balancing Chemical EquationsPage 75 Balancing Chemical Equations Make a list of each element on each side of the reaction Count how many of each element is present before and after Use coefficients to balance the reaction Only use coefficients to balance the reaction Don’t change the subscripts when balancing a reaction Keep polyatomic ions together Science 10/Kennedy/2016

84 Balancing chemical equationsPage 78 Balancing chemical equations Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016

85 Balancing chemical equationsPage 79 Balancing chemical equations Write the correct formulae for the products and the reactants Use coefficients to ensure you have the same amount of each type of atom on both sides of the equation 9. Balance the following equations using whole number coefficients. 2 Mg O > MgO 2 List and count atoms 2 1 2 Mg O Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016

86 Page 38 Reactants Products Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016

87 Balancing Chemical EquationsMake a list of each element on each side of the reaction Count how many of each element is present before and after Use coefficients to balance the reaction Only use coefficients to balance the reaction Don’t change the subscripts when balancing a reaction Keep polyatomic ions together Science 10/Kennedy/2016

88 Only use coefficients to balance – don’t change the subscripts!Write the correct formulae for the products and the reactants Use coefficients to ensure you have the same amount of each type of atom on both sides of the equation Page 79 4. Balance the following chemical reaction using the lowest possible whole number coefficients. Mercury(II) oxide decomposes to produce mercury and oxygen gas. 2 HgO Hg O2 2 Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016

89 CO2 3CO2 One carbon dioxide molecule One carbon atom Two oxygen atomsThree carbon dioxide molecules 3CO2 Three carbon atom Coefficient Six oxygen atoms subscript p. 78 #1 - 3 Do Science 10/Kennedy/2016

90 Reactants Products Li + AlCl3 Al + LiCl 3 3Page 79 8. Balance the following chemical reaction using the lowest possible whole number coefficients. Reactants Products 3 Li AlCl Al LiCl 3 Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016

91 3. Identify the reaction below that is properly balanced.Page 78 3. Identify the reaction below that is properly balanced. a. N H2 ⟶ NH3 b. N H2 ⟶ NH3 c. 2N H2 ⟶ NH3 d. N H2 ⟶ NH3 The lowest possible whole number coefficients must be used. Science 10/Kennedy/2016

92 Balancing Chemical EquationsMake a list of each element on each side of the reaction Count how many of each element is present before and after Use coefficients to balance the reaction Only use coefficients to balance the reaction Don’t change the subscripts when balancing a reaction Keep polyatomic ions together p. 79 #1 - 11 Do Science 10/Kennedy/2016

93 2 NaOH + H2SO4 H2O + Na2SO4 2 HOH 2 1 1 2 Na OH SO4 H 2 1 Page 8014. The following reactions contain polyatomic ions. Balance the following equations using the lowest possible whole number coefficients. Keep the polyatomic ions together 2 NaOH H2SO H2O Na2SO4 2 HOH 2 1 1 2 Na OH SO4 H 2 1 Science 10/Kennedy/2016

94 NaOH + H2SO4 H2O + Na2SO4 Page 80 Same question as a multiple choiceThe coefficients for the balanced chemical equation are: a. 2, 0, 2, 0 b. 1, 2, 1, 2 c. 2, 1, 2, 2 d. 2, 1, 2, 1 p. 80 #12 – 17 Do Science 10/Kennedy/2016

95 Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Remember!! Water H2O(l) or HOH(l) Hydrogen peroxide H2O2(l) Methane (natural gas) CH4(g) Propane C3H8(g) Ethanol C2H5OH(l) or CH3CH2OH(l) Methanol CH3OH(l) Ammonia NH3(g) Hydrogen sulfide H2S(g) Sucrose C12H22O11(s) Glucose C6H12O6(s) Hydrochloric acid HCl(aq) Sulfuric acid H2SO4(aq) Acetic acid CH3COOH(aq) Nitric acid HNO3(aq) Phosphoric acid H3PO4(aq) Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2 (g) Science 10/Kennedy/2016

96 Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2 (g)Page 66 Remember!! Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2 (g) Science 10/Kennedy/2016

97 Na(s) + HOH(l) H2(g) + NaOH(aq) 2 2Page 81 A chemical reaction may be expressed using words rather than symbols. Write the balanced chemical equation, including states of matter, for each of the following: 21. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide. 2 Na(s) HOH(l) H2(g) NaOH(aq) 2 2 2 Na OH H 2 1 2 Na OH H 1 Science 10/Kennedy/2016

98 Na(s) + HOH(l) H2(g) + NaOH(aq)Same question as a numeric response Page 81 21. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide. 2 Na(s) HOH(l) H2(g) NaOH(aq) The coefficients for the balanced chemical reaction, in order from left to right are _____, ______, ______, and _______, 1 6 7 8 9 2 3 4 5 p. 81 #18 – 26 Do Science 10/Kennedy/2016

