Course Package Form 2018 Outline
Mohave Community College
CHM 130 Fundamental Chemistry with Lab


Originator: Arac, Lale           Status: Approved           Department: CHM Chemistry
Date Created: 02/02/2015         Submitted: 02/02/2015         Completed: 03/11/2015        
Effective Semester: Fall  
Catalog Year: 2015-16  
Course Prefix: CHM  
Course Number: 130  
Course Full Title: Fundamental Chemistry with Lab  
Reason for Evaluation: Prerequisite Change    
Current Credit: 04  
Lecture Hours: 03  
Lab Hours: 03  
Clinical Hours:  
New Credit Hours:  
Lecture Hours:  
If the credit hour change box has been marked, please provide the new credit hour:  
New Lecture Hours:  
New Lab Hours:  
New Clinical Hours:  
New Internship Hours:  
New Externship Hours:  
SUN Course?: Yes  
AGEC Course?: Yes  
Articulated?: Yes  
Transfer: ASU   NAU   UA    
Prerequisite(s): Appropriate score on assessment test or successful completion of TRE 089, and TRM 091 or MAT 101  
Corequisite(s): CHM 130L  
Catalog Course Description: Fundamental chemistry covers principles of inorganic chemistry designed for programs requiring a year or less of chemistry, and for students proceeding on to one semester of organic chemistry.  
Course Learning Outcomes: By the end of the semester, the students will be able to
1. Analyze the perspectives and values of chemistry and the major principles and theories upon which these are based.(3,5)
2. Promote scientific literacy using the developments, methods and technologies of chemistry.(5,6)
3. Evaluate interrelationships between chemical principles and concepts. (2,3 )
4. Utilize critical thinking skills through direct experience with the methods and processes of inquiry (the scientific method).(3)
5. Appreciate the important contributions that chemistry has made and continues to make in today's society.(1, 3,4 )  
Course Competencies: 1. Recognize the coherence between the world we know and the chemical world via the application of the scientific method
1.1 Recognize that chemicals make up virtually everything we come into contact with in our world.
1.2 Recognize that all things are made of atoms and molecule.
1.3 Identify the key characteristics of the scientific method: observation, the formulation of hypotheses, the testing of hypotheses by experiment, and the formulation of laws and theories.
2. Utilize measurement and problem solving techniques in scientific calculations
2.1 Express very large and very small numbers using scientific notation.
2.2 Report measured quantities to the right number of digits.
2.3 Determine which digits in a number are significant.
2.4 Round numbers to the correct number of significant figures.
2.5 Determine the correct number of significant figures in the results of calculations involving addition/subtraction and multiplication/division.
