The Periodic Table is arranged on a grid system, with the columns being groups, and the rows being periods. The elements that are located in the same group have the same number of valence electrons. For example, the elements that are in group 18, all have 8 valence electrons. These elements are the Noble Gases, and they have similar chemical properties. This holds true for the elements in other groups; they have similar chemical properties as elements as other elements in the same group. The major different between elements in the same group, is the number of electron shells. Elements that are in the periods closer to the bottom of the periodic table have more electron shells, thus, the atom is larger. To sum it up, an atom that is in the bottom right corner of the Periodic Table will have a higher number of valence electrons and more electron shells than an element that is in the top left hand corner of the periodic table.
Atoms and Ions are fairly similar. Ions are atoms in a more stable state because they have either gained electrons to make their valence electron count 8, or have lost electrons to bring their valence electron count to 0. This transfer of electrons happens when 2 elements exchange valence electrons such that they will have opposite charges, and will bond together. A Magnesium ion is still Magnesium, it is just Magnesium that has been oxidized. You can predict the charge of an ion based on how many valence electrons it has. If an atom has 3 valence electrons, then its ion will have a charge of +3, because it is going to lose those three valence electrons. One can determine whether the charge of the ion will be positive of negative. Metals will lose their valence electrons, making their charge positive, and nonmetals will gain electrons, making their charge negative; with the exception of the noble gases, which cannot react with anything.
Friday, October 28, 2011
Thursday, October 20, 2011
Lab 2.1 Grouping of Elements
1. The two groups that I created at the end of the lab were metals and non metals.
2. Electrical conductivity is a chemical property because it is related to the subatomic particles (electrons) and how they react with one another. Malleability and appearance are physical properties because they are only how the elements look/appear. The way that the elements look, and the chemical make up of them are unrelated. Chemical reactivity is a chemical property. The name is very self explanatory; this determines if and how the elements reacted with the acid, based on their chemical make-up.
3. Elements that are metalloids are unique because they do not have only the properties of either side. They could exhibit come of the properties of a metal, and at the same time exhibit some properties of a non-metal.
3b. Silicon (Si) is a metalloid.
3c. The 7 metalloids are: Silicon (Si), Boron (B), Germanium (Ge), Arsenic (As), Antimony (Sb), & Tellurium (Te).
4. As you look from left to right on the Periodic Table, you see that the elements listed become less metal-like, that is, with the exception of hydrogen (i.e. Metals, Metalloids, Non-Metals, and finally, the Noble Gases). It seems to be that the elements with more valence electrons are less metal-like, and the elements with less valence electrons are more metal-like, or are metals.
4b. There is a less noticeable trend that appears when looking from the top of the Periodic Table to the bottom. Although the metalic characteristics of elements seem to show a trend from left to right, the Table also shows that, of the first 112 elements, there are more and more metals per row as the period number increases. This shows that elements with more electron shells with exhibit more metalic properties than an element with fewer electron shells.
Enrichment. Gold (Au), number 79 on the Periodic Table, is derived from the Latin word "Aurum" which is a direct translation to the English word "gold". (Bentor, Yinon. Chemical Element.com - Gold. Oct. 20, 2011 http://www.chemicalelements.com/elements/au.html.)
2. Electrical conductivity is a chemical property because it is related to the subatomic particles (electrons) and how they react with one another. Malleability and appearance are physical properties because they are only how the elements look/appear. The way that the elements look, and the chemical make up of them are unrelated. Chemical reactivity is a chemical property. The name is very self explanatory; this determines if and how the elements reacted with the acid, based on their chemical make-up.
3. Elements that are metalloids are unique because they do not have only the properties of either side. They could exhibit come of the properties of a metal, and at the same time exhibit some properties of a non-metal.
3b. Silicon (Si) is a metalloid.
3c. The 7 metalloids are: Silicon (Si), Boron (B), Germanium (Ge), Arsenic (As), Antimony (Sb), & Tellurium (Te).
4. As you look from left to right on the Periodic Table, you see that the elements listed become less metal-like, that is, with the exception of hydrogen (i.e. Metals, Metalloids, Non-Metals, and finally, the Noble Gases). It seems to be that the elements with more valence electrons are less metal-like, and the elements with less valence electrons are more metal-like, or are metals.
4b. There is a less noticeable trend that appears when looking from the top of the Periodic Table to the bottom. Although the metalic characteristics of elements seem to show a trend from left to right, the Table also shows that, of the first 112 elements, there are more and more metals per row as the period number increases. This shows that elements with more electron shells with exhibit more metalic properties than an element with fewer electron shells.
Enrichment. Gold (Au), number 79 on the Periodic Table, is derived from the Latin word "Aurum" which is a direct translation to the English word "gold". (Bentor, Yinon. Chemical Element.com - Gold. Oct. 20, 2011 http://www.chemicalelements.com/elements/au.html.)
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