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1 Firrst Last N Name P Per_____ _ Score ____/____ _ 11Ch hemical +1R + Rxn’s Æ Æ1Ch11R Rx _______________ __________ ___________ __________ __________________________________________________ om_______ ____ Syntthesis or Co Basic Pattern R Ro_ ____ _+ S___ S __ Æ A+B BÆ __________ ________ _______ _______ ____________________________________ Dec compositio on R R___ ____ ___y y Æ + ABÆ Æ __________ ________ _______ _______ ____________________________________ Sing gle Replacement + ÆB Æ _______yy + R R____ A + BC Æ __________ ________ _______ _______ ____________________________________ Dou uble Replac cement ÆR___ ____+ B___ ____ AAB + CDÆ Æ + ____ ____________ ___________ ___________ ___________ ____________ ___________ ___________ ___________ ____________ _ Com mbustion + O2 Æ C ____ __ + H ____ __ ___ _______ ________ _______ ________ _______ _______ ________ _______ _______ 1 05_CTR_ch11 7/9/04 3:33 PM Page 265 2 Name ___________________________ 11.1 Date ___________________ Class __________________ DESCRIBING CHEMICAL REACTIONS Section Review Objectives • Explain how to write a word equation • Describe how to write a skeleton equation • List the steps for writing a complete chemical equation Vocabulary • chemical equation • skeleton equation • catalyst • coefficients • balanced equation Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. A chemical reaction can be concisely represented by a chemical 1. 1 . The substances that undergo a chemical change are the 2. 2 . The new substances formed in a chemical reaction are the 3. 3 . In accordance with the law of conservation of 4 , 4. a chemical equation must be balanced. When balancing an equation, you place 5 5. in front of reactants and products so 6 that the same number of atoms of each 6. are on each side of 7. the equation. An equation must never be balanced by changing the 8. 7 in the chemical formula of a substance. 9. Special symbols are used to show the physical state of a substance in a reaction. The symbol for a liquid is a solid, 9 ; and for a gas, in water is designated 11 10 . If a 8 10. ; for 11. . A substance dissolved 12. 12 is used to increase the rate of a chemical reaction, its formula is written above the arrow. 2 Chapter 11 Chemical Reactions 265 05_CTR_ch11 7/9/04 3:33 PM Page 266 Name ___________________________ 3 Date ___________________ Class __________________ Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 13. In an equation, a substance is shown to be in the gaseous state by placing an upward-pointing arrow after its formula. ________ 14. The symbol placed over the arrow in an equation means that heat is supplied to the reaction. ________ 15. Atoms are destroyed in a chemical reaction. ________ 16. A skeleton equation is not a balanced equation. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B a. an equation in which each side has the same number of atoms of each element ________ 18. skeleton equation b. a substance that speeds up the rate of a reaction ________ 19. catalyst c. a symbolic way of describing a chemical reaction ________ 20. coefficients d. substances that undergo chemical change ________ 21. balanced equation e. a chemical equation that does not indicate the amounts of substances involved ________ 22. reactants f. new substances formed in a chemical reaction ________ 23. products g. numbers used to balance a chemical equation Part D Questions and Problems Answer the following in the space provided. 24. Write a balanced equation for each of these chemical reactions. Include appropriate symbols from Table 11.1. a. Aluminum reacts with aqueous hydrochloric acid to form hydrogen gas and aqueous aluminum chloride. b. Acetylene gas (C2H2) burns in a welding torch with oxygen to form carbon dioxide gas and water vapor. 266 Core Teaching Resources 3 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 17. chemical equation 05_CTR_ch11 7/9/04 3:33 PM Page 267 4 Name ___________________________ Date ___________________ Class __________________ TYPES OF CHEMICAL REACTIONS 11.2 Section Review Objectives • Describe the five general types of reactions • Predict the products of the five general types of reactions Vocabulary • combination reaction • decomposition reaction • single-replacement reaction • activity series • double-replacement reaction • combustion reaction Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1 It is possible to the products of some chemical 1. