Download presentation

Presentation is loading. Please wait.

Published byKendall Hillen Modified about 1 year ago

1
Unit 7: Chemical Quantities Moles Particles

2
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

3
Substances can be measured in different ways…. 1.Count – 5 apples, dozen eggs 2.Mass – 2lbs of bananas, 16oz box of cereal 3.Volume – gallon of milk, pint of cream The Mole can be related to each of these types of measurements.

4
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.”

5
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.

6
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.”

7
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.”

8
The mole (mol) as a unit in chemistry serves as a bridge between the atomic and macroscopic worlds. In Latin, mole means “huge pile.”

9
1 mole = 6.02x10 23 atoms, molecules, or formula units = 602,,,,,,, = six-hundred and two sex-tillion 000

10
This equality can be used as a conversion factor to convert particles into moles, or moles into particles.

11
Example: How many atoms are in a 1.22 mole sample of sodium? K: 1.22 mol Na U: ? atoms Na 1.22 mol Na 1 x 6.02x10 23 atoms Na 1 mol Na = 7.34x10 23 atoms Na K stands for what we know! U stands for what we are solving for!

12
Example: How many moles are equal to 4.79x10 24 molecules of CO? K: 4.79x10 24 molec. CO U: ? mol CO 4.79x10 24 molec. CO 1 x 6.02x10 23 molec. CO 1 mol CO. = 7.96 mol CO

Similar presentations

© 2016 SlidePlayer.com Inc.

All rights reserved.

Ads by Google