HONORS UNIT 3B : AIRBAGS

Below are the class objectives, correlated to the NC Essential Standards and page numbers within your textbook. In the far right column you will see the required vocabulary of the unit as well. At the end of each unit, you should be able to define and apply all the required vocabulary words in order to be successful on the unit test.

Unit / Section / Glencoe Pages / North Carolina Essential Standard / Student Objectives / Unit Vocabulary
Unit 3b: Airbags (Part B) / 3.4 / 385-390
419-420
309-341 / 2.1.5•
2.2.5• /
  • Define a mole & Avogadro’s number
  • Define and calculate molar mass
  • Define molecular mass and atomic mass as mass for 1 mole of particles
  • Perform calculations between number of particles, moles and masses(standard: 1 step conversions; Honors: multistep conversions
  • Apply 1 mole of any gas at STP=22.4 L
  • Calculate empirical formula from mass or percent using experimental data.
  • Calculate molecular formula from empirical formula using molecular weight
  • Determine percentage composition by mass of a given compound.
  • Perform calculations based on percent composition.
  • Determine the composition of hydrates using experimental data.
/ Required Vocabulary
  1. Kinetic Molecular Theory
  2. Dalton’s Law of Partial Pressures
  3. STP
  4. Combined Gas Law
  5. Ideal Gas Equation
  6. Ideal gas
  7. Real gas
  8. Mole
  9. Avogadro’s number
  10. Standard molar volume
Other Vocabulary
  1. Pressure
  2. Absolute temperature
  3. Boyle’s Law
  4. Charles’ Law
  5. Gay-Lussac’s Law
  6. Avogadro’s Law

3.5 /
  • Define pressure & atmospheric pressure
  • Qualitatively relate properties of gases: volume, pressure, temperature, number of particles
  • Define kinetic molecular theory
  • Distinguish between real and ideal gases
  • Understand movement of gas: effusion v diffusion

3.6 / 421-438 / 2.1.5• /
  • Apply formulas and concepts of kinetic molecular theory: 2. Ideal gas equation (PV=nRT), Combined gas law (P1V1/T1 = P2V2/T2) and applications holding one variable constant: for PV=k, P1V1 = P2V2; for V/T=k, V1/T1= V2/T2; for P/T=k, P1/T1 = P2/T2. Note: Students should be able to derive and use these gas laws, but are not necessarily expected to memorize their names.
  • Apply formulas and concepts of kinetic molecular theory: 3. Avogadro’s law (n/V=k), n1/V1 = n1/V2
  • Apply formulas and concepts of kinetic molecular theory: 4. Dalton’s law (Pt=P1+P2+P3 …)

3.7 /
  • Use the concept of calorimetry to measure heat changes in constant pressure system for chemical and physical changes.
  • Understand the difference between endothermic and exothermic reactions, using reaction pathway graphs and chemical equations