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. reactions. In order to do this, you must be able to recognize at least five general types of reactions. For example, in a 3 the reactants are two or more 4 there is always a 2 reaction, and/or compounds and 5 3. 4. reaction, a single 5. compound is broken down into two or more simpler substances. 6. In a 6 product. In a 2. reaction, the reactants and products are an 7 element and a compound. The 7. can be used to predict 8. whether most single-replacement reactions will take place. A 8 9. reaction involves the exchange of ions between two 10. compounds. This reaction generally takes place between two ionic compounds in 9 combustion reaction is solution. One of the reactants in a 10 11. 12. . The products of the complete combustion of a hydrocarbon are 11 and 4 12 . Chapter 11 Chemical Reactions 267 05_CTR_ch11 7/9/04 3:33 PM Page 268 Name ___________________________ 5 Date ___________________ Class __________________ Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 13. In a decomposition reaction, there is a single reactant. ________ 14. The activity series of metals can be used to predict products in doublereplacement reactions. ________ 15. Carbon dioxide and water are the products of the combustion of hexane (C6H14). ________ 16. A nonmetal can replace another nonmetal from a compound in a single-replacement reaction. ________ 17. One of the products of a double-replacement reaction is a gas that bubbles out of the mixture. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B a. reaction in which atoms of one element replace atoms of a second element in a compound ________ 19. decomposition reaction b. a reaction in which two or more substances combine to form a single substance ________ 20. single-replacement reaction c. reaction of a compound with oxygen to produce energy ________ 21. combustion reaction d. reaction in which a single compound is broken down into two or more products Part D Questions and Problems Answer the following in the space provided. 22. Identify the type of each of the following reactions. a. 2C6H14(l ) 19O2(g) y 12CO2(g) 14H2O(g ) b. 2Fe(s) 3Br2(l ) y 2FeBr3(s) 23. Complete and balance the following equation. What must be true of one of the products? Li3PO4 Zn(NO3)2 y 268 Core Teaching Resources 5 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 18. combination reaction 6 11 BALANCING CHEMICAL EQUATIONS Directions:. Label decomposition, synthesis (combination), single displacement, double displacement (or double replacement), combustion reaction or Neutralization (acid/base). Balance the Chemical Equation Reaction Type 1. 2 K + 1 Cl2 → 2 KCl COMBINATION 2. __SO2 + __O2 → __SO3 ________________ 3. __KClO3 → __KCl + __O2 ________________ 4. __CO2 + __C → __CO ________________ 5. __H2 + __O2 → __H2O ________________ 6. __MgCO3 → __MgO + __O2 ________________ 7. __H2O + __Cs → __CsOH + __H2 ________________ 8. __Fe2O3 + __Al → __Fe + __Al2O3 ________________ 9. __PbCl2 + __Li2SO4 → __PbSO4 + __LiCl ________________ 10. __NaOH + __H2SO4 → __Na2SO4 +__H-OH ________________ 12. __Pb(OH)2 +__HCl Æ __PbCl2 +__H-OH ________________ 13. __Na2CO3 + __HCl Æ__H2CO3 +__NaCl ________________ 14. __AgNO3 + __Cu → __Ag + __Cu(NO3)2 ________________ 15. __CH4 + __O2 → __CO2 + __H2O ________________ 16. __C2H6 + __O2 → __CO2 + __H2O ________________ 17. __C3H8 + __O2 → __CO2 + __H2O ________________ 18. __C4H10 + __O2 → __CO2 + __H2O ________________ 19. __C5H12 + __O2 → __CO2 + __H2O ________________ Bonus: Don’t unless given permission. Use decimal method if needed, for example “1.5 O2.” 