Periodic Trends

We spent the last week before our unit test reviewing periodic trends, and putting them to practice with a few activities. The first trend is atomic size, where atoms get larger because you move down a group, and also get bigger as you move from right to left, leaving the largest atoms in the bottom left corner. The next trend is ionization energy, which is the energy needed to remove an electron from a gaseous state atom, and it results in forming a cation. This trend is at its greatest in the top right. The third trend regarding only the s and p blocks, along with the two previous trends is electron affinity, which is the ease with which an electron may be added to an atom, creating an anion, otherwise, the energy given off when an electron joins an atom, and this gives off negative energy. This trend is also at its greatest in the top right. The final trend we learned about in our supplement is electronegativity, which is the tendency of an atom to draw electrons toward itself when chemically combined with another element, and this is greatest to the right and up, but does not include noble gases.
This overall demonstrates all the trends:

https://upload.wikimedia.org/wikipedia/commons/4/41/PERIODIC_TRENDS.jpg

Here is just atomic radius:

http://www.kentchemistry.com/links/PT/atomic_radii.jpg

Here are some practice links:
http://www.acschools.org/cms/lib07/PA01916405/Centricity/Domain/362/Periodic%20Trends%20Worksheet%20Answers.pdf
http://www.sfponline.org/uploads/71/periodictrendspracticesub1106.pdf

Quantum Numbers

The final lesson before our first quiz was quantum numbers. We learned that each element is assigned to four quantum numbers, being first the principal quantum number, n, which is the period number for all except d orbitals, and it labels the shell number. Second is the Angular Momentum Quantum Number, l, and this number is determined from the type of sublevel, either 0,1,2,3 for s,p,d,f. Third is the Magnetic Quantum Number, m1, which labels the orbital subtype, and corresponds with the number of orbitals in each orbital type. So, if it were an s orbital it would only be zero, with only one space for the two electrons to be  _ . If it were in the p orbital, it would have three spaces _ _ _ labeled left to right -1,0,1. This will expand each level one on each side with the two orbitals in each level. The fourth part of the Quantum number is the Spin Quantum Number, which is the direction in which the electron is facing in the last orbital. Therefore, if the electron in the figure is facing up, it is given the +1/2, and if it is facing down, it is given a -1/2.
Here are some links to help practice:
http://highered.mheducation.com/sites/0072396814/student_view0/chapter8/interactive_quiz_1.html
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.html

capthttp://www.chemistryland.com/CHM130S/10-ModernAtom/Spectra/PeriodicTableWithQuantumNumbers.jpg

Post Quiz

Since I did not do as well on the quiz as I had hoped, I found some extra links to help me practice. Many of the mistakes were misunderstanding the concept or what the question was asking for, but some others I did not properly use the conversion factors we were supposed to memorize .
Here are some of the practice links I found:
http://www.chemteam.info/Electrons/calc-energy-freq-wavelength.html

https://www.khanacademy.org/science/chemistry/electronic-structure-of-atoms/electron-configurations-jay-sal/v/electron-configurations-2#!

http://terpconnect.umd.edu/~wbreslyn/chemistry/electron-configurations/electron_configuration_worksheet.html