section on the periodic table composed of 8 groups including metals metalloids and nonmetals?????
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Here are the 'answers', in order you asked.\n\nfamily\nmetalloids\ngroup\ntransition elements\n\nGet an "A".
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Periodic table was invented by Mendeleev, a Russian while playing piano. Music has 7 notes, hence the periodic table consists of 7 families, ignoring the mid section, which no one has been able to figure out where to be placed, so is the case with many other elements invented. \n\nBase your project on a musical scale of 7
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I actually asked an inorganic chemist the very same question, and this is what he told me:\nI seperated out the section that I thought was the best reason he gave, and I think it's important to read the last paragraph.  His other reasoning seems good, too.  I'm not trying to say it doesn't make sense.  I just think the part I seperate is probably what they had in mind when designating the groups.\n\n When you say they are put into the same "group" I assume you mean the group B numbering within the transition metals columns, which would make the Fe, Co and Ni triads all part of group VIIIB.  Now with the main group, also termed group A, the significance of the roman numeral to signify the standard oxidation state of the element is obvious.  The oxidation states get more complex in the transition metal series and frequently multiple oxidation states are observed.  The Cu triad (Cu, Ag, Au) is termed IB due to stable +1 states that are common especially silver which is only found as elemental or +1, where copper may alos be found as a +2 and Au may be found as +3.  The Zn triad (Zn, Cd, Hg) are exclusively +2 and are thus labled IIB group.  You then skip back to the begining of the transition metals and number across due to stable +3 and +4 for Sc triad and Ti triad respectively.  There are a few reasons why in the classical B grouping Fe, Co, and Ni are lumped into a "group" in the middle of the transition metal series.  First as you go across the transition metals the +2 state is becomeing continuously more stable and prevalent.  For Fe there are several oxidations states that are common, however +2 and +3 are most stable and common.  When you move over to Co the +2 becomes the dominant oxidation state with +3 also commmon and very rare examples of higher oxidation states.  When you move over to Ni it is almost exclusively +2 or +3 with rare exceptions.  The second point that I would consider in grouping them together would be their adherence to the 18 elecron rule.  These elements in the middle of the transition metall series follow the rule almost always where earlier elements frequently violate the rule with lower electron counts or even odd number counts and the later elemnts are frequently content with 16 or even 14 electron counts, the later condition is common for group IIB.  \n\n\nAnother consideration to give this group the lable VIIIB is the d8 configuration that is common (Fe(0), Co(I), and Ni(II)) are all d8 systems and frequently analogous compounds can be made with the different metals.  \n\nI hope this shed some light on your question.  I also should note that the system that groups these elements together is an older group numbering system and the new and current grouping system avoids the grouping by groups A and B and simply numbers across the table from 1 to 18, with groups 3-12 being the transition metals.
428791
gold is and element, silver, copper, water is hydrogen and oxygen, everything is made of elements!  If your just having trouble finding the periodic table, try spelling it p-e-r-i-o-d-i-c.
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This is an answer I gave a few weeks ago. It helped me to get from failing Chemistry to University....maybe it will help you to understand the periodic table as well.\n\nMy Chemistry teacher taught me a great story which helped me learn the elements, which groups they were in, which periods, how many electrons they had etc and resulted in me going from a grade F to B. Every kid should learn this.\n\nHorrible Hairy Little Begger Boys Catch Newts On Friday Near Naples, Magnificent Albert Sits Planning Some Clever Arrangement Keeping Calm.\n\nOk, looks crazy until you break it down;\n\nH He Li Be B C N O F Ne Na, Mg Al Si P S CL Ar K Ca\n\nThen put it into the table\n\nH\nHe\nLi Be B C N O F Ne\nNa Mg Al Si P S Cl Ar \nK Ca\n\nYou will need to line them up because Yahoo has left align, but the trick is the story. \n\nThe groups 1-8 (across the table) tell you how many electrons are in the outer shell, the periods (down the table) tell you how many shells an element has. etc\n\neg Sodium (Na+, group 1) bonds with Chlorine (Cl- , group 7) because Chlorine has 7 electrons in its outer shell. It needs the one from sodium to become stable.....NaCl (kitchen salt). This is the basis for other compund formation....ie water H2O and so on.\n\nLearn the story above and everything will fall into place.\n\nHope this helps!
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This is an answer I gave a few weeks ago. It helped me to get from failing Chemistry to University....maybe it will help you to understand the periodic table as well.\n\nMy Chemistry teacher taught me a great story which helped me learn the elements, which groups they were in, which periods, how many electrons they had etc and resulted in me going from a grade F to B. Every kid should learn this.\n\nHorrible Hairy Little Begger Boys Catch Newts On Friday Near Naples, Magnificent Albert Sits Planning Some Clever Arrangement Keeping Calm.\n\nOk, looks crazy until you break it down;\n\nH He Li Be B C N O F Ne Na, Mg Al Si P S CL Ar K Ca\n\nThen put it into the table\n\nH\nHe\nLi Be B C N O F Ne\nNa Mg Al Si P S Cl Ar \nK Ca\n\nYou will need to line them up because Yahoo has left align, but the trick is the story. \n\nThe groups 1-8 tell you how many electrons are in the outer shell, the periods tell you how many shells etc\n\nHope this helps!