20. __C7H5N3O6 + __O2 → __ CO2 + __ H2O + __ N2 __ __ __ 6 __ __ ____________ 7 How To Write & Balance Chemical Reactions Equations must be balanced Atoms can be neither created nor destroyed in an ordinary chemical reaction, so there must be the same number of atoms on both sides of the equation. These numbers are found in a chemical equation 2H2 + O2 2H2O Subscripts Coefficients The small numbers to the lower right of chemical symbols. Subscripts represent the number of atoms of each element in the molecule. The large numbers in front of chemical formulas. Coefficients represent the number of molecules of the substance in the reaction. Balancing Equations By Inspection 1. 2. 3. 4. 5. 6. Balance Metals Balance Nonmetals Balance Ions Balance Oxygen Balance Hydrogen DOUBLE CHECK DIRECT COMBINATION REACTIONS A + B AB (also called “synthesis reactions”) A. In the Haber process, nitrogen gas and hydrogen gas are combined under high temperature and pressure to form ammonia (NH3). B. One of the rare reactions among the noble gasses that have been discovered is the formation of solid xenon tetrafluoride from the combination of xenon and fluorine gas. 7 8 C. Pure magnesium metal is burned to form magnesium oxide, a fine white Powder. D. Sodium metal and chlorine gas react to form table salt. E. Iron nails rust to form ferric oxide. F. Phosphorus is mixed with chlorine gas to form phosphorus pentachloride (PCl5) G. Water is added to ammonia to yield ammonium hydroxide. DECOMPOSITION REACTIONS AB A + B E. Electricity is run through water, liberating oxygen gas and hydrogen gas. F. Hydrogen peroxide decomposes in the presence of a catalyst (manganese), to liberate oxygen gas, leaving only water behind. HYDROCARBON COMBUSTION CnH2n+2 + O2 H2O + CO2 Methane CH4 Hexane C6H14 Ethane C2H6 Heptane C7H16 Propane C3H8 Octane C8H18 Butane C4H10 Nonane C9H20 Pentane C5H12 Decane C10H22 G. Combustion of methane H. Combustion of butane 8 I. Combustion of propane 9 SINGLE REPLACEMENT REACTIONS A + BC AB + C J. When Copper metal is added to silver nitrate, pure silver is deposited and a blue solution of copper (I) nitrate remains. K. (find one in the book or internet) L. Lead (II) sulfide is heated in the presence of oxygen to form solid lead (II) oxide and sulfur dioxide gas. DOUBLE REPLACEMENT REACTIONS AB + CD AC + BD M. Solid carbon is added to aluminum oxide in order to form pure aluminum metal and carbon dioxide gas. N. If solutions of potassium chromate and barium chloride are mixed, a bright yellow solid called barium chromate is formed, leaving potassium chloride in solution. O. Hydrochloric acid is added to sodium hydroxide to produce water and sodium chloride. P. (find one in the book or internet) 9 10Name Date Period ________ 11 Writing & balancing Chemical Reactions Here are some sample reactions. Can you write the unbalanced reaction? What type of reaction is taking place? (advanced: balance the rx's) 1. sulfur trioxide and water combine to yield sulfuric acid. 2. lead(II) nitrate and sodium iodide react to yield lead iodide and sodium nitrate. 3. calcium fluoride and sulfuric acid yield calcium sulfate and Hydrofluoric acid. 4. Sodium metal and chlorine gas yield sodium chloride. 5. ammonia gas, when bubbled into water, will yield ammonium hydroxide. 6. ethane is burned in oxygen to yield carbon dioxide and water. 7. zinc sulfide and oxygen yields zinc oxide and sulfur. 8. Aluminum metal reacts with Calcium oxide to produce calcium metal and aluminum oxide. 9. aluminum hydroxide and sulfuric acid yields water and aluminum sulfate. 10. Silver (I) nitrate reacts with copper metal to yield silver metal and copper (I) nitrate. 11. barium hydroxide and sulfuric acid yield water and barium sulfate. 12. aluminum sulfate and calcium hydroxide react to form aluminum hydroxide and calcium sulfate. 