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Active as of Fall Semester 2013
I. General Information
1. Course Title:
Fundamentals of Chemistry
2. Course Prefix & Number:
CHEM 1414
3. Course Credits and Contact Hours:
Credits: 4
Lecture Hours: 3
Lab Hours: 3
Internship Hours: 0
4. Course Description:
This course involves the study of general laws of chemistry, periodicity, atomic and molecular structure, physical and chemical changes.
5. Placement Tests Required:
6. Prerequisite Courses:
CHEM 1414 - Fundamentals of Chemistry
There are no prerequisites for this course.
9. Co-requisite Courses:
CHEM 1414 - Fundamentals of Chemistry
There are no corequisites for this course.
II. Transfer and Articulation
1. Course Equivalency - similar course from other regional institutions:
Bemidji State University, Chem 1111 General Chemistry, 4 credits
St. Cloud State University, Chem 160 Preparatory Chemistry, 4 credits
III. Course Purpose
MN Transfer Curriculum (General Education) Courses - This course fulfills the following goal area(s) of the MN Transfer Curriculum:
Goal 3 – Natural Sciences
IV. Learning Outcomes
1. College-Wide Outcomes
College-Wide Outcomes/Competencies |
Students will be able to: |
Demonstrate oral communication skills |
Make a presentation of lab group results and/or current events involving chemistry. |
Analyze and follow a sequence of operations |
Follow a given lab protocol to successfully complete a lab experiment in the time allowed. |
Apply abstract ideas to concrete situations |
Apply theories concerning particles which are not visible to construct atomic structure and calculate gram amounts to use in an experiment |
Work as a team member to achieve shared goals |
Interact with lab partners to successfully complete a lab experiment in the time allowed. |
2. Course Specific Outcomes - Students will be able to achieve the following measurable goals upon completion of
the course:
- Use dimensional analysis to convert from one unit or dimension of measurement to another. MnTC Goal 3
- Determine the number of significant figures in a number resulting from addition, subtraction, multiplication and division of measured values. MnTC Goal 3
- Describe the models and list the properties for the three states of matter. MnTC Goal 3
- Classify changes in matter as either physical or chemical. MnTC Goal 3
- Draw a Bohr model for any representative element and predict its chemical reactivity. MnTC Goal 3
- Solve various gas law problems involving the combined gas law. MnTC Goal 3
- Compare and contrast ionic and covalent bonds. MnTC Goal 3
- Draw Lewis electron dot structures for a given molecular formula. MnTC Goal 3
- Construct and name chemical formulas for various combinations of representative metals, nonmetals and polyatomic ions. MnTC Goal 3
- Balance chemical equations. MnTC Goal 3
- Perform various calculations involving grams, formula weight, moles, Avogadro’s number, percentage composition, empirical and molecular formulas. MnTC Goal 3
- Calculate the stoichiometric amounts in grams or moles for a given chemical equation when give an initial amount of a reactant. MnTC Goal 3
V. Topical Outline
Listed below are major areas of content typically covered in this course.
1. Lecture Sessions
- Matter and Measurement
- State the steps of the scientific method.
- Explain the difference between a fact and an inference.
- Recognize qualitative verses quantitative data.
- Define the term scientific law.
- Explain the difference between a hypothesis and a theory.
- State the two properties matter must possess.
- Define and recognize a physical verses a chemical change.
- Recognize the three states of matter.
- Define the terms homogeneous verses heterogeneous.
- Describe how matter can be classified by attempting to separate it by physical changes.
- Describe how matter can be further classified by attempting to separate it by chemical changes once it has been completely separated by physical changes.
- Express decimal numbers in scientific notation and vice versa.
- Express the results of multiplication and division of scientific numbers in scientific notation.
- Perform multiplication and division of scientific numbers on a scientific calculator.
- Write unit paths and solve any problem that involves converting from one unit of measurement to another—given a table of conversion factors.
- Interpret the meaning of proportionality and of a proportionality constant.
- Solve problems that involve the use of a proportionality constant as a conversion factor.
- Convert Fahrenheit temperatures to Celsius and vice versa.
- Convert Celsius temperatures to Kelvin and vice versa.
- Distinguish between units of the English system and Metric system.
- List the standard metric units of measurement and their abbreviations for length, mass and volume.
- Write equivalencies, with their correct abbreviations, between any standard metric unit and a prefixed metric unit of kilo, centi, or milli.
- Write equivalencies between metric units when utilizing a table of prefixed metric units.
- Determine the number of significant figures in a number by having memorized the rules for counting significant numbers.
- Determine the uncertainty in a given measured value.
