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Balancing Chemical Equations and Types of Chemical Reactions. Boon Chemistry. Objectives. I can compare and contrast different types of chemical reactions. I can define and identify a balanced chemical equation. I can balance simple chemical equations. Parts of a Chemical Reaction.

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Presentation Transcript
objectives
Objectives
  • I can compare and contrast different types of chemical reactions.
  • I can define and identify a balanced chemical equation.
  • I can balance simple chemical equations.
parts of a chemical reaction
Parts of a Chemical Reaction

Cu (s) + 2 AgNO3 (aq) → Cu(NO3)2 (aq) + 2 Ag (s)

Reactants

Products

Letters in parentheses show the state of matter.

Coefficients (numbers) in front of a chemical formula show “how many.”

The arrow separates the reactants and products.

balancing a chemical reaction equation
Balancing a Chemical Reaction Equation
  • Atoms are not createdor destroyedduring a chemical reaction.
  • Scientist know that there must be the samenumber of atoms on each sideof the arrow.
slide5

Is it balanced?

__Cu + __ AgNO3 → __Cu(NO3)2 + __ Ag

Cu = Cu =

Ag = Ag =

NO3 = NO3 =

balancing a chemical reaction equation1
Balancing a Chemical Reaction Equation
  • To balance the chemical equation, you must add coefficientsto the different parts of the equation.

Cu (s) + 2 AgNO3 (aq) → Cu(NO3)2 (aq) + 2 Ag (s)

steps for balancing chemical reaction equations
Steps for Balancing Chemical Reaction Equations
  • Determine number of atoms for each element for the reactants and products separately.
  • Try to add coefficients to the equation to get the same number of atoms on each side.
  • Note: Coefficients multiply the atoms in the compound. Keep the compound formulas the same. Do not change subscripts.
  • Hint: Balance anything that is not hydrogen or oxygen first. Then balance hydrogen. Balance oxygen last.
why do we balance chemical reactions
Why do we balance Chemical Reactions?
  • http://www.youtube.com/watch?v=ODf_sPexS2Q
  • http://www.youtube.com/watch?NR=1&v=92Mfric7JUc&feature=endscreen
  • http://www.youtube.com/watch?v=IgU4nwdBrIA&feature=related
  • Focus Questions:
    • How are the two reactions the same? How are they different? Why?
    • If you wanted to do these reactions at home, what would you need to know?
law of conservation of mass

+

H2

O2

H2O

(g)

(g)

(l)

O

O

O

H

H

H

H

H

H

O

H

H

Law of Conservation of Mass
  • Matter cannot be created or destroyed in a chemical reaction
  • The number of atoms on the reactant side must equal the atoms of the products

Unbalanced!

Balanced!

balanced chemical equations
Balanced Chemical Equations
  • A chemical equation is “balanced” when there are the same number of atoms of each element on both sides of the arrow.

NaHCO3 (s) + HC2H3O2 (aq) èNaC2H3O2 (aq) + CO2 (g) + H2O (l)

Is it balanced?

is it balanced practice
Is it balanced? Practice
  • Determine the number of atoms of each element in the reactants and products. Then, state whether the equation is balanced.
  • P4 + O2 → P2O5
  • C3H8 + O2 → CO2 + H2O
  • Ca2Si + Cl2 → CaCl2 + SiCl4
  • Si + CO2 → SiC + SiO2

Not balanced.

Not balanced.

Not balanced.

Not balanced.

balancing equations

coefficient

+

H2

O2

H2O

(g)

(g)

(l)

Balancing Equations

2

2

  • Only the coefficients can be changed!

H =

O =

2

4

H =

O =

2

4

2

1

2

balancing tips
Balancing Tips
  • Always balance non-Oxygen’s & Hydrogen’s first (ex. Chlorine)
  • Then balance Hydrogens
  • Balance Oxygens Last
balancing practice
Balancing Practice!

P4 + O2 → P2O5

P4 + 5 O2 → 2 P2O5

Ca2Si + Cl2 → CaCl2 + SiCl4

Ca2Si + 4 Cl2 → 2 CaCl2 + SiCl4

Si + CO2 → SiC + SiO2

2 Si + CO2 → SiC + SiO2

C3H8 + O2 → CO2 + H2O

C3H8 + 5 O2 → 3 CO2 + 4 H2O

overview of major chemical reaction types
Overview of Major Chemical Reaction Types
  • Synthesis
  • Decomposition
  • Single-Replacement
  • Double-Replacement
  • Combustion
1 synthesis reactions

+

H2

O2

H2O

(g)

(g)

(l)

H

H

O

O

H

H

H

H

H

H

1. Synthesis Reactions
  • Two substances combine to make one
  • Synthesismeans “to make”

O

O

a b ab
A + B  AB

SYNTHESIS

Na + Cl2 NaCl

2 decomposition reactions

NH3

(l)

N2

+

H2

(g)

(g)

2. Decomposition Reactions
  • One substance breaks down into 2
  • Decompositionmeans “to break down” or “decay”

H

H

H

H

N

N

H

H

ab a b
AB  A + B

Decomposition

NaCl  Na + Cl2

one element replaces another in a compound
one element replaces another in a compound

3. SINGLE REPLACEMENT

AB + C  AC + B

4 double replacement
4. DOUBLE REPLACEMENT

Both elements in two compounds switch places

AB + CD  AD + CB

slide24

Double Replacement

NaBr + Pb2S3 Na2S + PbBr3

K2SO4 + Ba(OH)2

KOH + BaSO4

5 combustion reactions

CH4

C2H4

+

+

O2

O2

CO2

CO2

+

+

H2O

H2O

C6H12O6

+

O2

CO2

+

H2O

5. Combustion Reactions
  • A hydrocarbon reacts with oxygen gas to produce carbon dioxide and water vapor
  • Combustionmeans to “burn in oxygen”