Chemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions
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1 Chemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions
2
3 A preview of things we will do Chemical Reactions are AWESOME!
4 Characteristics of Chemical Reactions A chemical reaction: is a process in which the chemical and physical properties of the original substance changes and new substances with different physical and chemical properties are formed. main menu
5 PIZZA!!!
6 Chemical Equations A chemical equation has two parts: reactants: the starting materials products: the substances formed in the reaction (ending) example: C + O CO 2 2 reactants products
7 Identifying Reactants and Products Identify the reactants and products in the following equation: 2Al(s) + 3Cl 2 (g) 2AlCl 3 (s) reactant(s) Al, Cl 2 products(s) AlCl 3 main menu
8 Reaction Symbols Yields or Produces Solid or precipitate Liquid Gas Aqueous (acids & bases) (s) or (l) (g) or (aq) Catalyst (speeds up) Ni Heat Added Reversible Reaction
9 Identifying parts of a Chemical Equation: 2 Mg + O 2 2 MgO Reactants Products 1. Which are the reactants? 2. Which are the products? 3. Which are the coefficients? 4. Which is the subscript? Mg + O 2 MgO # in front # on bottom
10 SRIRACHA!!!
11 Indications of a Chemical Reaction 1. Production of a gas. 2. Formation of a precipitate. (a solid that forms from two liquids) 3. Change in energy. Endothermic reaction energy is absorbed Exothermic Reaction energy is released 4. Change in color or odor. main menu
12 Why wet dogs stink!!!
13 Law of Conservation of Mass Chemical equations are balanced to satisfy the Law of Conservation of Mass The Law of Conservation of Mass states: mass cannot be created or destroyed by ordinary physical or chemical means. total mass of the reactants must equal the total mass of the products. main menu
14 Law of Conservation of Mass -Mass is neither created nor destroyed! The number of atoms (and total mass) on the reactant side must equal the number of atoms (and total mass) on the product side. Remember: Calculate formula mass. (1 C x 12) + (4 H x 1) = 16 g 1CH 4 + 2O 2 1CO 2 + 2H 2 O 16 g + 64 g = 44 g + 36 g 80 g = 80 g Example: In a chemical reaction, 4 g of hydrogen combine with 32 g of oxygen to form water (2H 2 + O 2 2H 2 O). What is the mass of the product formed? Answer: Reactants = Products 4 g + 32 g = 36 g H 2 O
15 Practice: 1. In a chemical reaction, 4 g of hydrogen combine with 32 g of oxygen to form water What is the mass of the product formed? 2H 2 + O 2 2H 2 O 36 g 4 g + 32 g =? g 2. If 60 g of ethane burns in 224 g of oxygen to produce 108 g of water, what is the mass of the remaining product? C 2 H 6 + O 2 CO 2 + H 2 O 60 g g = 176 g? g g
16 Homework/Do NOW: Conservation of Mass Practice Problems (12 questions) Due FRIDAY 1/29/16 Turn it in today if you finish!
17 Warm-Up: Answer the following 1. What are the two parts of a chemical equation? 2. What is the law of conservation of mass? 3. According to the law, what must be equal on both sides of the equation? (hint: there are TWO things that must be equal (the total number of and the total in grams)
18 Law of Conservation of Mass Remember that atoms don t change in a chemical reaction; they just rearrange. For a chemical equation to accurately represent a reaction, the same number of each kind of atom must be on the left side of the arrow as are on the right side. main menu
19 Counting Atoms in Chemical Compounds Before we can balance an equation, we must first make sure that everyone can count the atoms present in a compound. Here are some examples. KClO 3 Mg(OH) 2 Al 2 (SO 4 ) 3 2Al(NO 3 ) 3 K, 1 Cl, 1 O 3 Mg, 1 O, 2 H 2 Al, 2 S, 3 O 12 Al, 2 N, 6 O 18 main menu
20 You Try It Determine the number of each atom present in each of the following. AlPO 3 Ba(NO 3 ) 2 HC 2 H 3 O 2 3Fe 3 (PO 4 ) 2 Al, 1 P, 1 O 3 Ba, 1 N, 2 O 6 H, 4 C, 2 O 2 Fe, 9 P, 6 O 24 main menu
21 Identifying Balanced Chemical Equations An equation in which the number of atoms of each element is the same on both sides of the equation is called a balanced chemical equation. Pb(NO 3 ) 2 + 2KI PbI 2 + 2KNO 3 Reactant Side Element Product Side 1 Pb 1 2 N 2 6 O 6 2 K 2 2 I 2 main menu