- Determine the correct number of significant figures after adding and subtracting measured values.
- Determine the correct number of significant figures after multiplying and dividing measured values.
- Atoms and Elements
- Identify three subatomic particles by name, relative mass, and charge, and describe the structure of the atom.
- Write and name a given isotope and determine the number of subatomic particles it contains.
- Define an atomic mass unit, amu.
- Calculate the atomic mass of an element given a set of isotopes, masses and abundances.
- Distinguish between periods and families or groups in the periodic table.
- Describe why groups or families of elements have similar chemical and physical properties.
- Locate the alkali metals, halogens, and noble gases in the periodic table.
- Predict the relative sizes of atoms within a group or family and period.
- Identify the metals, nonmetals, and metalloids by their positions in the periodic table.
- Identify representative and transition elements by their positions in the periodic table.
- Molecules, Ions and Compounds
- Name molecules.
- Recognize the seven elements that form stable diatomic molecules.
- Name and know the charges of the polyatomic ions asked to memorize.
- Name the two types of ionic formulas that contain polyatomic ions.
- Describe how scientists arrived at Avogadro’s number.
- Define a mole in terms of mass and Avogadro’s number.
- Convert grams of a given substance to moles and vice versa.
- Convert grams of a given substance to numbers of atoms, molecules, or formula units or vice versa.
- Calculate the percentage by mass of each element in a given formula.
- Determine the empirical formula from percentage data.
- Determine the true molecular or ionic formula from percentage data and formula weight.
- Chemical Equations and Stoichiometry
- Balance chemical equations.
- Identify the abbreviations used in chemical equations for solids, liquids and gases.
- Classify balanced equations into one of the six types discussed in class.
- Identify common acids and bases.
- Solve the four types of possible stoichiometry problems.
- State the definitions of endothermic and exothermic reactions.
- Draw energy level diagrams for endothermic and exothermic reactions.
- Calculate percentage yield for a given stoichiometric reaction.
- Atomic Structure
- Describe the wave nature of electromagnetic radiation and how wavelength plays a role in its character.
- Describe how observations of a discharge tube can be used to make of model of electron energy levels.
- List the two types of energy an electron possesses.
- Describe how the total energy of an electron changes with increased average distance from the nucleus.
- Atomic Electron Configuration
- Describe the shapes of the s and p orbitals.
- List the various orbitals, sublevels, and principal energy levels and their capacities for electrons.
- Write the electron configuration for any element in the periodic table using the short-hand notation.
- Define valence electrons.
- Write electron-dot structures for any representative element.
- Bonding and Molecular Structure
- Define the terms cations and anions.
- Predict the number of electrons representative metals and nonmetals tend to loss or gain so as to acquire a noble gas electron configuration when they are involved in an ionic bond.
- Predict the charge the representative metals and nonmetal acquire when they are involved in an ionic bond.
- Use electron-dot structures to draw the electron transfers necessary between metals and nonmetals to form ionic bonds.
- Predict ionic formulas from those metals and nonmetals that have only one charge.
- Calculate the charge a transition metal when contained in an ionic bond.
- Name the nonmetal anions.
- Name ionic formulas that contain metals that have only one oxidation state and those that contain metals that can have more than one oxidation state.
- Draw electron-dot structures for covalently bonded substances.
- Draw electron-dot structures for polyatomic ions.
- Define electronegativity and apply it to determine if a formula contains ionic or covalent bonds.
- Define polar, nonpolar or essentially nonpolar covalent bonds and be able to use electronegativities to determine the type found in a formula.
- State the elements which disobey the octet rule.
- Predict the geometry of a molecule.
- Determine if a molecule is polar or nonpolar.
- Gases and Their Properties
- State the properties of gases.
- Describe the model for ideal gases.
- Describe a barometer and open ended monometer and how to make pressure measurements from each.
- Convert one pressure measurement to another given the relationship between the pressure measurements.
- State Boyle’s and apply it to solve applicable problems.
- State Gay-Lassac’s Law, Charles’ Law, and the combined gas law and apply them to solve applicable problems.
- State Avogadro’s Law.
- State the ideal gas law and apply it to solve applicable problems.
- State or derive the gas density equation from the ideal gas equation and apply it to solve applicable problems.
- State or derive the molar volume equation from the ideal gas equation and apply it to solve applicable problems.
- Define STP.
- Intermolecular Forces, Liquids, Solids
- Predict how vapor pressure, molar heat of vaporization, boiling point, viscosity, and surface tension varies with intermolecular forces of attraction.
- Identify the intermolecular forces of attraction in a substance from its formula.
