March 14th
Today we covered isotopes. We discussed how average atomic masses are determined for the periodic table based on the relative abundance of the elements isotopes.
Definitions to know from today:
Isotope: Atoms of the same element (same number of protons) with different number of neutrons.
Atomic Mass Unit:the unit that elements' weights are measured in. 1 amu is equal to the weight of a proton or neutron.
Atomic Mass: The weight of a particular atom. (equal to number of neutrons+the number of protons)
Average Atomic Mass: is the relative average atomic mass based on the abundance of particular isotopes of a certain element
To complete this outcome you must understand and be able to demonstrate your ability to do the following:
1. be able to calculate the average atomic mass of an element when given the relative abundance of the isotopes of an element
2. be able to differentiate between average atomic mass and atomic mass
3. Understand that different isotopes exist naturally in nature at specific ratios and that different isotopes can behave differently.
I hope you remember the penny activity we did to understand how average atomic mass is related to the percent abundance of each isotope. information on the penny from: http://en.wikipedia.org/wiki/Penny_(Canadian_coin)
The activities you can do to demonstrate your understanding are the following: (choose at least 2 and do a portfolio write up on 1)
1) Design an activity like the penny one to explain relative abundance using real life objects
2) Do the worksheet
3) Create a how to manual on how to determine the average atomic mass
4) Research on an element and create a presentation poster or explanation on its isotopes and the average atomic mass
5) Create 3 questions you may see on a test and provide a detailed answer sheet
If you want more information on this check out these sites:
http://www.chem4kids.com/files/atom_isotopes.html -simple explanation
http://digipac.ca/chemical/molemass/isotopes.htm -more detailed information
http://www.chem.ualberta.ca/~massspec/atomic_mass_abund.pdf -relative abundance of elements
Definitions to know from today:
Isotope: Atoms of the same element (same number of protons) with different number of neutrons.
Atomic Mass Unit:the unit that elements' weights are measured in. 1 amu is equal to the weight of a proton or neutron.
Atomic Mass: The weight of a particular atom. (equal to number of neutrons+the number of protons)
Average Atomic Mass: is the relative average atomic mass based on the abundance of particular isotopes of a certain element
To complete this outcome you must understand and be able to demonstrate your ability to do the following:
1. be able to calculate the average atomic mass of an element when given the relative abundance of the isotopes of an element
2. be able to differentiate between average atomic mass and atomic mass
3. Understand that different isotopes exist naturally in nature at specific ratios and that different isotopes can behave differently.
I hope you remember the penny activity we did to understand how average atomic mass is related to the percent abundance of each isotope. information on the penny from: http://en.wikipedia.org/wiki/Penny_(Canadian_coin)
The activities you can do to demonstrate your understanding are the following: (choose at least 2 and do a portfolio write up on 1)
1) Design an activity like the penny one to explain relative abundance using real life objects
2) Do the worksheet
3) Create a how to manual on how to determine the average atomic mass
4) Research on an element and create a presentation poster or explanation on its isotopes and the average atomic mass
5) Create 3 questions you may see on a test and provide a detailed answer sheet
If you want more information on this check out these sites:
http://www.chem4kids.com/files/atom_isotopes.html -simple explanation
http://digipac.ca/chemical/molemass/isotopes.htm -more detailed information
http://www.chem.ualberta.ca/~massspec/atomic_mass_abund.pdf -relative abundance of elements