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    Module in (Ge-Ad: General CHEMISTRY (Organic) ) : Palawan State University Roxas Campus (Department Name) Department

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    John Mark Juarez
    This module overview describes how chemical equations are used to represent chemical reactions, including writing and balancing equations. It outlines key concepts such as classifying reaction types, predicting solubility through solubility rules, and performing stoichiometric calculations. The module content will cover writing and balancing chemical equations, classifying reaction types, solubility rules, and stoichiometry calculations including theoretical yield and limiting reactants.

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    Module in (Ge-Ad: General CHEMISTRY (Organic) ) : Palawan State University Roxas Campus (Department Name) Department

    Uploaded by

    John Mark Juarez
    68 views50 pages
    This module overview describes how chemical equations are used to represent chemical reactions, including writing and balancing equations. It outlines key concepts such as classifying reaction types, predicting solubility through solubility rules, and performing stoichiometric calculations. The module content will cover writing and balancing chemical equations, classifying reaction types, solubility rules, and stoichiometry calculations including theoretical yield and limiting reactants.

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    Module4

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    This module overview describes how chemical equations are used to represent chemical reactions, including writing and balancing equations. It outlines key concepts such as classifying reaction types, predicting solubility through solubility rules, and performing stoichiometric calculations. The module content will cover writing and balancing chemical equations, classifying reaction types, solubility rules, and stoichiometry calculations including theoretical yield and limiting reactants.

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    © All Rights Reserved
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    Download as docx, pdf, or txt
    68 views50 pages

    Module in (Ge-Ad: General CHEMISTRY (Organic) ) : Palawan State University Roxas Campus (Department Name) Department

    Uploaded by

    John Mark Juarez
    This module overview describes how chemical equations are used to represent chemical reactions, including writing and balancing equations. It outlines key concepts such as classifying reaction types, predicting solubility through solubility rules, and performing stoichiometric calculations. The module content will cover writing and balancing chemical equations, classifying reaction types, solubility rules, and stoichiometry calculations including theoretical yield and limiting reactants.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
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    Republic of the Philippines

    PALAWAN STATE UNIVERSITY


    Tiniguiban Heights, Puerto Princesa City, Palawan

    ROXAS CAMPUS
    National Highway, Barangay New Barbacan (Retac), Roxas, Palawan

    [DEPARTMENT NAME] DEPARTMENT

    MODULE IN
    [GE-Ad: GENERAL
    CHEMISTRY (Organic)]

    [PICTURES/ILUSTRATION (OPTIONAL) WITH PROPER CITATION)]

    [JOHN MARK L. JUAREZ]


    Faculty
    [Module 4]
    [Molecular and Chemical Bonding]

    MODULE OVERVIEW

    Many modern rocket fuels are solid mixtures of substances combined in carefully
    measured amounts and ignited to yield a thrust-generating chemical reaction. The
    engines of these rockets rely on carefully prepared solid mixtures of chemicals combined
    in precisely measured amounts. Igniting the mixture initiates a vigorous chemical
    reaction that rapidly generates large amounts of gaseous products. These gases are
    ejected from the rocket engine through its nozzle, providing the thrust needed to propel
    heavy payloads into space. Both the nature of this chemical reaction and the relationships
    between the amounts of the substances being consumed and produced by the reaction are
    critically important considerations that determine the success of the technology. This
    chapter will describe how to symbolize chemical reactions using chemical equations,
    how to classify some common chemical reactions by identifying patterns of reactivity,
    and how to determine the quantitative relations between the amounts of substances
    involved in chemical reactions-that is, the reaction stoichiometry.

    LEARNING OUTCOMES

     Write and balance chemical equations in molecular, total ionic, and net ionic formats
     Classify chemical reactions as one of these three types given appropriate descriptions or
    chemical equations
     Predict the solubility of common inorganic compounds by using solubility rules
     Perform stoichiometric calculations involving mass, moles, and solution molarity
     Explain the concepts of theoretical yield and limiting reactants/reagents

     Derive the theoretical yield and percent yield for a reaction under specified conditions

     Describe the fundamental aspects of titrations and gravimetric analysis.