10 11 Combustion of Hydrocarbons A hydrocarbon is formed when a central carbon atom (or chain of carbon atoms) bond with hydrogen atoms. The simplest hydrocarbons are the alkanes, with a general formula of ... CnH2n + 2 For example, what is the formula for an alkane hydrocarbon with 3 carbons? Solution: Fill in the above general formula with the new numbers as follows: C3H(2 x 3) + 2 = C3H8 Alkanes are named as follows: n= Formula Name Acronym New Acronym 1 CH4 methane Mother M__________ 2 ethane eats E__________ 3 propane peanut P__________ 4 butane butter B__________ 5 pentane pizza. P_________ 6 hexane Hence H__________ 7 heptane her H__________ 8 octane office O__________ 9 nonane never N__________ 10 decane dines D__________ Most hydrocarbons, including all the alkanes undergo combustion (burning in oxygen) to form Carbon dioxide and water. For example, write the formula for the combustion of ethane: C3H8 + O2 CO2 + H2O 3CO2 + 4H2O Now, we just need to balance the reaction. C3H8 + 5O2 COMMON ACIDS Hydrochloric acid Hydrobromic acid Hydroiodidic acid Hydrofluoric acid Sulfuric acid Acetic acid HCl HBr HI HF H2SO4 HCH3CO Nitric acid Phosphoric acid Citric acid Carbonic acid Formic acid 11 HNO3 H3PO4 H3C6H5O7 H2CO3 HCO2H 12 Name Date Period Writing and balancing Chemical Reactions Here are some sample reactions. First write the chemical reaction, then determine the type of reaction taking place. Finally, balance the reaction. 1. Carbon dioxide and water combine to yield carbonic acid. CO2 + H2O H2CO3 2. Carbon disulfide reacts with oxygen to form carbon dioxide and sulfur dioxide. 3. When heated, calcium carbonate yields carbon dioxide and calcium oxide. 4. Calcium fluoride reacts with sulfuric acid to form calcium sulfate and hydrogen fluoride. 5. Lithium oxide reacts with water to form lithium hydroxide. 6. Pentane burns. 7. When water is exposed to electricity, oxygen and hydrogen are formed. 8. Aluminum reacts with iron (II) nitrate to form aluminum nitrate and iron. 9. Hydrochloric acid reacts with ammonium hydroxide. 12 13 10. Sodium reacts with bromine to form sodium bromide. 11. Decane burns. 12. When heated, potassium chlorate forms potassium chloride and oxygen. 13. Magnesium burns to form magnesium oxide. 14. Aluminum reacts with fluorine to form aluminum fluoride. 15. Hydrochloric acid reacts with calcium metal to produce calcium chloride and hydrogen gas. Name the following compounds: a. C3H8 b. H2PO4 c. FeCl d. Cu(NO3)2 e. SCl5 f. (NH4)O g. C8H18 h. Mg(OH)2 13 14Name Period Date 11 Writing and balancing Chemical Reactions II Name the following compounds: 1. C6H14 2. HCH3CO2 3. CuCl 4. Al(NO3)3 5. PF4 6. NH4OH 7. CH4 8. Fe(OH)2 IONIC COVALENT Here are some sample reactions. First write the chemical reaction, then determine the type of reaction taking place. Finally, balance the reaction. 9. Sodium metal reacts violently in water to form hydrogen gas and sodium hydroxide. 10. Chlorine gas reacts with magnesium iodide to form magnesium chloride and pure iodine. 11. Iron reacts with copper (II) sulfate to form iron (III) sulfate and pure copper 12. Hydroiodidic acid reacts with calcium hydroxide. 13. Combustion of heptane. 14. Solid iron reacts with chlorine gas to form iron (III) chloride. 15. Carbon monoxide burns to form 14 carbon dioxide. 15 ____________ ___ Predicting Reactions Worksheet 1 Combination Reactions - Predict the product and write balanced reactions for each of the following. 1. Hydrogen burned in oxygen. ___ H2 + ___ O2 Æ ___ H2O 2. Sodium plus iodine. Æ 3. Calcium burned in chlorine. Æ 4. Carbon burned in oxygen. Æ 5. Hydrogen combined with nitrogen. Æ 6. Sulfur burned in air. Æ 7. Magnesium burned in hydrogen. Æ 8. Zinc plus bromine. Æ 9. Water plus carbon dioxide. Æ 10. Sulfur dioxide plus water. Æ 11. Sodium plus hydrogen. Æ 12. Hydrogen burned in chlorine. Decomposition (decombination) - Predict products (if needed) and write balanced reactions for each: If you need to search the net to find the products, you can do that also with permission. 1. The heating of magnesium carbonate to form Magnesium Oxide & Carbon Dioxide. 2. The heating of sodium chlorate to form Sodium Oxide and Dichloro-oxide. 3. The electrolysis of water. __MgCO3(s) Æ __MgO(s) + __ CO2(g) Æ Æ 4. The decomposition of calcium carbonate to form Calcium Oxide and Carbon Dioxide. 