Balancing Equations
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Unit Four: Chemical Reactions 0 Unit Four: Chemical Reactions Table of Contents: Pg. 1 Table of Contents Pg. 2-3 Phases of Matter (Assign on Pg 18-19) Pg. 4-5 Solutions (Assign on Pg 20) Pg. 6 Chemical Reactions (Assign Pg 21-23) Pg. 7-9 Types of Chemical Reactions (Assign Pg 24) Pg. 10 Rates of Reactions Pg. 11-12 Rates of Reactions Lab Pg. 13-14 Balancing (Assign on Pg 25) Pg. 14 Balancing Word Equations (Assign on Pg 26) Pg. 15 Predicting Products (Assign on Pg 27) Pg. 15-16 Balancing Net Ionic Equations (Assign on Pg 28) Pg. 29-32 Pg. 33-34 Using Solubility and Reaction Types to Write Balanced Net Ionic Equations (Assign on Pg 29) Energy: Exothermic and Endothermic Processes (Assign on Pg 30) 1 Phases of Matter Phase Diagrams Pressure-temperature diagrams Summarizes the effect of temperature and pressure on a substance in a _________________________ container. AB line: rate at which solid sublimes to form a gas = rate at which gas condenses to form a solid The points along AB represent all combinations of temperature and pressure at which the solid is in _________________________ with the gas. BC line: rate at which liquid boils to form a ________________ = rate at which gas condenses to form a liquid BD line: rate at which solid melts to form a _________________________ = rate at which liquid freezes to form a solid The BD line is almost vertical because the melting point of a solid is not very sensitive to changes in _________________________ The solid-liquid phase boundary of most substances has a _________________________ slope. This is due to the solid phase having a _________________________ density than the liquid, so that increasing the pressure increases the melting temperature. Changes in pressure: Point B is the point at which a pure substance can exist simultaneously as a solid, a liquid, and a gas. This is called the _________________________ point. Point C is the _________________________ point of the substance, which is the highest temperature and pressure at which a gas and a liquid can _________________________ The “normal” boiling point and freezing point occur at ______ atm pressure. 2 Temperature vs. Energy Graph: Melting Point and Freezing Point Pure, crystalline solids have a characteristic ________________________ _________________________, the temperature at which the solid melts to become a liquid. When the solid is turning into a liquid it remains at a _________________________ temperature until all of the solid becomes a liquid. This is because the _________________________ being put into the solid is going into changing the state of the solid and therefore isn’t used to increase the _________________________ of the compound. Once all of the solid has become a liquid the temperature can _________________________. Liquids have a characteristic temperature at which they turn into solids, known as their _____________________________________________. In theory, the melting point of a solid should be the same as the freezing point of the liquid. Melting points are often used to help _________________________ compounds. Boiling Point When a liquid is heated, it eventually reaches a temperature at which the vapor pressure is large enough that bubbles form inside the body of the liquid. This temperature is called the ___________________________________________. Once the liquid starts to boil, the temperature remains _________________________ until all of the liquid has been converted to a gas. Pressure and temperature both affect the freezing and boiling points. Below is a chart that shows the freezing and boiling points of water at 1 atm. (See Phase Diagram Assign pg 18 & 19) 3 Solutions Components of a Solution A solution is composed of two or more _________________________ substances, one of which is a solvent and the other a solute. A cup of instant coffee is the _________________________, the hot water is the _________________________, and the instant coffee is the _________________________. Solutions in which water is the solvent are called _________________________ solutions. Water as a Solvent Most covalent liquids are only able to dissolve other covalent compounds; water can dissolve both _________________________ and covalent compounds. The attraction of water _________________________ for ions pulls ions out of a crystalline