How Small is an Atom? Ted Ed
Using Moles and Avogadro's number as a conversion factor
Moles as a conversion factor: How do we get from grams to number of atoms?
Overview
This module has two parts:
1- Introduction to the concept of a "mole" and Avogadro's number.
2- Application of the Mole (Avogadro's number) as a conversion factor relating mass in grams to number of atoms or molecules (formula unit for ionic compounds)
Introduction to the MOLE (chemist's dozen)
How do we count atoms? Since atoms are so small, we can't! We'd literally die first before we could count them all. Check out the Ted Ed video, How Small is an Atom? for a taste of the relative size of these tiny particles.
So, how about using mass in grams instead? We can easily weigh things, and since every pure element or compound has its own mass based on the number of protons and neutrons, we can convert from grams to atoms or molecules.
We use the MOLE, which is 6.022 x 1023 of anything. The Ted Ed video on What's a Mole? Is a great place to start.
Using Avogadro's number as a conversion factor
Now that you understand what moles represent and why it's useful to scale to that unit, let's explore the application of this new conversion factor.
In the video, we demonstrate converting atoms to moles to grams and grams to moles to atoms. If you need a refresher on Dimensional Analysis and Unit Conversions, skip over to the module on Unit Conversions. All our same rules apply.
Video also includes molar mass of compounds.