5. The heated of mercuric oxide. Æ 6. The electrolysis of sodium chloride. Æ 7. Ferric hydroxide heated. Æ 8. Aluminum hydroxide heated. Æ 9. Sodium carbonate heated. Æ 10. Barium hydroxide heated. Æ 11. The electrolysis of calcium bromide. Æ 12. The heating of carbonic acid. Æ 15 16 WORKSHEET ON SINGLE & DOUBLE REPLACEMENT REACTIONS Predict the products. Write formulas & balance each reaction. If there is no reaction, then just put NO RXN. Single Replacement: A + BC → B + AC or A + BC → C + BA (when A and C are negative ions) 1. Zinc + Hydrogen chloride Æ 2. Magnesium + Hydrogen Sulfate Æ 3. Copper (II) chloride + Flourine Æ 4. Silver + Sodium Hydroxide Æ 5. Potassium iodide + Bromine Æ 6. Calcium + Hydrogen hydroxide Æ 7. Iron IV oxide + Hydrogen Æ Double Replacement: AB + CD Æ AD + CB 1. Barium chloride + Aluminum sulfate Æ 2. Calcium nitride + water Æ 3. Calcium hydroxide + Hydrogen phosphate Æ 4. Hydrogen sulfate + Sodium hydrogen carbonate Æ 5. Calcium hydroxide + Ammonium chloride Æ 6. Potassium iodide + Lead II Nitrate Æ 7. Sodium acetate + Calcium sulfide Æ Complete each word equation, write formulas and balance the reaction equation. Then identify and place the type of reaction (single replacement or double replacement) in the blank provided. 1. Zinc + Silver nitrate → 2. Aluminum + Hydrogen chloride Æ 3. Magnesium oxalate + Ammonium carbonate → 4. Calcium + Aluminum nitrate Æ 5. Potassium flouride + Lead (II) Nitrate → 6. Calcium bromide + Silver nitrate → 7. Ammonium phosphate + Barium acetate → 8. Sodium chloride + Potassium → 9. Magnesium nitrate + ammonium chloride → 10. Iron (III) chlorate + calcium → 11. Chlorine + Sodium bromide → 12. Potassium chloride + Silver nitrate → 13. Calcium hydroxide + Hydrogen nitrate → 14. Lead II nitrate + Potassium chloride Æ 15. Strontium carbonate + Hydrogen nitrate Æ 16. Gold + Potassium nitrate Æ 17. Zinc + Silver nitrate Æ 18. Aluminum + Copper II sulfate Æ 16 17 11-1 Comparing Synthesis and Decomposition Reactions Formative Assessment 1. a. An equation with the “A + B Æ AB” format is which of the following types of reaction? combustion b. synthesis/combination c. c. decomposition 2. a. b. Which of the following reactions is an example of the above unbalanced reactions? H2 + O2 Æ H2O c. CH4 + O2 Æ H2O + CO2 H2O2 Æ H2O+ O2 d. Na + H2O Æ NaOH + H2 3. 4. 5. Which above reaction in #2 is a decomposition reaction? ______________________ Which above reaction is a single replacement reaction? ________________ Which above reaction is a combustion reaction? ______________ Directions - Write the following reactions equation noting the states. For example, note a gas as (g). Then balance the equation by placing coefficients in front of the formula. For example, 2 CO2. 6. Hydrogen gas reacts with oxygen gas to form water vapor? _________ _______ Æ ____________ Score ___/10 11-2 Chemical Reaction Formative Assessment Approaching 1. Circle the letter of the reactions below that are balanced equations. a. 2PbO2 b. (NH4)2CO3 c. PbO + Pb(NO3)2 O2 2NH3 + + 2NaI H2O + CO2 PbI2 + 2NaNO3 + H2O Meets 2. Balance the following equations: Fe3O4 a. Fe + O2 b. C2H6 + O2 CO2 Exceeds 3. Write an equation of the chemical reaction when we burned Magnesium in Oxygen. ______ + _______ Æ _________ Score ___/10 11-2 Writing Equations- Formative Assessment 1. Convert the following unbalanced equation into the written form (See number 2): Methane_______________________________________ CH4 (g) + O2 (g) Æ H2O (g) + CO2 (g) ____________________________________________________________________________________ ____________________________________________________________________________________ 2. Convert the following into a balanced chemical equation: Hydrogen peroxide is catalyzed by Manganese IV Oxide decomposes to form water & Oxygen gas. Æ 3. Which is the correct balanced equation for the combustion of Methane? a. CH4 (g) + O2 (g) Æ H2O (g) + CO2 (g) c. CH4 (g) + 2O2 (g) Æ 2H2O (g) + CO2 (g) b. C2H6 (g) + 3.5 O2 (g) Æ 3H2O (g) + 2CO2 (g) d. C3H8 (g) + 5O2 (g) Æ 4H2O (g) + 3CO2 (g) 4. Balance the following equation by filling in the missing numbers and letters. ___BaO( ) + ____ O2 ( ) Æ ____ BaO ( ) Score ___/10 17 18 ___________________________ First Name, Last ________ Period SCORE: ___/10 pts 11 Chemical Naming Formative Assessment 1 Directions – Circle the best answer for each. 1. 2. 