Module 6 Intro
1. Module 6 Intro
1.4. Page 2
Module 6—Stoichiometry
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Read
Read “2.5 Classifying Chemical Reactions” on pages 58 and 59 of your textbook, and then turn to pages 62 and 63 and read about single replacement and double replacement reactions. To summarize what you have read, copy into your notebook the information in “Table 3: Reaction Generalizations” on page 63. Place a copy of your summary in your course folder so that it is convenient for you to access it.
Self-Check
SC 1. For each of the reactants listed in question 9 on pages 66 and 67 of your textbook, identify the type of reaction that would occur. Justify your classification.
Self-Check Answers
SC 1.
|
Reaction Type |
Justification |
(a) |
simple decomposition |
Only one reactant, a compound, is undergoing change. |
(b) |
formation |
Both reactants are elements. |
(c) |
complete combustion |
One of the reactants is oxygen. |
(d) |
double replacement |
Both reactants are ionic compounds. |
(e) |
single replacement |
One reactant is an element and the other is an ionic compound. |
(f) |
complete combustion |
One of the reactants is oxygen. |
(g) |
simple decomposition |
Only one reactant is shown. |
formation |
Both reactants are elements. |
|
(i) |
double replacement |
Both reactants are ionic compounds. |
(j) |
double replacement |
Both reactants are ionic compounds. |
Read
Understanding the different types of chemical reactions is an important step in becoming able to predict the changes that may occur when reactants are combined. Review the products for each type of reaction listed in "Table 3 Reaction Generalizations" on page 63 of your textbook.
Predicting the products of a chemical reaction requires knowledge of the different types of chemical reactions as well as knowledge of how to write chemical formulas for the products. The information below summarizes some of major aspects for writing formulas for chemical compounds. You may wish to add this information to the summary of types of chemical reactions you completed earlier in this lesson.
Some things to be aware of when writing chemical formulas are as follows:
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Some elements exist as molecular elements (e.g., H2, O2, Cl2, and P4).
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The net charge of a compound must be zero.
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Some metal ions can have more than one charge.
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The state of any ionic compound in an aqueous system is (s) or (aq).
Review your understanding of these aspects by reading the following pages in your textbook:
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“Names and Formulas of Ionic Compounds” on pages 29 to 31
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“Molecular Elements” on page 33
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how to use a solubility chart to determine the solubility of ionic compounds in aqueous systems and "Table 1: Solubility of Ionic Compounds at SATP–Generalizations," both on page 61
Self-Check
SC 2. For each of the reactants listed in question 9 on pages 66 and 67 of your textbook, predict the products of the reaction by writing their chemical formulas and respective names.
Self-Check Answers
SC 2.
|
Chemical Formula(s) of Product(s) |
Name(s) of Products |
(a) |
K(s) + Cl2(g) |
solid potassium and chlorine gas |
(b) |
CuCl2(s) |
solid copper(II) chloride (Note: The 2+ charge is the most common charge for copper.) |
(c) |
CO2(g) + H2O(g) |
carbon dioxide gas and water vapour |
(d) |
AgCl(s) + NaNO3(aq) |
solid silver chloride and aqueous sodium nitrate |
(e) |
Al(NO3)3(aq) + Cu(s) |
aqueous aluminium nitrate and solid copper |
(f) |
CO2(g) + H2O(g) |
carbon dioxide gas and water vapour |
(g) |
Al(s) + O2(g) |
solid aluminium and oxygen gas |
FeBr3(aq) |
aqueous iron(III) bromide (Note: The 3+ charge is the most common charge for iron.) |
|
(i) |
Cu(OH)2(s) + NaNO3(aq) |
solid copper(II) hydroxide and aqueous sodium nitrate |
(j) |
H2O(l) + Ca3(PO4)2(s) |
liquid water and solid calcium phosphate |