1 / 48

Introduction to Chemical Reactions

Learn about the observable changes and energy changes that occur during chemical reactions, as well as the production of new materials. Understand how chemical bonds are broken and formed, and how chemical reactions can be written using symbols.

aguon
Download Presentation

Introduction to Chemical Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Introduction to Chemical Reactions (c) S. Coates 2012

  2. Observing chemical Reactions • Everything around us is made of atoms. These atoms are constantly interacting with each other. • We call those interactions chemical reactions, and they are happening EVERYWHERE. (c) S. Coates 2012

  3. Observing chemical Reactions • Evidence for Chemical Reactions • Chemical reactions involve observable changes. Make a List: What are some OBSERVABLE CHANGES that take place while roasting marshmallows? (Think of the fire and the marshmallow) (c) S. Coates 2012

  4. Observing chemical Reactions • Evidence for Chemical Reactions • The list you just came up with can be sorted into TWO lists… 1. Changes in Properties 2. Changes in Energy These are the TWO Main kinds of Observable Changes that take place in a chemical reaction. (c) S. Coates 2012

  5. Observing chemical Reactions • Changes in Properties include: • Gases Produced • Bubbles may appear in liquid • Color Change • Smell Change • Solid may appear when 2 solutions are mixed (*THIS IS CALLED A PRECIPITATE) (c) S. Coates 2012

  6. Watch the video below and look for CHANGES IN PROPERTIES. (c) S. Coates 2012

  7. Observing chemical Reactions • Changes in Properties • Q: What change in property did the Diet Coke go through during the chemical reaction in the video? • A: Increased “fizziness” or CO2 was the most observable change. (c) S. Coates 2012

  8. For example, sometimes TWO liquids will mix together and will form a SOLID. We call this solid a PRECIPITATE. (c) S. Coates 2012

  9. Observing chemical Reactions 2. Changes in Energy: • Some reactions ABSORB energy • Other reactions RELEASE energy • You can usually tell if something is absorbing or releasing energy because there is a CHANGE IN TEMPERATURE. (c) S. Coates 2012

  10. Observing chemical Reactions 2. Changes in Energy: • Reactions that ABSORB energy are called ENDOTHERMIC • Reaction that RELEASE energy are called EXOTHERMIC (c) S. Coates 2012

  11. Observing chemical Reactions • The BIGGEST observable characteristic of a chemical reaction is the production of NEW MATERIALS • The NEW MATERIALS will have properties that are different from those of the starting materials. (c) S. Coates 2012

  12. Observing chemical Reactions • Chemical Reactions occur when chemical bonds break or when new bonds form! Magnesium Metal (Mg) Magnesium oxide (MgO) Oxygen(O) (c) S. Coates 2012

  13. Observing chemical Reactions 2. Changes in Energy • Chemical Reactions happen because of the way chemicals are stuck together or “bonded”. • Some bonds are strong and hard to change…think of Glass. • Some bonds are weak…think of Wood. (c) S. Coates 2012

  14. Observing chemical Reactions • STOP AND REVIEW • What are some examples of evidence for a chemical reaction? • What two kinds of energy changes can take place during a chemical reaction? • What happens to the chemical bonds in a substance during a chemical reaction? • When a solid forms as two solutions are mixed together, what is that solid called? (c) S. Coates 2012

  15. Understanding Written equations (c) S. Coates 2012

  16. Understanding chemical Reactions • Group Activity! • Materials needed per group: • 20 different coins, each of any value • Paper and Pencil to record results (c) S. Coates 2012

  17. Procedure: • As a group arrange the coins on your desk into four random piles. • Count the value of each pile, then count the TOTAL value of the piles, and record it on your paper. • Do this TWO more times (rearrange the piles and count) for a total of 3 times. (c) S. Coates 2012

  18. Understanding Written Equations Understanding chemical Reactions • Analysis: • Did rearranging the coins change any individual coin? • Did rearranging the coins change the TOTAL value of the coins? • If you think of the coins as representing different types of atoms, what does this activity suggest about chemical reactions? (c) S. Coates 2012

  19. Understanding chemical Reactions • Think about our class. We have a group of students and a teacher. (c) S. Coates 2012

  20. Understanding chemical Reactions • When the bell rings, you all leave and a new group of students comes in, and all of you go to a new class room. (c) S. Coates 2012

  21. Understanding chemical Reactions • The number of students and teachers in the school has notchanged. But their arrangement is different and the new groups interact differently. (c) S. Coates 2012

  22. Writing chemical Reactions • We use symbols when writing chemical reactions. • Using these symbols makes it easier and faster to read and write reactions. • How else do you use symbols as a short-cut in daily life? (c) S. Coates 2012

  23. What do these symbols mean? (c) S. Coates 2012

  24. Writing chemical Reactions These one or two letter abbreviations are unique for each element (or type of atom). • A chemical equation is a shorter, easier way to show chemical reactions, using symbols instead of words. • These symbols come from the Periodic Table of the Elements. (c) S. Coates 2012

  25. Writing chemical Reactions Use a Periodic Table to determine what each of these symbols stand for: Record the symbol and what it stands for. Au Pb Ag Sn Fe Al Ca C (c) S. Coates 2012