2.6 Convert between units.
2.7 Convert units raised to a power.
2.8 Calculate the density of a substance.
2.9 Use density as a conversion factor.
3. Differentiate between matter and energy.
3.1 Classify matter as element, compound, or mixture.
3.2 Distinguish between physical and chemical properties.
3.3 Distinguish between physical and chemical changes.
3.4 Apply the law of conservation of mass.
3.5 Convert among energy units.
3.6 Convert between Fahrenheit, Celsius, and Kelvin temperature scales.
3.7 Relate energy, temperature change, and heat capacity.
4. Integrate historical discoveries and modern concepts which define the nature of atoms and elements
4.1 Recognize that all matter is composed of atoms.
4.2 Explain how the experiments of Thomson and Rutherford led to the development of the nuclear theory of the atom.
4.3 Analyze the respective properties and charges of electrons, neutrons, and protons.
4.4 Determine the atomic symbol and atomic number for an element using the periodic table.
4.5 Use the periodic table to classify elements by group.
4.6 Determine ion charge from numbers of protons and electrons.
4.7 Determine the number of protons and electrons in an ion.
4.8 Determine atomic numbers, mass numbers, and isotope symbols for an isotope.
4.9 Determine number of protons and neutrons from isotope symbols.
4.10 Calculate atomic mass from percent natural abundances and isotopic masses.
5. Differentiate between types of molecules and compounds through classification and nomenclature
5.1 Restate the law of constant composition.
5.2 Apply the law of constant composition with calculations.
5.3 Write chemical formulas.
5.4 Determine the total number of each type of atom in a chemical formula.
5.5 Classify elements as atomic or molecular.
5.6 Classify compounds as ionic or molecular.
5.7 Write formulas for ionic compounds.
5.8 Distinguish between common and systematic names for compounds.
5.9 Name binary ionic compounds containing a metal that forms only one type of ion.
5.10 Name binary ionic compounds containing a metal that forms more than one type of ion.
5.11 Name ionic compounds containing a polyatomic ion.
5.12 Name molecular compounds.
5.13 Name binary acids.
5.14 Name oxyacids containing an oxyanion ending in -ate and-ite.
5.15 Calculate formula mass.
6. Demonstrate the numerical and conceptual skills to carry out chemical composition calculations
6.1 Convert between moles and number of atoms.
6.2 Convert between grams and moles.
6.3 Convert between grams and number of atoms or molecules.
6.4 Convert between moles of a compound and moles of a constituent element.
6.5 Convert between grams of a compound and grams of a constituent element.
6.6 Use mass percent composition as a conversion factor.
6.7 Determine mass percent composition from a chemical formula.
6.8 Determine an empirical formula from experimental data.
6.9 Calculate a molecular formula from an empirical formula and molar mass.
7. Differentiate between types of chemical reactions according to molecular or chemical properties.
7.1 Identify a chemical reaction.
7.2 Write balanced chemical equations.
7.3 Determine if a compound is soluble.
7.4 Write equations for precipitation reactions.
7.5 Write molecular, complete ionic, and net ionic equations.
7.6 Write equations for acid/base reactions.
7.7 Write equations for gas evolution reactions.
7.8 Identify redox reactions.
7.9 Write equations for combustion reactions.
7.10 Classify chemical reactions.
8. Apply numerical and conceptual skills to the determination of quantities in chemical reactions.
8.1 Recognize the numerical relationship between chemical quantities in a balanced chemical equation.
8.2 Perform mole-to-mole conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation.
8.3 Carry out mass-to-mass conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation and molar masses.
8.4 Calculate limiting reactant, theoretical yield, and percent yield for a given amount of reactants in a balanced chemical equation.
8.5 Calculate the amount of thermal energy emitted or absorbed by a chemical reaction.
9. Relate the arrangement of electrons in atoms to the organization and structure of the periodic table.
9.1 Explain the nature of electromagnetic radiation.
9.2 Explain the key characteristics of the Bohr model of the atom.
9.3 Explain the key characteristics of the quantum-mechanical model of the atom.
9.4 Predict relative wavelength, energy, and frequency of different types of light.
9.5 Write electron configurations and orbital diagrams for atoms.
9.6 Identify valence electrons and core electrons.
9.7 Write electron configurations for an element based on its position in the periodic table.
9.8 Recognize that the chemical properties of elements are largely determined by the number of valence electrons they contain.
9.9 Identify periodic trends such as atomic size, ionization energy, and metallic character.
10. Explain chemical bonding theory and its relationship to predicting molecular shapes.
10.1 Write Lewis structures for elements.
10.2 Write Lewis structures of ionic compounds.
10.3 Use Lewis theory to predict the chemical formula of an ionic compound.
10.4 Write Lewis structures for covalent compounds.
10.5 Write resonance structures.
10.6 Predict the shapes of molecules.
10.7 Determine whether a molecule is polar.
11. Distinguish between the different laws governing the properties of gases with respect to pressure, volume and temperature.
11.1 Convert pressure units.1
11.2 Use simple gas laws.
11.3 Use the combined gas law.
11.4 Use the ideal gas law.
11.5 Relate total pressure and partial pressure.
11.6 Calculate stoichiometry for gases in chemical reactions.
12. Differentiate between the properties of liquids and solids that affect their intermolecular and intramolecular forces of attraction that account for the differences in their behavior.
12.1 Use heat of vaporization in calculations.
12.2 Use heat of fusion in calculations.
12.3 Determine the types of intermolecular forces in a compound.
12.4 Determine melting and/or boiling points using intermolecular forces.
13. Apply Numerical and conceptual skills to the determination of solution concentrations.
13.1 Calculate mass percent.
13.2 Use mass percent in calculations.
13.3 Calculate molarity.
13.4 Use molarity in calculations.
13.5 Calculate solution dilution.
13.6 Use solution stoichiometry.
13.7 Calculate molality.
13.8 Calculate freezing point depression and boiling point elevation.
14. Compare the properties and theories governing the behavior of acids and bases.
14.1 Identify common acids and bases by their key characteristics.
14.2 Identify Arrhenius acids and bases.
14.3 Identify Br?nsted/Lowry acids and bases and their conjugates.
14.4 Write equations for neutralization reactions.
14.5Write equations for the reactions of acids with metals and with metal oxides.
14.6 Using acid/base titration to determine the concentration of an unknown solution.
14.7 Determine [H3O+] and [OH-] in solutions.
14.8 Identify strong and weak acids and strong and weak bases.
14.9 Find the concentration of H3O+ or OH- from Kw.
14.10 Calculate pH or pOH from [H3O+] or [OH-].
14.11 Calculate [H3O+] or [OH-] from pH or pOH.
15. Analyze chemical equilibrium through chemical principles and mathematical concepts.
15.1 Write equilibrium expressions for chemical reactions.
15.2 Calculate equilibrium constants.
15.3 Determine the concentration of a reactant or product at equilibrium by using the equilibrium constant.
15.4 Restate Le Ch?telier?s principle.
15.5Write an expression for the solubility-product constant.
15.6 Use Ksp to determine molar solubility.
16. Differentiate between oxidation and reduction reactions.
16.1 Define oxidation and reduction.
16.2 Identify oxidizing agents and reducing agents.
16.3 Assign oxidation states.
16.4 Balance redox reactions.
16.5 Predict spontaneous redox reactions.