CH 104 Chemistry for Allied Health

1. Apply basic chemical principles.
2. Describe the chemistry of living cells.
3. Perform scientific measurements.
4. Evaluate atomic and molecular structure.
5. Describe chemical reactions and stoichiometry.
6. State the units of length, mass, volume and temperature in the metric and SI systems.
7. Perform calculations with experimental data, maintaining the correct number of significant figures.
8. Convert measurements between the metric and English systems.
9. Define density and specific gravity and calculate these quantities when told the mass of a given volume of a substance.
10. Describe the structure of an atom, listing three subatomic particles, their relative mass, their charge, and their location in the atom.
11. Define atomic number and mass number, and given the atomic number and mass number of any element, indicate the number of protons, neutrons, and electrons in an atom of that element.
12. Describe how isotopes of an element differ.
13. Define atomic weight.
14. Describe the Bohr model of the atom and indicate the maximum number of electrons possible in energy levels 1 through 7.
15. List the various sublevels found within each principle energy level.
16. Use the periodic table to state the symbol, atomic number, atomic weight, and electron configuration of an element.
17. Given one element in a period or group, name another member of that same period or group.
18. State the number of valence electrons in an atom of any representative element.
19. Identify on a periodic table the elements that are metals, nonmetals, metalloids, representative elements, transition elements, and inner transition elements.
20. Define periodicity and predict how atomic size will change across a period and down a group.
21. Define ionization energy and electron affinity and predict how each will change across a period or down a group.
22. State the octet rule.
23. Describe an ionic bond and an ionic compound.
24. Describe a covalent bond and an ionic compound.
25. Describe a single, double, and triple covalent bond and give examples of each.
26. Draw the electron dot diagram for an ionic or a covalent compound formed from the representative elements.
27. Define electronegativity and describe how electronegativity changes on the periodic table.
28. Describe the difference between a polar and a non-polar covalent bond.
29. Define polyatomic ion.
30. Define oxidation number and determine the oxidation numbers of the elements in a given compound or polyatomic ion.
31. Write the formula for an ionic or covalent compound when given its name and write the name of the compound when given its formula.
32. Given its shape, predict whether a simple molecule will be polar or non-polar.
33. Describe the hydrogen bond.
34. Write a balanced chemical equation given the names of the reactants and products.
35. Define a mole.
36. Calculate the formula weight of a chemical compound.
37. Calculate the number of moles in a given mass of a substance.
38. Calculate the number of grams in a given number of moles of a substance.
39. Use a balanced chemical equation to determine the amount of reactants necessary to produce a given amount of product.
40. List three special properties of water and explain each in terms of the hydrogen bonding in water.
41. Describe the five properties of ideal gases stated by the kinetic-molecular theory.
42. List five units used to measure pressure.
43. State, in his/her own words, five laws of gas behavior and give everyday examples of each.
44. Perform calculations using Boyle’s law, Charles’ law, the general gas law, and Dalton’s law.
45. Describe and compare suspensions, colloids, and solutions and state three properties that are unique to colloids.
46. Define solute, solvent, and aqueous solution.
47. Describe in his/her own words the process by which sodium chloride dissolves in water.
48. Define electrolyte and nonelectrolyte and state the difference between a strong and weak electrolyte.
49. Predict whether a precipitate will form when two ion-containing solutions are combined.
50. Define saturated, unsaturated, and supersaturated.
51. Explain how to prepare a solution of a given molarity or a given percentage of solute.
52. Determine the concentration of a solution in parts per million or parts per billion.
53. Given an ion, state its gram-equivalent weight, and calculate the number of milliequivalents of that ion in a given weight/volume percent solution.
54. Describe how to prepare a specific volume of a given concentration from a stock solution.
55. Define osmosis, osmolarity, osmol, isotonic, hypertonic, and hypotonic.
56. Describe a laboratory procedure for separating cellular colloids such as proteins from the crystalloid contents of the cell.

Statewide General Education Outcomes:

1. Gather, comprehend, and communicate scientific and technical information in order to explore ideas, models, and solutions and generate further questions.
2. Apply scientific and technical modes of inquiry, individually, and collaboratively, to critically evaluate existing or alternative explanations, solve problems, and make evidence-based decisions in an ethical manner.
3. Assess the strengths and weaknesses of scientific studies and critically examine the influence of scientific and technical knowledge on human society and the environment.

• Matter
  • Composition and classification of matter
  • Elements and their properties
  • The scientific method
  • Precision, accuracy, and significant figures
  • Unit factoring and the SI system
  • Length, mass, volume
  • Temperature, density and specific gravity
• Atomic Structure
  • The parts of the atom and isotopes
  • Atomic number, mass number and atomic weight
  • The Bohr model and electron configuration
  • Ions
  • Atomic orbitals (optional)
  • The periodic table
• Combination of Atoms
  • The octet rule
  • The ionic bond, Lewis dot diagrams
  • Chemical formulas
  • The covalent bond, multiple bonds electronegativity
  • Polyatomic ions, oxidation numbers
  • Chemical compounds, formulas and shapes
  • Polarity and hydrogen bonding
• Chemical Equations and the Mole
  • Writing chemical equations
  • Balancing chemical equations
  • Balancing equations with oxidation numbers (optional)
  • The mole
  • Formula weight
  • The mole in problem solving
  • Calculations using balanced equations
• Solution Concentrations
  • Saturated and unsaturated solutions
  • Percent concentration and molarity
  • Parts per million and parts per billion
  • Equivalents and dilutions
• States of Matter
  • Solids, liquids
  • Changes of state
  • Gases and the kinetic-molecular theory
  • Units of pressure, volume and temperature
  • Gas laws
• Water, Solutions, Colloids
  • Solvent properties
  • Density and surface tension
  • Heats of vaporization and fusion
  • Specific heat
  • Solutions, suspensions, colloids and their properties
  • Electrolytes and nonelectrolytes
  • Solubilities and factors affection solubilities
  • Colligative properties, molality
  • Osmosis and dialysis

Laboratory Content:

• Laboratory Techniques
  • The Bunsen burner
  • Filtration
  • Evaporation
• The Metric System
  • Metrics
  • Balances and volumetric flasks
  • Density, specific gravity
• Chromatography
  • Separation of components
  • Paper chromatography
  • Thin layer chromatography
• Chemical Periodicity
  • Trends and relationships in the periodic table
• Relative Mass and the Mole
  • The law of conservation of mass
  • Atomic weights
  • Avogadro’s number and the mole
• Stoichiometry
  • The law of conservation of mass
  • Atomic weights
  • Avogadro’s number and the mole
• Properties of Gases
  • Boyle’s law
  • Henry’s law
  • Charles’ law
  • Graham’s law
• Electrolytes, Acids and Bases
  • Electrolytes
  • Water properties
  • Osmosis