  26. Writing chemical Reactions Au Pb Ag Sn Gold Lead Silver Tin Fe Al Ca C Iron Carbon Calcium Aluminum (c) S. Coates 2012

  27. Writing chemical Reactions • You have already seen many chemical formulas… H2O • What does the “H” stand for? • What does the “O” stand for? • What does the little “2” stand for? Hydrogen Oxygen There are TWO hydrogen atoms (c) S. Coates 2012

  28. Here are some familiar items. Use a Periodic Table of the Elements to record what these compounds are made of… Lowercase “L”, not an I. (c) S. Coates 2012

  29. Understanding Written Equations Writing chemical Reactions (c) S. Coates 2012

  30. Writing chemical Reactions • Structure of a chemical equation: Every chemical equation is written THE SAME WAY… Reactant + Reactant Product + Product Sometimes there are more than 2 reactants. Sometimes there is only 1 reactant. Sometimes there are more than 2 products. Sometimes there is only 1 product. (c) S. Coates 2012

  31. Writing chemical Reactions • See if you can answer the following questions for this chemical reaction: CaCO3CaO + CO2 (Heated) How many reactants are there? What is/are the reactant(s)? How many products are there? What is/are the product(s)? (c) S. Coates 2012

  32. Writing chemical Reactions CaCO3CaO + CO2 * Notice that the atoms we began with are the same atoms we end with, just in a different order! (Heated) Ca C O O O 3 2 (c) S. Coates 2012

  33. Understanding chemical Reactions • The amount of matter involved in a chemical reaction does not change. • The total mass of the reactants MUST EQUAL the total mass of the products. • We call this principle Conservation of Mass. (c) S. Coates 2012

  34. Writing chemical Reactions • How do you know if the mass of the products is equal to the mass of the reactants? • Subscript Numbers! • If you add up the NUMBER of EACH element on the reactant side and compare it to the NUMBER of the SAME element on the product side you can tell if the mass of the reactants is equal to the mass of the products. CaCO3CaO + CO2 (c) S. Coates 2012

  35. Understanding chemical Reactions • For example: Na + Cl NaCl 1. Count up the number of Na and Cl atoms on the reactant side. Na = 1 Cl = 1 2. Count up the number of Na and Cl atoms on the product side. Na = 1 Cl = 1 3. Compare the numbers. Are they the same? If so then the mass of the reactants and the products is equal. Yes! The masses are equal! (c) S. Coates 2012

  36. Understanding chemical Reactions • Here’s another: Fe2 + S2 Fe2S2 1. Count up the number of Fe and S atoms on the reactant side. Fe = 2 S = 2 2. Count up the number of Fe and S atoms on the product side. Fe = 2 S = 2 3. Compare the numbers. Are they the same? If so then the mass of the reactants and the products is equal. Yes! The masses are equal! (c) S. Coates 2012

  37. Understanding chemical Reactions • But what if the numbers are NOT equal? H2 + O2 H2O 1. Count up the number of H and O atoms on the reactant side. H = 2 O = 2 2. Count up the number of H and O atoms on the product side. H = 2 O = 1 3. Compare the numbers. Are they the same? NO! The masses are NOT equal! That makes this equation “unbalanced” (c) S. Coates 2012

  38. Understanding chemical Reactions • Try another one… CO2 + H2O  C6H12O6 + O2 1. Count up the number of C, H, and O atoms on the reactant side. C = 1 H = 2 O = 3 2. Count up the number of H and O atoms on the product side. C = 6 H = 12 O = 8 3. Compare the numbers. Are they the same? NO! The masses are NOT equal! That makes this equation “unbalanced” (c) S. Coates 2012

  39. Understanding chemical Reactions • What do you do when an equation is “unbalanced?” • That’s something you’ll be learning in high school Chemistry. • For now you just need to understand whether and equation is balanced or unbalanced. (c) S. Coates 2012

  40. Understanding chemical Reactions • Activity! “Is it Balanced?” • Materials Needed: • 1 envelop of activity cards per group (c) S. Coates 2012

  41. Understanding chemical Reactions • You are going to “build” each chemical reaction on your desks: • Example: Na + Cl NaCl (c) S. Coates 2012

  42. Understanding chemical Reactions • Build this equation: Analyze: Is your equation balanced? (Do you have the same number of Fe molecules on both sides of the equation on your desk? What about the S molecules?) (c) S. Coates 2012

  43. Understanding chemical Reactions • Build the following equations and identify whether they are balanced or unbalanced: (c) S. Coates 2012

  44. Understanding chemical Reactions • Now you can practice on your own! • Do the “Chemical Reactions” worksheet. • This will be due: _____________ (c) S. Coates 2012

  45. Understanding chemical Reactions • Build the following equations and identify whether they are balanced or unbalanced: (c) S. Coates 2012

  46. Understanding chemical Reactions • Need more practice? (c) S. Coates 2012

  47. Understanding chemical Reactions • Need more practice? (c) S. Coates 2012

  48. Understanding chemical Reactions • Let’s summarize: • Chemical reactions can cause changes in properties and changes in energy. • Chemical reactions occur when the bonds between atoms break, or when new bondsbetween atoms are formed. • We can write equations for chemical reactions by using symbols • Chemical reactions must follow the Law of Conservation of Mass. (c) S. Coates 2012

More Related