99 6 Balancing Quiz Balance the following reactions. (2 marks each) 1.8 HgS Hg S8 6 2. 2 NaF Ba(OH) NaOH BaF2 3. Aluminium reacts with sodium hydroxide to produce sodium metal and aluminium hydroxide Al NaOH Na + Al(OH)3 3 Science 10/Kennedy/2016

100 4.2 The Mole Concept Page 82 1 mole = 6.02 x 1023 particlesDealing with individual atoms is not typically practical in chemical reactions. A larger amount called the mole is used. The number of particles called Avogadro’s number is equal to one mole:  Notes: 1 mole = 6.02 x 1023 particles Science 10/Kennedy/2016

101 Amount Science 10/Kennedy/2016

102 The amount of a substance can be expressed in numerous ways:couple 2 few 3 dozen 12 score 20 ream 500 mole 6.02 x 1023 A mole is an amount: Science 10/Kennedy/2016

103 1 mole = 6.02 x 1023 particles atoms molecules ions Page 82Science 10/Kennedy/2016

104 1 mole = 6.02 x 1023 Is a very large number!Page 82 1 mole = 6.02 x 1023 Is a very large number! Dealing with individual atoms is not typically practical in chemical reactions. Science 10/Kennedy/2016

105 6.02 x 1023 Avogadro’s number 1 mol of watermelon Seeds: Would fit inside a hollow sphere the size of the moon 1 mol of Timbits: Would cover the Earth and be 8 km deep 1 mol of dimes: Would make at least 7 stacks that would reach the moon 1 mol of grains of sand: Would be more than all of the sand on Miami Beach Science 10/Kennedy/2016

106 4.2 The Mole Concept Page 82 1 mole = 6.02 x 1023 particlesDealing with individual atoms is not typically practical in chemical reactions. A larger amount called the mole is used. The number of particles called Avogadro’s number is equal to one mole:  Notes: 1 mole = 6.02 x 1023 particles A mole is defined as the number of atoms in 12 g of carbon. Science 10/Kennedy/2016

107 A mole is defined as the number of atoms in 12 g of carbon.Page 82 The Mole A mole is defined as the number of atoms in 12 g of carbon. Unit mole Symbol mol Science 10/Kennedy/2016

108 Sulfur atoms are 3 times heavier than carbon atoms.Page 83 4. One mole of carbon has a mass of 12 g but one mole of sulfur is measured as 36 g. The mass of one sulfur atom must be ______ times larger than the mass of one carbon atom 3 36 g sulfur 12 g carbon = 3 Sulfur atoms are 3 times heavier than carbon atoms. Science 10/Kennedy/2016

109 Page 84 The amount of a substance in a balanced chemical reaction may be communicated as moles. 7. Note the balanced chemical equation below. Four mol of FeCl3 will produce _____ mol of BaCl2. 6  2FeCl BaBr FeBr BaCl2 Two moles of iron(III) chloride react with 3 moles of barium bromide to produce 2 moles of iron(III) bromide plus 3 moles of barium chloride p. 83 #1 – 7 Do Science 10/Kennedy/2016

110 Molar Mass (pg 95) To calculate the molar mass of the substance.Determine the chemical formula (if necessary) Count the number of each atom. Look up molar mass of each atom and multiply by number of atoms Add Science 10/Kennedy/2016

111 Mass to moles and Moles to Mass (pg 95)Determine the conversion Identify the conversion factor Set up conversion line and set up conversion to cancel units Ex) 5.00g of sodium in moles ? _5.00g__1 mol____0.217 mol 22.99g p. 95 #1 – 3 Do Science 10/Kennedy/2016

112 4.3 Reaction Types Page 85 Chemical reactions can be classified according to type. Knowledge of reaction type may make it possible to predict the products of a chemical reaction.  Notes: Reaction types: Formation Decomposition Single Replacement Double replacement Combustion Other (any reaction that does not match the above types) Science 10/Kennedy/2016

113 element + element ----> compoundPage 85 Formation: element element > compound Decomposition: compound > element + element Single replacement: element compound > compound + element Double replacement: compound compound > compound compound Science 10/Kennedy/2016

114 element + element ----> compoundPage 85 Formation: element element > compound Decomposition: compound > element element p. 86 #1 – 12 Do Science 10/Kennedy/2016

115 Predicting Reactions requires:Ionic Nomenclature Solubility Multivalent charges Polyatomic ions Molecular Nomenclature Acid/base Nomenclature Memorized compounds Balancing Reactions Science 10/Kennedy/2016

116 Predictions of Formation & Decomposition ReactionsPage 87 Predictions of Formation & Decomposition Reactions Predict the missing substances Identify the reaction as either formation (f) or decomposition (d) Balance using whole number coefficients Formation: element element > compound Decomposition: compound > element element Science 10/Kennedy/2016

