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Chemical Reactions

Learn how to classify compounds, interpret and balance chemical equations, and identify types of reactions and energy changes involved. Explore the Law of Conservation of Mass.

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Chemical Reactions

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  1. Chemical Reactions

  2. Chemistry (2/25) • Acid/Base Quiz • Interpreting and Balancing chemical equations Due: • Acid/Base Nomenclature worksheet for partial credit

  3. Chemical Reactions Objectives 1.Classify and name compounds in chemical reactions 2.Describe chemical reactions in word and chemicalequations. 3.Balance chemical equations based on the Law of Conservation of Mass. 4.Identify and classify types of chemical reactions and energy changes involved. 5.Predictproducts and energy changes in a chemical reaction. 6.Identify and testfactors that affect the rate of chemical reactions.

  4. Chemistry (2/26) Infinite Campus Update: • Acid/Base Nomenclature Worksheet (10pts.) • Acid/Base Quiz (15pts.) *Check infinite a lot of missing assignments!* Objectives: • Interpreting and Balancing chemical equations Homework: • Check for missing assignments on infinite campus • Balancing chemical equations worksheet

  5. Chemical Reaction Pre-Test • What is a chemical reaction? • If matter is conserved during a chemical reaction, how is it new matter is “created”? 3. Complete the questions below on the following word equation: Fe(s) + O2 (g) ----> FeO (s) • Give an example of a reactant from this reaction. • Give an example of a product from this reaction. • Balance the chemical equation if needed. • Circle the type of chemical reaction you think this represents. synthesis decomposition replacement neutralization combustion

  6. Chemical Reactions Substances chemically interact to form different substances. A substance can be an element or a compound. Chemical bonds are broken and created. Example: Fe(s) + O2 (g) ----> FeO (s)

  7. Chemical Equations Fe + O2 ------> FeO Reactants: Starting substances. Chemically interact with one another. Usually located to the left of the arrow. Products: Ending substances. Substances formed from the chemical reaction. Usually located to the right of the arrow.

  8. Chemical Equations Fe(s) + O2 (g) ------> FeO (s) Abbreviations for state of matter in an equation. (s)= substance in solid state (g)= substance in gaseous state (l)= substance in liquid state (aq)= substance dissovled in water. (aqueous solution)

  9. Law of Conservation of Mass Fe(s) + O2 (g) ------> FeO (s) • Are atoms destroyed or created during a chemical reaction? • No, they are just rearranged to produce new substances.

  10. Law of Conservation of Mass Fe(s) + O2 (g) ------> FeO (s)

  11. Balancing Chemical Equations Why? Observe the Law of Conservation of Mass Rules: 1. Add coefficients in front of substances, do NOT change subscripts. 2. First balance elements that only appear once on each side of the equation. 3. Make sure coefficients are expressed in lowest terms.

  12. Chemistry (2/27) Objectives: • Interpreting and Balancing chemical equations • Review acid/base quiz Homework: • Balancing equations worksheet(due Thursday) • Law of Conservation of Mass pre-lab qts. and hypothesis • Review acids/bases nomenclature • Check for missing assignments in infinite campus Lab: Law of Conservation of Mass Lab: (Thursday)

  13. Law of Conservation of Mass Lab Homework: • Read through the background and procedures section. • Complete pre-lab questions and hypothesis.

  14. Balancing Chemical Equations a. K + MgCl2 ---------> KCl + Mg b. Ag2O ---------> Ag + O2 c. CH4 + O2 -------> CO2 + H2O

  15. Chemical Equations

  16. Chemistry (2/28) Objectives: • Interpreting and Balancing Chemical Equations • Validate the Law of Conservation of Mass with scientific evidence. Due Today: • Balancing chemical equations worksheet (turn in tray) • Law of Conservation of Mass pre-lab qts. and hypothesis Homework: • Balancing Chemical Equations practice problems (Fri.) • Check for missing assignments in infinite campus

  17. Balancing Chemical Equations Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide

  18. Law of Conservation of Mass Lab Purpose: Validate the Law of Conservation of Mass Lab Reminders: • Follow ALL lab procedures carefully. • Use the same balance for all measurements.

  19. Acid/Base Nomenclature Quiz

  20. Exit Slip: Interpret and Balance Chemical Equations Cl2 (g) + KBr (aq) ----> KCl (aq) + Br2 (l) Balance the equation if needed CH4 (g) + O2 (g)  CO2(g) + H2O(g) Balance the equation if needed. Identify the diatomic molecule in this reaction.