3. Chemical Reaction occur when atoms are: separated or joined Which is correct: rearranged both correct a. Reactant 1 + Reactant 2 Æ Product 1 + Product 2 b. Product 1 + Product 2 c. None correct Æ Reactant 1 + Reactant 2 Which must be written as “diatomic”, “double-atoms” or “Siamese Twins”? a. Br2 I2 N2 Cl2 H2 O2 F2 b. H2 O2 F2 Br2 Au2 4. Which is the correct skeleton equation considering the diatomic atoms above? a. H2 + O2 Æ H2 O b. H + O Æ H2 O 5. In an equation how does one write a catalyst which speeds up the reaction? a. 6. MnO2 Æ b. ∆ Æ Which is correct for: Fe (s) + O2 (g) Æ Fe2O3 (s) a. Solid Iron reacts with Oxygen gas to form solid Iron III Oxide b. Solid Iron reacts with Oxygen to produce Iron II Oxide. Write True of False for each when using the below true equation: Cu (s) + HCl (l) ∆ Æ CuCl2 (s) + H2 (g) 7. Copper metal reacts with liquid Hydrochloric Acid to form solid Copper (I) Dichloride and Hydrogen Gas. 8. Copper metal reacts with liquid Hydrochloric Acid to form solid Copper (II) Chloride and Hydrogen Gas. 9. This reaction was done without a catalyst but with added heat. 10. A “2” in front of the __HCl would balance this equation. 18 19 Name _____________________ 11 CHEMICAL REACTION LAB – DECOMPOSITION Directions: Make sure to balance all Chemical equations and fill in all boxes correctly for full credit. Information: In this type of chemical reaction a compound decomposes into other compounds or elements. Examples: AB → A + B. AB is the reactant; A and B are the products. Sucrose (C12H22O11, decomposes into Carbon and Water Procedure: Place two pinches of sucrose on one end of an aluminum foil scoop. Heat gently at first. Hold a metal jar lid over the decomposing sugar to observe one decomposition product. The charred carbon in the scoop is the other product. Wear goggles. Word Equation Chemical Equation Physical Property Blue Copper Sulfate Hydrate(CuSO4 h5H2O) Crystals produces Water and anhydrous CuSO4 Procedure: Heat two pinches of the crystal in aluminum foil 1cm above a candle flame to avoid sooting. Wear goggles. Observe the color of the crystal and the product. Note any vapor (H20) leaving. Then add a drop of water to the product to re produce the original substance. Word Equation Chemical Equation Physical Property Calcium (Ca) in Water produces Calcium Hydroxide [Ca(OH)2] and H2 Gas Procedure: Fill a test tube half with water. Place a calcium turning into the water. To catch the H2 gas, place another test tube upside down over the mouth of the first test tube until the reaction is complete. To prove there was H2 gas produced place mouth of the upside down test tube over the flame. The 2nd reaction is H2 gas & oxygen becomes water. (Write both RXNs) Word Equation Chemical Equation Physical Property Hydrogen Gas burns in Oxygen to Produce Water (Chemical Combination) Word Equation Chemical Equation Physical Property Poppers/Gun Powder Potassium Nitrate, Carbon and Sulfur produce Potassium Sulfide, Nitrogen & CO2 Procedure: After balancing the below, inspect the color of a party popper. Then throw the party popper on the ground. Observe the color difference. The grey is Potassium Sulfide. The explosion is from the many molecules of Nitrogen gas and Carbon Dioxide gas produced. Word Equation Chemical Equation Physical Propert 19 20 Name _____________________ CHEMICAL COMBINATION Information: In a combination reaction, two chemicals combine to from a new compound. Example: A + B → AB. Chemical A and B are the “reactants” and AB is the “product.” Copper and Sulfur Procedure: With all your strength quickly rub a pinch of sulfur powder on the copper copper is not shiny. Observe color of copper and your fingers. Word Equation: until the Chemical Equation: Physical Property: Copper and Oxygen Procedure: Tie your hair back. Clean one end of copper wire with steel wool till shiny. Heat shiny part of copper wire 1cm above candle flame until the copper is no longer shiny. Wear goggles. Hold copper with small piece of paper to avoid burning fingers. Word Equation: Chemical Equation: Physical Property: Iron (Steelwool) and Oxygen produces Iron II Oxide and Fe3O4 Complex Information: Iron reacts with oxygen in different combinations to form products such as FeO grey, ferrous oxide, Fe2O3 reddish, ferric oxide; and Fe3O4 black, magnetic iron oxide. All are forms of rust. You only have room below for 2 of the 3 products mentioned