lattice and into aqueous solution. Solutions: A ____________________________________is a solution that contains the maximum amount of solute dissolved in a solvent. A __________________________________________________ is a solution where conditions have been changed to allow more solute to dissolve than would at room temperature (this is done by heating the solvent or solution). When the solvent and solutes are liquids we can use the terms miscible and immiscible. _________________________ means that the two liquids will mix together, and _________________________means that the two liquids will not dissolve in one another. Sometimes when we mix two dissolved salts together, we end up with a _________________________. This is because a new ionic compound is formed that is insoluble in water. We can use solubility charts or solubility tables to determine if a solid will be formed. 4 Solubility Table Ion NO3– ClO4– Cl– I– SO42CO32PO43OH– S2Na+ K+ NH4+ Solubility soluble soluble soluble soluble soluble insoluble insoluble insoluble insoluble soluble soluble soluble Exceptions none none except Ag+, Hg22+, *Pb2+ except Ag+, Hg22+, *Pb2+ except Ca2+, Ba2+, Sr2+, Hg2+, Pb2+, Ag+ except Group IA and NH4+ except Group IA and NH4+ except Group IA, *Ca2+, Ba2+, Sr2+ except Group IA, IIA and NH4+ none none none * = slightly soluble Ex. If we mix sodium ions with hydroxide ions will a precipitate form? Ex. If we dissolved sodium hydroxide in calcium chloride, will a precipitate form? 2NaOH + CaCl2 2NaCl + Ca(OH)2 Ex. Calcium nitrate with sodium carbonate Ca(NO3)2 + Na2CO3 CaCO3 + 2NaNO3 Ex. Silver Perchlorate and Calcium Iodide Examples/Demonstrations (see Solubility Assign Pg 20) 5 Chemical Reactions The Importance of Chemical Reactions Many chemical reactions occur naturally, although some take place so slowly that we do not notice them. Biochemical Reactions The natural chemical reactions that we observe occurring in _________________________ things are known as biochemical reactions. 2 important chemical reactions are shown below: Respiration: Photosynthesis: Manufacture Important Chemicals Many important chemicals are created through chemical reactions. Examples: Harmful Chemical Reactions There are also chemical reactions that harm living organisms and harm the environment. Review Chemical Reactions: Indicator that a chemical change has occurred: Other signs of a chemical change: Change in electrical conductivity Change in melting point or boiling point Change in density Change in taste 6 Types of Chemical Reactions Chemical Reactions A _________________________ occurs when two or more molecules _________________________ and a chemical change occurs. A chemical change MUST occur in order for a chemical reaction to occur. Chemical reactions start with the _________________________ and go to the _________________________. Types: Synthesis/ Combination: A synthesis reaction is when two or more simple compounds _________________________ to form a more complicated one. These reactions come in the general form of: A + B ---> AB One example of a synthesis reaction is the combination of iron and sulfur to form iron (II) sulfide: Decomposition: A decomposition reaction is the opposite of a synthesis reaction - a complex molecule ___________________ ___________________ to make simpler ones. These reactions come in the general form: AB ---> A + B One example of a decomposition reaction is the electrolysis of water to make oxygen and hydrogen gas: Single displacement: This is when one element ______________________ _________________________with another element in a compound. These reactions come in the general form of: A + BC ---> AC + B One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas: The Activity Series: The activity series of an element is used to determine whether or not a single displacement reaction will _________________________. Each metal will displace any metal ion that appears _________________________ it in the series. 