Chemistry I – Midterm Exam Review Chapter 1 The nature of chemistry – What is chemistry? How is chemistry done? Scientific method hypothesis, law, theory lab safety The five branches of chemistry Chapter 2 Matter mass, volume, density, temperature physical vs. chemical properties physical vs. chemical changes The Law of Conservation of Mass homogeneous solutions vs. heterogeneous solutions elements, compounds, substances

Chemistry I – Midterm Exam Review Chapter 3 Qualitative vs. quantitative measurements Scientific notation vs. standard form Simple mathematical operations using scientific notation Significant figures Mathematical operations and significant figures (multiplication, division, addition, and subtraction.) Precision vs. accuracy Density calculations Chapter 4 Metric Metric Conversions Metric  English conversions Chapter 5 Dalton’s atomic theory Protons, neutrons, and electrons The cathode ray experiment

Chemistry I – Midterm Exam Review Chapter 5 The gold foil experiment mass number vs. atomic number isotopes metals vs. nonmetals metalloids The Periodic Table Chapter 13 various atomic models – (Rutherford, Bohr, quantum mechanical, etc) electron configurations orbitals wave mechanics electromagnetic spectrum Chapter 14 Periodic Trends – atomic radius and electronegativity

Chemistry I – Midterm Exam Review Bonus Questions: 1. Draw a periodic table. Indicate, by color, the s-block, p-block, d-block, and f-block. Use a different color for each block. List the colors of light from longest wavelength to shortest wavelength List the five signs that a chemical reaction has occurred. Calculate the average atomic mass, given the following data: Isotope 1 : 78.88 % abundant ; mass = 34.55 amu Isotope 2: 21.13% abundant; mass = 36.88 amu