In today's lesson, we learned about masses of subatomic particles. First, we learned the labels of an element in a periodic table because that is what we use to determine a lot of things in this unit. (see picture below). The letters in the middle are the Element symbol, the name below is the element name, the number at the top is the atomic number (the number of protons and electrons), and the number at the bottom (usually a decimal) is the average atomic mass. Then we leaned the notation for recording different isotopes of an element. Which is done by using the element symbol and two numbers on the right (see picture below). The number on the top is the mass number and the number on the bottom is the atomic number (number of protons/electrons). The number of neutrons can be determined by subtracting the atomic mass by the number of protons. Then, we learned about calculating average masses and percent abundances of isotopes. The formula for calculating average atomic mass is (mass of one isotope)*(% abundance)+(mass of other isotope)*(%isotope). This same formula can be used to figure percent abundances when average mass and isotope masses are known.
Element on periodic table labels
Isotope notation
Extra resources:
calculating practice:
http://www.chemteam.info/Mole/AverageAtomicWeight.html
http://blog.wsd.net/hewaite/2014/10/
http://ehschemcorner.blogspot.com/2012/09/the-atom-isotopic-notation.html
As a visual learner, your picture help me greatly in knowing where and what is found on an element. On our quiz i struggled with which numbers represented protons/electrons/neutrons. If I had looked here I may have been more prepared. I will use this for future reference.
ReplyDeleteAs a visual learner, your picture help me greatly in knowing where and what is found on an element. On our quiz i struggled with which numbers represented protons/electrons/neutrons. If I had looked here I may have been more prepared. I will use this for future reference.
ReplyDelete