22 You try it: Handout Balancing Practice I Worksheet 15 minutes. GO!
23 Balancing Chemical Equations Example: Mg + 2HCl MgCl 2 + H 2 What coefficient must be added in front of HCl in order to balance the chlorine and the hydrogen? main menu
24 Ex. 1: 1 Mg + 2 HCl 1 MgCl H 2 1 Mg 12 H 1 Mg 2 H 12 Cl 2 Cl Ex. 2: 2 KClO 3 2 KCl + 3 O 2 21 K 21 Cl 63 O 12 K 12 Cl 26 O
25 Writing Balanced Chemical Equations If the skeleton equation is not written for you, you must write your own. Example** When an electric current is passed through water, the water molecules break down to produce hydrogen and oxygen. Bubbles of each gas are evidence of the reaction. 2H 2 O(l) 2H 2 (g) + O 2 (g) main menu
26 You Try It Write a balanced equation for each of the following reactions. **When magnesium metal and oxygen gas react, the product is solid magnesium oxide. 2Mg(s) + O 2 (g) 2 MgO(s) **When nitrogen and hydrogen gas react, the product is ammonia gas. N 2 (g) + 3H 2 (g) 2NH 3 (g) main menu
27 Challenge: **Writing Balanced Chemical Equations Example 2. Solutions of aluminum sulfate and barium chloride react to produce solid barium sulfate and aqueous aluminum chloride. aluminum sulfate = Al 3+, SO 4 2- = Al 2 (SO 4 ) 3 barium chloride = Ba 2+, Cl - = BaCl 2 barium sulfate = Ba 2+, SO 4 2- = BaSO 4 aluminum chloride = Al 3+, Cl - = AlCl 3 Al 2 (SO 4 ) 3 (aq) + 3BaCl 2 (aq) 3BaSO 4 (s) + 2 AlCl 3 (aq) main menu
28 You Try It Write a balanced equation for each of the following reactions. **Aluminum metal reacts with oxygen gas to produce solid aluminum oxide. 4Al(s) + 3O 2 (g) 2 Al 2 O 3 (s) **Solutions of calcium chloride and sodium sulfate react to produce aqueous sodium chloride and solid calcium sulfate. CaCl 2 (aq) + Na 2 SO 4 (aq) 2 NaCl(aq) + CaSO 4 (s) main menu
29 Homework/DO NOW: 14 practice problems TO BE TURNED IN when completed
30 [[you need a computer]] Room code: KILBANESTP Enter your name
31
32 Types of Reactions 1. Synthesis A + B AB 2. Decomposition AB A + B 3. Single Replacement A + BC B + AC 4. Double Replacement AB + CD CB + AD 5. Combustion Reaction C x H y + O 2 CO 2 + H 2 O
33 Synthesis (Combination) Reactions two substances either elements or compounds combine to form a single compound. The general equation for a synthesis reaction is: A + B C chemical reactions menu
34 Practice: Synthesis Reactions Write the product and balance the equation. Remember, if you have a metal + nonmetal, you have to balance the charges!!! 1) H 2 + O ) Zn + S 3) H 2 + Cl 2 ZnS Zn 2+ S 2- Zn 2+ S H 2 O HCl H + Cl - H + Cl - 4) K(s) + Cl 2 (g) 2 KCl K + Cl - K + Cl - Balanced 5) N 2 + H NH 3 ammonia
35 II. Decomposition Reaction: A compound breaks down into simpler products. AB A + B 2 HgO 2 Hg + O 2 Diatomic
36 Metal Carbonates: break down into the metal oxide and carbon dioxide. CaCO 3 CaO + CO 2 Ca 2+ O 2- Na 2 CO 3 Na 2 O + CO 2 Na + O 2- PbCO 3 PbO + CO 2 Pb 2+ O 2-
37 III. Single Replacement Reaction One element replaces another element. Remember: The positive ion always goes with the negative ion! A + BC B + AC
38 A) Metal replaces Metal Cu + AgNO 3 Cu(NO 3 ) 2 + Ag Cu 2+ Ag + NO 3 1- Cu 2+ NO 3 1- Ag + Pos. ion goes with neg. ion! B) Nonmetal replaces Nonmetal Br 2 + KI KBr + I 2 Br 1- K + I 1- K + Br 1- I 1- Diatomic
