Unit 04b: Chemical Reactions
|
|
- Brent York
- 5 years ago
- Views:
Transcription
1 1 Unit 04b: Chemical Reactions Author: S. Michalek Introductory Resources: Zumdahl v. 5 Chapter 4 Main Ideas: Classification of reactions Balancing reactions Prediction of products Writing net ionic equations Duration: 10 days Last Revision: September 5, 2007
2 2 Outline 4b.1 Classifying Reactions There are 5 basic chemical reactions. Synthesis or composition o A + B AB o Two or more reactants are combined to form one compound Decomposition o AB A + B o One reactions is broken into two or more products o Decomposition reactions are endothermic meaning the reaction absorbs heat. Single Replacement or Single Displacement o Element + Compound Element + Compound o A + BC AC + B o Single replacement reactions are reactions that involve an element replacing one part of a compound. The products include the displaced element and a new compound. An element can only replace another element that is less active than itself. Double Replacement, Double Displacement, or Metathesis o AB + CD AD + BC o In many reactions between two compounds in aqueous solutions, the cations and anions appear to switch partners. The two compounds form two new compounds. No changes in oxidation numbers. o All double replacement rations must have a driving force or a reason why the reaction occurs. The driving force in a double replacement reaction is the removal of at least one pair of ions from solution. o Removal of ions can occur in one of three ways: Formation of a precipitate a solid has formed that is insoluble in water. Formation of a gas gases may form directly from the reaction or a side decomposition reaction occurs causing the gas to form. Reactions that produce three of the gases (CO 2, SO 3, NH 3 ) involve the initial formation of a substance that breaks down to give the gas and water. H 2 SO water + SO 2 H 2 CO water + CO 2 NH 4 OH --- water + NH 3 Formation of water water is formed from an acid/base reaction. Combustion reactions o Chemical + O 2 chemical oxides o C x H y + O 2 CO 2 + H 2 O o S 8 + O 2 SO 3 o Combustion reactions are exothermic reactions that release heat.
3 3 Outline 4b.2 Balancing Reactions Now comes the fun part, balancing the reaction. The Law of Conservation of Mass states that in a chemical reaction there is no loss of mass. Each type of element will have the same mass before the reaction and after the reaction, or as reactant and product. But you can t change the materials that participate in the reaction, so you must write an integer coefficient in front of (to the left of) each material in the reaction to make sure every type of atom has the same number on each side of the reaction. Tips for Balancing Equations Be sure each molecular formula is written correctly and each compound is neutral (meaning no charge). Mentally count or tally how many of each type of atom is present on each side of the equation. Begin balancing elements that are only found in one substance on each side. Balance oxygen and hydrogen last. If there is an odd number of an element on one side and an even number on the other, the odd will need to be evened out so use a coefficient of 2 for that substance. When tallying, be sure to adjust the count for each and every element that an added coefficient affects. Combustion reactions that don t seem to balance will often turn out better if a coefficient of 2 is used for the hydrocarbon. Keep polyatomic ions grouped together in double replacement reaction. Nitrogen gas and hydrogen gas react under high pressure high temperature to form ammoni _ N 2 + _ H 2 _ NH 3 Begin with nitrogen. There are two nitrogen atoms on the left and only one on the right. In order to balance the nitrogen atoms, place a 2 in front of the ammoni _ N 2 + _ H 2 2 NH 3 There are two hydrogens on the left and six on the right. We balance the hydrogens by placing a 3 in front of the hydrogen gas. _ N H 2 2 NH 3 Now go back and check to make sure everything is balanced. There are two nitrogen and six hydrogens on both sides of the reaction. It is balanced. There is no coefficient shown in front of the nitrogen. There is no need to write ones as coefficients. The reaction equation is: N H 2 2 NH 3