7 The Activity Series lithium potassium barium These metals displace hydrogen from water calcium sodium magnesium aluminum zinc iron These metals displace hydrogen from acids nickel tin lead hydrogen copper mercury These metals do not react with acids or pure water silver gold Examples: Cu(s) + FeSO4(aq) Zn(s) + 2 HCl(aq) 2 Na(s) + 2 H2O(l) The Halogen Displacement Series The Halogen Displacement Series Each halogen will fluorine displace any halide chlorine ion that appears below it bromine iodine Examples: determine whether a reaction will occur, if so, what are the products? Br2(aq) + 2 NaCl(aq) Zn(s) + NiCl2(aq) I2(aq) + 2 KF(aq) F2(aq) + 2 KI(aq) Cu(s) + 2 AgNO3(aq) 8 Double displacement: This is when the anions and cations of two different molecules _____________________ _________________________, forming two entirely different compounds. These reactions are in the general form: AB + CD ---> AD + CB One example of a double displacement reaction is the reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate: How can we predict when a double displacement reaction will occur? Such reactions usually result in the formation of a _________________________, a gas, or water. Sometimes included as types of reactions: Acid-base: This is a special kind of __________________________________________________reaction that takes place when an acid and base react with each other. The H+ ion in the acid reacts with the OH- ion in the base, causing the formation of _________________________. Generally, the product of this reaction is some ionic salt and water: HA + BOH ---> H2O + BA One example of an acid-base reaction is the reaction of hydrobromic acid (HBr) with sodium hydroxide: The base is under a salt: NaCl NaOH Combustion: A combustion reaction is when _________________________ combines with another compound to form water and carbon dioxide. These reactions are exothermic, meaning they produce heat. An example of this kind of reaction is the burning of napthalene: C10H8 + 12 O2 ---> 10 CO2 + 4 H2O Steps to determine types of reactions: Follow this series of questions. When you can answer "yes" to a question, then stop! 1) Does your reaction have oxygen as one of its reactants and carbon dioxide and water as products? If yes, then it's a combustion reaction 2) Does your reaction have two (or more) chemicals combining to form one chemical? If yes, then it's a synthesis reaction 3) Does your reaction have one large molecule falling apart to make several small ones? If yes, then it's a decomposition reaction 4) Does your reaction have any molecules that contain only one element? If yes, then it's a single displacement reaction 5) Does your reaction have water as one of the products? If yes, then it's an acid-base reaction 6) If you haven't answered "yes" to any of the questions above, then you've got a double displacement reaction 9 Rates of Chemical Reactions The rate of reaction is the _________________________ at which reactants combine to form products. Remember that in order for a bond to form a collision must occur. This means that the more collisions the more molecules will bond and the _________________________ the rate will be. What influences the rate of reaction? Surface area: The greater the surface area of the reactants, the _________________________ collisions will occur, and the faster the reaction will take place. So if you increase the surface area of a reactant you will _________________________ the rate of the reaction. Temperature: When the temperature is increased the atoms/molecules move around more so there are _________________________ collisions. Because there are more collisions, the rate of the reaction _________________________. So an increase in temperature results in an increase in the rate of the reaction and vice versa. Concentration: The more molecules or atom you have to combine with another atom or molecule, the _________________________ chance you have of a collision occurring between the molecules. This means there is a greater chance of bonding and therefore an _________________________ in the rate of the reaction. So if you increase the concentration of a reactant, you will increase the rate of the reaction. Pressure: Pressure effects the rate of a reaction but this can be difficult to visualize with a solid or liquid, so think of a gas. The more you increase the pressure, the less area the gas molecules have to move around, so the more likely they are to _________________________ each other. Since an increase in the pressure increases the number of collisions, it also _________________________ the rate of the reaction. Catalyst: A caltalyst is something that is added to the reaction to increase the rate without changing the products. This means that whatever amount of catalyst you put into the reaction, will be the _________________________ amount you get out. Reactions need a certain amount of _________________________ in order to occur. If they do not get enough energy, they cannot occur. What a catalyst does is lowers the amount of energy required for the reaction to take place. The energy needed for a reaction to take place is called the _________________________energy. Keep in mind that energy is not matter. In fact energy is anything that is not matter. 