The Mole

-Equal volumes of different gases had a constant ratio
Relative Mass
-expressed by comparing it mathematically to the mass of another object

Avogadro's hypothesis
-equal volumes of different gases at the same temperature and pressure have the same unmber of particle
-if they have same number of particles, the mass tatio is due to the mass of particle

FORMULA MASS
-total mass of all the atoms in he formula of an ionic compound in atomic mass units
K39.1u+F19.0u =KF58.1u

MOLECULARR MASS
-total mass of all the atoms that make up a molecule of a covalent compound organic compound or a polyyatomic element in atomic mass units
canbon dioxide
C 12.0g+O2 32g=44g

MOLAR MASS
mass of 1 mole of substane and is the same numerical value of atomic mass, formula mass, or molecular mass but expressed in Grams Per Mole
-1mole of oxygen=16.0g/mol
-1mole of carbon=12.0g/mole

the molar atomic mass of an element is the mass of 1 mole that element
the units of molar are grams per mole (g/mole)

Avogadro's number
-the number of particles in 1 mole of any amount of substance
6.022*10 to the 23
-the mole is extremely important to chemists because it allows them to sount atoms and molecules