     Determine the concentration of a sample using acid-base titration


    CONTENT

    4.1 Writing and Balancing Chemical Equations

    4.1.1 writing Chemical Equations

    An earlier chapter of this module introduced the use of element symbols to represent
    individual atoms. When atoms gain or lose electrons to yield ions, or combine with other
    atoms to form molecules, their symbols are modified or combined to generate chemical
    formulas that appropriately represent these species. Extending this symbolism to
    represent both the identities and the relative quantities of substances undergoing a
    chemical (or physical) change involves writing and balancing a chemical equation.
    Consider as an example the reaction between one methane molecules (CH4) and two
    diatomic oxygen molecules (O2) to produce one carbon dioxide molecule (CO2) and two
    water molecules (H2O). The chemical equation representing this process is provided in
    the upper half of Figure 4.1, with space-filling molecular models shown in the lower half
    of the figure.
    EVALUATION

    1. Balance the following equations:


    (b) PCl5(s) + H2O(l) ⟶ POCl3(l) + HCl(aq)
    (c) Cu(s) + HNO3(aq) ⟶ Cu (NO3)2(aq) + H2O(l) + NO(g) (d) H2(g) + I2(s) ⟶ HI(s)
    (e) Fe(s) + O2(g) ⟶ Fe2O3(s)
    (f) Na(s) + H2O(l) ⟶ NaOH(aq) + H2(g)
    (g) (NH4)2Cr2O7(s) ⟶ Cr2O3(s) + N2(g) + H2O(g) (h) P4(s) + Cl2(g) ⟶ PCl3(l)
    (i) PtCl4(s) ⟶ Pt(s) + Cl2(g)

    2. Write a balanced molecular equation describing each of the following chemical reactions.
    (a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon
    dioxide gas.
    (b) Gaseous butane, C4H10, reacts with diatomic oxygen gas to yield gaseous carbon
    dioxide and water vapor.
    (c) Aqueous solutions of magnesium chloride and sodium hydroxide react to produce solid
    magnesium hydroxide and aqueous sodium chloride.
    (d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and
    hydrogen gas.

    3. Colorful fireworks often involve the decomposition of barium nitrate and potassium chlorate
    and the reaction of the metal’s magnesium, aluminum, and iron with oxygen.

    (a) Write the formulas of barium nitrate and potassium chlorate.

    (b) The decomposition of solid potassium chlorate leads to the formation of solid potassium
    chloride and diatomic oxygen gas. Write an equation for the reaction.
    (c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide,
    diatomic nitrogen gas, and diatomic oxygen gas. Write an equation for the reaction.
    (d) Write separate equations for the reactions of the solid metals magnesium, aluminum, and
    iron with diatomic oxygen gas to yield the corresponding metal oxides. (Assume the iron
    3+
    oxide contains Fe ions.)

    4. From the balanced molecular equations, write the complete ionic and net ionic equations
    for the following:
    (a) K2C2O4(aq) + Ba(OH)2(aq) ⟶ 2KOH(aq) + BaC2O4(s) (b)
    Pb(NO3)2(aq) + H2SO4(aq) ⟶ PbSO4(s) + 2HNO3(aq) (c)
    CaCO3(s) + H2SO4(aq) ⟶ CaSO4(s) + CO2(g) + H2O(l)
    5. Classify the following as acid-base reactions or oxidation-reduction reactions: (a) Na2S(aq) +
    2HCl(aq) ⟶ 2NaCl(aq) + H2S(g)
    (b) 2Na(s) + 2HCl(aq) ⟶ 2NaCl(aq) + H2(g)
    (c) Mg(s) + Cl2(g) ⟶ MgCl2(s)
    (d) MgO(s) + 2HCl(aq) ⟶ MgCl2(aq) + H2O(l) (e) K3P(s) +
    2O2(g) ⟶ K3PO4(s)
    (f) 3KOH(aq) + H3PO4(aq) ⟶ K3PO4(aq) + 3H2O(l)

    REFERENCES

    1. R. Chang, General Chemistry: The Essential Concepts, 5th ed., 2008


    2. J.W. Hill and R.H. Petrucci, General Chemistry: An Integrated Approach, 2nd ed.,
    1999.
    3. Patricia Eldredge, R.H. H and, LLC, General Chemistry-Principles, Patterns, and
    Applications, 2011. (http://www.saylor.org/books)
    4. David W. Ball, Introductory Chemistry, Cleveland State University,2011,
    (http://www.saylor.org/books)
    5. J. E. Brady, J. W. Russel and J.R. Holum, General Chemistry: Principles and
    Structure,
    5th ed., 2006.
    6. S. S. Zumdahl and S.A. Zumdahl, Chemistry, 7th ed., 2007
    7. J. McMurry, Organic Chemistry, 8th ed., 20P

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