39 Double Replacement Solutions of ionic compounds trade ions Outside two go together; Inside two go together. (+ion with ion) AB + CD CB + AD
40 Double-Replacement Reactions KBr + NaCl KCl + NaBr MgCl 2 + 2LiF MgF 2 + 2LiCl HCl + NaOH NaCl + H 2 O (This is an example of a special type of double-replacement reaction known as an acid-base neutralization reaction.) chemical reactions menu
41 Combustion Reactions A burning of a hydrocarbon compound in oxygen produces carbon dioxide and water. C x H y + O 2 (g) CO 2 + H 2 O
42 Complete Combustion Reactions CH 4 + 2O 2 CO 2 + 2H 2 O 2C 3 H 7 OH + 9O 2 6CO 2 + 8H 2 O chemical reactions menu
43 Welcome to FRIDAY! Make sure you picked up the handout by the door.
44 Practice Sheet: your options Single replacement Double replacement Synthesis Decomposition Acid-base neutralization Combustion YOU HAVE 10 MINUTES. MAY THE ODDS BE EVER IN YOUR FAVOR
45 35 minutes of PUTTING IT TOGETHER: Complete and balance the following equations. Label the type of reaction. 1. 2HgO 2Hg + O C 5 H O 2 10CO H 2 O 3. AgNO 3 + NaCl Decomposition Combustion Double-Replacement AgCl + NaNO Li + N 2 2Li 3 N Synthesis 5. 2K + Ba(C 2 H 3 O 2 ) 2 2KC 2 H 3 O 2 + Ba 6. 2H 2 O 2H 2 + O 2 Decomposition 7. Mg(NO 3 ) 2 + 2KOH Mg(OH) 2 + 2KNO C 6 H O 2 12CO H 2 O Combustion 9. 2Al + 3S Al 2 S 3 Synthesis 10. 3F 2 + 2AlCl 3 2AlF 3 + 3Cl 2 Single-Replacement Double-Replacement Single-Replacement main menu
46 Activity Series Not all single-replacement reactions will occur. Mg + ZnCl 2 Zn + MgCl 2 MgCl 2 + Zn No Reaction How can you determine if a single-replacement reaction will occur or not? main menu
47 Activity Series of Metals Whether or not a singlereplacement reaction will occur can be determined by using an activity series. The activity series of metals lists metals in order of chemical reactivity. A reactive metal will replace any metal found below it in the activity series. WRITE THIS DOWN! main menu
48 Activity Series of Halogens The halogens can also take place in single-replacement reactions. The order of reactivity for the halogens from highest to lowest reactivity: is fluorine, chlorine, bromine, iodine. Activity of Halogens F 2 Cl 2 Br 2 I 2 main menu
49 Single-Replacement Reactions Increasing activity Activity of Halogens F 2 Cl 2 Br 2 I 2 Will the first element replace the second? Remember: In order to replace an element, the first element (reactant) has to be HIGHER on the activity series then the second 1.Mg Ag 2.Br F 3.Pb Cu 4.Cl I Yes No Yes Yes main menu
50 Single-Replacement Reactions Use the activity series to determine whether or not the following reactions will occur. If the reaction will occur spontaneously, complete and balance the reaction. If it does not occur, write no reaction. 1. Zn + Na 2 O No Reaction 2. Li + AgNO 3 3. Fe + CuSO 4 Ag + LiNO 3 Cu + FeSO 4 4. Cl 2 + 2KBr 2KCl + Br 2 main menu
51 The equation says no reaction, plus the picture shows that nothing is happening. That must mean WHAT? The metal ion originally in the solution is MORE reactive (higher on the activity series list) then the metal that was dropped into the solution. You could also say that the metal dropped into the solution was lower on the list than the original metal.