- Draw an kinetic energy distribution curve for molecules in a liquid.
- Explain how escape energy of molecules in a liquid is related to the intermolecular forces of attraction and how its value relates to the liquids vapor pressure.
- Explain how the kinetic energy distribution curve changes with temperature and how that affects the vapor pressure of the liquid.
- Write a reversible equation to represent the equilibrium between a liquid and its vapor state.
- Define boiling point of a liquid in terms of the liquids vapor pressure and the total gaseous pressure exerted on the liquid and explain how the boiling point of a liquid can be changed.
- Identify the five types of solids and their respective physical properties.
- Define heats of vaporization, condensation, fusion, and solidification.
- Calculate the amount of energy required to vaporize a given mass of liquid at its boiling point or condense the same amount of gas at its condensation temperature.
- Calculate the amount of energy required to melt a given mass of solid at its melting point or freeze the same amount at its freezing point.
- Identify melting, freezing, boiling, or condensation as endothermic or exothermic processes.
- Define specific heat.
- Calculate the amount of energy required to be added or removed to change the temperature of a given amount of solid, liquid, or gas.
- Calculate the amount of energy required to be added or removed to make any variation in temperature including any combination of phase changes.
- Solutions and Their Behavior
- Explain the electric properties of polar and nonpolar molecules.
- Know what hydrogen bonding is and when it occurs.
- Know the definitions of homogeneous and heterogeneous mixtures, solutions, solute, and solvent.
- Know how polar and nonpolar molecules effect the mixing process between solute and solvent.
- Know how to calculate % wt., ppm, and molarity of a solute in a solution.
- Know how to use molarity as a conversion factor to solve the four types of molarity problems discussed in class.
- Know how to calculate dilution problems.
2. Laboratory/Studio Sessions
- Laboratory Techiques
- Introduction to Quantitative Measurement
- Effect of Temperature on Solubility of a Salt
- Separation Techniques
- Freezing and Melting of Water
- Chemical and Physical Changes
- Properties of Solutions: Electrolytes and Non-Electrolytes
- Chemical Changes and Equations
- Endothermic and Exothermic Reactions
- Determining the Concentration of a Solution: Beer’s Law
- Acid-Base Titration
- Gravimetric Determination
- Boyle’s Law
- Preparation of Soap
I. General Information
1. Course Title:
Fundamentals of Chemistry
2. Course Prefix & Number:
CHEM 1414
3. Course Credits and Contact Hours:
Credits: 4
Lecture Hours: 3
Lab Hours: 3
Internship Hours: 0
4. Course Description:
This course involves the study of general laws of chemistry, periodicity, atomic and molecular structure, physical and chemical changes.
5. Placement Tests Required:
6. Prerequisite Courses:
CHEM 1414 - Fundamentals of Chemistry
There are no prerequisites for this course.
9. Co-requisite Courses:
CHEM 1414 - Fundamentals of Chemistry
There are no corequisites for this course.
II. Transfer and Articulation
1. Course Equivalency - similar course from other regional institutions:
Bemidji State University, Chem 1111 General Chemistry, 4 credits
St. Cloud State University, Chem 160 Preparatory Chemistry, 4 credits
III. Course Purpose
2. MN Transfer Curriculum (General Education) Courses - This course fulfills the following goal area(s) of the MN Transfer Curriculum:
Goal 3 – Natural Sciences
IV. Learning Outcomes
1. College-Wide Outcomes
College-Wide Outcomes/Competencies |
Students will be able to: |
Demonstrate oral communication skills |
Make a presentation of lab group results and/or current events involving chemistry. |
Analyze and follow a sequence of operations |
Follow a given lab protocol to successfully complete a lab experiment in the time allowed. |
Apply abstract ideas to concrete situations |
Apply theories concerning particles which are not visible to construct atomic structure and calculate gram amounts to use in an experiment |
Work as a team member to achieve shared goals |
Interact with lab partners to successfully complete a lab experiment in the time allowed. |
2. Course Specific Outcomes - Students will be able to achieve the following measurable goals upon completion of
the course:
- Use dimensional analysis to convert from one unit or dimension of measurement to another. MnTC Goal 3
- Determine the number of significant figures in a number resulting from addition, subtraction, multiplication and division of measured values. MnTC Goal 3
- Describe the models and list the properties for the three states of matter. MnTC Goal 3
- Classify changes in matter as either physical or chemical. MnTC Goal 3
- Draw a Bohr model for any representative element and predict its chemical reactivity. MnTC Goal 3
- Solve various gas law problems involving the combined gas law. MnTC Goal 3
- Compare and contrast ionic and covalent bonds. MnTC Goal 3
- Draw Lewis electron dot structures for a given molecular formula. MnTC Goal 3
- Construct and name chemical formulas for various combinations of representative metals, nonmetals and polyatomic ions. MnTC Goal 3
- Balance chemical equations. MnTC Goal 3
- Perform various calculations involving grams, formula weight, moles, Avogadro’s number, percentage composition, empirical and molecular formulas. MnTC Goal 3
- Calculate the stoichiometric amounts in grams or moles for a given chemical equation when give an initial amount of a reactant. MnTC Goal 3
V. Topical Outline
Listed below are major areas of content typically covered in this course.
