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Page 61 Science 10/Kennedy/2016 1 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 2 Page 61 International International Union Union ofof Pure Pure and and Applied Applied Chemistry Chemistry IUPAC Science 10/Kennedy/2016 3 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 4 Alloys Alloys are combinations of metals: e.g., steel Alloys 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 5 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 6 Page 61 Atoms are bonded together using valence electrons. Science 10/Kennedy/2016 7 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 Ionic compounds • sharing Molecular compounds Science 10/Kennedy/2016 8 3.1 Binary Ionic Compounds Page 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. Properties: metal-nonmetal 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 9 Page 61 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. + _ + _ + _ + _ + _ + _ + _ + All the ions are interconnected with each other Single units of ionic compounds do not exist by themselves Science 10/Kennedy/2016 10 Page 62 Nomenclature Science 10/Kennedy/2016 11 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 12 Page 62 Nomenclature Notes: Cation name/space/anion name Science 10/Kennedy/2016 e.g., sodium chloride 13 Page 63 Cation name/space/anion name 2. Name the following binary ionic substances. IUPAC Name Formula a. sodium chloride NaCl b. magnesium chloride MgCl2 c. strontium bromide SrBr2 p. 63 #1, 2 Do Science 10/Kennedy/2016 14 Page 63 Ionic substances All the atoms are interconnected with each other + _ + _ + _ + _ + _ + _ + _ + 2:1 Ratio 1:1 Ratio e.g., NaCl Na2Cl2 Always use the lowest possible numbers Na4Cl4 Science 10/Kennedy/2016 Ca2+ Cl- CaCl2 15 Page 63 Ca2+ + Cl- 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+ Na+ Na+ BrO2- NaBr Na2O K+ K+ K+ N3- K3N P3- Mg3P2 Mg2+ Science 10/Kennedy/2016 16 Page 63 Superscripts are different than subscripts Superscripts – the charge on each ion Mg2+ + 3P Mg3P2 Subscripts – how many ions are in the compound p. 63 #3 Science 10/Kennedy/2016 Do 17 Page 62 Multivalent Ions Notes: 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 18 Page 63 The total charge must = zero 4. Determine the formula for each of the following binary ionic substances. Name Formula FeBr2 a. iron(II) bromide Fe2+ Br- b. iron(III) bromide Fe3+ Br- h. gold(I) oxide i. gold(III) oxide Au3+ Au3+ O2- O2- O2- Au+ Au+ BrBr- Br- O2- FeBr3 Au2O Au2O3 p. 63 #4 Science 10/Kennedy/2016 Do 19 Page 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 c. d. Name niobium(III) oxide niobium(V) oxide Nb2O3 Nb2O5 First consider negative charge on nonmetal ion Science 10/Kennedy/2016 20 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 Science 10/Kennedy/2016 Do 21 Classical Nomenclature Latin: Ferric and Ferrous Fe3+ Fe2+ Latin: cupric and cuprous Cu2+ Cu+ Science 10/Kennedy/2016 22 Page 62 Notes: Polyatomic ions Groups of atoms may form an ion and form ionic bonds with other ions. Science 10/Kennedy/2016 sulfate SO42- ammonium NH4+ 23 Page 274 Science 10/Kennedy/2016 24 Memorize Common Polyatomic Ions hydroxide OH- sulfate SO42- acetate CH3COO- nitrate NO3- phosphate PO43- ammonium NH4+ No Quiz Science 10/Kennedy/2016 25 Page 64 Metal name(roman numeral) nonmetal name 6. Determine the name for each of the following polyatomic substances. Name Formula a. sodium carbonate Na2CO3 b. sodium nitrite NaNO2 g. aluminium hydroxide Al(OH)3 i. iron(III) sulfate Fe2(SO4)3 p. 64 #6 Science 10/Kennedy/2016 Do 26 Page 