Chem notes 1-3

Chem notes 1-3 - 1.4-1.7 Sig Figs: 0.004004500 4.50 Bolded...

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Unformatted text preview: 1.4-1.7 Sig Figs: 0.004004500 4.50 Bolded are significant x or / Same sig fig + or – same decimal places Density P = m/v Density times volume = mass Intensive: independent of mass ex. Density Extensive property: dependent on mass Conversion kg to g then you multiply by 1000g/kg - Systematic error: built into instrument - Random Error: human error - Precision: how closely bundled are results - Accuracy: how close to real value 2.3-2.8 - Atomic number = proton number (z)BOTTOM - Mass number (a) = protons+neutrons TOP - Isotopes= massXabundance add it all up = periodic table number - Periodic table: ME transit into halogas LA 3.2-3.6 (3.5 not included) - Formula mass (ionic compounds) = Molecular mass (covalent) = mass of 1 mole - Be careful of units H O N F CL Br I are all diatomic 2 form *atomic mass of H = 1 Molar mass = 2 % element = [(no. of atoms) (Molar mass of element) ]/ molar mass of compound X100 - Empirical=Simplest - Molecular = multiple of empirical -1 mole= 6.02*1023 atoms aka Molar Mass Convert % to grams, divide by molar mass of compound to get moles, divide by smallest one and multiply to make it a whole no. Figure out H and C amount and grams of oxygen = sample – C – H 1)Free element ex. C has an Oxidation State =0 2) Compound OS=0, Ion: sum of OS = charge 3) Group1 OS +1, Group 2 OS +2 4) Flourine in compound has OS = -1, H +1, O -2 Group 17 -1, 16 -2, 15 -3 *OS can be fraction Naming compounds: metal/nonmetal = ide ending 1st if its mono) *positive OS element 1st Covalent = dinitrogen monoxide (both, not ...
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This note was uploaded on 04/02/2010 for the course AECH 110 taught by Professor Cherestes during the Winter '10 term at McGill.

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