CHM 103 1st Edition Exam 1 Study Guide Lectures 1 9 Chapter 1 Lectures 1 3 The Scientific Method hypotheses laws and theories o Hypothesis a tentative interpretation of observations o Scientific Law summarize observations to predict other ones o Scientific Theory model for the way nature is to explain why Classification of Matter o state solid liquid gas o composition pure substance element or compound mixture homogeneous or heterogeneous Properties of Matter o physical properties can be observed without changing the composition o chemical properties observed only during a chemical change physical chemical changes be able to distinguish between them Converting between Fahrenheit Celsius and Kelvin equations will be given Density o d m V m d V V m d o be able to calculate the volume of a regularly shaped solid given the appropriate equation Significant figures o when are zeroes significant Interior zeroes always are Trailing zeroes are if after a decimal o rules for addition subtraction Keep the lowest number of decimal points o rules for multiplication division Keep the lowest number of significant digits o combining the two sets of rules Conversion factors o know the metric prefixes o English to metric conversion factors will be given o know how to handle squared or cubed units Chapter 2 Lectures 4 6 Modern Atomic Theory o Law of Conservation of Mass Law of Definite Proportions Law of Multiple Proportions o Dalton s Atomic Theory Discovery of subatomic particles o Thomson s Cathode Ray Tube discovery of electrons o Millikan s Oil Drop Experiment charge of electrons o Rutherford s Gold Foil Experiment structure of atoms discovery of protons Structure of atoms o nucleus very dense core of protons and neutrons makes up most of the atom s mass o electrons travel around the nucleus in clouds make up most of the atom s volume Terminology o atomic number Z of protons in nucleus defines the element o chemical symbol 1 or 2 letters be able to identify the names chemical symbols for the first 36 elements periodic table will be included with exam o mass number A of protons of neutrons Isotopes atoms of the same element with different numbers of neutrons o be able to calculate the average atomic mass of an element given the appropriate data Ions neutral atoms that have either gained or lost electrons o Elements in groups 1A 2A and 3A tend to form 1 2 and 3 cations respectively noble gas electron counts o Elements in groups 5A 6A and 7A tend to form 3 2 and 1 anions respectively noble gas electron counts The Periodic Table o arranged so elements in groups columns have similar properties rows are called periods o know the locations of metals vs nonmetals main group elements transition metals alkali metals alkaline earth metals halogens noble gases Converting between MASS MOLES and OF PARTICLES o units on Avogadro s Number 6 022 1023 particles mole o be able to do these conversions for pure elements and for compounds Chapter 3 Lectures 7 9 Chemical bonds know the difference between ionic and covalent bonds and how to identify whether a compound is ionic or molecular Chemical formulas know the difference between empirical and molecular formulas Ionic compounds o review the naming handout memorize names and charges polyatomics o be able to write formulas based on names and vice versa Molecular compounds o Greek prefixes denote the number of atoms of each element in the molecule o be able to turn formulas into names and vice versa o special rules for naming acids Composition of compounds o be able to calculate the molar mass of a compound o be able to calculate mass percent based on formulas o be able to use mole ratios based on formulas o be able to determine the empirical formula of a compound based on composition o be able to determine the molecular formula given the empirical formula and the molar mass Writing and balancing chemical equations Combustion reactions using combustion reactions to determine the empirical formula of a hydrocarbon