Chapter 5 Chemical Reactions and Quantities. Type of Reactions. Formation of MgO. Combination. Decomposition of HgO. Decomposition
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1 Chapter 5 Chemical Reactions and Quantities Type of Reactions 5.3 Types of Reactions Chemical reactions can be classified as Combination reactions. Decomposition reactions. Single Replacement reactions. Double Replacement reactions. 1 Combination 2 Formation of MgO In a combination reaction, Two or more elements (or simple compounds) combine to form one product A + B A B 2Mg(s) + O2(g) 2MgO(s) 2Na(s) + Cl2(g) 2NaCl(s) SO3(g) + H2O(l) H2SO4(aq) 3 Decomposition 4 Decomposition of HgO In a decomposition reaction, One substance splits into two or more simpler substances. 2HgO(s) 2Hg(l) + O2(g) 2KClO3(s) 2KCl(s) + 3O2(g) 5 6 1
2 Single Replacement In a single replacement reaction, One element takes the place of a different element in a reacting compound. Classify the following reactions as 1) combination or 2) decomposition: A. H2(g) + Br2(g) 2HBr(l) B. Al2(CO3)3(s) Al2O3(s) + 3CO2(g) C. 4Al(s) + 3C(s) Al4C3(s) Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Fe(s) + CuSO4(aq) FeSO4(aq) + Cu(s) 7 Zn and HCl is a Single Replacement Reaction 8 Double Replacement In a double replacement, Two elements in the reactants exchange places. AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) ZnS(s) ZnCl2(aq) + H2S(g) + 2HCl(aq) 9 Example of a Double Replacement 10 Classify the following reactions as 1) single replacement 2) double replacement 11 A. 2Al(s) + 3H2SO4(aq) Al2(SO4)3(s) + 3H2(g) B. Na2SO4(aq) + 2AgNO3(aq) Ag2SO4(s) + 2NaNO3(aq) C. 3C(s) + Fe2O3(s) 2Fe(s) + 3CO(g) 12 2
3 Identify each reaction as 1) combination 2) decomposition 3) single replacement 4) double replacement Chapter 5 Chemical Reactions and Quantities 5.4 Oxidation-Reduction Reactions A. 3Ba(s) + N 2 (g) Ba 3 N 2 (s) B. 2Ag(s) + H 2 S(aq) Ag 2 S(s) + H 2 (g) C. SiO 2 (s) + 4HF(aq) SiF 4 (s) + 2H 2 O(l) D. PbCl 2 (aq) + K 2 SO 4 (aq) 2KCl(aq) + PbSO 4 (s) E. K 2 CO 3 (s) K 2 O(aq) + CO 2 (g) Oxidation and Reduction Electron Loss and Gain An oxidation-reduction reaction Provides us with energy from food. Provides electrical energy in batteries. Occurs when iron rusts. 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) An oxidation-reduction reaction Transfers electrons from one reactant to another. A Loss of Electrons is Oxidation Zn(s) Zn 2+ (aq) + 2e - (LEO) A Gain of Electrons is Reduction (GER) Cu 2+ (aq) + 2e - Cu(s) Oxidation and Reduction Zn and Cu 2+ oxidation Zn(s) Zn 2+ (aq) + 2e- Silvery metal Cu 2+ (aq) + 2e- Blue reduction Cu(s) orange
4 Electron Transfer from Zn to Cu 2+ Oxidation: electron loss Identify each of the following as 1) oxidation or 2) reduction: A. Sn(s) Sn 4+ (aq) + 4e B. Fe 3+ (aq) + 1e Fe 2+ (aq) C. Cl 2 (g) + 2e 2Cl - (aq) Reduction: electron gain Writing Oxidation and Reduction Reactions Write the separate oxidation and reduction reactions for the following equation. 2Cs(s) + F 2 (g) 2CsF(s) Each cesium atom loses an electron to form cesium ion. 2Cs(s) 2Cs + (s) + 2e oxidation Fluorine atoms gain electrons to form fluoride ions. F 2 (s) + 2e - 2F (s) reduction In light-sensitive sunglasses, UV light initiates an oxidation-reduction reaction. uv light Ag + + Cl Ag + Cl A. Which reactant is oxidized? B. Which reactant is reduced? Identify the substances that are oxidized and reduced in each of the following reactions: TYPES OF CHEMICAL REACTIONS Chemical reactions are often classified into categories according to characteristics of the reactions. The following is a useful classification scheme: A. Mg(s) + 2H + (aq) Mg 2+ (aq) + H 2 (g) B. 2Al(s) + 3Br 2 (g) 2AlBr 3 (s) 23 4
