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Introduction to Chemical Reactions

Learn about chemical reactions and how they are everywhere in our daily lives. Discover different indicators of a chemical reaction and how to represent them using chemical equations. Understand the importance of balancing equations and the law of conservation of mass.

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Introduction to Chemical Reactions

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  1. Introduction to Chemical Reactions Making new substances

  2. Chemical Reactions are Everywhere Cooking Respiration

  3. Chemical Reactions are Everywhere Hair Dye Auto Fuel

  4. Demo Universal Indicator – shows pH Dilute ammonia + effervescent tablet (e.g. Alka Seltzer) What do you think is going to happen?

  5. What Happened during Demo? What did you observe during demonstration? Share your observations with someone sitting next to you

  6. How do you know when a chemical reaction takes place? Color Change Precipitate Formation

  7. How do you know when a chemical reaction takes place? Gas Formation Odor

  8. How do you know when a chemical reaction takes place? Temperature Change Change in Acidity

  9. Representing Chemical Reactions • Chemists observe chemical reactions and have come up with a way to represent or model what is happening. • Making NaCl • https://www.youtube.com/watch?v=2mzDwgyk6QM • Solid Sodium combines with Chlorine gas to make solid Sodium Chloride: 2Na (s) + Cl2 (g)  2NaCl

  10. Chemical Equations are different from Numerical Equations • Numerical Equation: 3x + 2y = 47 • Chemical Equation 2Na + Cl2  2NaCl • ReactantA + Reactant B  Product • The reactants are used up in forming the product • The arrow  shows the direction of the reaction

  11. Law of Conservation of Mass • In a chemical reaction, matter is neither created nor destroyed. • Atoms won’t change their identity (e.g. a Carbon atom can’t become an Iron atom) • This means that you have to have the same number of each type of atom on each side of the chemical equation. • Conservation of Mass Video

  12. Balancing Equations After you write a chemical equation you have to balance it to make sure that the same number of atoms of each element are on each side. How would you balance this equation? ____Ca + ____O2 ____ CaO

  13. Another Example • _____CH4 + ____O2  ____CO2 + ____H2O 7 ≠ 6! Where did our atoms go?

  14. Example Continued • CH4 + 2 O2  CO2 + 2H2O • Are your coefficients in their simplest ratio? • Count your atoms again to check your work:

  15. Try These! • C2H6 + O2 CO2 + H2O • N2 + H2 NH3 • Cu2O + C Cu + CO2 Think – Pair - Share

  16. Exit Ticket • Write the Law of Conservation of Mass. • List evidence that a chemical reaction has taken place. • Explain why chemists have to balance equations. • Balance this equation: ____Na + ____MgF2 ____NaF + ____Mg

  17. Review Matter is not destroyed or created Atoms are rearranged in chemical reactions Chemical equations represent chemical reactions You have to have the same number of each type of atom on the left and right hand side of a chemical equation

  18. WARNING! Don’t mess with the insides of polyatomic ions – put a square around them, or label them as X – treat the WHOLE polyatomic ion as though it were an element! Don’t ever play around with subscripts (those little numbers that tell you how many atoms are in a molecule) e.g. C6H22O11

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