117 Predicting Reactions:Page 87 Predicting Reactions: Formation: element + element > compound Decomposition: compound > element + element 13. Mg(s) O2(g)  2 MgO(s) p. 87 #13 – 20 Do Science 10/Kennedy/2016

118 element + compound ----> compound + elementPage 85 Single replacement: element compound > compound element Double replacement: compound compound > compound compound Page 88 NaOH(aq) HCl(aq) HOH(l) NaCl(aq) 23. dr May also be called a neutralization reaction Neutralization reaction: Acid plus base Science 10/Kennedy/2016

119 element + compound ----> compound + elementSingle replacement: element compound > compound element Double replacement: compound compound > compound compound Page 88 25. Aqueous iron(II) hydroxide reacts with aqueous aluminium chloride to produce a solution of aluminium hydroxide and iron(II) chloride. 3 2 Fe(OH)2(aq) AlCl3(aq) Al(OH)3(s) FeCl2(aq) p. 88 #21 – 27 Do Need to check solubility table Science 10/Kennedy/2016

120 Predictions of Single & Double Replacement ReactionsPage 89 Predictions of Single & Double Replacement Reactions Predict the missing substances Identify the reaction as either single replacement (sr) or double replacement (dr) Balance using whole number coefficients Single replacement: element + compound > compound + element Br2(aq) NaI(aq) 29. 2 2NaBr(aq) l2(s) Science 10/Kennedy/2016

121 Predictions of Single & Double Replacement ReactionsPage 89 Predictions of Single & Double Replacement Reactions Predict the missing substances Identify the reaction as either single replacement (sr) or double replacement (dr) Balance using whole number coefficients Page 89 32 Iron reacts with copper(II) chloride (use the most common ion charge for iron). 3 2 Fe(s) CuCl2(aq) Cu(s) FeCl3(aq) p. 89 #28 – 34 Do Science 10/Kennedy/2016

122 Combustion (oxidation):Page 90 Combustion (oxidation): Add oxygen burns rusts tarnish compound + oxygen > most common oxides Science 10/Kennedy/2016

123 Combustion (oxidation):Page 90 Combustion (oxidation): Science 10/Kennedy/2016

124 Combustion (oxidation): burns rusts tarnishPage 90 Combustion (oxidation): burns rusts tarnish Science 10/Kennedy/2016

125 Fossil Fuel CombustionPage 90 Fossil Fuel Combustion The combustion of fossil fuels is exothermic producing carbon dioxide and water Usually the combustion is incomplete resulting in carbon monoxide – very poisonous Need winter picture of car exhaust Science 10/Kennedy/2016

126 C5H12(l) + O2(g) CO2(g) + H2O(g)Page 90 41. Liquid pentane (C5H12) reacts with oxygen gas in the air to undergo complete combustion to produce carbon dioxide and water vapour. C5H12(l) O2(g) CO2(g) H2O(g) 8 5 6 42. Liquid pentane (C5H12) reacts with oxygen gas in the air to undergo incomplete combustion to produce carbon monoxide and water vapour. 2 C5H12(l) O2(g) CO(g) H2O(g) 11 10 12 p. 90 #35 – 42 Do Science 10/Kennedy/2016

127 Rusts, oxidation, explodes Add oxygenPage 91 Burns, tarnish Rusts, oxidation, explodes Add oxygen Predictions of Combustion Reactions Predict the missing substances Balance using whole number coefficients compound + oxygen > most common oxides H H2O(g) N NO2(g) C CO2(g) S SO2(g) Metals form their metal oxides p. 91 #43 – 47 Do Science 10/Kennedy/2016

128 Cobalt(II) chloride paperPage 94 Chemical Tests Evidence Hydrogen Burning splint Explode (pop) Carbon dioxide Burning splint Extinguishes fire Lime water Precipitate (cloudy) Ca(OH)2 + CO2  CaCO3(s) Oxygen Glowing splint Splint catches fire Water Blue paper turns pink Cobalt(II) chloride paper Acidity Acid: Blue turns red pH paper Base: Red turns blue Science 10/Kennedy/2016

129 Writing Chemical EquationsPredict the missing chemicals based on reaction type Know the most common oxides Know your memorized substances Use coefficients to balance the reaction: Only use coefficients to balance the reaction Don’t change the subscripts when balancing a reaction Keep polyatomic ions together Check solubility of products Balance oxygen last in combustion reactions p. 92 # Do Science 10/Kennedy/2016

130 8 Balancing Quiz Balance the following equations. HgS Hg + S8 2 marksCl Na NaCl 2 Barium reacts with aluminium hydroxide to produce aluminium metal and barium hydroxide Ba Al(OH) Al Ba(OH)2 2 3 Science 10/Kennedy/2016

131 The End Science 10/Kennedy/2016