10 Lab 5: Alka-Seltzer Rates of Reaction Lab Background information: Today we are going to be observing what occurs when an Alka-seltzer tablet is dissolved in water. An Alkaseltzer tablet produces Carbon dioxide gas when dissolved in water. It is obvious then that the reaction is as follows: Alka-seltzer + H2O → CO2 + products However there is a lot more going on than just this simple (looking) reaction. Alka Seltzer is an effervescent tablet used to relieve pain or an upset stomach. Alka-Seltzer’s primary ingredients are acetylsalicylic acid (aspirin), citric acid (C6H8O7), and sodium bicarbonate (NaHCO3). When the Alka-seltzer is in tablet form, the ingredients of the tablet do not form any sort of reaction, but when dissolved, the citric acid and sodium bicarbonate are able to react. When the Alka-seltzer tablet dissolves in water, the sodium bicarbonate dissociates to form a bicarbonate ion (HCO3-) and a sodium ion (Na+). + 1. - NaHCO (s) → Na (aq) + HCO (aq) 3 3 (Notice the state of the sodium bicarbonate starts out as a solid and then it dissolves so it become aqueous.) + Citric acid (C6H8O7) also dissolves, donating an H+ to water to create a hydronium ion (H O (aq)) which is an 3 acid. The by-product of this reaction is citrate (C6H7O7-). 2. C6H8O7(aq) + H2O (l) → C6H7O7-(aq) + H3O+(aq) Since the Citric acid allowed for a hydronium ion (H3O+) to be present in the solution, the following reaction takes place between the hydronium ion and the bicarbonate ion: - 3. + HCO (aq) + H O (aq) → 2H O(l) + CO (g) 3 3 2 2 (The sodium ion does not take part in this reaction, so is not included in the equation) The Complete reaction that occurs is as follows: Sodium bicarbonate + citric acid carbon dioxide (gas) + water + sodium citrate NaHCO (aq) + C6H8O7(aq) + H2O (l) → NaC6H7O7(aq) + 2H2O(l) + CO2 (g) 3 The complete reaction above can be simplified by writing only the reactant and products that have an active role in the reaction. The first step to doing this is to write any products or reactants in the form of the ions they create when they dissociate in water: + - + Na (aq) + HCO (aq) + C6H7O7- (aq) + H3O+(aq) → 2H2O(l) + CO2 (g) + Na (aq) + C6H7O7- (aq) 3 We then cancel and ions that appear in both the products and the reactants side of the equation. + - + Na (aq) + HCO (aq) + C6H7O7- (aq) + H3O+(aq) →2H2O(l) + CO2 (g) + Na (aq) + C6H7O7- (aq) 3 By cancelling out the ions that appear on both the reactants and products side of the reaction, we are cancelling out any ions that are not an active part of the reaction. This is called writing the net ionic equation of a reaction: - + HCO (aq) + H O (aq) → 2H O(l) + CO (g) 3 3 2 11 2 Purpose: The objective of this experiment is to examine ways to increase or decrease the rate of the reaction of an Alka-seltzer tablet and water. Materials: Film canister (with lid) Spatula Water Paper towel 2 Alka-seltzer tablets (There are 2 in one package, so only on package needed) Procedure: 1. Gather the materials needed for the lab (Don’t forget to wear your safety glasses). 2. Break one Alka-seltzer tablet in half (or less) 3. Place water in your film canister. 4. Drop a piece of Alka-Seltzer tablet into your water in the film canister (you should not need more than one half of the tablet, but you may try varying amounts). 5. Place the lid on the film canister. (You may want to be quick about this). 6. Stand back (the lid can shoot off at extreme speeds which could be harmful if it hits you) 7. Vary the amounts of tablets, the tightness of the lid, the time the lid is placed on, the surface area of the tablet and the temperature of the water to try to get the lid to pop off of the canister in exactly 10 seconds. 