4 4 Outline 4b.3a Predicting Reactions When prediction reactions you will need to follow steps in order to get the correct final balanced reaction. 1. Write out the reactants. Remember ionic compounds need to have there charges balanced. Remember your diatomic elements (H 2, O 2, N 2, Cl 2, Br 2, I 2, F 2 ) 2. Classify the reaction. 3. Use the prompts to figure out the products. Remember ionic compounds need to have there charges balanced. 4. Balance the reaction Synthesis Reactions o Element + Element Zn + Cl 2 ZnCl 2 o Compound + Compound Formation of an Acid Gas + Water Acid CO 2 + H 2 O H 2 CO 3 Formation of a Base Metal Oxide + Water CaO + H 2 O Ca(OH) 2 Metal Hydroxide Decomposition Reactions o Binary Compound a compound with two elements Compound Element + Element 2AlCl 3 2Al + 3Cl 2 o Metal Carbonate Metal Carbonate Metal Oxide + Carbon Dioxide Na 2 CO 3 Na 2 O + CO 2 o Metal Oxide Metal Oxide Metal + Oxygen Gas 2FeO 2Fe + O 2 o Metal Peroxide Metal Peroxide Metal Oxide + Oxygen Gas 2PbO 2 2PbO + O 2 o Metal Hydroxide Metal Hydroxide Metal Oxide + Water 2LiOH Li 2 O + H 2 O o Acid Acid Water + Gas Left Over H 2 SO 4 H 2 O + SO 3 o Metal Chlorate Metal Chlorate Metal Chloride + Oxygen Gas 2KClO 3 2KCl + 3O 2
5 5 Outline 4b.3b Predicting Reactions Single Replacement Reactions o Active metals replace less active metals from their compounds in aqueous solutions (SEE ACTIVITY SERIES HANDOUT). Magnesium turnings are added to a solution of iron (III) chloride. Reactants: Mg + FeCl 3 Mg is higher on the activity Series than Fe so it replaces the iron Equation: 3Mg + 2FeCl 3 2Fe + 3MgCl 2 o Active metals replace hydrogen in water. Sodium is added to water. Reactants: Na + H 2 O Equations: 2 Na + 2 H 2 O H 2 + NaOH o Active metals replace hydrogen in acids Lithium is added to hydrochloric acid Reactants: Li + HCl Equation: Li + HCl H 2 + LiCl o Active nonmetals replace less active nonmetals from their compounds in aqueous solutions (SEE ACTIVITY SERIES HANDOUT). Chlorine gas is bubbled into a solution of potassium iodide. Cl 2 + KI KCl + I 2 Double Replacement Reactions o AB + CD AD + BC o Metals will interchange and new products will be formed. Use solubility rules to find if a precipitate will form. o AgNO 3 + NaCl NaNO 3 + AgCl All chlorides are soluble except silver chloride. AgCl is the solid. Combustion Reactions o Chemical + O 2 chemical oxides o C 3 H 8 + 5O 2 3CO 2 + 4H 2 O o S 8 + O 2 SO 3 o 2C 8 H O 2 16CO H 2 O
6 6 Outline 4b.4 Writing Net Ionic Equations Net Ionic Equations In overall ionic equations, formulas of the reactants and products are written to show the predominant form of each substance as it exists in aqueous solution. Soluble salts, strong acids, and strong bases are written as separate ions. Insoluble salts, suspensions, solids, weak acids, weak bases, gases, water and organic compounds are always written as compounds. Strong Acids HCl, HI, HBr, HNO 3, H 2 SO 4. HClO 3 Net ionic Reactions 1. Write the equation and put the phases (s, l, g, aq) of each chemical. 2. Balance the equation 3. Rewrite the equations splitting the (aq) substances Overall ionic equation. 4. Cancel any ions that are found on both sides of the equation spectator ions. 5. Rewrite what is left in the reaction net ionic equation. 6. Reduce if needed Aqueous solutions of sulfuric acid and excess sodium hydroxide are combined. 1. H 2 SO 4 (aq) + NaOH (aq) H 2 O (l) + Na 2 SO 4 (aq) 2. H 2 SO 4 (aq) + 2NaOH (aq) 2H 2 O (l) + Na 2 SO 4 (aq) 3. 2H +1-2 (aq) + SO 4 (aq) + 2Na +1 (aq) + 2OH -1 (aq) 2H 2 O (l) + 2Na +1-2 (aq) + SO 4 (aq) 4. Na +1 and SO -2 4 are spectator ions and are canceled 5. 2H +1 (aq) + 2OH -1 (aq) 2H 2 O (l) 6. Reduce: H +1 (aq) + OH -1 (aq) H 2 O (l)
7 7 Handout 4b.1a Activity Series Metals: Lithium Cesium Rubidium Potassium Barium Strontium Calcium Sodium Magnesium Aluminum Manganese Zinc Chromium Iron Cadmium Cobalt Nickel Tin Lead Hydrogen Copper Silver Mercury Platinum Gold (highest reactivity) (lowest reactivity) Metals from Lithium to Sodium will replace Hydrogen from acids and water; from Magnesium to Lead they will replace Hydrogen from acids only. Activity Series of Halogens: F 2 Cl 2 Br 2 I 2 (highest reactivity) (lowest reactivity)