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 Science 10/Kennedy/2016 Do 27 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) molecular C12H22O11(s) Dissociates when it dissolves Separates into ions Does not dissociates when it dissolves Science 10/Kennedy/2016 28 Page 62 Soluble – dissolves in water aqueous Breaks apart into ions as it dissolves dissociates Science 10/Kennedy/2016 29 Ionic 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 30 Ionic substances + - + - - + - + + - + - Salt Dissociate – individual ions areScience formed 10/Kennedy/2016 Molecular substances Sugar 31 Ionic substances Molecular substances Both dissolve Salt solution - Sugar solution - + + - + + + - + Dissociate – individual ions are formed Science 10/Kennedy/2016 32 Compounds that include group I ions or NH4+ are generally soluble Using Solubility Table Only works for ionic substances Page 274 aq s Science 10/Kennedy/2016 33 Use solubility table Page 64 8. Use your solubility table to determine the solubility for each of the following. Formula Solubility (s or aq) a. Na2CO3 c FeSO4 aq aq f. Al(OH)3 s aq s Not all substances are in the solubility table p. 64 #8 Compounds that include group I ions are always soluble Science 10/Kennedy/2016 Do 34 Use solubility table Page 65 10. 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 #10 - 13 Science 10/Kennedy/2016 Do 35 Ionic Nomenclature Quiz: Provide the name or formula for the following. (1 mark each) Science 10/Kennedy/2016 36 Ionic 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 MgBr2 2. nickel(II) hydroxide Ni(OH)2 3. sodium carbonate 4. gold(III) borate Na2CO3 Au2(B03)3 5. ZnCl2 6. zinc chloride ammonium sulfate 7. iron(III) hydroxide Fe(OH)3 8. vanadium(IV) dichromate V(Cr2O7)2 Use your solubility table to determine the solubility for each of the following. Name 9. Lithium carbonate 10. 10 (NH4)2SO4 calcium hydroxide Science 10/Kennedy/2016 Solubility (s or aq) aq s 37 3.2 Molecular Compounds 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 38 Ionic 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 39 Molecular Compounds Page 66 Atoms join to form individual molecules that are not connected with other molecules O H H Science 10/Kennedy/2016 40 Ionic Substances Page 66 All the atoms are interconnected with each other Molecular Substances The atoms join to form molecules that are not connected with other molecules H O H Science 10/Kennedy/2016 41 H H O HC H O C H H C H H O H H O C H C C O O H H C H C O H O H H H C C O O C H C H OH H Science 10/Kennedy/2016 Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- 42 Science 10/Kennedy/2016 Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- Na+ Cl- 43 Nomenclature Ionic Compounds • Metal, nonmetal • Balance charges Molecular Compounds Page 66 • Nonmetal, nonmetal • Use prefix system Science 10/Kennedy/2016 44 3.2 Molecular Compounds Page 66 Notes: Molecular compounds are combinations of nonmetals • Molecular elements contain only one type of atom: • Monoatomic atoms can exist on their own e.g., Ar, Ni, Cr Science 10/Kennedy/2016 Ozone O3(g) Sulfur S8(s) Phosphorus P4(s) Diatomic elements: O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) 45 Page 66 Some elements tend to come together as groups. Ozone Sulfur Phosphorus O3(g) S8(s) P4(s) Diatomic elements O2(g) H2(g) Cl2(g) Br2(l) I2(g) F2(g) N2(g) Memorize Science 10/Kennedy/2016 46 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 propane BBQ fuel hydrogen peroxide Hydrogen peroxide H2O2 • • • Baking soda Sodium bicarbonate Cleaning, baking, putting out fires, absorbing