1. Lecture Sessions
- Matter and Measurement
- State the steps of the scientific method.
- Explain the difference between a fact and an inference.
- Recognize qualitative verses quantitative data.
- Define the term scientific law.
- Explain the difference between a hypothesis and a theory.
- State the two properties matter must possess.
- Define and recognize a physical verses a chemical change.
- Recognize the three states of matter.
- Define the terms homogeneous verses heterogeneous.
- Describe how matter can be classified by attempting to separate it by physical changes.
- Describe how matter can be further classified by attempting to separate it by chemical changes once it has been completely separated by physical changes.
- Express decimal numbers in scientific notation and vice versa.
- Express the results of multiplication and division of scientific numbers in scientific notation.
- Perform multiplication and division of scientific numbers on a scientific calculator.
- Write unit paths and solve any problem that involves converting from one unit of measurement to another—given a table of conversion factors.
- Interpret the meaning of proportionality and of a proportionality constant.
- Solve problems that involve the use of a proportionality constant as a conversion factor.
- Convert Fahrenheit temperatures to Celsius and vice versa.
- Convert Celsius temperatures to Kelvin and vice versa.
- Distinguish between units of the English system and Metric system.
- List the standard metric units of measurement and their abbreviations for length, mass and volume.
- Write equivalencies, with their correct abbreviations, between any standard metric unit and a prefixed metric unit of kilo, centi, or milli.
- Write equivalencies between metric units when utilizing a table of prefixed metric units.
- Determine the number of significant figures in a number by having memorized the rules for counting significant numbers.
- Determine the uncertainty in a given measured value.
- Determine the correct number of significant figures after adding and subtracting measured values.
- Determine the correct number of significant figures after multiplying and dividing measured values.
- Atoms and Elements
- Identify three subatomic particles by name, relative mass, and charge, and describe the structure of the atom.
- Write and name a given isotope and determine the number of subatomic particles it contains.
- Define an atomic mass unit, amu.
- Calculate the atomic mass of an element given a set of isotopes, masses and abundances.
- Distinguish between periods and families or groups in the periodic table.
- Describe why groups or families of elements have similar chemical and physical properties.
- Locate the alkali metals, halogens, and noble gases in the periodic table.
- Predict the relative sizes of atoms within a group or family and period.
- Identify the metals, nonmetals, and metalloids by their positions in the periodic table.
- Identify representative and transition elements by their positions in the periodic table.
- Molecules, Ions and Compounds
- Name molecules.
- Recognize the seven elements that form stable diatomic molecules.
- Name and know the charges of the polyatomic ions asked to memorize.
- Name the two types of ionic formulas that contain polyatomic ions.
- Describe how scientists arrived at Avogadro’s number.
- Define a mole in terms of mass and Avogadro’s number.
- Convert grams of a given substance to moles and vice versa.
- Convert grams of a given substance to numbers of atoms, molecules, or formula units or vice versa.
- Calculate the percentage by mass of each element in a given formula.
- Determine the empirical formula from percentage data.
- Determine the true molecular or ionic formula from percentage data and formula weight.
- Chemical Equations and Stoichiometry
- Balance chemical equations.
- Identify the abbreviations used in chemical equations for solids, liquids and gases.
- Classify balanced equations into one of the six types discussed in class.
- Identify common acids and bases.
- Solve the four types of possible stoichiometry problems.
- State the definitions of endothermic and exothermic reactions.
- Draw energy level diagrams for endothermic and exothermic reactions.
- Calculate percentage yield for a given stoichiometric reaction.
- Atomic Structure
- Describe the wave nature of electromagnetic radiation and how wavelength plays a role in its character.
- Describe how observations of a discharge tube can be used to make of model of electron energy levels.
- List the two types of energy an electron possesses.
- Describe how the total energy of an electron changes with increased average distance from the nucleus.
- Atomic Electron Configuration
- Describe the shapes of the s and p orbitals.
