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a. Looking at the trends in first ioniaztion energies across period 3, there is a sudden unusual dip with Al and S. First ionization energy is the energy required to remove the first electron from an atom. This means that it is much easier to remove an electron from S than it is to remove one from Al, because the extra electron in the p shell of S repels the other electron, making it much easier to remove.
b. Electronegativity is the ability of an atom to attract another electron. Electronegativity increases across the groups and decreases down the periods, which makes the halogens the most electronegative group. The noble gases have an electronegativity of zero, because all of their electron shells are filled, and they don't want to attract another electron.
c. Atomic radius is the average distance to the nucleus of the atom from the edge of its surrounding electron cloud. Oxygen would have the smallest atomic radius becuse atomic adius increases down the periods, but decreases across the groups.
Great blog! You discussed everything well. The only thing I would add is in part a and part c. You talk about first Ionization energy you say that it is easier to remove but why? It is because the balance of electrons in orbitals and shell layers. In part c, you don’t mention why the atomic radius is greater or less.
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Awesome post!
ReplyDeleteThe only thing I would add would be in part B how the halogens are the most electronegative because they are the closest to becoming a noble gas, besides that great job!
Great job, Abigail. I was just wondering in part B why electronegativity increases across the groups and decreases down the periods. The reason for this is that down the groups the effective positive charge is weakened by shielding inner shells. Also, across the periods there is no added shielding from energy levels and the positive charge increases with additional protons so the element is more able to attract an electron. Other than that, fantastic job!!
ReplyDeleteGreat post, Abigail! The only thing I would add to your blog post would be a little more explanation on part B. You might want to include why the electronegativity trends occur on the periodic table. Weakening shield layers are caused by the inner shells and across periods shielding isn't added because the electrons filling in are still in the same sublevel. Also, you may want to add that the noble gases don't attract more electrons and are satisfied by a full sublevel because at that point they are in complete equilibrium and are at their most stable state. Overall, your blog posting was very thorough and clearly answered the test review questions! Good job!
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