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# CHM 107 - Chemistry For Engineering Technology

Credits: 4

Develops a foundation in chemistry for engineering technicians and designers so they can make better informed decisions. Builds connections of understanding between engineering material selection, design, and manufacturing processes. Uses fundamental principles including atomic theory, structure of metals and polymers, periodic properties, states of matter, gas laws, nomenclature, and common chemical reactions to make connections.

Prerequisite(s): READING LEVEL 2 and WRITING LEVEL 2 and MATH LEVEL 6
Corequisite(s): None
Lecture Hours: 45 Lab Hours: 30
Meets MTA Requirement: Natural Science Lab
Pass/NoCredit: Yes

Outcomes and Objectives 1.    Relate the effects of temperature and pressure on the volume of a gas and the moles of any gas
at standard temperature and pressure.

A.         Convert between temperatures expressed in Celsius and Kelvin

B.         Convert between pressure expressed in atmospheres, torr, mm Hg

C.         Observe the relationship between volume and pressure for a gas

D.         State Boyle's Law and express mathematically

E.         Given a change of pressure, calculate the change of volume and the reverse

F.          Recognize the significance of the partial pressure of water vapor in measuring the pressure of a
gas collected by displacement of water

G.         Observe the relationship between temperature and volume for a gas

H.         State Charles’ Law and express mathematically

I.           Given a change of temperature, calculate the change of volume and the reverse

J.          Combine application of Boyle’s Law and Charles’ Law; use Combined Gas Law

K.          Use the Ideal Gas Law to solve for pressure, volume, number of moles, or temperature

L.          Recognize Avogadro’s Law and understand that at any given temperature and pressure,

there are an equal number of moles of any gas in an equal volume

M.         Recognize that at standard temperature and pressure (273 Kelvin, 760 mm Hg), 1 mole of a

gas has a volume of 22.4 L

N.         Use the density relationship to calculate molar mass (g/mole) using the Ideal Gas Law

O.         Use molar mass and the Ideal Gas Law to calculate density of a gas at a given temperature and
pressure

P.          Given a balanced chemical equation, the mass of one reactant or product, and the T and P of a
gaseous reactant or product, calculate the volume of the gaseous reactant or product.

Q.         Given a balanced chemical equation, the volume of a gaseous reactant or product and a given T
and P, calculate the mass of another reactant or product

R.          Understand the applications of Kinetic Molecular Theory to gases

S.          Recognize the relationship of the Kinetic Molecular Theory to Boyle’s Law, Charles’ Law, and
Dalton’s Law of Partial Pressures

T.          Define and be able to use the following terms: atmosphere, torr, partial pressure, standard
temperature, standard pressure, molar gas volume, universal gas constant, ideal gases

U.         Recognize the difference between an Ideal Gas and a real gas.

2.    Express concentration of solution by various methods and use units of concentration to calculate
quantities of solute.

A.          Define solute and solvent

B.          Define and be able to use the following terms: soluble, insoluble, solubility, saturated, unsaturated, dilute, concentrated, miscible, immiscible, concentration, molarity

C.          Express concentration of a solution as a % (m/m)

D.          Given a %(m/m) concentration, calculate the mass of solute in a given volume

E.          Calculate the mass of solute and solvent to prepare a given % (m/m) solution.

F.          Calculate the mass of solute and volume of solvent to prepare a given % (m/v) solution

G.         Calculate the volume of solute and solvent to prepare a given % (v/v) solution

H.         Convert between % and ppm

I.           For a given molarity solution, calculate the mass of solute required / L

J.          For a given molarity and volume, calculate the number of moles of solute

K.          Calculate the volume of a solution with a specified molarity to deliver a given amount of solute

L.          Given the molarity and volume of a concentrated solution, calculate the volume required to
prepare a dilute solution of a specified molarity

