Accuracy and Precision

CHEMISTRY FINAL EXAM 2014-2015 - TOPICS TO REVIEW

Fundamental concepts in chemistry  accuracy and precision  percent yield (calculations)  factor labeling/dimensional analysis  sig figs – why and how to use them  metric units/conversions  temperature: average kinetic energy of the molecules  units of temperature Kelvin and Celsius (K = ˚C + 273)  percent error (calculations)

KMT and energy changes  phase changes and heating curves  heat absorbed/lost during heating/cooling/phase changes -be able to draw a heating curve graph for water  heat of fusion, heat of vaporization, specific heat -temperature and phase changes during heating (calculations) -potential and kinetic energy changes during  be able to find Physical Constants for Water in data book heating/cooling and phase changes  know all the terminology for phase changes

Atomic structure  know the basic structure of the atom – protons,  electron configurations and the periodic table neutrons, electrons -understand stability  nuclear chemistry (types of decay) -predict oxidation numbers from the periodic table  represent an atom with different types of diagrams -predict the charge on an ion and/or symbols -how an atom becomes an ion (metal or non-metal)  distinguish between different isotopes

Ionic and covalent bonding  distinguish between ionic and covalent compounds  understand how bonding relates to stable electron  name and write correct (electrically neutral) configurations formulas for ionic compounds using oxidation  know the four types of intermolecular forces numbers/charges  use the “criss-cross” shortcut  explain how the characteristics of water related to  Use Roman numerals correctly intermolecular forces  use Ref Table F for polyatomic ions  name and write formulas for covalent compounds using  recognize the diatomic elements (HONClBrIF) prefixes

The Periodic Table  know how it is organized  distinguish between groups/families and periods  know the phases of the elements  characteristics of groups/families

Chemical reactions  write complete, balanced equations from word  use Ref Table N to determine if a single replacement reaction descriptions will occur.  recognize the five main types of reactions  use Ref Table E to determine if a precipitate is formed  What is combustion?  be able to write equations all three ways: molecular, complete  predict products if given the reactants ionic, and net ionic

Mathematics of chemistry ; stoichiometry  simple calculations involving mass/moles/particles/gas  stoichiometry problems using mole ratios from balanced volume/ chemical equations  Definitions of mole and standard pressure (earlier?).  Limiting reagent problems

Solutions  explain the difference between concentrated and  When a solution is cooled, identify how much precipitate saturated may be formed  be able to identify solvent and solute in a solution  Explain why a supersaturated solution is unstable  Define Molarity (M) = moles of solute/liters of solution  Recognize the effect of temperature on the solubility of  Calculate amount of stock solution needed to make a dilute a solute

solution (using M1V1 = M2V2)  Explain why gases are less soluble at higher temperatures  use solubility table/graph (D&E) to describe solutions  Use table E to predict whether or not a salt will dissolve  Use graph D to identify unsaturated, saturated and in water supersaturated solutions 00d7bfe6fc751854d337826f49755793.doc - 1 Gases TBA

Equilibrium TBA

CONSTANTS and EQUATIONS

sig figs indicate the precision of original --Know dimensional analysis/factor labeling measurements method for conversions add/sub: sig figs determined by least precise --Conversions can include metric conversions as number well as other things like mole conversions: ex.: 23.56 mL  mol to g (using molar mass) - 2.2 mL = 21.4 mL  mol to number of particles (1 mol = 21.36 mL 6.02x1023 particles) mult/div: sig figs determined by least # of sig figs  mol of a gas to L of a gas (1 mol = 22.4L) ex.: --Particles can include atoms, f. u., molecules, or 23. 56 cm x 2.2 cm = 51.832 cm2 = 52 cm2 ions --Understand mole ratios in stoichiometry to % error = (experimental-theoretical) x 100 set up the equation for calculations. theoretical % yield = experimental x 100 theoretical 1 mole = molar mass of substance M = mol Solutions 1 mole = 6.02 x 1023 particles (atoms or molecules) L

1 mole of gas = 22.4 L at STP M1V1 = M2V2 Dilutions (STP) standard temp and pressure = 0 ˚C and 1 atm Solubility tables and graph. Heat and it’s equations: c = 1 cal Q = mcΔT g · oC

Q = mHf Hf = 79.72 cal Hv = 539.4 cal g g Q = mHv

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