Unit 6 chemical reactions
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Unit 6 Chemical Reactions. Objectives. Write chemical equations to describe chemical reactions Balance chemical equations Classify and identify chemical reactions Predict products from chemical reactions. I. Reactions and equations. Chemical reactions: A chemical change has occurred

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Unit 6 chemical reactions

Unit 6 Chemical Reactions


Objectives
Objectives

  • Write chemical equations to describe chemical reactions

  • Balance chemical equations

  • Classify and identify chemical reactions

  • Predict products from chemical reactions


I reactions and equations
I. Reactions and equations

  • Chemical reactions:

    • A chemical change has occurred

  • Evidence of a chemical reaction

    • Temperature change (energy

      change)

    • Change in color




  • Representing chemical reactions:

    • Reactants: starting substances (written on the left side)

    • Products: substances that result from the reaction (written on the right side)

    • Anarrowiswrittenbetweenreactants and products and isread as “yields”



  • Word Equations

    • Statementsusedtoindicatereactants and products

    • Lackimportantinformation

    • Ex.Hydrogen (g) + oxygen (g)  water (l)

  • Skeletonequations

    • Chemical formulas are usedtorepresentreactants and products

    • Ex. H2 (g) + O2 (g)  H2O (l)


Learning check
Learning Check:

  • Write the skeleton equations for the following:

  • Hydrogen (g) + Bromine (l)  hydrogen bromide (g)

  • Carbon monoxide (g) + oxygen (g)  carbon dioxide (g)


Practice
Practice:

  • Write the skeleton equations for the following:

  • Hydrogen (g) + Bromine (l)  hydrogen bromide (g)

    H2 (g) + Br2 (l)  HBr (g)

  • Carbon monoxide (g) + oxygen (g)  carbon dioxide (g)

    CO (g) + O2 (g)  CO2 (g)

    CW p 284 # 3, p 980 9.1 #1,2


Ii balancing chemical equations
II. Balancing chemical equations

  • Chemical equations:

    • Must obey “law of conservation of matter”

    • Must show that the number of atoms of each substance is the same before and after the reaction.

    • A chemical equation has to be BALANCED

    • To balance chemical equations, COEFFICIENTS (whole number)are written in front of a reactant or product.

    • If coefficient is 1, it is not written


  • Steps for balancing equations

  • Write the skeleton equation for the reaction. Ex. Hydrogen gas reacts with chlorine gas and yields gaseous hydrogen chloride.

    H2 (g) + Cl2 (g)  HCl(g)

  • Count the atoms of each substance for the reactants and products.


  • Place coefficients (ONLY IN FRONT OF A REACTANT OR PRODUCT) to make number of atoms of each element equal on both sides of the equation. (#atoms= coefficient x subscript)

H2 (g) + Cl2 (g)  HCl(g)



Practice1
Practice

1. Write a balanced chemical equation if sulfur trioxide when heated yields sulfur dioxide and oxygen.





Cw p balancing equations handout
CW p balancing equations handout


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