8 8 Handout 4b.1b Activity Series The Activity Series is a list of many of the metals found in nature, and will help you predict whether or not a single replacement reaction will occur. The metals at the top of the list are highly reactive, and the metals at the bottom are largely inert. For the purposes of this activity, we shall consider the following abridged activity series: Lithium Magnesium Gold (highest reactivity) (lowest reactivity) Lithium, the most active metal, will replace either magnesium or gold in any compound, due to its relatively high activity. Magnesium will replace gold, but not lithium. Gold will not replace either of the other two metals. So: However, Li + MgCl 2 Mg + LiCl (lithium replaces magnesium in MgCl 2 ) Mg + LiCl No Reaction (magnesium will not replace lithium in LiCl) Confused? Well, it might be instructive to personify our metals and nonmetals with more human characteristics. Our assumptions: 1. Atoms are people dancing at a party. 2. Metals are men, and nonmetals are women. 3. Reactivity is equal to attractiveness. 4. Atoms are shallow, and are hung up on good looks. So, now, let s take another look, with a slightly modified activity series. Metals: Nonmetal: Lithium Most reactive Magnesium Gold Least reactive Chlorine
9 9 Handout 4b.1c Activity Series Once again, consider the reaction: Li + MgCl 2 Mg + LiCl This equation implies that Lithium was at the party alone, and saw Magnesium dancing with Chlorine. Lithium asked to cut in, and Chlorine said yes. Lithium then proceeded to dance with Chlorine, and Magnesium went off and cried in the corner, alone and dejected. + + Lithium Magnesium with Chlorine Magnesium Lithium with Chlorine So, given our earlier assumptions, the activity series implies that a nonmetal will leave a metal with low activity for a metal with high activity. However, the opposite is not true. Consider the opposite reaction: Mg + LiCl No Reaction This equation implies that Magnesium was at the party alone, and saw Lithium dancing with Chlorine. Magnesium asked to cut in, and Chlorine said no. Lithium then continued to dance with Chlorine, and Magnesium went off and cried in the corner, yet again. + + Magnesium Lithium with Chlorine Magnesium Lithium with Chlorine Using this technique, we can predict whether or not any single replacement reaction will occur. An attractive (highly reactive) single atom will replace a less attractive (less reactive) atom that is already in a couple. It gets a bit absurd, but it works. And don t feel bad for Gold. He ll be just fine. In fact, here s a picture of him with Lithium s ex-wife.
10 10 Handout 4b.2 Solubility Rules: Water-Soluble Salts: 1. All salts of the chloride ion, Cl -1, bromide ion, Br -1, and iodide ion, I -1, are soluble except those of Ag +1, Hg 2 +2, Pb +2, Cu +1, and Tl +1. BiI 3 and SnI 4 are insoluble. PbCl 2 is three to five times more soluble in hot water than in cold water. 2. All salts of the acetate ion CH 3 CO 2-1, nitrate ion, NO 3-1, chlorate ion, ClO 3-1, perchlorate ion, ClO 4-1, and permanganate ion, MnO 4-1, are soluble. 3. All common salts of the Group 1A cations and ammonium ion, NH 4 +1, are soluble. 4. All common salts of the sulfate ion, SO 4-2, are soluble except those of Ba +2, Sr +2, Pb +2, and Hg All Group 1A and 2A salts of the bicarbonate ion, HCO 3-1, are soluble. 6. Most salts of the fluorosilicate ion, SiF 6-2, thiocyanate ion, SCN -1, and thiosulfate ion, S 2 O 3-2, are soluble. Exceptions are the Ba +2 and Group 1A fluorosilicates, the Ag +1, Hg 2 +2, and Pb +2 thiocyanates, and the Ag +1 and Pb +2 thiosulfates. Water-Insoluble Salts: 1. All common salts of the fluoride ion, F -1, are insoluble except those of Ag +1, NH 4 +1, and Group 1A cations. 2. In general, all common salts of the carbonate ion, CO 3-2, phosphate ion, PO 4-3, borate ion, BO 3-3, arsenate ion, AsO 4-3, arsenite ion, AsO 3-3, cyanide ion, CN -1, ferricyanide ion, [Fe(CN) 6 ] -3, ferrocyanide ion, [Fe(CN) 6 ] - 4, oxalate ion C 2 O 4-2, and the sulfite ion, SO 3-2, are insoluble, except those of NH 4 +1 and the Group 1A cations. 3. All common salts of the oxide ion, O -2, and the hydroxide ion, OH -1, are insoluble except those of the Group 1A cations, Ba +2, Sr +2, and NH Ca(OH) 2 is slightly soluble. Soluble oxides produce the corresponding hydroxides in water. 4. All common salts of the sulfide ion, S -2, are insoluble except those of NH 4 +1 and the cations that are isoelectronic with a noble gas. 5. Most common salts of the chromate ion, CrO 4-2, are insoluble except those of NH 4 +1, Ca +2, Cu +2, Mg +2, and the Group 1A cations. 6. All common salts of the silicate ion, SiO 3-2 are insoluble except those of the Group 1A cations.