- List the various orbitals, sublevels, and principal energy levels and their capacities for electrons.
- Write the electron configuration for any element in the periodic table using the short-hand notation.
- Define valence electrons.
- Write electron-dot structures for any representative element.
- Bonding and Molecular Structure
- Define the terms cations and anions.
- Predict the number of electrons representative metals and nonmetals tend to loss or gain so as to acquire a noble gas electron configuration when they are involved in an ionic bond.
- Predict the charge the representative metals and nonmetal acquire when they are involved in an ionic bond.
- Use electron-dot structures to draw the electron transfers necessary between metals and nonmetals to form ionic bonds.
- Predict ionic formulas from those metals and nonmetals that have only one charge.
- Calculate the charge a transition metal when contained in an ionic bond.
- Name the nonmetal anions.
- Name ionic formulas that contain metals that have only one oxidation state and those that contain metals that can have more than one oxidation state.
- Draw electron-dot structures for covalently bonded substances.
- Draw electron-dot structures for polyatomic ions.
- Define electronegativity and apply it to determine if a formula contains ionic or covalent bonds.
- Define polar, nonpolar or essentially nonpolar covalent bonds and be able to use electronegativities to determine the type found in a formula.
- State the elements which disobey the octet rule.
- Predict the geometry of a molecule.
- Determine if a molecule is polar or nonpolar.
- Gases and Their Properties
- State the properties of gases.
- Describe the model for ideal gases.
- Describe a barometer and open ended monometer and how to make pressure measurements from each.
- Convert one pressure measurement to another given the relationship between the pressure measurements.
- State Boyle’s and apply it to solve applicable problems.
- State Gay-Lassac’s Law, Charles’ Law, and the combined gas law and apply them to solve applicable problems.
- State Avogadro’s Law.
- State the ideal gas law and apply it to solve applicable problems.
- State or derive the gas density equation from the ideal gas equation and apply it to solve applicable problems.
- State or derive the molar volume equation from the ideal gas equation and apply it to solve applicable problems.
- Define STP.
- Intermolecular Forces, Liquids, Solids
- Predict how vapor pressure, molar heat of vaporization, boiling point, viscosity, and surface tension varies with intermolecular forces of attraction.
- Identify the intermolecular forces of attraction in a substance from its formula.
- Draw an kinetic energy distribution curve for molecules in a liquid.
- Explain how escape energy of molecules in a liquid is related to the intermolecular forces of attraction and how its value relates to the liquids vapor pressure.
- Explain how the kinetic energy distribution curve changes with temperature and how that affects the vapor pressure of the liquid.
- Write a reversible equation to represent the equilibrium between a liquid and its vapor state.
- Define boiling point of a liquid in terms of the liquids vapor pressure and the total gaseous pressure exerted on the liquid and explain how the boiling point of a liquid can be changed.
- Identify the five types of solids and their respective physical properties.
- Define heats of vaporization, condensation, fusion, and solidification.
- Calculate the amount of energy required to vaporize a given mass of liquid at its boiling point or condense the same amount of gas at its condensation temperature.
- Calculate the amount of energy required to melt a given mass of solid at its melting point or freeze the same amount at its freezing point.
- Identify melting, freezing, boiling, or condensation as endothermic or exothermic processes.
- Define specific heat.
- Calculate the amount of energy required to be added or removed to change the temperature of a given amount of solid, liquid, or gas.
- Calculate the amount of energy required to be added or removed to make any variation in temperature including any combination of phase changes.
- Solutions and Their Behavior
- Explain the electric properties of polar and nonpolar molecules.
- Know what hydrogen bonding is and when it occurs.
- Know the definitions of homogeneous and heterogeneous mixtures, solutions, solute, and solvent.
- Know how polar and nonpolar molecules effect the mixing process between solute and solvent.
- Know how to calculate % wt., ppm, and molarity of a solute in a solution.
- Know how to use molarity as a conversion factor to solve the four types of molarity problems discussed in class.
- Know how to calculate dilution problems.
2. Laboratory/Studio Sessions
- Laboratory Techiques
- Introduction to Quantitative Measurement
- Effect of Temperature on Solubility of a Salt
- Separation Techniques
- Freezing and Melting of Water
- Chemical and Physical Changes
- Properties of Solutions: Electrolytes and Non-Electrolytes
- Chemical Changes and Equations
- Endothermic and Exothermic Reactions
- Determining the Concentration of a Solution: Beer’s Law
- Acid-Base Titration
- Gravimetric Determination
- Boyle’s Law
- Preparation of Soap