Chapter 2; Understanding The Periodic Table Of Elements And Electron Configurations
Chapter 2; Understanding The Periodic Table Of Elements And Electron Configurations Chemistry 101
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This 4 page Bundle was uploaded by Becca LeBoeuf on Friday February 12, 2016. The Bundle belongs to Chemistry 101 at University of Wisconsin - Oshkosh taught by George Vater Olsen in Spring 2016. Since its upload, it has received 41 views. For similar materials see General, Organic, Biological Chemistry in Chemistry at University of Wisconsin - Oshkosh.
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Date Created: 02/12/16
Chapter 2 Periodic Elements: NOT FOR EXAM 1, FOR EXAM 2! Protons : Mass: 1 amn. Charge: 1+. Neutrons : Mass: 1 amn. Charge: 0. Electrons: Mass 1/1875 amn. Charge: 1. Please refer to the periodic table of elements above: Follow these simple rules when trying to find protons, neutrons, and electrons for an element: For any element: Number of Protons = Atomic Number Number of Electrons = Number of Protons = Atomic Number Number of Neutrons = Mass Number Atomic Number Finding the number of protons (ALSO THE ATOMIC NUMBER): whatever number that is shown above the symbol, is the number of protons the element has. Example: H 1 He 2 Cr 24 Mn 25 Ar 18 Na 11 Be 4 Os 76 Ir 77 P 15 S 16 O 8 Finding the number of e lectrons: electrons are always equaled to the number of protons which are also equaled to the atomic number. Example: The element C (carbon). Protons: 6 Electrons: 6 Neutrons: 8 ELECTRONS CAN CHANGE IF GIVEN A NEGATIVE CHARGE! Example: The element given is C^3 Protons: 6 Electrons: 9 Neutrons: 8 So basically, when you are given a negative charge such as C^3....you add another 3 electrons onto the number of electrons you would normally if the 3 was not given! Finding the number of neutrons: to find the number of neutrons, take the number of protons and subtract it from the atomic mass..that will give you the number of neutrons and element has. Example: The element Kr (krypton). Kr has 36 protons (also called atomic number). Kr has an atomic mass of 83.798. You can round this number up to 84 Write an equation: Mass # = (# of protons) + (# of neutrons) 84 = 36 + (# of neutrons) 8436 = 48 Now, try a few out for yourself! I would definitely suggest printing off a period table! Please refer to the periodic table of elements above: First two columns: S orbitals. Six columns on the right: P orbitals. Middle rows: D orbitals. Bottom rows: F orbitals. We will not be tested on the f orbital block, so just ignore those. Example: He = 1S^2. This is because it is in the 1st row, S orbital, & is the 2nd element in that row. H = 1S^1 or 1S. This is because it is in the 1st row, S orbital, & is the 1st element in that row. As you go farther down the periodic table, they get much more complicated. Example: Li = 1S^2 2S Be = 1S^2 2S^2 B = 1S^2 2S^2 2P^1 And then even more complicated.. Example: Na = [Ne] 3S^1 → this is basically saying that Sodium (Na) is equaled to all of the configurations of Ne (1S^2 2S^2 2P^2) AND 3S^1 (which is the one more step (configuration) to get to Na). Cr = [Ar] 4S^2 3D^4 → this is basically saying that Chromium (Cr) is equaled to all of the configurations of Ar (1S^2 2S^2 2P^6 3S^2 3P^6 ) AND 4S^2 3D^4 (which is the two more steps (configurations) to get to Cr). PRACTICE PRACTICE PRACTICE! The more you study where the orbitals are and what configuration each element acquire, the more you will understand this. It is very confusing at first!
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