8. Be sure to make observations about what you are varying and how it works 9. LEAVE ENOUGH TABLET TO REPEAT THE EXPERIMENT ON FINAL TIME AS A CLASS 10. Near the end of the lab class I will start the timer and all students will have to place their Alka-seltzer tablet into the water in the film canister at this time. I will count the time as it passes and you will have to write out the time that your lid popped off in the final reaction. Analysis Questions: 1. What are some of the variables you changed to try to adjust your lid to pop off at exactly 10 seconds? Which combinations worked best for you? 2. Which combinations of variables worked best for other students’ whose lid popped off at exactly 10 seconds? 3. Label the reaction types for the following reactions: + - NaHCO (s) → Na (aq) + HCO (aq) 3 3 - + HCO (aq) + H O (aq) → 2H O(l) + CO (g) (you should have 2 types for this reaction) 3 3 2 2 Post a comment on our VC discussion board about what you liked most and what you like least in today’s experiment. 4. 12 Balancing! Recall Balancing: Chemical Equations: The Law of _________________________ of Mass states that in a chemical reaction the total mass of reactants is equal to the total mass of the _________________________. Matter cannot be created or destroyed. Also, elements cannot change to become other elements (exception: unstable elements). This means the number of atoms of each element in the reactants must be the same as the _________________________. Ex. If there are 3 oxygen atoms in the reactants, there must be exactly _____ oxygen atoms in the products. o What is a chemical equation? Whenever matter is _________________________ changed, an equation can be written to describe its effects. It is a representation of what occurs during the reaction. A balanced chemical equation represents the identities and relative _________________________ of reactants and products in a chemical reaction. The total number of each type of atom remains the same. A chemical equation represents the reactants and products in a chemical reaction using their symbols or formulas. How to balance chemical equations: You cannot change the number of atoms/each element in the compound (subscripts), but you can multiply the ____________________________________________by a number (add a coefficient). Remember: # of atoms in reactants must = # atoms in products Can only add _________________________, you cannot change subscripts Tips: If there is ever an element that is alone, we usually balance this one last. If you ever get stuck, try _________________________ everything. Examples: ____ H2 + ____O2 ____H2O ____KMnO4 + ____HCl ____KCl + ____MnCl2 + ____H2O + ____Cl2 13 ____ Fe + ____ Cl2 ____ FeCl3 Balancing Practice: http://funbasedlearning.com/chemistry/chemBalancer/default.htm Balancing Word Equations: A word equation identifies the reactants and products in a chemical reaction using only the _________________________ of the elements and compounds. Things to know: Diatomic elements: These elements come in _________________________. o In a word equation, if it states a lone element (not in a compound), this means it is just that element on its own… not with a _________________________ (only ions have charges). Examples: Zinc: Iodine: Chlorine: Helium: Calcium: Hydrogen: How to… Write out the pluses and arrow for produces. Write out all of the lone elements (don’t forget about diatomics) Write out the chemical formula (criss cross) for each of the compounds. Balance Examples: Zinc and lead (II) nitrate produces zinc nitrate and lead Aluminum bromide and chlorine yield aluminum chloride and bromine 14 Determining Products of a reaction: Look to see if the reactants are going to produce a synthesis, decomposition, single displacement or double displacement reaction. Remember that with double displacement or single displacement, a cation will be paired with an anion, you will not have 2 cations or 2 anions paired together in a compound. Examples: Aluminum bromide and calcium chloride: Mercury (II) oxide heated Write a word equation that states the reaction that will occur between Zn(s) and Pb(NO3)2 (aq) Hydrogen and oxygen Net Ionic Equations Balancing Net Ionic Equations: Before learning how to write balanced net ionic equations, we must first learn about electrolytes. Electrolytes If an _________________________ solution of a compound conducts _________________________, it is called an electrolyte. The ability to conduct electricity results when an aqueous solution contains dissolved ions. There are two types of electrolytes: 1. __________________________________________________- These compounds are the ones that completely _________________________ and exist as ions in solutions. They include strong acids (HCl, HBr, HI, HNO3, H2SO4 and HClO4, etc.), strong bases (Hydroxides etc.) and all soluble salts. 