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Physical Science

Physical Science. Chapter 6 Chemical Reactions. Section 1 Observing Chemical Change. Objectives: Describe properties and changes in matter Explain how you can tell whether a chemical reaction has occurred. Changes in Matter.

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Physical Science

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  1. Physical Science Chapter 6 Chemical Reactions

  2. Section 1 Observing Chemical Change Objectives: Describe properties and changes in matter Explain how you can tell whether a chemical reaction has occurred

  3. Changes in Matter • Physical Change -A change that alters the form of a substance but not the chemical makeup of the substance, a change of state • Words like: crush, smash, tear, evaporate, slice, breakdown, dissolve, absorb, swell, burst • Chemical Change - One or more substances combine or decompose to form a chemically different substance • Words like: react, burns, forms, decomposed, rusting, sours, rotting, digesting, cooked, molecular change

  4. Matter & Its Changes Physical Changes – Alters form or appearance but doesn’t change it into another substance ie. Water evaporates into water vapor, a rock is broken into pieces It’s like printing a word in a different font, it’s the same word just looks different! stampedes  stampedes

  5. Matter & Its Changes • Chemical change- changes the material into a new substance i.e. hydrogen and oxygen combine to form water. • Chemical reactions take place when chemical bonds are either formed or broken. • Strong chemical bonds resist change: glass • Weak chemical bonds breakdown easily: wood • A chemical change is like scrambling letters to form new words made + steps  stampedes

  6. Chemical Reactions • Chemical reactions occur when chemical bonds are formed or broken • 2. Strong chemical bonds resist change: glass • 3. Weak chemical bonds breakdown easily: wood

  7. Evidence for Chemical Reactions • Chemical reactions produce new substances that can usually be detected by observing the evidence: • Color change • Precipitation • Temperature change • Property change • Gas produced

  8. Changes in Energy in Chemical Reactions • Every chemical reaction involves a change in energy. • Some reactions release energy in the form of heat (exothermic) • Some reactions absorb energy & the container holding the reaction gets colder to the touch (endothermic)

  9. Section 2 Describing Chemical Reaction Objectives: • Identify what information is in a chemical equation • Write a balanced chemical equation • Identify three categories of chemical reactions

  10. A. Chemical Reaction • A change in which one or more substances are converted to different substances. A+BC+D REACTANTS PRODUCTS

  11. Writing Chemical Reactions • Elements are represented by a one or two letter symbol • a. When symbol is a single letter: always capitalize: Hydrogen=H • b. When symbol is two letters, capitalize first letter & lower case second letter: Sodium = Na

  12. Writing Chemical Reactions C2H6 H2O C2H4 C2H2 • Chemical formulas show the ratio of elements found in molecules and compounds • a. Subscript numbers designate how many atoms of each element are present: H2O2 ; 2 Hydrogen atoms and 2 Oxygen atoms are present in this molecule • b. When no subscript number is shown: it is understood that there is only one atom present: H2O = 2 Hydrogen atoms and only one Oxygen atom are present in this molecule

  13. Structure of an Chemical Equation: Conservation of Mass - Matter cannot be created nor destroyed so there must be the same number of atoms on each side of the equation Beginning materials are reactants Ending materials are products Example of Chemical reaction: Reactant + Reactant Product + Product

  14. p. 444 C. Chemical Equations

  15. Structure of an Equation: yields

  16. Counting Atoms in an Equation CaCl2 Ca=1 Cl=2 Ca3(PO4)2 Ca=3 P=2 O=8 2Ca3(PO4)2 Ca=6 P=4 O=16 It’s best to list the # of atoms under the molecules as we are doing in these examples If no subscript present it is assumed to be 1 atom If elements in brackets or parenthesis, treat same as in math. Coefficients multiple the entire molecule atoms You must add all reactant atoms together & compare w/ all atoms in the products

  17. Balancing Equations This reaction IS NOT balanced 4 Reactant Hydrogens = 4 Product Hydrogens 2 Reactant Oxygens = 2 Product Oxygens This reaction is balanced! • Remember matter cannot be created or destroyed • Therefore the # of reactant atoms must equal the # of product atoms