52 In order to replace hydrogen, the unknown element must be ABOVE the known element. Nickel is the only metal listed that is above Hydrogen on the list (gold is below)
53 I need you to FOCUS today! We have a LOT to do!!! Please make sure you have the pink half sheet
54 Oxidation-Reduction Reactions (Redox) Oxidation-Reduction reactions occur when electrons are transferred between reactions. Examples include: the burning of gasoline and the rusting of a nail. main menu
55 Oxidation Oxidation originally meant the combination of an element with oxygen to give oxides. However, today it is defined as: the loss of electrons. (Oxygen does not have to be present for oxidation to occur.) main menu
56 Reduction Reduction originally meant the loss of oxygen from a compound. Today it is defined as: the gain of electrons. main menu
57 Helpful Mnemonics Leo the Lion says Ger L Loss e of electrons o is oxidation G Gain e of electrons r is reduction main menu
58 Helpful Mnemonics OIL RIG O Oxidation R Reduction I Is I Is L LOSS G Gain main menu
59 TIPS for Assigning Oxidation Numbers 1. The oxidation number of a monatomic ion (by itself) is equal to its given charge. Examples: Br - equals Fe 3+ equals main menu
60 Rules for Assigning Oxidation Numbers 2. For a polyatomic ion, the sum of the oxidation numbers must equal the ionic charge of the ion. Examples: SO 4 2- equals NO 3- equals -2-1 main menu
61 Rules for Assigning Oxidation Numbers 3. The oxidation number of a metal cation is the same as its ionic charge. Examples: sodium ion is calcium ion is main menu
62 Rules for Assigning Oxidation Numbers 4. The oxidation number of hydrogen in a compound is usually +1. Exception: In metal hydrides, (ex. NaH) hydrogen is -1. main menu
63 Rules for Assigning Oxidation Numbers 5. The oxidation number of oxygen in a compound is usually -2 Exception: In peroxides (ex. H 2 O 2 ) oxygen is -1. main menu
64 Rules for Assigning Oxidation Numbers 6. The oxidation number of an uncombined element is 0. For example, the oxidation number of the potassium atoms in potassium metal, K, and of the nitrogen atoms in nitrogen gas, N 2, is zero. main menu
65 Rules for Assigning Oxidation Numbers 7. For any neutral compound, the sum of the oxidation numbers of the atoms in the compound must equal 0. main menu
66 Rules for Assigning Oxidation Numbers When assigning oxidation numbers to the elements in neutral compound or ion (positive + negative), assign them in the following order: 1. Lone elements (not in a compound): 0 2. metal use the charge from the periodic table 3. hydrogen +1 (or -1 in metal hydrides) 4. oxygen -2 (or -1 in peroxides) 5. everything that is left over
67 1. What is the oxidation number of each element in the following? +4-2 SO 2 S = +4 O= =0 main menu
68 2. What is the oxidation number of each element in the following? KClO =0 K = +1 O= -2 Cl = +5 main menu
69 3. What is the oxidation number of each element in the following? KClO =0 K = +1 O= -2 Cl = +3 main menu
70 4. What is the oxidation number of each element in the following? +4-2 CO 3 2- C = +4 O= = -2 main menu
71 You Try It. Determine the oxidation number of each element in each of the following on your own. 5. Na 2 Cr 2 O 7 Na = +1 Cr = +6 O= BaH 2 Ba = +2 H = (Hint: BaH 2 is a metal hydride.) Li 2 O 2 Li = +1 O = -1 (Hint: Li 2 O 2 is a peroxide.) 8. ClO - 3 Cl = +5 O = -2 main menu
