Periodic table Review

Metals, nonmetals, and metalloids, oh my! Categorize the following elements as metals, nonmetals, or metalloids by clicking on the element and selecting from the drop down menu. Metals Pd Be Ta Ca Bi Sn Ga Al Nonmetals F N O C P S Cl Br Metalloids Si Ge As Sb Te B When you're here, you're family... because you have the same valence electrons as me! Categorize the following elements by the periodic table family they belong to by clicking on the element and selecting from the drop down menu. Alkali Metals Li K Cs Alkaline Earth Metals Mg Sr Ba Transition Metals Mn Mo Hg Halogens F Br At Noble Gases He Kr Xe I don't always know my Periodic Table trends, but I know them periodically. Categorize the statements as Increases, Decreases, or Stays the Same by clicking and selecting from the drop down menu. Increases EN across a period with increasing atomic number Atomic radius as you do down a group IE considered in group with decreasing atomic number Decreases Atomic radius in a period considered with increasing atomic number Metallic character in a period considered with increasing atomic number EN within a group in order of increasing atomic number Stays the Same The number of valence electrons as you proceed up a group The number of PELs as you proceed from left to right across a period Atomic structure is EXTREMELY important when explaining why trends occur. Please fill in the blanks with the word that makes the sentences true by clicking on the blank selecting from the drop down menu. Good Luck! When considering any group from top to bottom, it is important to recognize the atomic structural differences between those elements. As you proceed down a group, the total number of Principle Energy Levels (PELs) increases by 1 with each element. This means that the distance from the nucleus to the valence electrons (atomic radius) increases as you proceed down a group. Additionally, the total number of shielding electrons increases. The number of protons or the nuclear charge does increase as you proceed down a group, BUT this is overshadowed by the effect the additional PEL has on the structure. Now, because of the observed changes to structure within any group, it's important to recognize the change in the attraction from the nucleus to the valence electrons. The attraction between the nucleus and valence electrons decreases within a group as you proceed down the group. Because of this, atomic radius increases. Electronegativity and first ionization energy both decrease you you proceed down a group.When considering a period from left to right, the number of PELs stays the same, but the nuclear charge increases because you have more protons in the nucleus. Since PELs stay the same, there is also no change in the number of shielding electrons. So the focus on atomic structure within a period is all about the protons. Because of the increase in protons, the attractions from the nucleus to the valence electrons increases as you proceed from left to right across a period. Because of this, the atomic radius actually decreases as the electrons are pulled closer to the nucleus due to the increased attraction. The ability of the atom to attract electrons (electronegativity) increases proceeding left to right across a period. This makes sense as more protons causing an increase in attraction would also increase the atom's ability to attract more electrons. Since the attraction between the nucleus and valence electrons increases left to right, it also makes sense that the ionization energy would increase as well since it would take more energy to remove an electron that is more attracted to the nucleus.