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1 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 __ __ __ 1 __ __ ____________ 2 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. 2 3 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 3 I. Combustion of propane 4 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) 4 5 Name 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. 5 6 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 6 HNO3 H3PO4 H3C6H5O7 H2CO3 HCO2H 7 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. 7 8 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 8 9 Name 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 carbon 9 dioxide. 10 ____________ ___ 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 10 11 9 IONIC COMPOUND NAMING CHART Directions: Write the formala name of each compound. F ClSO42CO32NO3- NH4+ PO43- Ammonium Flouride CrO42- CH3CO23Ammonium Acetate (vinegar) K+ Na+ Ag Ca 2+ Mg 2+ Ba 2+ Al 3+ Fe 2+ Fe 3+ Iron III Flouride Iron III Phosphate 9 IONIC COMPOUND FORMULA CHART Directions: NH4+ Write the chemical formula of each compound. Make sure the oxidation number add up to zero. ClSO42CO32NO3PO43CrO42CH3CO23FNH4 F K+ Na+ Ag+ Ca2+ Mg2+ Ba2+ Al3+ Fe2+ Fe3+ Fe3 (PO4)2 FeCl3 11 12 9 IONIC REACTION LAB CHART Directions: 1) Write the entire chemical formula of each anion & cation below to be used (look at NaCl/AgNO3). 2) Put one drop of each chemical on the plastic grid sheet. Record your observations below. Anions Cations ! A AgNO3 F- ClNaCl White ppt SO42- 3 4 CO32- NO3CaNO3 PO43- CrO42 CH3CO23 - - 8 9 No (NR) Reaction B C D E F G H I J 1 2 5 6 7 10 11 Directions: 1) Pick one reaction which made a Precipitate from each column and write the ionic reaction. 2) Use the solubility rule to determine which product formed the precipitate & which was soluble. 3) Cross out the products which were soluble because they’re spectators as reactants & products. column A 2 Reactants Products AgNO3 + NaCl AgCl + NaNO3 Ag++NO3- + Na++Cl- AgCl +Na++NO3Ag++ Cl- AgCl B C D E F G H I J 12 Rule # states that Chlorides are soluble except with Ag, Pb & Hg. Total ionic equation 13 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 13 14 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 14 15 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_______________________ 15 16 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: 16 First Last Name___Per__ Cornell Question & Ans Directions: Make 5 questions & answers that are different than the Anticipatory Response 1. 2. 3. 4. 5.