72 Oxidation Number Changes The changes in oxidation number can be used to determine which elements are oxidized and which elements are reduced. Remember an increase in the oxidation number of an atom signifies oxidation and a decrease in the oxidation number signifies reduction. main menu
73 Oxidation Number Changes Use the change in oxidation number to identify which elements are oxidized and reduced in each of these reactions F 2 (g) + 2HBr(aq) 2HF(aq) + Br 2 (l) +1-1 = =0 Fluorine: 0 to -1; reduced Bromine: -1 to 0; oxidized main menu
74 Oxidation Number Changes Use the change in oxidation number to identify which elements are oxidized and reduced in each of these reactions. Also identify the oxidizing (OA) and reducing (RA) agents SO 3 (g) + H 2 O(l) H 2 SO 4 (aq) = = =0 Since there is no change in oxidation number, this is not a redox reaction. main menu
75 Oxidation Number Changes Use the change in oxidation number to identify which elements are oxidized and reduced in each of these reactions. Also identify the oxidizing (OA) and reducing (RA) agents KClO 3 (s) 2KCl(s) + 3O 2 (g) = =0 Chlorine: +5 to -1; reduced Oxygen: -2 to 0; oxidized main menu
76 You Try It Use the change in oxidation number to identify which elements are oxidized and reduced in each of these reactions. Also identify the oxidizing (OA) and reducing (RA) agents H 2 (g) + O 2 (g) 2H 2 O(g) +2-2 =0 hydrogen: 0 to +1; oxidized oxygen: 0 to -2; reduced main menu
77 You Try It Use the change in oxidation number to identify which elements are oxidized and reduced in each of these reactions. Also identify the oxidizing (OA) and reducing (RA) agents Al(s) + 6HCl(aq) 2AlCl 3 (s) + 3H 2 (g) +1-1= =0 aluminum: 0 to +3; oxidized hydrogen: +1 to 0; reduced main menu
78 You Try It
79 You Try It DO MORE
80 OH SNAP! Last day before the EXAM! Today s agenda: 1. Double Replacement and Solubility Rules (you need a purple chart if you don t have one yet) 2. Solubility Practice 3. Test Review Announcements: Our exam is on WEDNESDAY Feb. 17 th Please check your home access to determine what you re missing. The 6 weeks ends on Friday Feb. 19th
81 Soluble and Insoluble Salts Ionic compounds that dissolve in water are soluble salts do not dissolve in water are insoluble salts 82
82 Solubility Rules Soluble salts typically contain at least one ion from Groups 1A(1), NO 3, or C 2 H 3 O 2 (acetate). Most other combinations are insoluble. You have this chart (or you should). Yours is purple!! 83
83 How do you use this crazy looking thing?>! 1. Look at the second element/ion in the given compound. NaOH 2. Find in under soluble or insoluble NaOH OH is insoluble, unless it s paired with an exception. 3. Check to see if it is paired with an exception. If it IS with an exception, it becomes the opposite (soluble becomes insoluble) NaOH Na is an alkali metal, which means that it s an exception. This means that NaOH is SOLUBLE!!
84 Learning Check Use the solubility rules to determine if each salt is: (S) soluble or (I) insoluble. A. Na 2 SO 4 B. MgCO 3 C. PbCl 2 Soluble Insoluble Insoluble D. MgCl 2 Soluble 85
85 For the rest of the period: you are to work on your study guide. This will be EXTRA CREDIT if you complete it and turn it in on test day.
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