M.         For a given molality solution, calculate the mass of solute required/ 1000 g of solvent

3.    Explain the structure, nomenclature and some reactions of carboxylic acids and esters.

A.          Give the common and IUPAC names of selected carboxylic acids

B.          Write the structural formulas for saturated, unsaturated, aromatic and dicarboxylic carboxylic
acids

C.          Understand correlation between molecular mass and the properties of solubility in water and
boiling point

D.         Write equations for the preparation of carboxylic acids by:

1.    Oxidation of alcohols and aldehydes

2.    Hydrolysis of esters

3.    Saponification of fats

4.    Oxidation of aromatic hydrocarbons

E.          Write equations for the reactions of carboxylic acids to form salts and esters

F.          Write common names, IUPAC names and formulas of esters

G.         Identify the portion of an ester that is derived from a carboxylic acid and the portion derived

from an alcohol

H.         Compare and contrast the cleansing action of a soap and synthetic detergent

I.           Recognize differences in the composition of natural fats and oils and the effect on the

properties of the triacylglycerols (triglycerides, fats).

J.          Differentiate between: fat and oil; salt of a carboxylic acid and a soap; hydrogenation,

hydrogenolysis, hydrolysis and saponification; cationic, anionic and nonionic surfactants,

4.    Differentiate characteristics of the atomic structure and molecular arrangement of common
engineering materials.

A.          Identify characteristics of the following lattice structures of metals and why they form from a

molten state:

1.    Face-center-cubic (FCC)

2.    Body-center-cubic (BCC)

3.    Hexagonal close packed (HCP)

B.          List at least 3 common metals within each group (FCC, BCC, HCP).

C.         Compare the formation of a pure metal from a molten state with that of an alloy.

D.         Identify characteristics of the amorphous structure of glass and ceramics.

5.    Explain the utility of polymers and of the relationship between structure and function.

A.          Recognize naturally occurring polymers including fibers

B.          Represent polymers in terms of their repeating units

C.          Write formulas for condensation polymers, given the monomer

D.         Identify polymers from their tradenames using standard reference materials

E.          Recognize characteristics of common polymeric materials and thereby classify the polymer

into major categories such as polyethylene, polystyrene, polyurethane, silicone polymer, PET,

etc.

F.          Demonstrate understanding of the functional characteristics of common polymers

G.         Understand the difference between addition and condensation polymers

H.         Understand thermoset vs. thermoplastic resins

I.          Differentiate between a polymeric fiber, resin and film.

J.          Understand the role of polymer additives

K.         Recognize the role of polymer properties in determining recycling capability

6.    Identify the relative importance of chemical bonding in engineering materials.

A.          Differentiate between the 4 types of bonds-Covalent, Ionic, Metallic, Vanderwaal.

B.          Identify how each of the 4 bonds can be most easily broken.

C.          Explain how slip planes and lattice structure defects in metals can be used to break bonds and
reshape metals.
7.    Explain how engineering materials degrade over time.

A.          Explain what happens when you place 2 dissimilar metals in contact with each other.

B.          Explain the process involved in the rusting of ferrous metals.

C.          Explain the process of oxidation of aluminum.

D.          Explain the process of degradation of plastics due to chemicals and heat.

8.    Explain the relationship between structure and function of carbohydrates and lipids.

A.          Recognize optical isomers

B.          Classify carbohydrates as monosaccharide, disaccharide, oligosaccharide and polysaccharide

C.          Differentiate between glucose and fructose

D.          Describe hydrolysis of disaccharides

E.          Recognize the significance of sugars and sugar substitutes

F.          Discuss the utility of polysaccharides (polymers) starch and cellulose

G.         Recognize the classification of lipids as being simple lipids, compound lipids, steroids or fat-

soluble vitamins

9.    Explain the operation of commonly-used batteries.

A.          Identify the role of the anode, cathode, and electrolyte.

B.          Explain how a common flashlight battery works.

C.          Compare lead-acid storage battery operation with more recently-developed battery types.

10. Explain the process of chemical etching in manufacture.

A.          Explain how chemical etching is done on flat surfaces.

B.          Explain how chemical etching is used in building printed circuit boards for microchips in the

semiconductor industry.

11. Identify the characteristics of liquid engineering materials.

A.          Compare the chemical formulations of the following hydraulic fluids:

1.    petroleum oils
2.    phosphate esters
3.    chlorinated hydrocarbons
4.    alcohol

B.          Identify whether the fluids in (1) above are chemically compatible with the following seal materials:

1.    rubber
2.    thermoplastic
3.    thermoset
4.    cork
5.    wood
6.    cast iron