Unit 7: Chemical Quantities Moles <--> Particles After today, you will be able to… • Using dimensional analysis, calculate how many atoms, molecules, or formula units are in one mole of that substance • Use correct significant figures and units in these calculations • Identify key scientists in the development of the mole Substances can be measured in different ways…. The Mole can be 1.Count – 5 apples, dozen eggs related each16oz of 2.Mass – 2lbs ofto bananas, box of cereal these types of 3.Volume – gallon of milk, pint of measurements. cream A Brief History on the Mole… Avogadro: (1811) An Italian scientist who studied the behavior of gases. Theorized:“The volume of a gas at a specific temperature and pressure contains equal numbers of atoms or molecules regardless of the nature of the gas.” Loschmidt (1865): Estimated the average diameter of the molecules in air and was able to calculate the number of particles in a given volume of gas. Millikan (1910): Measured the charge on an electron. From the charge on a mole of electrons, he divided the two and obtained Avogadro’s number. Perrin (1926): Earned the Nobel Prize for computing Avogadro’s number using many different methods and named this constant in honor of Avogadro. Used oxygen as a standard and proposed “Avogadro’s number is the number of molecules in exactly 32-grams of oxygen.” The standard was later changed to the carbon-12 isotope. The presently accepted definition of the mole is: “The amount of any substance that contains as many elementary entities as there are in 12 grams of pure carbon-12.” The mole (mol) as a unit in chemistry serves as a bridge between the atomic and macroscopic worlds. In Latin, mole means “huge pile.” 1 mole = 23 6.02x10 atoms, molecules, or formula units = 602,000 ,000,000,000,000,000 ,000 = six-hundred and two sex-tillion This equality can be used as a conversion factor to convert particles into moles, or moles into particles. Example: How many atoms are in a 1.22 mole sample of sodium? K: 1.22 mol Na U: ? atoms Na K stands for what we know! U stands for what we are solving for! 1.22 mol Na x 6.02x1023 atoms Na = 1 1 mol Na 7.34x1023 atoms Na Example: How many moles are equal to 4.79x1024 molecules of CO? K: 4.79x1024 molec. CO U: ? mol CO 4.79x1024 molec. CO x 1 mol CO . = 6.02x1023 molec. CO 1 7.96 mol CO