odours vinegar Acetic acid disinfectant for wounds (3 %) Hair bleach (6 %) Rocket fuel (> 70 %) Cooking, cleaning Science 10/Kennedy/2016 47 Memorized Compounds Science 10/Kennedy/2016 48 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 49 Compound Quiz: Provide the name or symbol for the following elements. (1 mark each) Science 10/Kennedy/2016 50 Compound Quiz: Provide the name or symbol for the following compounds. (1 mark each) CH4(g) Methane C12H22O11(s) Sucrose NH3(g) Ammonia O3(g) Ozone CH3OH(l) Methanol Propane C3H8(g) Ethanol C2H5OH(l) HOH water Glucose C6H12O6(s) H2O2(l) Hydrogen peroxide or CH3CH2OH(l) Science 10/Kennedy/2016 10 51 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 52 Page 66 Nomenclature: The number of atoms in a molecule must be indicated using a prefix: 1 – mono 2 – di 3 – tri 4 – tetra 5 – penta 6 – hexa 7 – hepta 8 – octa 9 – nona 10 – deca 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 53 Page 67 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. 3. Name each compound. IUPAC Name Formula c. dinitrogen monoxide d. diphosophorus pentoxide N2 O P2O5 Double vowels that sound the same - drop the first one The “a” is dropped 2. Provide the formula for each molecular compound Name formula a. nitrogen dioxide NO2 b. dinitrogen dioxide N2O2 p. 67 #1 - 3 Science 10/Kennedy/2016 Do 54 Page 68 3.3 Acids & Bases 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 H+ ion while in solution Science 10/Kennedy/2016 55 Page 68 3.3 Acids & Bases 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 56 Page 68 3.3 Acids & Bases The strength of an acid or base is measured on the pH scale. pH means power of the hydrogen H+ OH- Neutral Basic (alkaline) Acidic 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 57 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 58 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) HCl(g) Organic acids contain carbon and a COOH HCl(aq) Acids will always be aqueous p. 70 #1, 2 Science 10/Kennedy/2016 Do 59 Page 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. a. Ionic Name IUPAC Acid name Formula hydrogen nitrite aqueous hydrogen nitrite HNO2 p. 70 #3 Science 10/Kennedy/2016 Do 60 Page 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 61 Page 247 Science 10/Kennedy/2016 62 Page 71 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. 4. Complete the chart. Ionic Name hydrogen thiosulfate b. hydrogen sulfide c. hydrogen chlorate a. Classical Acid Name Formula thiosulfuric acid hydrosulfuric acid H2S2O3(aq) chloric acid HClO3 H2S(aq) p. 71 #4 Science 10/Kennedy/2016 Do 63 Page 68 The strength of an acid or base is measured using the pH scale pH = power of the hydrogen H+ acidic 0 1 2 3 OHbasic neutral 4 5 6 7 8 9 10 11 12 13 14 pH may be measured using: • a pH meter • dyes that change colour such as indicators or pH paper Science 10/Kennedy/2016 64 Nomenclature Quiz: Provide the name or formula for the following. (1 mark each) Name Formula 1. diphosophorus pentoxide P2O5 2. nickel(II) hydroxide Ni(OH)2 3. glucose 4. 5. gold(III) tetraborate dinitrogen heptaoxide C6H12O6 Au2(B4O7)3 N2O7 6. sulfurous acid H2SO3(aq) aqueous hydrogen sulfite Science 10/Kennedy/2016 6 65 Nomenclature Quiz: Provide the name or formula for the following. (1 mark each) Name Formula 1. triphosophorus heptoxide P3O7 2. nickel(II) nitrite Ni(NO2)2 3. sucrose 4. 