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Chemical Equations

Learn about chemical equations, a shorthand notation for representing chemical reactions using chemical formulas and symbols. Understand how to balance equations and ensure the number of atoms on each side is equal.

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Chemical Equations

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  1. Chemical Equations

  2. Chemical symbol: A Quick Review… A shorthand notation for an element’s name. • Chemical formula: A shorthand notation for a compound or a molecule.

  3. Chemical reaction: A Quick Review… The process by which one or more substances undergo change to produce one or more different substances. • Writing out a chemical reaction can take a long time and isn’t universal, so there exists a simpler way to represent a chemical reaction called a…

  4. Chemical equation: Chemical Equations A shorthand notation of a chemical reaction using chemical formulas and symbols. • Example: C + O2 CO2

  5. C + O2 CO2 Parts of a Chemical Equation Reactants: the starting materials in a chemical reaction. (LEFT) - Written before the arrow. Products: the substances formed in a reaction. (RIGHT) - Written after the arrow.

  6. C + O2 CO2 Parts of a Chemical Equation Plus sign: reads: ‘reacts with’. Carbon reacts with dioxide Arrow: Reads ‘to produce’ or ‘to yield’ Carbon reacts with dioxide to yield Carbon dioxide.

  7. C + O2 CO2 Why We Counted Atoms The number of atoms we start with (reactants side) must equal the number of atoms we end up with (products side). All equations must be balanced. The number of atoms of each element in a reactant must equal the number of the same elements in the product. Reactants = Products

  8. C + O2 C O2 Why We Counted Atoms When counting atoms for each side, think of the yield sign as an equal sign. C + O2 = C O2 • The number of Carbon in the reactants must equal the number of Carbon in the product. • The number of Oxygen in the reactants must equal the number of Oxygen in the product.

  9. C + O2 C O2 Balancing the Equation • Divide the equation into a chart.

  10. C + O2 C O2 Balancing the Equation C O O • Count the number of atoms of each element on the reactants side using symbols to represent the number of atoms. • Are all atoms counted for on the left side? If so, we can move to the right side of the arrow.

  11. C + O2 C O2 Balancing the Equation C O C O O O • Repeat the same process for the right side as you did with the left side.

  12. C + O2 C O2 Balancing the Equation C O C O O O 1 1 • Start with Carbon and count each side. • Do we have an equal amounts of Carbon? Let’s move on to Oxygen

  13. C + O2 C O2 Balancing the Equation C O C O O O 2 2 • Now Count the Oxygen on each side. • Do we have an equal amounts of Oxygen? We have a BALANCED equation.

  14. C + O2 C O2 Balancing the Equation

  15. C O2 Balancing the Equation O2 + C

  16. A Balanced Equation C + O2 C O2

  17. H2 + O2 H2 O Balancing Example Dihydrogen reacts with Dioxideto yield Dihydrogen monoxide.

  18. H2 + O2 H2 O Balancing Example H O H O • Count the number of atoms of each element on the reactants side using symbols to represent the number of atoms.

  19. H2 + O2 H2 O Balancing Example H O H O H O H • Repeat the same process for the right side as you did with the left side.

  20. H2 + O2 H2 O Balancing Example H O H O H O H 2 2 • Start with Hydrogen and count each side. • Do we have an equal amounts of Hydrogen?

  21. H2 + O2 H2 O Balancing Example H O H O H O H 1 2 • Now count Oxygen on each side. • Do we have equal amounts of Oxygen?

  22. O H2 Balancing Example O2 + H2 • We cannot leave an equation unbalanced. What can be done to fix it?

  23. H2 + O2 H2 O Balancing Example H O H O H O H H H O

  24. H2 + O2 Balancing Example H2 O • The equation is still unbalanced. What can be done to fix it?

  25. H2 + O2 H2 O Balancing Example H H O H O H H O H H H O • Are Oxygen atoms equal on both sides? • Are Hydrogen atoms equal on both sides? Let’s try and fix Hydrogen.

  26. 2 H2 + 1 O2 2 H2 O Balancing Example H H O H O H H O H H H O • The number of boxes represents the coefficient. • What is the coefficient in front of H2O? • What is the coefficient in front of H2?

  27. A Balanced Equation 2 H2 + 1 O2 2 H2 O

  28. 1 H2 + 1 Cl2 2 H Cl Practice H Cl H Cl H Cl H Cl Dihydrogen reacts with dichloride to yield Hydrogen monocholoride.

  29. 1 N2 + 3 H2 2 N H3 Practice N H H H N H H H N H H H N H H H Dinitrogen reacts with dihydride to yield Nitrogen trihydride.

  30. 2 Na F + 1 Cl2 2 Na Cl + 1 F2 Practice Na F Cl Na Cl F Na F Cl Na Cl F Sodium Fluoride reacts with Dichloride to yield Sodium Chloride and Difluoride

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