5 Chapter 5 Chemical Reactions and Quantities 5.5 The Mole Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans A Mole of Atoms A mole is a collection that contains The same number of particles as there are carbon atoms in 12.0 g of carbon 12 C x atoms of an element (Avogadro s number). 1 mole element Number of Atoms 1 mole C = 6.02 x C atoms 1 mole Na = 6.02 x Na atoms 1 mole Au = 6.02 x Au atoms A Mole of a Compound A mole Of a covalent compound has Avogadro s number of molecules. 1 mole CO 2 = 6.02 x CO 2 molecules 1 mole H 2 O = 6.02 x H 2 O molecules Of an ionic compound contains Avogadro s number of formula units. 1 mole NaCl = 6.02 x NaCl formula units 1 mole K 2 SO 4 = 6.02 x K 2 SO 4 formula units Particle in One-Mole Samples Avogadro s Number TABLE 5.3 Avogadro s number 6.02 x can be written as an equality and two conversion factors. Equality: 1 mole = 6.02 x particles Conversion Factors: 6.02 x particles and 1 mole 1 mole 6.02 x particles
6 Using Avogadro s Number Avogadro s number is used to convert moles of a substance to particles. How many Cu atoms are in 0.50 mole Cu? Using Avogadro s Number Avogadro s number is used to convert particles of a substance to moles. How many moles of CO 2 are in 2.50 x molecules CO 2? 0.50 mole Cu x 6.02 x Cu atoms 1 mole Cu = 3.0 x Cu atoms 2.50 x molecules CO 2 x 1 mole CO x molecules CO 2 = 4.15 moles CO Subscripts and Moles 1. The number of atoms in 2.0 moles Al is A. 2.0 Al atoms B. 3.0 x Al atoms C. 1.2 x Al atoms 2. The number of moles of S in 1.8 x atoms S is A. 1.0 mole S atoms B. 3.0 moles S atoms C. 1.1 x moles S atoms The subscripts in a formula give The relationship of atoms in the formula. The moles of each element in 1 mole of compound. Glucose C 6 H 12 O 6 In 1 molecule: 6 atoms C 12 atoms H 6 atoms O In 1 mole: 6 moles C 12 moles H 6 moles O Subscripts State Atoms and Moles Factors from Subscripts Subscripts used for conversion factors Relate moles of each element in 1 mole compound. For aspirin C 9 H 8 O 4 can be written as: 9 moles C 8 moles H 4 moles O 1 mole C 9 H 8 O 4 1 mole C 9 H 8 O 4 1 mole C 9 H 8 O 4 and 1 mole C 9 H 8 O 4 1 mole C 9 H 8 O 4 1 mole C 9 H 8 O 4 9 moles C 8 moles H 4 moles O 1 mole C 9 H 8 O 4 = 9 moles C 8 moles H 4 moles O
7 A. How many moles O are in mole aspirin C 9 H 8 O 4? 5.6 Molar Mass The molar mass is The mass of one mole of a substance. The atomic mass of an element expressed in grams. B. How many O atoms are in mole aspirin C 9 H 8 O 4? Molar Mass of CaCl 2 Give the molar mass to the nearest 0.1 g. A. K = For a compound, the molar mass is the sum of the molar masses of the elements in the formula. We calculate the molar mass of CaCl 2 to the nearest 0.1 g as follows. B. Sn = Element Number of Moles Atomic Mass Total Mass Ca g/mole 40.1 g Cl g/mole 71.0 g CaCl g Molar Mass of K 3 PO 4 Determine the molar mass of K 3 PO 4 to 0.1 g. Calculate the molar mass to the nearest 0.1g A. K 2 O = g Element Number of Moles Atomic Mass Total Mass in K 3 PO 4 K g/mole g P g/mole 31.0 g O g/mole 64.0 g K 3 PO g B. Al(OH) 3 = g
8 Conversion Factors from Molar Mass Prozac, C 17 H 18 F 3 NO, is an antidepressant that inhibits the uptake of serotonin by the brain. What is the molar mass of Prozac? 1) 40.0 g/mole 2) 262 g/mole 3) 309 g/mole Methane CH 4 known as natural gas is used in gas cook tops and gas heaters. 1 mole CH 4 = 16.0 g The molar mass of methane can be written as conversion factors g CH 4 and 1 mole CH 4 1 mole CH g CH Calculations Using Molar Mass Acetic acid C 2 H 4 O 2 gives the sour taste to vinegar. Write two molar mass conversion factors for acetic acid. Mole factors are used to convert between the grams of a substance and the number of moles. Grams Mole factor Moles Calculating Grams from Moles Aluminum is often used for the structure of lightweight bicycle frames. How many grams of Al are in 3.00 moles of Al? 3.00 moles Al x 27.0 g Al = 81.0 g Al 1 mole Al mole factor for Al The artificial sweetener aspartame (Nutri-Sweet) C 14 H 18 N 2 O 5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 g of aspartame?
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