5. gold(III) thiosulfate dinitrogen heptachloride C12H22O11 Au2(S2O3)3 N2Cl7 6. sulfurous acid H2SO3(aq) 6 aqueous hydrogen sulfite Science 10/Kennedy/2016 66 Empirical Classification of Compounds ionic molecular s, l, or g at SATP Solids at SATP Conducts electricity when dissolved in water Do not conduct electricity when dissolved in water p. 71 #5, 6 Science 10/Kennedy/2016 Do 67 Water Hydrogen peroxide Methane (natural gas) Propane Ethanol Methanol Ammonia Hydrogen sulfide Sucrose Glucose Hydrochloric acid Sulfuric acid Acetic acid Nitric acid Phosphoric acid Ozone Sulfur Phosphorus Diatomic elements H2O(l) or HOH(l) H2O2(l) CH4(g) C3H8(g) C2H5OH(l) or CH3CH2OH(l) CH3OH(l) NH3(g) H2S(g) C12H22O11(s) C6H12O6(s) HCl(aq) H2SO4(aq) CH3COOH(aq) HNO3(aq) H3PO4(aq) O3(g) S8(s) P4(s) O2(g) H2(g) Cl2(g) Br2(l) I2(g) N2 (g) Science 10/Kennedy/2016 F2(g) 69 4 Chemical Change Page 77 Science 10/Kennedy/2016 70 Introduction 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: Theoretical: A chemical reaction occurs when atoms rearrange themselves into new molecules Particles must collide with a minimum speed/energy and orientation. Science 10/Kennedy/2016 KMT Kinetic molecular theory Particles are in constant and random motion 71 4.1 Chemical Reactions Page 77 Chemical reactions are changes that may be defined theoretically or empirically: Reactants Chemicals you start with Products Chemicals you end up with Science 10/Kennedy/2016 72 Physics 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 73 4.1 Chemical Reactions Page 77 Notes: Empirical: reaction Evidence of a chemical change: • colour change • odor change • gas produced • state change • energy change (the substance changes temperature) Science 10/Kennedy/2016 Exothermic: heat is given off (surrounding temp increases) Endothermic: heat is absorbed (surrounding temp decreases) 74 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 75 Page 77 Notes: Mass is conserved in all chemical reactions Theoretical 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 76 Chemical Reactions Page 77 Reactants Chemicals you start with Reactant 1 + Reactant 2 Products Chemicals you end up with Product 1 + Science 10/Kennedy/2016 Product 2 77 Page 77 Methane and oxygen react to form water and carbon dioxide CH4 + O2 H H C H H + O O ----> H 2O H O + H CO2 + O C O 2H 1C 3O 4H 1C 2O The number of atoms on each side do not add up!!!??? They must add up!! Science 10/Kennedy/2016 78 Page 75 CH4 + O2 10 g of reactants ----> H 2O + CO2 10 g of products Mass is conserved Science 10/Kennedy/2016 79 Page 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. CH4 H H C H H + + 2 O2 O O ----> 2 H2 O H O O H O O H + + CO2 O C O H Science 10/Kennedy/2016 80 One water molecule H O H2O H Two hydrogen atoms One oxygen atom Two water molecules H O H H O H 2H2O Four hydrogen atoms Two oxygen atoms Coefficient subscript Science 10/Kennedy/2016 81 Page 78 Law of Conservation of Mass It must be balanced. CH4 + 2 O2 ----> 2 H2 O + CO2 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 82 Page 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 83 Page 78 Balancing chemical equations Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016 84 Page 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 + 2 O2 1 Mg 2O ----> 2 MgO 2 1 Mg 1O List and count atoms Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016 85 Page 38 Products Reactants Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016 86 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 87 • 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 2 Hg + O2 Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016 88 One carbon dioxide molecule CO2 One carbon atom Two oxygen atoms Three carbon dioxide molecules Coefficient 3CO2 Three carbon atom Six oxygen