  18. Balance this… Step 1: Count the atoms on both sides of the equation & compare ** you can only add or change whole # coefficients to balance equations. Never change subscripts Step 2: apply a coefficient to a molecule to balance an “easy” atom (in this case, we can add a 2 coefficient to the product water to balance the H’s) Step 3: Recount

  19. Balance this… (continued) Step 4: apply a coefficient to a molecule to balance the next off balanced atom (in this case, the oxygens are not yet balanced. We can add a coefficient of 2 in front of the reactant oxygen to correct this) Step 5: Recount Step 6: Continue doing this until all atoms are balanced BALANCED!!

  20. Classifying Chemical Reactions Objectives: • Define the three types of chemical reactions • Classify a chemical reaction based reviewing a chemical equation

  21. Classifying Chemical Reactions Synthesis/Combination: When two or more substances combine to form a more complex substance 2H2 + O2 2H2O Decomposition: When a complex substance is broken into two or more simpler substances: 2H2O 2H2 + O2 Replacement: When one element replaces another or when two elements in different compounds change places: 2CuO + C 2Cu + CO2

  22. Synthesis Reactions

  23. Decomposition Reactions

  24. Replacement Reactions • 2 types: • Single Replacement • Double Replacement

  25. Section 3 Controlling Chemical Reactions Objectives: • Explain how activation energy is related to chemical reactions • Identify factors that affect the rate of a chemical reaction

  26. Controlling Rates of Reaction Increase Surface Area Increased Temperature Increased Concentration Add a catalyst

  27. Getting Reactions Started The activation energyis the energy needed by a system to initiate the reaction. It is the minimum energy needed for a specific chemical reaction to occur. Once achieved, the reaction continues until reactants are extinguished.

  28. Catalysts (Enzymes are an example) • Help reactions happen but are not part of the reactants or the final product

  29. Combustion Reactions: Burning of any material in the presence of O2 Exothermic reaction Usually requires activation energy in the form of heat When carbon burns products are CO2 & H20 CH4 + 2O2  CO2 + 2H2O Combustion Reactions

  30. Enough is enough….Stop already!!OK

  31. Chapter Review • What is the difference between a chemical change and a physical change? • Chemical change makes a new substance • Physical Change changes only changes the form of a substance • Chemical reaction can usually be detected by observing what evidence? • Color change • Precipitation • Temperature change • Property change • Gas produced

  32. Chapter Review • Reactions that release energy in the form of heat are called? • Exothermic • Reactions that absorb energy & reduce the surrounding temperature are called? • Endothermic • In the chemical equation below, which are the products and the reactants? • A + B  C + B • A+ B = Reactants & C + B = Products • What do subscript numbers designate in a chemical formula? • How many atoms of each element are present in the molecule

  33. Chapter Review • What does the coefficient in front of an element or compound in a chemical equation designate? • How many of that element or compound are present in the equation • What does Conservation of Mass mean in a chemical equation? • Matter cannot be created nor destroyed so there must be the same number of atoms on each side of the equation • How do you balance the following: • CH4 + O2 CO2 + H2O • CH4 + 2O2 CO2 + 2H2O

  34. Chapter Review Name the reaction types: • 2H2 + O2 2H2O • Synthesis: When two or more substances combine to form a more complex substance • 2H2O 2H2 + O2 • Decomposition: When a complex substance is broken into two or more simpler substances • 2CuO + C 2Cu + CO2 • Replacement: When one element replaces another or when two elements in different compounds change places • CH4 + 2O2 CO2 + 2H2O • Combustion: When a substance reacts with oxygen and releases heat

  35. Chapter Review • What is the minimum energy needed for a chemical reaction to occur? • Activation energy is the energy needed by a system to initiate a reaction. • What controls the rate of a chemical reaction? • Temperature • Surface area • Concentration • Catalysts • Inhibitors

  36. Jeopardy Review Game • http://www.superteachertools.com/jeopardyx/jeopardy-review-game.php?gamefile=1320268214

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