above. Procedure: Burn steelwool by holding a small ball of it in the tip of a candle flame with a paperclip. Wear goggles. Fill in the spaces below for the formation of FeO and Fe2O3. Word Equation: Chemical Equation: Fe2O3 Physical Property: Word Equation: Chemical Equation: Fe3O4 Physical Property: 20 21 Name _____________________ DOUBLE DISPLACEMENT (REPLACEMENT) Lead II Nitrate and Sodium Hydroxide produce Lead II Hydroxide and Sodium Nitrate Directions: Add several drops of two ionic solutions in one container or well. Read the solubility rules one through six and determine which two ions are Soluble (dissolved) and which two are insoluble or precipitate (clump up). Write the balanced reaction below: Word Equation: Chemical Equation: Physical Property: Write the net ionic reaction below canceling the spectators ions on both sides of the arrow Na+ + Example NO3 - + Pb2+ + 2OH- Pb(OH)2 + Na+ + NO3 - Word Equation: Chemical Equation: Physical Property: Word Equation: Chemical Equation: Physical Property: SINGLE DISPLACEMENT Silver in Silver Nitrate is Replaced by Copper and Lead Directions: Add enough drops of the solution to half cover the metal chunk. Observe And then write the balanced reaction. Word Equation: Chemical Equation: Physical Property: Word Equation: Chemical Equation: Physical Property: Conclusions: 1. For your double displacement reaction, which Solubility Rule(s) predicts the precipitate? 2. 3. Which predicts the ions which will be soluble in the double displacement reaction? If the single replacement reaction, where on the activity chart series is the more Reactive metal? Top middle bottom (circle one). Which metal is more valuable? 21 22 Jeopardy 9 & 111 1-10 00 equation which each side has the same # off atoms of ea ach elementt 1-20 00 what is a new substa ance formed in a chemic cal reaction Product Reacttion Ca atalyst e above None of the 1-30 00 a starting g substance in a chemic cal reaction __________ _ ________ 1-40 00 A reactio on in which oxygen o reactts with anoth her substancce, often producing heat or light 2-10 00 a reaction in which th he atoms of one elemen nt replace the e atoms of a seco ond elementt in a compo ound AB + CÆ C 2-20 00 The ioniz zation energy of which fo ollowing grou up is arrang ed from sma allest to grea atest. Explaiin a. Na, N Si, Cl b. Na, K, Cs 2-30 00 How man ny electrons does nitrogen gain in order to achie eve a noble--gas electron n configuratiion? 2-40 00 What typ pe of ions alw ways have names n ending in -ide? __ __________ ___ like ____ _____ & ___ ________ 2-50 00 Which off the followin ng are arrang ged with all electronegat e tivities from greatest to ssmallest exp plain a. K, Se, Kr b. Li, Na, Cs 33-10 00 What is the t correct name n for the N ion? 3-20 00 When na aming a trans sition metal ion that can have more than one co ommon ionicc charge, the e numerical value of the t charge is s indicated by b a ____. 3-30 00 The electron configuration of a fluoride ion, F, F is ____ 3-40 00 Calculate e the charge e on each ion n. X2Y3 3-50 00 How man ny valence electrons e doe es each X & Y have? 4-20 00 In AlCl3 Al A loses ___ ___ electrons s & Cl gains _____ elecctrons. D. 1, 2 1, 3 E. A. 3, 2 B. 3, 1 C. 2, 4-30 00 What is the t balanced d rxn betwee en. (hint: sing gle replacem ment) __Br2 & ___NaI Æ Æ___ ___ + _ ___ ___ 4-40 00 What is the t formula unit u of sodium nitride? 4-50 00 What typ pe of bond would w the below two subs stances form m? Why?1s2 2 2s2 2p5 &1 1s2 2s2 2p6 6 3s2 5-10 00 What is the t formula for f sodium sulfide? s 5-20 00 Which 2 of the follow wing are NOT T cations? A. iron(III) ion c. Ca b. sulfate s d. mercurous ion 3+ 5-30 00 Which of the following g compound ds contains the t Mn ion n? MnO b. MnBr2 d. Mn2 O3 a. MnS c. 5-40 00 Which sh hows correcttly an ion pa air and the io onic compou nd the two io ons form? 5-50 00 Draw the e electron do ot structure for f Hydrogen n Sulfide? 6-10 00 What is th he name of the t ionic com mpound form med from lith hium and bro omine? 