11 11 Worksheet 4b.1 Classifying Reactions Name Classify and balance the following reactions. 1. S 8 + O 2 SO 2 2. Fe(OH) 3 + H 2 SO 4 Fe 2 (SO 4 ) 3 + H 2 O 3. Zn + HCl ZnCl 2 + H 2 4. KClO 3 KCl + O 2 5. AgNO 3 + H 2 S Ag 2 S + HNO 3 6. P 4 + O 2 P 2 O 5 7. C 9 H 20 + O 2 CO 2 + H 2 O 8. C 3 H 8 + O 2 CO 2 + H 2 O 9. H 2 O 2 H 2 O + O Na + H 2 O NaOH + H S 8 + O 2 SO Zn + NaOH Na 2 ZnO 2 + H MgCl 2 + NaOH Mg(OH) 2 + NaCl 14. C 6 H 14 + O 2 CO 2 + H 2 O 15. NaNO 3 NaNO 2 + O 2
12 12 Worksheet 4b.2 Double Replacement NAME Put numbers in the blanks to balance the following equations. Using the Solubility Rules, rewrite the equations as overall equations, ionic equations, and net-ionic equations. Be sure to include identification of phases, like (s), (l), (g), or (aq) in the reactions. DOUBLE REPLACEMENT (also known as METATHESIS): REACTION: Na 2 SO 4 + Ba(NO 3 ) 2 NaNO 3 + BaSO 4 CuHCO 3 + KBr CuBr + KHCO 3 MgCrO 4 + BaI 2 MgI 2 + BaCrO 4 NH 4 CN + Fe(NO 3 ) 3 NH 4 NO 3 + Fe(CN) 3
13 13 Worksheet 4b.3 Synthesis Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O 1. Solid beryllium is left in a container with liquid bromine. 2. Solid bismuth is burned in air. 3. Cesium is put in a container with chlorine gas. 4. Phosphorus trichloride is placed in a chlorine rich atmosphere. 5. Solid magnesium oxide is placed in water 6. Sulfur trioxide is bubbled through water. 7. Solid gold is added to fluorine gas. 8. Solid calcium oxide is added to water. 9. Nitrogen monoxide gas is bubbled through water. 10. Hydrogen and oxygen gases are mixed.
14 14 Worksheet 4b.4 Decomposition Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O 1. Potassium hydroxide is heated. 2. Lithium chlorate decomposes by heating. 3. Sodium carbonate is heated. 4. Sulfurous acid is boiled. 5. Molten aluminum chloride is electrolyzed. 6. A sample of magnesium carbonate is heated. 7. A sample of ammonium carbonate is heated. 8. Carbonic acid is boiled. 9. Hydrogen peroxide decomposes. 10. Ammonium hydroxide is heated.
15 15 Worksheet 4b.5a Single Replacement Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O 1. A piece of copper is dropped into a container of water. 2. Liquid bromine is added to a container of sodium iodide crystals. 3. An aluminum strip is immersed in a solution of silver nitrate. 4. Zinc pellets are added to a sulfuric acid solution.
16 16 Worksheet 4b.5b Single Replacement Predictions 5. Fluorine gas is bubbled into a solution of aluminum chloride. 6. Magnesium turnings are added to a solution of lead (II) acetate. 7. Iodine crystals are added to a solution of sodium chloride. 8. Calcium metal is added to a solution of nitrous acid. 9. A pea-size piece of lithium is added to water. 10. A solution of iron (III) chloride is poured over a piece of platinum wire.
17 17 Worksheet 4b.6a Double Replacement Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O 1. Ammonium sulfate and potassium hydroxide are mixed together. 2. Ammonium sulfide is reacted with hydrochloric acid. 3. Cobalt (II) chloride is combined with silver nitrate. 4. Solid calcium carbonate is reacted with sulfuric acid.
18 18 Worksheet 4b.6b Double Replacement Predictions 5. Potassium sulfite is reacted with hydrobromic acid. 6. Potassium sulfide is reacted with nitric acid. 7. Ammonium iodide is mixed with magnesium sulfate. 8. Solid titanium (IV) carbonate is added to hydrochloric acid. 9. Solid calcium sulfite is mixed with acetic acid. 10. Strontium hydroxide is added to ammonium sulfide.
