CH 105 Chemistry for Allied Health

1. Define energy.
2. Describe the difference between kinetic energy and potential energy and give several examples of each.
3. State which molecules have greater kinetic energy; those in a sample of water at 20EC, or in the same sample of water at 100EC?
4. List four different forms of energy.
5. Define calorie and use experimental data to calculate the number of calories in a food sample.
6. Define the melting point and the boiling point of a substance.
7. Describe the changes that occur at the molecular level as an ice cube is warmed from -5E to 110EC.
8. Define heat of fusion and heat of vaporization.
9. Define and explain the role of a catalyst in a chemical reaction.
10. Define and explain the difference between kinetic stability and thermodynamic stability.
11. State the Bronsted-Lowry definition of an acid and base and identify the conjugate acid-base pairs in a chemical reaction.
12. State in his/her own words the difference between a strong and weak acid, and a strong and weak base.
13. Write a balanced equation for a neutralization reaction between an acid and base.
14. Name an acid or acid salt when given its formula.
15. Write the equation for the ionization of water.
16. Given the pH of a solution, calculate the hydrogen ion concentration and hydroxide ion concentration and state whether the solution is acidic, acid, or neutral.
17. Define normality and calculate the normality of a specified solution of acid or base.
18. Perform the equivalence point calculations for a titration.
19. Define buffer and give an example of the way in which the blood plasma is protected against large changes on pH.
20. Define acidosis and alkalosis and describe conditions in the body that will cause acidosis to occur.
21. Define organic chemistry.
22. Describe the difference between molecular and structural formulas of a compound.
23. Define structural isomer and, given the molecular formula of a compound, draw the structural formulas of its isomers.
24. Define alkane and saturated hydrocarbon.
25. Draw the structural formula of an alkane when given its IUPAC name, and state the IUPAC name when shown the alkane’s structural formula.
26. Write the chemical equations for the combustion and substitution reactions of a given alkane.
27. Determine whether a hydrocarbon is saturated or unsaturated, given its structural formula.
28. Describe the difference between the alkanes, alkenes, and alkynes, and give examples of compounds found in each class.
29. Draw the structural formula of a hydrocarbon when given its IUPAC name, and state its IUPAC name when given its structural formula.
30. Define geometric isomer, and give examples of the cis- and trans- structures of an alkene and a cyclic hydrocarbon.
31. Compare the chemical reactivity of the alkanes and alkenes.
32. Write the equations for the combustion, addition, and polymerization.
33. Write the equation for the substitution reaction of benzene with a halogen.
34. Classify the organic compounds having oxygen-containing functional groups, and given the structural formula of a compound, state its IUPAC name.
35. Compare the polarity and water solubility of alcohols, ethers, aldehydes, ketones, and carboxylic acids.
36. State the difference between a primary, secondary, and tertiary alcohol.
37. Describe two methods for preparing alcohols in the laboratory.
38. Write the equations for the dehydration and oxidation reactions of an alcohol.
39. State the difference in structure between aldehydes and ketones.
40. Describe one method of preparing aldehydes and ketones.
41. Compare the ease with which aldehydes and ketones can be oxidized.
42. Write the equations for the production of a carboxylic acid and an ester.
43. Define esterification, hydrolysis, and saponification, and give an example of each reaction.
44. Classify organic compounds having nitrogen-containing functional groups.
45. Given the structural formula of an amine or amide when given its IUPAC name, and state the IUPAC name when given its structural formula.
46. Write the structural formula of an amine or amide when given its IUPAC name, and state the IUPAC name when given its structural formula.
47. Write the equations for the reaction of an amine with water, with an acid, and with an alkyl halide.
48. Describe two ways of preparing an amide in the laboratory.
49. Write the equation for the hydrolysis of an amide.
50. Define heterocyclic ring.
51. Describe three uses of alkaloids in drug therapy.

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.

• Energy
  • Definition of energy
  • Kinetic energy
  • Potential energy
  • Reaction rates
  • Energy diagrams
  • Chemical equilibrium
• Acids and Bases
  • Acid/base definitions
  • Strength of acids and bases
  • Nomenclature
  • Neutralization and titrations
  • pH: defined and control
  • Normality
  • Buffers
• Organic Chemistry: Saturated Hydrocarbons
  • The role of carbon
  • Organics defined
  • Hydrocarbons and their bonds
  • Writing structural formulas
  • Alkanes
  • Nomenclature
• Organic Chemistry: Unsaturated Hydrocarbons
  • Unsaturated hydrocarbons
  • Alkenes and their nomenclature
  • Geometric isomers
  • Alkynes and cyclic hydrocarbons
  • Aromatic hydrocarbons and nomenclature
• Organic Chemistry: Functional Groups
  • Alcohols: reactions and descriptions
  • Aldehydes and ketones
  • Carboxylic acids
  • Esters, ethers
  • Amides and amines

Laboratory Content:

• Energy Measurements
  • Specific heat
  • Temperature/energy changes
  • Exothermic and endothermic reactions
• Chemical Reactions
  • Rates and factors
  • Catalysis
  • Equilibrium
• Electrolytes, Acids, and Bases
  • Electrolytes, acids, bases, buffers
  • Solvent properties of water
  • Standardizations
• Acids and Bases
  • Neutralization
  • Titrations
  • Standardizations
• Properties of Organic and Inorganic Compounds
  • Solubility, flammability, melting points, boiling points
  • Reactions
  • Formulas from molecular models
• Hydrocarbons
  • Molecular models
  • Isomerism
  • Saturation
  • Combustion
• Organic Oxygen Compounds
  • Alcohol structures
  • Physical and chemical properties
  • Aldehydes and ketones
  • Synthesizing esters
• Analysis of Aspirin
  • Rate of disintegration
  • Stability
  • Percentage and composition
  • Saponification
• Organic Nitrogen Compounds
  • Primary, secondary, tertiary amines
  • Physical and chemical properties
  • Preparing acetanilide
  • Extraction of caffeine