15 2. __________________________________________________- in aqueous solution, these compounds yield some _________________________ in solution. They include: weak acids (any acid that isn't strong), and weak bases (any base that isn't strong). 3. ______________________________________– These are solutions that do not dissociate into _________________________. This includes water. Balancing Net Ionic: Net ionic equations are _________________________ equations that represent chemical reactions with aqueous solutions involved. Aqueous solutions are solutions created by salts dissolving in water, and their ions dissociating. Solids, liquids and gases do not _________________________ into ions. They stay in their compound or formula unit form. There are 3 steps to writing out a Balanced Net Ionic Equation. Step 1: Write a _________________________ General Equation. Step 2: Write the _________________________ Ionic Equation. This means to look at each product and reactant and determine if it dissociates into its ions. If it does, you must write out these ions. Step 3: Write the _________________________ equation. That is to remove all ions that do not undergo a change. These are called spectator ions and these can be identified if they appear as ions in both the products and the reactants. Ex. NaOH(aq) + HCl(aq) H2O(l) + NaCl(aq) When writing net ionic equations we separate anything that is aqueous into its ions. Anything that is solid, liquid or gas stays as it is. Examples: KCl(aq) + AgNO3(aq) AgCl(s) + KNO3(aq) Total ionic equation Net ionic equation NaOH(aq) + CuCl2(aq) Cu(OH)2(s) + NaCl(aq) Not only do the atoms/elements need to balance but _________________________ must also ALWAYS balance. If they do not then there is an error. 16 Bringing it all together: Using reaction types to predict the products and solubility to write a balanced net ionic equation Lead (II) Nitrate and Potassium Chloride Energy! Balancing reactions with energy terms: Exothermic: An exothermic reaction is one where energy is __________________. This does not mean that energy is not required to start the reaction, it just means that more energy is released than absorbed. This means that energy is a _______________ of the reaction. Examples: Endothermic: An endothermic reaction is one where energy is _________________. This means energy is required in order for the reaction to occur so energy is a _________________. Examples: Example Questions: Determine if the following are exothermic reactions or endothermic reactions: Ice melting: Baking bread: Photosynthesis: Burning propane: 17 Name:_____________________ Phase Diagrams Assignments For the graph above answer the following questions: 1. At what temperatures is the substance represented in the graph above a gas? 2. At what temperatures is the substance represented in the graph above a liquid? 3. At what temperatures is the substance represented in the graph above a solid? 4. What is the substance`s melting point? 5. What is the substance`s freezing point? 6. What is the substances boiling point? 7. At 10oC what state is the substance in? 18 8. For the phase diagram above, label the area of the graph where the substance is solid, liquid and gas. 9. Explain what a triple point is. 10. For the phase diagram above, label the triple point. At what temperature and pressure does this occur? 11. What is a critical point? 12. For the phase diagram above what is the highest temperature that a liquid can exist at? 13. What is the normal boiling point of this substance? 14. What is the normal melting point? 15. For the substance graphed above, circle the state that is more dense. Solid Liquid 16. At 1.5atm and 100oC what state would this substance be in? 17. At 50oC, if you started at 0.5 atm and increased the pressure to 1.5atm which of the following changes of state would occur? (circle) Condensation melt boil freeze 19 sublimation stay the same Name:_______________________ Solubility Assignment 1. Determine whether the following compounds are soluble or insoluble: a. NaNO3 b. AgCl c. K2CO3 d. CaSO4 e. Na3PO4 f. Ca(OH)2 g. Fe(OH)2 h. PbSO4 2. Write the states for all of the reactants and products in the reactions below: a. 2KCl + Pb(NO3)2 b. HCl + NaOH c. FeCl3 + K3PO4 d. BaCl2 + Na2SO4 2KNO3 → NaCl + PbCl2 + H2O FePO4 + 3KCl BaSO4 20 + 2NaCl Name:________________________ Types of Reactions Assignment State which type of reaction the following reactions are 1. NaOH + KNO3 NaNO3 + KOH 2. CH4 + 2 O2 CO2 + 2 H2O 3. 