Fall Mid-term Exam Review To study, make sure to look over (and possibly redo) all homework assignments, old labs. Make sure to read through, recopy and study all class notes. Chapter reviews at the end of each chapter (even if they weren’t assigned) will be very helpful for you to use as practice questions. Chapter 1 1. Alchemy and Aristotle’s theory 2. Matter a. General properties—mass and volume b. What is an atom, element, compound? 3. Physical property vs. Chemical property with examples a. Identify a chemical change vs. a physical change 4. What is a change of state? 5. Identify types of matter—heterogeneous, homogeneous, pure substance (hint: Study chart at bottom of p. 15 in textbook) 6. Be able to label the different areas of the periodic table a. Groups and periods and how the elements within them are related b. Properties of metals, nonmetals, metalloids, noble gases Chapter 2 1. Qualitative vs. quantitative 2. Mass vs weight 3. Density calculations (know formula) 4. Conversion Factors 5. How to calculate Percent Error (know formula) 6. Significant figures 7. Scientific notation Chapter 3 1. Dalton’s Atomic Theory vs. Modern Atomic Theory 2. The three laws: 1. Conservation of mass, Law of definite proportions and Law of multiple proportions 3. Discovery of electrons: Cathode ray 4. Discovery of the nucleus: Gamma rays and gold foil 5. Avogadro’s Number, atomic mass vs. molar mass, atomic number, isotopes, finding number of neutrons, electrons, protons (and know their properties) 6. Units for molar mass vs. atomic mass 7. Calculations for elements and molecules a. moles atoms b. moles grams c. atoms grams (remember mol is in between these!) d. average atomic mass from isotopes e. molar mass of molecules Chapter 4 Section 4-1: 1. What are waves? electromagnetic radiation, electromagnetic spectrum, 2. frequency, wavelength and their relationship to the speed of light 3. continuous spectrum vs. line spectrum; what causes a line spectrum 4. black light vs. white light 5. Excited state vs. ground state 6. What is a photon? Section 4-2: 1. Heisenberg Uncertainty Principle 2. Atomic orbitals and what they look like; how we know what they look like 3. 4 Quantum numbers a. principal quantum number (n) b. angular momentum quantum number (l) & how to get them (n-1) and how to write them c. magnetic quantum number (m) how many possible orientations each orbital has and be able to identify what the first three may look like d. spin quantum number (+1/2 and –1/2); Section 4-3: 1. The 3 rules that govern electron configuration of a ground state electron a. Aufbau principle b. Pauli exclusion principle c. Hund’s Rule 2. What an excited electron looks like in orbital notation and be able to identify which rule/s are being violated 3. How to write a. orbital notation b. electron configuration notation c. Noble gas notation Chapter 5: The Periodic Law 1. Mendeleev and Mosley 2. Modern Periodic Table 3. Periodic Law 4. properties, noble gas, lanthanides, actinides 5. s-block characteristics (alkali and alkaline-earth metals) 6. hydrogen and helium exceptions 7. d-block characteristics 8. p-block characteristics-halogens and noble gases 9. atomic radii—period and group trends 10. ionization energy—period trends and difficulty of removing e- from A+ 11. electron affinity—two possibilities, periodic trends, adding e- to A- 12. cation vs. anions a. their sizes in comparison to a neutral atom—ionic radii period and group trends b. Elements on which side of the periodic table is most likely to turn into which 13. valence electrons 14. electronegativity—periodic trends Laboratory 1. Lab Safety and Lab Equipment 2. Introduction to Measurements Lab 3. Conservation of Mass Lab 4. Flame Test Lab 5. Density is a Periodic Property Lab