Chemistry I Final Exam Review Topics

Unit 1 *Lab safety – fire, spills – acid/base, broken glass, chemical disposal, goggles *SF rules for +/- and x/division – how to report answer *Density formula *Identifying substances based on characteristics found on ref tables *Difference between accuracy and precision

Unit 2 *Elements cannot be decomposed by a chemical change, compounds can, mixtures can be separated by a physical change *Physical vs. chemical properties and changes *Laws of definite composition and multiple proportions

Unit 3 *Moles <----> Grams <----> Atoms/Molecules conversions # *Determine # of neutrons, protons and electrons when given symbol # Sym *Average atomic mass – why they are not whole numbers? *Atomic theory scientists: Rutherford, Bohr, Thompson, Dalton *Electron cloud model *Understand what this notation tells you - Carbon-14 *1 mole of an element (compound) = 6.02 x 1023 atoms (molecules)

Unit 4 *Interpret Bohr model of hydrogen atom on last page of ref tables *Orbital notation: Hund’s rule *E = h., c = . calculations *Excited state – where are electrons, how did they get there *Be able to determine the number of valence electrons from an electron configuration *Be able to draw dot diagrams (Lewis dot structures)

Unit 5 *Ions – notation, formation, what they mean *Periodic trends (atomic radius, ionization energy, electronegativity)

Unit 6 *Bonds – ionic vs. covalent: what they mean/ how they are formed, types of elements involved *Shapes vs. Lewis structures (know up through tetrahedral) *Molecular polarity compared to bond polarity *How are solid and liquid properties affected by types of bonding and intermolecular forces (IMF)

Unit 7 *Determine oxidation # of element in polyatomic ions and compounds *Nomenclature – roman numerals esp. *% by mass *Empirical formula – definition /calculation *Finding the molecular formula from the empirical formula

Unit 8 *Types of reactions *Symbols in chemical reactions: (s), (l), (g), (aq),  = heat added, formula over arrow = catalyst *Use activity series to predict whether a reaction occurs or not *Be able to balance equations *Coefficients in a balanced equation tell you the relative amount of MOLES!

Unit 9 *Stoichiometry: all types involving moles, mass, volume, # of atoms/molecules *% yield = (actual yield/theoretical yield) x 100 *moles to moles, moles to grams, grams to moles, grams to grams

Unit 10 *K-M Theory points (behavior of ideal gases), (at what two conditions do gases not behave ideally) *Ideal gas equation – note about “STP” – remember that there are numbers associated with this abbreviation... it may seem like there is not enough information to solve a problem (usually involving gases), but if STP is included, there is. Always use Kelvin temperatures! *Gas law problems: Boyle, Charles, Gay-Lussac, Combined, Ideal, Dalton’s, Graham

Unit 11 *Q = m . Cp . T * Q for phase change *Phase diagrams – state of matter at different locations – each section not labeled *Interpret a heating/cooling curve graph – phase changes vs. temperature changes *Heat transfer between objects

Unit 12 *Solubility rules – interpret (check reference tables!) *Molarity definition/calculation * Dilution math M1V1=M2V2 WATCH UNITS!!!! *Write net ionic equations *vanHofft factor (dissociation) – the i in freezing point depression problems *Solubility curves – be able to interpret – ie, how many grams can dissolve, etc

Unit 13 *Acid-Base titration (calculation) *pH  [H+1] and pOH  [OH-] and pH  pOH conversions *Characteristics of strong acids and bases: completely ionize, strong electrolytes *Products of a neutralization reaction *Acid-Base definitions, especially Bronsted/Lowry

Unit 14 *Methods of increasing the rate of a reaction in general – esp. how using a catalyst increases rate by lowering the activation energy *PE diagram: know what each part represents, know how diagram changes if a catalyst is added *Recognize how to determine exo/endothermic (∆H)(side of equation w/ energy on it), positive or negative S (be able to predict sign) *collision theory – the molecules need sufficient energy in order to react

Unit 15 *Half-reactions: pick out from overall equation given, be sure e- are written on correct side (be able to label as being oxidized or reduced) *Definition of anode/cathode – what processes occur there, how electrons flow

Unit 16 *Nuclear particles – know the notation of emitted particles (alpha, beta, gamma, positron) *Balance nuclear equations *Half-life calculations