2 Fe + 6 NaBr 2 FeBr3 + 6 Na 4. CaSO4 + Mg(OH)2 Ca(OH)2 + MgSO4 5. NH4OH + HBr H2O + NH4Br 6. Pb + O2 PbO2 7. Na2CO3 Na2O + CO2 8. 2H2 + O2 2H2O 9. 2H2O 2H2 + O2 10. Zn + H2SO4 ZnSO4 + H2 11. 2CO + O2 2CO2 12. 2HgO 2Hg + O2 13. 2KBr + Cl2 2KCl + Br2 14. AgNO3 + NaCl AgCl +NaNO3 Determine whether the following single displacement reactions will occur. If so, predict the products and balance the equation: 15. Al(s) + H2O(l) → 16. Cu(s) + Hg(NO3)2(aq) → 17. Br2(aq) + MgI2(aq) → 18. Au(s) + FeSO4(aq) → 19. Al(s) + ZnSO4(aq) → 20. Sn(s) + AgNO3(aq) → 21 Name:_________________________________ Balancing Equations 1. ____Al + ____Fe3O4 ____Al2O3 + ____Fe 2. ____CH3OH + ____O2 ____CO2 + ____H2O 3. ____P4O10 + ____H2O ____H3PO4 4. ____PCl5 + ____H2O ____H3PO4 + ____HCl 5. ____SbCl5 + ____H2O ____SbOCl3 + ____HCl 6. ____MgO + ____Si ____Mg + ____SiO2 7. ____CaCl2 + ____Na2CO3 ____CaCo3 + ____NaCl 8. ____C6H6 + ____O2 ____CO2 + ____H2O 9. ____Al2S3 + ____H2O ____Al(OH)3 + ____H2S 10. ____C2H6 + ____O2 ____CO2 + ____H2O 11. ____KClO3 ____KCl + ____KClO4 12. ____KBr + ____Cl2 ____KCl + ____Br2 13. ____ (NH4)2SO4 + ____NaOH ____NH3 + ____H2O + ____Na2SO4 22 Name:_______________________________ Balancing Word Equations Write out the balanced chemical reaction for the following reactions. 1. Zinc and lead (II) nitrate yield zinc nitrate and lead 2. Aluminum bromide and chlorine produces aluminum chloride and bromine 3. Sodium phosphate and calcium chloride yield calcium phosphate and sodium chloride 4. Potassium chlorate when heated produces potassium chloride and oxygen gas 5. Aluminum and hydrochloric acid yield aluminum chloride and hydrogen gas 6. Calcium hydroxide and phosphoric acid yield calcium phosphate and water 7. Copper and sulfuric acid yield copper (II) sulfate, water and sulfur dioxide 8. Hydrogen and nitrogen monoxide yield water and nitrogen 23 Name:____________________________ Predicting Products of Chemical Reactions Predict the products of the reactions below. Then, write the balanced equation and classify the reaction. 1. Magnesium bromide and chlorine 2. Aluminum and iron (III) oxide 3. Silver nitrate and zinc chloride 4. Hydrogen peroxide (catalyzed by manganese dioxide) 5. Zinc and hydrochloric acid 6. Sulfuric acid and sodium hydroxide 7. Sodium and hydrogen 8. Acetic acid and copper 24 Name:________________________________ Net Ionic Equations Write the total and net ionic equations for the following. 1. ___Zn (s) +___ HCl (aq) ___ ZnCl2 (aq) + ___H2 (g) 2. ___FeCl3 (aq) +___ AgNO3 (aq) ___ AgCl (s) +___ Fe(NO3)3 (aq) 3. ___KOH (aq) + ___H3PO4(aq) ___ K3PO4(aq) +___ H2O (l) 4. ___HCl (aq) + ___ Na2CO3 (aq) ___ H2O(l) + ___CO2(g) + ___NaCl (aq) 5. ___Ba(OH)2 (aq) + ___Fe2(SO4)3 (aq) ___ Fe(OH)3 (s) + ___ BaSO4 (aq) 6. ___Mg (s) + ___AgNO3 (aq) ___Ag (s) + ___ Mg(NO3)2 (aq) 7. ___NaOH (aq) + ___CO2 (g) ___Na2CO3 (aq) + ___H2O (l) 8. ___BaCl2(aq) + ___Na2CO3(aq) ____BaCO3(s) + ____ NaCl(aq) 9. ___NaOH(s) + ___ HNO3(aq) ___H2O(l) + ___NaNO3(aq) 10. ___NaCl(aq) + ___AgNO3(aq) ___AgCl(s) + ___NaNO3(aq) 25 Name:_____________________________ Using Solubility and Reaction Types to Write Balanced Net Ionic Equations For the following examples, write the balanced equation (Reactants AND products) including states. Then write the balanced net ionic equation. 1. Mercury (I) Nitrate and Potassium Iodide 2. Lithium Sulfide and Silver (I) Perchlorate 3. Barium Hydroxide and Sodium Sulfate 4. Strontium (II) Chloride and Sodium Sulfate 5. Calcium Chloride and Potassium Carbonate 26 Name:__________________________________ Exothermic Vs. Endothermic Assignment Put the word “Exothermic” by the processes which are exothermic and the word “Endothermic” by the processes that are endothermic. 1. Making ice cubes: 2. Melting ice cubes: 3. Frost turning into water vapour: 4. Evaporation of water: 5. Melting wax: 6. A candle flame: 7. Cooking an egg: 8. HC2H3O2 + NaHCO3 + Energy CO2 + NaC2H3O2 (aq) + H2O 9. HCl H+ (aq) + Cl1- (aq) + Energy : 10. 2H2O + energy 2H2 + O2 11. 2 H2 + O2 2H2O + heat 27
