Chemical Reactions
Chemical Reactions
Learning Targets:
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I can describe evidence of a chemical reaction from experimental observations.
I can balance chemical equations to fulfill the Law of Conservation of Mass
I can interpret changes in matter and energy from complete chemical equations
I can write chemical reactions by interpreting word equations
I can classify reaction types (synthesis, decomposition, single replacement, double replacement, combustion)
I can predict the products of chemical reactions in writing complete chemical equations
(synthesis, decomposition, single replacement, double replacement, and combustion)
Chemical Reactions
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Chemical Reaction: a process in which one or more substances are converted into new substances with different
chemical and physical properties
? Reactants ¡ú Products
? ¡ú means ¡°_________¡±
? chemical equation example: Fe(s) + O2(g) ? Fe2O3(s)
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Balanced Equations ¨C both sides of the equation must have the same _____________________ for each element
? Law of Conservation of Mass
? only _________________ may be adjusted to balance an equation
? NEVER change the _________________ which identify the substance (ex: H2O2 vs. H2O)
? example:
__ C(s) + __ O2(g) ¡ú __ CO2(g)
__ H2(g) + __ O2(g) ¡ú __ H2O (l)
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Word Equations use the name of the chemical to describe what is happening in the reaction
? example: Iron and oxygen react to produce iron (III) oxide
Basic Types of Reactions
examples:
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Synthesis/ Combination
2 Mg + O2 ? 2 MgO
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Decomposition
CaCO3 ? CaO + CO2
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Single Replacement
2 K + 2 H2O ? 2 KOH + H2
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Double Replacement
K2CO3 + BaCl2 ? 2 KCl + BaCO3
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Combustion
CH4 + 2 O2 ? CO2 + 2 H2O
5 signs/evidence of chemical reactions:
1. _______________________________
2. _______________________________
3. _______________________________
4. _______________________________
5. _______________________________
Honors Chemical Reactions 1 ?
Types of Chemical Reactions
To help make sense of all the different chemical reactions that exist, we classify reactions into several types.
There are five basic types of reactions.
Types
Pattern
Example
Synthesis
X + Y ? XY
2H2 + O2 ? 2H2O
Decomposition
AB ? A + B
H2CO3 ? H2O + CO2
Single Replacement
XY + A ? AY + X
Zn + 2HCl ? H2 + ZnCl2
Double Replacement
XY + AB ? XB + AY
2AgNO3 + K2CrO4 ? Ag2CrO4 + 2KNO3
Combustion
CxHy + O2 ? CO2 + H2O
C3H8 + 5 O2 ? 3 CO2 + 4 H2O
Classify each of the following reactions as S, D, SR, DR, or C and then balance the equation.
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1.
__ZnS + __HCl ? __ZnCl2 + __H2S
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2.
__H2CO3 ? __H2O + __CO2
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3.
__Al + __Fe3O4 ? __Al2O3 + __Fe
(page 2, 3, or 4) to practice
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4.
__H2 + __Br2 ? __HBr
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5.
__NaCl + __I2 ? __NaI + __Cl2
balancing equations and check
your progress
___
6.
__AlCl3 + __Na2CO3 ? __Al2(CO3)3 + __NaCl
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7.
__H2O ? __H2 + __O2
___
8.
__Ca(OH)2 + __H3PO4 ? __Ca3(PO4)2 + __H2O
___
9.
__NH4OH ? __H2O + __NH3
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10.
__NaOH + __(NH4)2SO4 ? __Na2SO4 + __H2O + __NH3
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11.
__C4H10 + __O2 ? __CO2 + __H2O
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12.
__C7H6O2 + __O2 ? __CO2 + __H2O
___
13.
__P4O10 + __H2O ? __H3PO4
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14.
__Fe + __HCl ? __H2 + __FeCl2
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15.
__H2O2 ? __H2O + __O2
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16.
__Fe2O3 + __H2SO4 ? __Fe2(SO4)3 + __H2O
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17.
__Zn + __HCl ? __H2 + __ZnCl2
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18.
__Fe + __CuSO4 ? __FeSO4 + __Cu
Evidence of Learning:
Complete any 15 problems
Honors Chemical Reactions 2 ?
Balance the equation and classify each reaction as synthesis, decomposition, singlereplacement, or double-replacement.
Balance the equation¡
¡and classify it.
1.
____ Sb + ____ Cl2 ? ____SbCl3
________________________
2.