atoms subscript Science 10/Kennedy/2016 p. 78 #1 - 3 Do 89 Page 79 8. Balance the following chemical reaction using the lowest possible whole number coefficients. Reactants 3 Li + AlCl3 Products Al + 3 LiCl Only use coefficients to balance – don’t change the subscripts! Science 10/Kennedy/2016 90 Page 78 3. Identify the reaction below that is properly balanced. a. b. c. d. N2 N2 2N2 N2 + + + + H2 H2 6H2 3H2 ⟶ ⟶ ⟶ ⟶ NH3 2NH3 4NH3 2NH3 The lowest possible whole number coefficients must be used. Science 10/Kennedy/2016 91 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 p. 79 #1 - 11 Science 10/Kennedy/2016 Do 92 Page 80 14. The following reactions contain polyatomic ions. Balance the following equations using the lowest possible whole number coefficients. Keep the polyatomic ions together 2 NaOH + H2SO4 2 HOH H 2O + 1 2 Na 2 Na 1 2 OH 2 1 OH 2 H 2 1 H 1 SO4 1 SO4 Science 10/Kennedy/2016 Na2SO4 93 Page 80 Same question as a multiple choice NaOH + H2SO4 H 2O + Na2SO4 The coefficients for the balanced chemical equation are: a. b. c. d. 2, 0, 2, 0 1, 2, 1, 2 2, 1, 2, 2 2, 1, 2, 1 p. 80 #12 – 17 Science 10/Kennedy/2016 Do 94 Remember!! Water Hydrogen peroxide Methane (natural gas) Propane Ethanol Methanol Ammonia Hydrogen sulfide Sucrose Glucose Hydrochloric acid Sulfuric acid Acetic acid Nitric acid Phosphoric acid Ozone Sulfur Phosphorus Diatomic elements H2O(l) or HOH(l) H2O2(l) CH4(g) C3H8(g) C2H5OH(l) or CH3CH2OH(l) CH3OH(l) NH3(g) H2S(g) C12H22O11(s) C6H12O6(s) HCl(aq) H2SO4(aq) CH3COOH(aq) HNO3(aq) H3PO4(aq) O3(g) S8(s) P4(s) O2(g) H2(g) Cl2(g) Br2(l) I2(g) Science 10/Kennedy/2016 N2 (g) F2(g) 95 Page 66 Remember!! Ozone Sulfur Phosphorus Diatomic elements O3(g) S8(s) P4(s) O2(g) H2(g) Cl2(g) F2(g) N2 (g) Science 10/Kennedy/2016 Br2(l) I2(g) 96 Page 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) + 2 HOH(l) H2(g) + 2 NaOH(aq) 1 Na 1 Na 2 1 H 2 2 H 2 1 OH 2 1 OH Science 10/Kennedy/2016 97 Same question as a numeric response Page 81 21. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide. 2 Na(s) + 2 HOH(l) H2(g) + 2 NaOH(aq) The coefficients for the balanced chemical reaction, in order from left to right are _____, ______, ______, and _______, 2 21 2 p. 81 #18 – 26 Do Science 10/Kennedy/2016 0 0 0 0 1 1 1 1 2 2 2 2 3 3 3 3 4 4 4 4 5 5 5 5 6 6 6 6 7 7 7 7 8 8 8 8 9 9 9 9 98 Balancing Quiz Balance the following reactions. (2 marks each) 1. 8 HgS 2. 2 NaF 3. 8 Hg + + Ba(OH)2 S8 6 2 NaOH + BaF2 Aluminium reacts with sodium hydroxide to produce sodium metal and aluminium hydroxide Al + 3 NaOH 3 Na + Al(OH)3 Science 10/Kennedy/2016 99 4.2 The Mole Concept Page 82 Dealing 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 100 Amount Science 10/Kennedy/2016 101 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 102 Page 82 1 mole = 6.02 x 1023 particles atoms molecules ions Science 10/Kennedy/2016 103 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 104 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 105 4.2 The Mole Concept Page 82 Dealing 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 106 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 107 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 108 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 6 mol of BaCl2. will produce _____ 2FeCl3 + 3BaBr2 2FeBr3 + 3BaCl2 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 Science 10/Kennedy/2016 Do 109 Molar Mass (pg 95) • To calculate the molar mass of the substance. 