chemistry chapter 10 study guide – Flashcards
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Gram-atomic mass
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the molar mass of an element expressed in grams per mole (g/mol)
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Gram-formula mass
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The mass of a mole of formula units in a ionic compound bond.
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Mole
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the simplest structural unit of an element or compound A group of atoms bonded together
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Empirical formula
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A formula showing the lowest whole number ratio of atoms in a compound
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STP
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0 degrees C and 1 atm
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Molar mass
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The mass in grams of 1 mol of a substance
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Molar volume
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the volume occupied by 1 mole of a gas at standard temperature and pressure (STP); 22.4 L
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Avogadro's number
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6.022 x 10^23
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Gram-molecular mass
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the mass in grams of a mole of molecular units; a value numerically equivalent to the average molecular mass expressed in grams
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% Composition
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(Mass of X in formula)/(Formula Weight of Compound) x 100%
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What are the representative particles?
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Atom, molecule, count
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What are the diatomic elements?
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Hydrogen Nitrogen Oxygen Fluorine Chlorine Iodine Bromine
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What is the value of Avogadro's number
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6.022 x 10^23
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What is relationship between A's number & the mole
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They are equal to each other
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What is the molar volume of a gas @ STP
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22.4
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What are the values of STP in SI units
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0 Celsius, 101.3 kilopascals (Kpa)
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Be able to recognize if an empirical formula or not
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[[to be emp., must have lowest whole number ratio; IF it can be simplified, it is a molecular formula; NEVER REDUCE SUBSCRIPTS OF A POLYATOMIC ION!!]]
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What are 3 ways quantities can be measured in chemistry
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Mass Volume Count
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Be able to determine moles of atoms in a molecular formula. o Ex: 0.2 mol H2O
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How many moles of hydrogen? 2 x .2= .4 total moles= 3 x .2=.6
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Empirical Formula
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o divide amount given by element's atomic mass o divide these answers by whichever is the smallest o correct for any decimal fractions o ratio becomes subscripts for empirical formula
