Review Sheet

Chemistry Review Sheet Unit 1 major concepts: Basics 1) Physical vs. chemical properties (density vs. reactivity) [pg7-10] 2) Physical vs. chemical changes (melting vs. burning) [pg7-10] 3) Conservation of energy (mass) [pg7-10] 4) Classification of matter [pg11-13] 5) Families vs. periods (columns vs. rows) [pg17] 6) Characteristics of metals, nonmetals, and metalloids [pg18-20] 7) Qualitative vs. quantitative (red vs. 440nm) [pg29] 8) Mass vs. weight (unchanged by gravity vs. depends on gravity) [pg34-35] 9) Density Calculations (d=m/v) [pg38-39] 10) Unit conversions [pg34-37 & 40-42] 11) Accuracy vs. precision (around correct “point” vs. close together) [pg44-45] 12) Sig figs [pg46-50] 13) Scientific notation [pg50-52] 14) Inverse vs. direct proportions (one goes ↑ the other goes ↓ vs. both go ↑)[pg55-57] Unit 2 major concepts: The atom, electrons, and the periodic table 1) Dalton’s atomic theory (the solid sphere model) [pg68-69] 2) The cathode ray experiment (discovery of electrons) [pg72-73] 3) Rutherford’s experiment and atomic model (gold foil nucleus) [pg74-76] 4) Protons, neutrons, and electrons (you should know this) [pg76] 5) Moles, Avogadro’s number, and molar mass [pg80-81] 6) Mole conversions (# atomsmolegrams and back) [pg84-87] 7) Speed, wavelength, frequency, and energy of electromagnetic radiation [pg97-99] 8) Particle vs. wave nature of light (excites electrons vs. has a frequency) [pg97-100] 9) Photoelectric effect (light excites electrons) [pg99-100] 10) Bohr model of hydrogen (only certain light frequencies emitted) [pg100-103] 11) Electron energy levels and orbitals (s, p, d, f) [pg111] 12) Electron configurations (orbital, electron-configuration, noble gas notation) [pg112-113] 13) The periodic table [pg133-136] 14) The four blocks (s, p, d, f) relate the electron configurations to column [pg138-149] 15) Atomic radii, ionization energy, electronegativity (how they change as you move down and across the periodic table and why) [pg151-164] Unit 3 major concepts: Chemical bonding 1) 2) 3) 4) 5) 6)

Bonds (why they form, what they are) [pg175] Ionic vs. covalent (stealing vs. sharing valence electrons) [pg175-177] Electron negativity difference  bonding type [pg176-177] Covalent bonding (electrons are shared) [pg178-179] The octet rule (main group elements “want” to have 8 valence electrons) [pg182-183] Lewis structures [pg184-188]

7) Resonance structures [pg189] 8) Ionic bonds (valence electrons are stolen) [pg190] 9) Properties of ionic compounds (brittle, strong bonds, high melting point) [pg193] 10) Types of packing (cubic close, face centered, etc.) [not in book] 11) Polyatomic ions (NO3-, SO42-, etc.) [pg194] 12) Metallic bonding (electrons sea, malleable, ductile, conductive) [pg195-196] 13) VSEPR theory (3D molecules) [pg197-198] 14) Molecular geometries (the sheet with all the geometries) [pg200] 15) Polarity and intermolecular forces [pg203-206] Unit 4 major concepts: Ions and math 1) 2) 3) 4) 5) 6) 7) 8) 9)

Ions (you don’t need them memorized, a sheet will be on the test) [pg221 & 2226] Al2(SO4)3  aluminum sulfate & back (remember roman numerals for metals [pg222-225] Naming binary molecules (N2O5 is dinitrogen pentoxide) [pg227-229] Acids (hydrogen bonded to any anion) [pg230] Oxidation numbers (S = +6 in H2SO4) [pg232-234] Calculating molar mass of molecules (molar mass of H2O is 18 g/mol) [pg238-239] Mole conversions in molecules (2 mole of H2O weighs 36 grams) [pg240-242] Percent composition (H2O is 2/18 or 1/9 hydrogen by mass) [pg242-244] Determining empirical and molecular formula (CH3 vs. C2H6) [pg245-249]

Unit 5 major concepts: Reactions and stoichiometry 1) 2) 3) 4)

Signs a reaction took place (color change,  solid or gas, heat or light) [pg261-262] Word  formula equation (Methane + Oxygen  Carbon Dioxide + Water) [pg263-265] Balancing chemical equations (__ H2O2  __H2O + __O2) [pg270-274] Reaction types (synthesis, decomposition, single and double displacement, and combustion) [pg276-284] 5) The activity series (will Co(s) + 2NaCl(aq) yield a reaction? Answer = no) [pg285-286] 6) Mole ratios [pg299-301] 7) Stoichiometry (we’ll practice) [pg304-311] Unit 6 major concepts: States of matter, especially gasses 1) 2) 3) 4) 5) 6)

The kinetic-molecular theory of matter and gasses (in constant motion) [pg285-286] Solids, and liquids [pg333-341] Changes of state (endothermic or exothermic) [pg348] Phase diagrams [pg347-348] Pressure conversions [pg364] Dalton’s law of partial pressures (oxygen is collected by water displacement…)[pg365-367]  P1V1 P2V2 = T2  T1

7) The gas laws, esp. the combined gas law  8) The ideal gas law PV=nRT [pg383-385]

  [pg374-375] 

Unit 7 we just completed. I trust you have all the completed handout to study. If not, you may print them off the internet at the course website: chemguide.wikispaces.com