1. Determine the chemical formula (if necessary) 2. Count the number of each atom. 3. Look up molar mass of each atom and multiply by number of atoms 4. Add Science 10/Kennedy/2016 110 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 Science 10/Kennedy/2016 p. 95 #1 – 3 Do 111 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 112 Page 85 Formation: element + element Decomposition: compound ----> ----> compound element + element Single replacement: element + compound ----> compound + element Double replacement: compound + compound ----> compound Science 10/Kennedy/2016 + compound 113 Page 85 Formation: element + element Decomposition: compound ----> ----> element compound + element p. 86 #1 – 12 Science 10/Kennedy/2016 Do 114 Predicting Reactions requires: • Ionic Nomenclature • Solubility • Multivalent charges • Polyatomic ions • Molecular Nomenclature • Acid/base Nomenclature • Memorized compounds • Balancing Reactions Science 10/Kennedy/2016 115 Page 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 Decomposition: compound ----> ----> element Science 10/Kennedy/2016 compound + element 116 Page 87 Predicting Reactions: Formation: element + element Decomposition: compound ----> 13. 2 Mg(s) + ----> compound element + element O2(g) 2 MgO(s) p. 87 #13 – 20 Science 10/Kennedy/2016 Do 117 Page 85 Single replacement: element + compound ----> compound + element Double replacement: compound + compound ----> compound + compound Page 88 23. NaOH(aq) + dr HCl(aq) HOH(l) + NaCl(aq) May also be called a neutralization reaction Neutralization reaction: Acid plus base Science 10/Kennedy/2016 118 Single replacement: element + compound ----> compound Double replacement: compound + compound + element ----> 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 Fe(OH)2(aq) + 2 AlCl3(aq) 2 Al(OH)3(s) Need to check solubility table Science 10/Kennedy/2016 + 3 FeCl2(aq) p. 88 #21 – 27 Do 119 Page 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 29. Br2(aq) + 2 NaI(aq) Science 10/Kennedy/2016 2NaBr(aq) + l2(s) 120 Page 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). 2 Fe(s) + 3 CuCl2(aq) 3 Cu(s) + 2 FeCl3(aq) p. 89 #28 – 34 Science 10/Kennedy/2016 Do 121 Page 90 Combustion (oxidation): burns rusts tarnish compound + oxygen Add oxygen ----> most common oxides Science 10/Kennedy/2016 122 Page 90 Combustion (oxidation): Science 10/Kennedy/2016 123 Page 90 Combustion (oxidation): burns rusts tarnish Science 10/Kennedy/2016 124 Page 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 Science 10/Kennedy/2016 125 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) + 8 O2(g) 5 CO2(g) + 6 H2O(g) 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) + 11 O2(g) 10 CO(g) + 12 H2O(g) p. 90 #35 – 42 Science 10/Kennedy/2016 Do 126 Page 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 N C S H2O(g) NO2(g) CO2(g) SO2(g) Metals form their metal oxides p. 91 #43 – 47 Science 10/Kennedy/2016 Do 127 Page 94 Chemical Tests Evidence Hydrogen Explode (pop) Burning splint Carbon dioxide Burning splint Lime water Ca(OH)2 + CO2 CaCO3(s) Extinguishes fire Precipitate (cloudy) Oxygen Splint catches fire Glowing splint Water Cobalt(II) chloride paper Blue paper turns pink Acidity Acid: Blue turns red pH paper Science 10/Kennedy/2016 Base: Red turns blue128 Writing Chemical Equations Predict 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 #48 - 69 Science 10/Kennedy/2016 Do 129 Balancing Quiz Balance the following equations. 8 HgS Cl2 + 2 Na 8 Hg + S8 2 marks 2NaCl 2 marks 8 Barium reacts with aluminium hydroxide to produce aluminium metal and barium hydroxide 4 marks 3 Ba + 2 Al(OH)3 2 Al Science 10/Kennedy/2016 + 3 Ba(OH)2 130 The End Science 10/Kennedy/2016 131