6-20 00 What is th he correct fo ormula for po otassium sulfate? K2SO O4 KSO4 K2SO3 Non ne of the abo ove 6-30 00 Which off the followin ng is a binary y molecular compound ((not ionic)? b. a. BeHCO3 B c. AgI PCl5 d. MgSO4 6-50 00 Sugar burrns under fire e and salt do oesn’t. Why y?What type e of bonds? 7-10 00 What is the t name forr N2O5 Din nitrogen Hex xoxide Binittrogen Pento oxide Dinitrrogen Pentoxxide None 7-20 00 Which on ne has a sing gle covalent bond? CO2 O2 N2 F2 Na2S 7-40 00 What is th he correct name for the compound CoCl2?? C 7-50 00 How man ny Neutrons, Electrons & Protons do oes Potassiu um have in tthat order? Which has the most? 8-10 00 What doe es an -ite or -ate ending in a polyato omic ion mea an? No 8-20 00 Which is correct Tin IV Flouride e SnF4 Sodium Oxide NaO Bariium Nitride BaN one 8-30 00 What kind d of reaction n is the follow wing? __H2O2 Æ _ __H2O + __O2 8-40 00 What kind of reaction n is the follow wing?__Fe + __Cl2 Æ _ __FeCl3 Th hen Balance them with ccoefficient. 8-50 00 22 23 First Last Name Per 4 –11 & 25 Cumulative & Reteaching Score ___/20 4 Atomic Structure Problem Symbol Isotope Number Name 25 1. 12 Magnesium‐?__ ? Avg Atomic Mass # Mass 24.3 Atomic Number = ‐ Neutrons Electrons Protons = 2. From the above chart, Isotopes of the same element have different: 3. Elements are always Identified by the same: 4. Ions are formed because of a losing or gaining protons, neutrons, electrons protons, neutrons, atomic mass protons, neutrons, none correct 25 Nuclear Chemistry 5. Mass Letter Charge P 6. __________ He Fill missing numbers 7. Reaction type Radioisotope Beta Decay Oxygen Reactants 17 Reacts To Form Æ O 8. How much material is left after 3 half‐lives: 100% 50% 25% Products ‐1 e Fission Or Fusion + 12.5% None correct 5&6 Electron Configuration Element Electron Configuration 9. 1s2 2s2 2p6 3s2 3p3 Noble Gas Shorthand Highest Energy Level with Electrons # electrons in highest level Lewis Dot 10. In “2s2 “, the 2 represents which 3 Æ (column, group, family, period, row or energy level). 7 Ions and Bonding 11. Which 2 have 3 valence electron? 12. Aluminums’ charge after reacting would be 13. Which formula is correct? (Aluminum, magnesium, Group 1A, Group 3A) (0, 1+, 2+ 3+) (AlCl, MgCl2, AlCl3) 8 Covalent Bonding 14. What type of bond is Aluminum Chloride? (covalent, ionic, metallic) Type 1 9 Naming 15. 16. 17. 18. Type II Type III What is the name of MgCl2? Magnesium Chloride Magnesium II Chloride Manganese Dichloride What is the name of Fe2O3? Iron Oxide Iron III Oxide Di‐Iron Tri‐oxide Nitrogen Iodide Nitrogen III Iodide Nitrogen Tri‐iodide What is the name of Nl3? From the above, Type I is (alkalis, transitions), Type II is (transitions, non‐metals) & Type III is (alkalis, nonmetals) 11 Reactions 19. The missing product in the reaction:__HCl +__ Ba(OH)2 Æ _ ___ + _ BaCl2 is: [H‐OH HBa Cl‐OH] 20. The above reaction is a: single replacement double replacement combustion 21. To balance the above reaction, the coefficients would be: (1,1,1,1 2,1,2,1 3,1,3,1) 10 Moles 22. 24 grams of Carbon is how many moles: 23. 24 grams of Carbon is how many molecules: 24. 8.0 grams of Hydrogen is how many liters: 25. Show work for the # 8 above. 0.5 1.0 3.01 x 10 23 22.4 44.8 2.0 4.0 6.02 x 10 23 12.04 x 10 23 none correct 89.6 none correct = Corrected by_______________________ 23 24 11CHEMICAL RXN’S __ /__ pts burns is a combustion? Y N 5.Double replacement reactions A + B ÆAB Anticipatory Response 1.Chemical reactions occur only when atoms are joined or rearranged? Y N 2. In the above equation, the the rt. side are reactants? Y N 3. Æ means “to produce”, “to make”, or “to yield”? Y N 4.Skeleton equations are not Balanced? Y N 5. Hydrogen can be written as “H” in an equation? Y N 6. Catalysts & heat are always written on the arrow? Y N 7. Aqueous (aq), liquid(l) & gas (g) should be written? Anticipatory Response 1. A + B ÆAB is the pattern for a decomposition reaction? Y N 2. H2 + O2 Æ H2O fits the pattern for synthesis? Y N 3. Photosynthesis is called so because chlorophyll combines CO2+H2O to makeÆsugar? Y N 4The reverse of #3 when sugar Involve cations & anions? Y N Summary Section: 24 First Last Name___Per__ Cornell Question & Ans Directions: Make 5 questions & answers that are different than the Anticipatory Response 1. 2. 3. 4. 5.