19 19 Worksheet 4b.7 Combustion Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O 1. Ethanol is burned completely in air. 2. Propane is heated with oxygen gas. 3. Octane is burned in oxygen gas. 4. Copper (II) Sulfide is burned in air. 5. Solid Phosphorus is burned in air. 6. Barium sulfide is burned in air. 7. Iron is added to an oxygen rich environment. 8. Ethane is burned in oxygen gas. 9. Methane is burned in air. 10. Propanol is burned in air.
20 20 Worksheet 4b.8 Mixed Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O REACTION: C 5 H 12 + O 2 Zn + HCl Na 2 O Li + Cl 2 Na 2 SO 4 + LiCl C 4 H 10 + O 2 Al 2 O 3 Al + I 2 Zn(OH) 2 + Al 2 (CO 3 ) 3 FeCl 3
21 21 Worksheet 4b.9 Mixed Predictions NAME Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B AB AB A + B AX + B BX + A AX + BY BX + AY C x H y + O 2 CO 2 + H 2 O REACTION: CuCl 2 + Na 3 PO 4 C 12 H 26 + O 2 FeCl 3 K 2 SO 4 + Li Na + O 2 C 3 H 8 + O 2 KMnO 4 + Li Na 3 P + Ba(OH) 2 H 2 O HCl + Ca(OH) 2
22 22 Worksheet 4b.10 Mixed Predictions NAME Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. REACTION: Mg + O 2 AlCl 3 Na + O 2 HCl + NaOH Pb(SO 4 ) 2 + Al(C 2 H 3 O 2 ) 3 C 4 H 10 + O 2 H 3 PO 4 + MgCO 3 HgCl 2 + NaSCN PtO 2 + H 2 CaCO 3 + NaCl Ag + HNO 3 NCl 3 MgSO 4 7H 2 O
23 23 Worksheet 4b.11 Mixed Predictions NAME Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. REACTION: Sr + O 2 Na + H 2 O Zn + HCl ICl Fe(OH) 3 + H 2 SO 4 C 6 H 14 + O 2 Au(OH) 3 + Na 2 CO 3 SrCl 2 + NaOH OCl 2 AgNO 3 + H 2 SO 4 Zn + O 2 Mg(OH) 2 + NaF C 30 H 62 + O 2 Mg(NO 3 ) 2 + H 2 O Au 2 S 3 Ti(MnO 4 ) 4 + Fe 2 O 3 MnF 2 + O 2 CO 2
Balancing Equations Notes
. Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationelemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
More informationChemical Reactions and Equations
Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new
More informationSCH4U Chemistry Review: Fundamentals
SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.
More informationCHAPTER Describing Chemical Reactions Reactants Products. New substances produced The arrow means yields TYPES OF EQUATIONS.
CHAPTER 11 Chemical Reactions 11.1 Describing Chemical Reactions Reactants Products New substances produced The arrow means yields Where do Chemical Reactions occur? Everywhere!!! In living organisms In
More informationBalancing Equations Notes
. Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting
More informationPart 01 - Notes: Reactions & Classification
Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationBALANCING EQUATIONS NOTES
BALANCING EQUATIONS NOTES WHY DO WE NEED TO BALANCE CHEMICAL EQUATIONS? The LAW OF CONSERVATION OF MASS says that matter cannot be created or destroyed. In other words, you cannot end up with any more
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationUnit Learning Targets (L.T.):
Unit 9: Chemical Equations and Reactions Chapters 8 and 19 Name Block Unit Learning Targets (L.T.): By the end of the unit, students will be able to: Chapter 8: 1. Correctly write and balance chemical
More informationUnit IV: Chemical Equations & Stoichiometry
Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations
More informationSCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4
Lesson Topics Covered 1 Note: Chemical Reactions and Chemical Equations definition of chemical reaction four signs of chemical change the Law of Conservation of Mass balancing chemical equations SCH 3UI
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
More informationReaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
More informationThe names of the reactants are: The names of the products are: The name of the product is:
CLASSIFICATION OF EQUATIONS WORKSHEET Chemical reactions produce new substances with new properties. The starting materials in a chemical reaction are called reactants while the materials that are formed
More informationName HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are
More informationExam 3. Objectives: Nomenclature
Exam 3 Objectives: o Nomenclature m-nm, m(vos)-nm, nm-nm o Evidence for Chemical Reactions o Writing Chemical Equations o Balancing Chemical Equations o Classifying Chemical Reactions o Combination Reactions
More informationTypes of Reactions. There are five types of chemical reactions we observed in the lab:
Chemical Reactions Acids and Bases Acids: Form hydrogen ions (H + ) when dissolved in water. HCl (aq) H + (aq) + Cl - (aq) Examples: HCl (hydrochloric acid), HNO 3 (nitric acid), H 2 SO 4 (sulfuric acid),
More informationUnit 8 Chemical Reactions- Funsheets
Part A- Balancing Equations and Types of Reactions Balance AND identify the following reactions: Unit 8 Chemical Reactions- Funsheets 1) Mg + Zn(NO 3) 2 Zn Mg(NO 3) 2 2) Ba + AgNO 3 Ag + Ba(NO 3) 2 3)
More informationUnit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
More informationTypes of Reactions. There are five main types of chemical reactions we will talk about:
Chemical Reactions Types of Reactions There are five main types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement
More information26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O
Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationChemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
More informationWRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included.
WRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationEXPERIMENT 10: Precipitation Reactions
EXPERIMENT 10: Precipitation Reactions Metathesis Reactions in Aqueous Solutions (Double Displacement Reactions) Purpose a) Identify the ions present in various aqueous solutions. b) Systematically combine
More informationYou try: 2) HC 7H 6O 2 3) N 2O 5. 5) HClO 4. 7) Rb 2C 2O 4 8) H 3PO 4 9) AgI 10) Sr(OH) 2. What kind of compound is it? NON ELECTROLYTE (NE)
Solubility: Solubility is the measure of how much of a solute will dissolve in a solvent. In general chemistry, we usually talk about water as the solvent, so we are talking about what compounds will dissolve
More informationName: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products)
Unit 8: Balancing and Identifying Chemical Reactions Packet Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products) C O 2 CO
More informationTypes of Chemical Reactions
Types of Chemical Reactions There are five types of chemical reactions: 1. Formation (combination) 2. Decomposition 3. Single Displacement 4. Double Displacement 5. Combustion 1 Formation (Combination)
More informationChapter 5 Classification and Balancing of Chemical Reactions
Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical
More informationChapter 8. Chemical Equations and Reactions
Chapter 8 Chemical Equations and Reactions Chemical Equations Represents, w/ symbols & formulas, the reactants & products in a chemical reaction Requirements Must represent the known facts Must contain
More informationIonic Compound Solubility. Ionic Compound Solubility. Nitrates (NO 3 - ) Chlorates (ClO 3 - ) Ionic Compound Solubility. Ionic Compound Solubility
Nitrates (NO 3 - ) Chlorates (ClO 3 - ) Perchlorates (ClO 4 - ) Acetates (C 2 H 3 O 2 - ) Alkali Metal Compounds (Li +,Na +,K +,Rb +,Cs + ) Ammonium Compounds (NH 4 + ) Chlorides (Cl - ) Bromides (Br -
More informationCHEMICAL REACTIONS WORDS, SYMBOLS AND ABBREVIATIONS
CHEMICAL REACTIONS All chemical reactions have two parts: (1) A substance that undergoes a reaction is called a. In other words, reactants are the substances you start with. (2) When reactants undergo
More informationVarious Types of Reactions
Various Types of Reactions Matthew Park Outline: 1. Synthesis / Replacement / Decomposition Reactions 2. Precipitation Reactions 3. Acid-Base Reactions 4. Summary: Metathesis Reactions NOTE: Not all of
More information1. Parts of Chemical Reactions. 2 H 2 (g) + O 2 (g) 2 H 2 O(g) How to read a chemical equation
Unit 6 Chemical Reactions 1. Parts of a Chemical Reaction 2. Indicators of a Chemical Reaction 3. Enthalpy 4. Balancing Chemical Equations 5. Word Equations 6. Classifying Chemical Reactions 7. Predicting
More informationTypes of Chemical Reactions (rxns.)
Types of Chemical Reactions (rxns.) Introduction Chemical reactions occur when bonds (between the electrons of atoms) are formed or broken Chemical reactions involve changes in the chemical composition
More informationIdentify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.
Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric
More informationIntro to Reactions/ Balancing Equations
Intro to Reactions/ Balancing Equations Chemical Reactions Chemical reactions involve change. Evidence of a chemical reaction could include the following Evolution of heat, light, and/or sound Production
More informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More information1. Naming and Writing Formulas 2. Writing Chemical Equations 3. Balancing Reactions
Chemistry 11 Stoichiometry I Name: Date: Block: 1. Naming and Writing Formulas 2. Writing Chemical Equations 3. Balancing Reactions Naming and Writing Formulas Key Points for naming ionic compounds: Cations
More informationIndicators of chemical reactions
Indicators of chemical reactions Emission of light or heat Formation of a gas Formation of a precipitate Color change Emission of odor All chemical reactions: have two parts Reactants - the substances
More informationCh. 8 Chemical Reactions
Ch. 8 Chemical Reactions Intro to Reactions I II III IV V Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change Law of Conservation of Mass
More informationCHEMICAL REACTIONS. Types of Reactions. Steps to Writing Reactions
Types of Reactions CHEMICAL REACTIONS There are five types of chemical reactions we will talk about: 1. Synthesis reactions 2. reactions 3. Single displacement reactions 4. reactions 5. Combustion reactions
More informationHonors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationFunsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017
Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +
More informationHonors Chemistry - Unit 7 Chapter 11 Chemical Reactions
Honors Chemistry - Unit 7 Chapter 11 Chemical Reactions Vocab Assignment Due: Unit 7 Packet - Page 1 of 15 UT Quest(s): Quiz on Diatomic Molecules & Balancing: Prediction Quiz : Test Date: VOCABULARY Assignment
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationHonors Chemistry - Unit 5 Chapter 8 Chemical Equations Quiz on Diatomic Molecules: Tues., Nov. 15th Test Date: Fri., Nov. 26th
Honors Chemistry - Unit 5 Chapter 8 Chemical Equations Quiz on Diatomic Molecules: Tues., Nov. 15th Test Date: Fri., Nov. 26th VOCABULARY Assignment Use the Two-column Notes format/strategy to study/complete
More informationH 2 O. Chapter 9 Chemical Names and Formulas
H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:
More informationChemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
More information2. Indicators of Chemical Rxns. Abbreviations of State (g) gas (l) liquid (s) solid (aq) aqueous a substance dissolved in water
Unit 6 Chemical Reactions 1. Parts of a Chemical Reaction 2. Indicators of a Chemical Reaction 3. Enthalpy 4. Balancing Chemical Equations 5. Word Equations 6. Classifying Chemical Reactions 7. Predicting
More informationUnit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
More informationNet Ionic Equations. Making Sense of Chemical Reactions
Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are
More informationName Honors Chemistry / / Chemical Equations Reactions
Name Honors Chemistry / / Chemical Equations Reactions Like everything else in chemistry, chemical equations follow a few basic patterns. Today we will begin to look at the first of these patterns and
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More information7.01 Chemical Reactions
7.01 Chemical Reactions The Law of Conservation of Mass Dr. Fred Omega Garces Chemistry 100 Miramar College 1 Chemical Reactions Making Substances Chemical Reactions; the heart of chemistry is the chemical
More informationBalancing CHEMICAL EQUATIONS
Balancing CHEMICAL EQUATIONS CHEMICAL REACTIONS involves a chemical change in the identity of one or more chemical species Ex. Rusting of iron (Fe): chemical rxn btwn water and iron involve the breaking
More informationUnit 6.3 Types of Chemical reactions
Unit 6.3 Types of Chemical reactions Most chemical reactions can be classified into one of five types of reactions. It depends on both the reactants used and the products formed. The possible chemical
More informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
More informationReactions in aqueous solutions Redox reactions
Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and
More informationChapter 7: Chemical Reactions
C h a p t e r 7, C h a p t e r 1 6 ( 2-5 ) : C h e m i c a l R e a c t i o n s P a g e 1 Chapter 7: Chemical Reactions Read Chapter 7 and Check MasteringChemistry due dates. Evidence of Chemical Reactions:
More informationChapter 9. Vocabulary Ch Kick Off Activity. Objectives. Interpreting Formulas. Interpreting Formulas
Chapter 9 Chemical Vocabulary Ch. 9.1 Chemical reaction Reactant Product Word Equation Skeleton Equation Chemical equation Coefficient 1 2 Objectives Write chemical equations to describe chemical reactions
More information7.01 Chemical Reactions
7.01 Chemical Reactions The Law of Conservation of Mass Dr. Fred Omega Garces Chemistry 152 Miramar College 1 Chemical Reactions Making Substances Chemical Reactions; the heart of chemistry is the chemical
More informationAP CHEMISTRY SUMMER ASSIGNMENT
For: Students enrolled in 2014-2015 AP Chemistry Course From: Mrs. Vanessa Urteaga (L-154) *This assignment is a recommendation. It is a review of things you should have mastered in Chemistry I or Pre-AP
More informationAP Chemistry Summer Assignment
AP Chemistry Summer Assignment Due Date: Thursday, September 1 st, 2011 Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number of significant
More informationChemical Reaction Types
Chemical Reactions Chemical Reaction Types There are 5 types of chemical reactions that you need to know Combination reaction Decomposition reaction Combustion reaction Single replacement (redox) reaction
More informationThe photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
More informationChemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions
Chemical Reactions and Equations Types of Reactions Predicting Products Activity Series Identifying Oxidation-Reduction Reactions A preview of things we will do Chemical Reactions are AWESOME! Characteristics
More informationChapter 9. Chemical Reaction
Chapter 9 Chemical Reaction Everyday Chemical Reaction O Can you name some? O Cooking Pizza O Changes the ingredients O Combustion O Driving to school burns gasoline O Wheelbarrow rusting (especially in
More informationQuestion 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate
Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O
More informationAP CHEMISTRY SUMMER ASSIGNMENT
For: Students enrolled in 2017-2018 AP Chemistry Course From: Mrs. Vanessa Urteaga (L-154) Edmodo Code: https://www.edmodo.com/home#/join/nidt95 or aszj8baszj8b This assignment is a review of things you
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationNomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds
PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common
More informationChemical Reactions. All chemical reactions can be written as chemical equations.
