Why is Fluorine the most reactive non metal?
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1) Highest electrotronegativity.In Pauling scale flourine's electronegativity is 4. Consequently F atom has a strong tendency to attract electrons from the other elements.Fluorine thus compels the other elements to combine with it.Due to its strong electronegativity & small size Fluorine has a strong tendency to accept electrons from other atoms or ions. As a result it oxidises all other substances.\n\n\n2) The bond dissociation energy of F2 is very low, due to this Fluorine easily comes to reactive atomic state. The low bond dissociation energy can be explained in the following ways\n\na] since F atom do not contain any d orbital d(pi)-p(pi) bond in F2 molecule is not possible( which is possible in other halogens). This cause was proposed by Mulliken.\n\nb] According to Coulsan, The F-F bond distance in F2 molecule is  least because of the small size of F atom.The non-bonding electrons in 2p subshell of one F atom exerts great repulsion on that of another F atom. Which causes easy bond cleavage.\n\nc] the bond existing between two F atoms is a single covalent bond. So the bond dissociation energy is minimum.\n\n3) The bond energy of Fluorine in Fluoride compound is very high & so it requires a great amount of energy to break this bond, consequently the tendency to form Fluoride compounds is much higher.
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Just in general\n\nAlkali Earth Metals- Pretty reactive they are found in many compounds\n\nBoron group- Low reactivity\n\nCarbon group- More reactive then boron group but still pretty low\n\nNitrogen group- More reactive then Carbon group\n\nOxygen group- Very reactive oxygen has an unually high affinty for electrons relative to where it is on the periodic table\n\nHalogen group- Even more reactive than oxygen th&#92;ey have very hi\naffinity for electrons\n\nNoble gases- Basically inert, they have a full outer orbital of electrons and will only react in rare cases such as with flourine
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An atom is only considered 'reactive' when it needs to lose it valence electrons (for metals) or gain electrons (for non-metals) so as to achieve stability with a full outermost electron shell.\n\nThe first atom you have, [2,8,8], it has a full outermost shell (last number is 8, meaning it has an octet). Thus it is not likely to react and gain or give away any valence electrons. Similarly for your 2nd atom, [2,8].\nThe 3rd atom has only 2 electrons in its 1 and only shell. It has a full outermost shell too (duplet, since 1st shell can only take in max 2 electrons), hence it is stable.\nThe last atom belongs to Group I, with 1 valence electron. Hence it will be very willing to give away its one valence electron to obtain a stable octet.  Thus the last atom is reactive.\nBy the way, the first 3 atoms belong to the noble gases (Group 0).
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Under ordinary conditions xenon will not react.  Under very low temperatures and very high pressure it can be forced to react with oxygen and fluorine forming xenon trioxide (XeO3) and xenon tetrafluoride (XeF4).  These compounds are extremely unstable and will decompose into their elements easily and explosively.
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Because most metals are susceptible to oxidation, having low electronegativities, prefering to be in a cationic form vs. the neutral element.  Only metals such as gold, which is resistant to oxidation, will be found pure in nature.
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Zirconium is a metal (transitional metal, to be precise).\nChlorine is a non-metal (halogen).\nGold is a metal (also a transitional metal).\nUnunnilium (now called darmstadtium) is a metal (transitional metal, too.).
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only Sodium Chloride is not.\n\nsimple answer:\ncovalent bonds are between non-metals\nionic bonds are between a metal and a non-metal\n\nthis is because of the large difference in electronegativity between metals and non-metals.\n\nonly sodium chloride has a metal.  the rest are all made only of non-metals and thus covalently bonded.
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After looking over the literature I have available, I can't come up with one.  None of the noble gases would, and other gases such as nitrogen are nonreactive as well.  That's why they state to run certain reactions in a nitrogen atmosphere.\n\nNoble gases are able to react with some materials, but they often contain halogens, which are highly reactive.  Check out the links to see some compounds of xenon and krypton.
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According to a book I read some time back, "Mellor's Modern Inorganic Chemistry," fluorine is stored in copper lined cylinders.  The F reacts with the Cu, forming a layer of CuF2, which prevents further attack.  Here's a good document on everything you ever wanted to know about handling fluorine:\nhttp://www.llnl.gov/es_and_h/hsm/doc_14.06/doc14-06.html\nI couldn't find anything on cost.
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Typically the metals and hydrogen. Non-metals usually give negative ions.
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Ignoring the inert gases, the highest electronegativity is at the top right corner (fluorine), and the lowest is at the bottom left (francium)
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The Halogens are very, very reactive chemicals, and tend to hook up and form salts with the other elements rather than hanging around in a pure elemental form.  They tend to pick up extra charge very well which makes them prime candidates for bonding.
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Iodine is the least likely to form an iodide anion because it is the lest electronegative of the halogens. \n \nTHe halogens tend to want to draw and electron towards their neucleus.  Fluorine has the highest electronegativity.  It has a small electron cloud, so the outer most electrons are close to the nucleus and are more strongly pulled there.  Iodine has a large electron cloud.  The outer most electrons of iodine are much further away from the neuleus, so it can't pull electrons in as close.\n\nHope that helps.\n\nPS.  F, Cl, Br, and I all are diatomic, so they all form F2, Cl2, Br2, and I2.
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The nonmetals are halogens, noble gases and the following elements in order of atomic number (nonmetals as chemical series):\n\nhydrogen (H) \ncarbon (C) \nnitrogen (N) \noxygen (O) \nphosphorus (P) \nsulfur (S) \nselenium (Se) \n\nhere's an example:\n\nhttp://en.wikipedia.org/wiki/Periodic_table_%28metals_and_non-metals%29
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Bromine is the only non-metal that is a liquid at room temperature and is a highly volatile and unstable compound.  The reason for this is due to the fact that it has 7 valence electrons, 1 away from being a stable noble gas.  Therefore, bromine is highly reactive in order to obtain the extra electron it needs to be happy.  \n\nPlus it smells terrible.  Another reason why it must be unstable.
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chlorine is more electronegative. it is in the '2nd column from right in the periodic table' it is a halogen. the halogen group contains chlorine, flourine, bromine, iodine etc. They are the most electronegative elements of all. nitrogen is placed to the left of chlorine & hence is less negative than Cl. With respect to, say carbon, nitrogen is electronegative [as in CN - cynide] while, in compounds like NO/NO2/ N2O4/ NO3 etc. Nitrogen is electropositive [as compared with oxygen].\n\nu can IM me at YahooMessenger [my ID is fizanaqsh] or email me at my email address which is  fizanaqsh@yahoo.co.in  or even chat via Skype where my ID is homewornetguru, in case u got any more difficulties with chemistry/english/math or physics etc.
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Francium, metals are located to the left of the staircase and as you move further left and down, the element more easily loses electrons giving it higher reactivity.