____ Mg + ____O2 ? ____MgO
________________________
3.
____ CaCl2 ? ____ Ca + ____ Cl2
________________________
4.
____ NaClO3 ? ____ NaCl + ____ O2
________________________
5.
____ Fe + ____ HCl ? ____ FeCl2 + ____ H2
________________________
6.
____ CuO + ____ H2 ? ____ Cu + ____ H2O
________________________
7.
____ Al + ____ H2SO4 ? ____ Al2(SO4)3 + ____ H2
________________________
8.
____ MgBr2 + ____ Cl2 ? ____ MgCl2 + ____ Br2
________________________
9.
____ SnO2 + ____ C ? ____ Sn + ____ CO
________________________
10.
____ Pb(NO3)2 + ____ H2S ? ____ PbS + ____ HNO3
________________________
11.
____ HgO ? ____ Hg + ____ O2
________________________
12.
____ KClO3 ? ____ KCl + ____ O2
________________________
13.
____ N2 + ____ H2 ? ____ NH3
________________________
14.
____ NaBr + ____ Cl2 ? ____ NaCl + ____ Br2
________________________
15.
____ Zn + ____ AgNO3 ? ____ Zn(NO3)2 + ____ Ag
________________________
16.
____ Sn + ____ Cl2 ? ____ SnCl4
________________________
Honors Chemical Reactions 3 ?
Balance the equation¡
¡and classify it.
17.
____ Ba(OH)2 ? ____ BaO + ____ H2O
________________________
18.
____ Mg(OH)2 + ____ HCl ? ____ MgCl2 + ____ H2O
________________________
19.
____ Na2CO3 + ____ HCl ? ____ NaCl + ____ H2CO3
________________________
20.
____ NH4NO2 ? ____ N2 + ____ H2O
________________________
21.
____ N2 + ____ O2 ? ____ N2O5
________________________
22.
____ MgCO3 ? ____ MgO + ____ CO2
________________________
23.
____ KBr + ____ Cl2 ? ____ KCl + ____ Br2
________________________
24.
____ Zn + ____ CuSO4 ? ____ Cu + ____ ZnSO4
________________________
25.
____ P + ____ O2 ? ____ P4O6
________________________
26.
____ K + ____ H2O ? ____ KOH + ____ H2
________________________
27.
____ Al + ____ Pb(NO3)2 ? ____ Al(NO3)3 + ____ Pb
________________________
28.
____ Fe + ____ O2 ? ____ Fe3O4
________________________
29.
____ Li + ____ O2 ? ____ Li2O
________________________
30.
____ ZnCl2 + ____ KOH ? ____ Zn(OH)2 + ____ KCl
________________________
31.
____ Fe3O4 + ____ H2 ? ____ Fe + ____ H2O
________________________
32.
____ Pb(NO3)2 ? ____ Pb + ____ NO2 + ____ O2
________________________
33.
____ H2O ? ____ H2 + ____ O2
________________________
Honors Chemical Reactions 4 ?
Writing Word Equations
Ionic Formulas
metal + nonmetal
balance the charges
example: aluminum oxide
Al+3
O-2
Al2O3
Evidence of Learning:
Complete any 4 problems to practice writing
word equations and check your progress
Covalent Formulas
nonmetal + nonmetal
covalent prefix system
example: nitrogen dioxide
NO2
key words:
yields or produces or forms ?
combines or combines +
decomposes ? (for decomposition reactions)
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look out for ¡°HONClBrIF¡± elements! They are diatomic in their pure form.
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pure forms of sulfur and phosphorus are S8 and P4, respectively.
Write the formulas for the chemical reaction, balance, and classify the reaction type:
1. Sulfur dioxide gas combines with oxygen gas to produce sulfur trioxide.
2. When heated, calcium carbonate decomposes to form calcium oxide and carbon dioxide.
3. Barium oxide reacts with water to form barium hydroxide.
4. When heated, calcium sulfite decomposes to form calcium oxide and sulfur dioxide.
5. Iron reacts with sulfuric acid (H2SO4) to form Iron (III) sulfate and hydrogen gas.
6. Dinitrogen pentoxide reacts with water to produce nitric acid (HNO3).
7. Carbon reacts with zinc oxide to produce zinc and carbon dioxide
8. Bromine reacts with sodium iodide to form sodium bromide and iodine.
Honors Chemical Reactions 5 ?
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