Chemical Reactions All chemical reactions can be written as chemical equations. What is a Chemical Reaction? Chemical reactions represent chemical changes A chemical change occurs when a substance has
More informationName CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are two
More informationTopic: Chemical Equations
Chemical Equations Lesson Objectives List evidence that suggests that a chemical reaction has occurred and evidence that proves that a chemical reaction has occurred. Describe a chemical reaction by using
More informationHonors Chemistry - Unit 5
Honors Chemistry - Unit 5 Chapter 8 Chemical Equations Unit 5 Packet - Page 1 of 18 Quiz on Diatomic Molecules: Tues., Nov. 9 th Vocab Assignment Due: Tues., Nov. 9 th Problem Set Due: Wed., Nov. 17th
More informationEquations. Chemical Reactions #1
Equations Chemical Reactions #1 equations show the complete chemical formulas. Does not indicate ionic character equation shows all ions. Actually how the particles exist in the solution Steps for Writing
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationUNIT 9 - STOICHIOMETRY
General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount
More informationCHEM 1364 Test #1 (Form A) Spring 2010 (Buckley)
Name CHEM 1364 Test #1 (Form A) Spring 2010 (Buckley) If you get stuck on one item, just go to the next and come back later. Point possibilities are indicated in parentheses to the right of each problem
More informationCHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
More informationNotes: Chemical Reactions. Diatomic elements: H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 I Bring Clay For Our New Hut OR HOBrFINCl
Name Chemistry-PreAP Notes: Chemical Reactions Period Review: Some elements do not occur as single atoms when uncombined with other elements. They will bond with themselves, forming a molecule. In any
More informationCHEMICAL REACTION. Engr. Yvonne Ligaya F. Musico 1
CHEMICAL REACTION Engr. Yvonne Ligaya F. Musico 1 Chemical Reaction Engr. Yvonne Ligaya F. Musico 2 Introduction Chemical reactions occur when bonds between the outermost parts of atoms are formed or broken
More informationPractice Packet Unit 3: Moles & Stoichiometry
PRACTICE PACKET: Unit 3 Moles & Stoichiometry Regents Chemistry: Mr. Palermo Practice Packet Unit 3: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson
More informationExam III Material Chapter 7-CHEMICAL REACTIONS, continued
Exam III Material Chapter 7-CHEMICAL REACTIONS, continued A chemical reaction occurs when there is a change in chemical composition. I. Double Replacement/Double Exchange/Metathesis Reactions In an double
More informationSNC2D Chemistry Review
SNC2D Chemistry Review 1. For each of the following elements: (a) Draw the Bohr-Rutherford diagram for the neutral atom (b) Determine the charge of the ion each element forms (c) Draw the Lewis dot diagram
More informationTypes of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
More informationFe(s) + O2(g) Chapter 11 Chemical Reactions. Chemical Equations. Fe + O2. January 26, What is a chemical reaction?
Chapter 11 Chemical Reactions What is a chemical reaction? Chemical Reaction: process by which one or more substances are changed into one or more different substances. Indications of a chemical reaction
More informationREVIEW OF BASIC CHEMISTRY ANSWER KEY
REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F
More informationIONIC CHARGES. Chemistry 51 Review
IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from
More informationChapter 6 Chemical Names and Formulas
Chemistry/ PEP Name: Date: Chapter 6 Chemical Names and Formulas Chapter 6: 1 9, 12, 14 24, 26 28, 31 36, 40, 42, 49, 52, 53, 56, 58, 62, 67 (37 total) 1. Provide the name and symbol of the ion formed
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationChapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
More information