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OVERSIMPLIFIED ANSWER\n\nActually, the periodic table was a stunning predictor of properties of elements. When it was first formulated, many of the elements we know of today had not been discovered, and so it contained many blank spots. Interestingly enough, it turns out that the groupings predicted properties of elements in groups. For instance, you could be reasonably certain that if 12 new halogens are found in the future, they will all have similar properties to the halogens that are grouped together today.\n\nHow do we know this? How were the elements grouped by properties before we knew what those properties were? Simply put, the periodic table is organized like this\n\nRight to left: number of electrons in the outermost orbital\n\nTop to bottom: atomic weight\n\nThis is oversimplified, but it works here. Electron configuration in the outer orbital is what determines an element's reactivity, the bulk of its chemical properties. Since there are 8 rows from left to right in the table, elements read from top to bottom all have the same number of electrons in their outer orbitals, so they all have similar properties.\n\nWhat's important to remember is that much of the periodic table was organized in its modern state BEFORE we knew this. Pretty nifty.
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the periodic table is great because it ditinguishes the different shells (s, p, d and f) that are filled as you add electrons. eg. He has 2 s electrons (full shell)\nNe has 1s2, 2s2 and 2p6 (full shell).\nIt gets a little more complicated at d electrons (transition metals) but Mendeleev did a great first shot.
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Check ur previous question's answer given by me.The site given in it contains all ur answer based on the Periodic Table of the elements.If U want the site in this answer too,then here it is:-\nhttp://mtsu32.mtsu.edu:11233/111-ch3.html
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Together with the metals and nonmetals, the metalloids (in Greek metallon = metal and eidos = sort - also called semimetals) form one of the three categories of chemical elements as classified by ionization and bonding properties. They have properties intermediate between those of metals and nonmetals. There is no unique way of distinguishing a metalloid from a true metal but the most common is that metalloids are usually semiconductors rather than conductors.\n\nThe known metalloids (and their atomic symbols) are:\n\nBoron (B) \nSilicon (Si) \nGermanium (Ge) \nArsenic (As) \nAntimony (Sb) \nTellurium (Te) \nPolonium (Po) \nAstatine (At) \nIn the periodic table, metalloids occur along the diagonal line from boron to polonium. Elements to the upper right of this line are nonmetals; elements to the lower left are metals.\n\nSemi-metallic behaviour is not confined to the elements, but is also found in alloys and compounds. Mercury (II) telluride is one example.\n\nOne definition of semi-metallic behavior would be if the conduction band and valence band overlap. This is also true of metals, so semi-metals must additionally have a relatively low carrier density.
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Investigate the origins of the periodic table.
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metal: simple element at room temp. except galium, mercury and cesium\n\nnonmetal: simple elemnent at the three states of matter
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mercury\n\nmercury is a liquid metal\nand its composed of potassium, sodium, oxygen, argon, helium, nitrogen, Carbon dioxide, water, and hydrogen
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http://www.schoolscience.co.uk/periodictable.html\nhttp://www.webelements.com/
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Nobody knows the answer to this exept for Mendeleev himself, and he isn't talking. The first periodic table had 64 elements, although 3 or 4 of those were still purely theoretical. Since there were more than 50 in the first periodic table, you can't really discuss the first 50 added very well. Several models of organization were proposed, but there were around 60 known elements before it was deemed necessary to organize them. Only Mendeleev's used periodicity, and it is the closest to our modern periodic table.\n\nThe only 2 elements in my periodic table are:\n\nWOMANIUM (XX)\nPhysical properties: Generally soft and round in form. Boils at nothing and may freeze any time. Very bitter if not used well.\nChemical properties: Very active and highly unstable. Possesses strong affinity with gold, silver, platinum, and precious stones. Violent when left alone. Turns slightly green when placed next to a better specimen.\nUsage: An extremely good catalyst for dispersion of wealth.\nCaution: Highly explosive in inexperienced hands!\n\nMANIUM (XY)\nPhysical properties: Solid at room temperature but gets bent out of shape easily. Difficult to find a pure sample. Due to rust, aging samples are unable to conduct electricity as easily as young samples.\nChemical properties: Attempts to bond with XX any chance it can get. Also tends to form strong bonds with itself. Becomes explosive when mixed with Childrium for prolonged period of time.\nUsage: Possibly good methane source.\nCaution: In the absence of XX, this element rapidly decomposes and begins to smell.
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oxygen, nitrogen, every fuckin mineral and more on the periodic table...take chemistry
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the periodic table. and all that stuff that has to deal with chemistry. compounds. atoms. matter.\n\n\ni am in 8th grade