  21. Exit Slip: Interpret and Balance Chemical Equations Cl2 (g) + KBr (aq) ----> KCl (aq) + Br2 (l) Which reactant is a molecule? What is the chemical name of the product that is an ionic compound? What does (aq) mean? Balance the equation if needed CH4 (g) + O2 (g)  CO2(g) + H2O(g) Balance the equation if needed. Identify the diatomic molecule in this reaction.

  22. Balancing Chemical Equations Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide • convert to chemical equation • Balance equation if needed.

  23. Law of Conservation Of Mass Matter is not created or destroyed. Matter is just rearranged. (mass of reactants = mass of products) That is why it is important to balance chemical equations.

  24. Law of Conservation of Mass Inquiry Lab • Purpose: To prove mass is conserved in chemical reactions. • Materials and Procedures: Groups will establish • Record and analyze data • Establish a conclusion

  25. Open vs. Closed System http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

  26. pre-AP Chemistry (2/20) Objectives: • Clarify misconceptions with writing and balancing chemical equations. • Validate the Law of Conservation of Mass (Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

  27. States of Matter Abbreviations Fe(s) + O2 (g) ------> FeO (s) Abbreviations for state of matter in an equation. (s)= substance in solid state (g)= substance in gaseous state (l)= substance in liquid state (aq)= substance dissovled in water. (aqueous solution)

  28. Chemical Equations • magnesium chloride + fluorine yields magnesium fluoride + chlorine 2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

  29. Pre-AP Chemistry (2/21) Reminder: • Quiz tomorrow over writing and balancing chemical equations. (complete extra practice problems from paper or webpage) Objective: • Validate the Law of Conservation of Mass (Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

  30. Pre-AP Chemistry (2/22) Reminder: • Quiz today over writing and balancing chemical equations. (complete extra practice problems from paper or webpage) Objective: • Validate the Law of Conservation of Mass (Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

  31. Chemical Equations

  32. Chemical Equations magnesium chloride + fluorine yields magnesium fluoride + chlorine 2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

  33. Law of Conservation of Mass Inquiry Lab • Purpose ,Background, Hypothesis: completed Objectives: • List materials needed for each experiment. • List procedures specific enough for someone else to repeat. (sign-off by Ms. Leeper) • Perform experiments and record data. (record all qualitative and quantiative data)

  34. Open vs. Closed System http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

  35. Chemical Reactions Bell Ringer 1. N2 (g) + H2(g) --------> NH3(g) • What is the chemical name of one of the reactants? b. What is the chemical name of the product? c. What state of matter is all the substances in this reaction? d. Balance the chemical equation if needed.

  36. Balancing Chemical Equations

  37. Types of Chemical Reactions 1. Synthesis (A+ B ----> AB) 2. Decomposition (AB------> A + B) 3. Single Replacement (A+ BC ---> B + AC) 4. Double Replacement (AB + CD ---> CB + AD) 5. Combustion (CxHx + O2 ----> CO2 + H2O) 6. Neutralization (Acid + Base--> H2O + Salt) *Each letter represents a substance*

  38. Chemical Reactions Objectives Identify and classify types of chemical reactions. 2. Identify energy changes involved with chemical reactions. 3. Predict products and energy changes in a chemical reaction.

  39. Synthesis (Combination) Reaction 2 or more substances chemically combine to form a single substance. A + B ---> AB + energy Energy released into surroundings is more than energy absorbed by the system. ( Energy of surroundings > Energy of system)

  40. Decomposition Reaction A compound breaks down into simpler substances. AB + energy ----> A + B Energy of system > Energy of surroundings Why?

  41. Single Replacement Reaction An element replaces another element in a compound. A + BC --------> B + AC + energy Energy of surroundings > Energy of system

  42. Double Replacement Reaction Exchange of cations between two compounds. AB + CD + energy ----> CB + AD + more energy Energy of Surrounding > Energy of System

  43. Combustion Reaction Fuel (hydrocarbons) reacts with oxygen to produce predictable substances and energy. CxHx + O2 ----> CO2 + H2O + ENERGY Energy of Surroundings > Energy of System

  44. Neutralization Acid and Base react to produce predictable products. Changes the pH to 7 (neutral). Acid + Base -------> H2O + Salt Salt:An ionic compound. The cation comes from the base and the anion from the acid.

  45. Class Reminders: • Acid Rain Article (15pts.) • Balance Chemical Equations Worksheet (10pts.) (balance and classify equations) • Word Equation Worksheet (10pts.) *3rd Quarter Ends: March 8th*

  46. Chemical Reaction Lab Purpose: • Perform and observe types of chemical reactions. • Determine reactants and predict products. • Classify chemical reactions. • Balance chemical reactions. • Write a formal lab report

  47. Chemical Equations to Lab

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