Materials Chemistry high school buddy in class XII would have to know the main elements of what con

Materials Chemistry high school buddy in class XII would have to know the main elements of what constitutes a halogen element. Take a look back at the periodic table. Based on electron configuration, halogen occupying group VIIA in the periodic table. Halogen atoms have high electron affinity so easily accept electrons to form electron configuration of a noble gas. Therefore, the halogen elements never found in a free element in nature. Abundance of Halogen Halogen Elements commonly found in the form of salts. Therefore, the elements of group VIIA called halogen, meaning salt formers night guard (and genes halos, halos = salt; genes = formers or creators). Fluorine and chlorine are halogens elements are abundant in nature. Fluorine minerals contained in fluorapatit, 3Ca 3 (PO 4) 2. CaF 2 and the mineral fluorite, night guard CaF 2. The second form of the mineral is shown in the picture. Chlorine is abundant in the form of NaCl dissolved in the oceans as well as the salt deposits. Bromine is less abundant, there is a Br ions in seawater. Iodine contained in small amounts in seawater as NaI and NaIO 3 as nitrate salt together. Astatine element not found in nature because it is radioactive so easily transformed night guard into other more stable night guard elements. Halogen Element Properties All halogen elements are a diatom molecule, ie F 2, Cl 2, Br 2, and I 2. Gaseous fluorine and chlorine, fluorine and chlorine night guard are pale yellowish greenish yellow. Bromine is a volatile, colorless liquid and vapor-reddish brown. Iodine is a solid shiny black sublimate produces steam that can be colored purple. Halogen elements are easily recognizable from the smell and color. Halogens are generally foul-smelling, night guard especially chlorine and bromine (bromos, meaning urine). Both of these gases are toxic and should be handled carefully. If the container is leaking bromine then in a moment, the room will appear reddish-brown. Melting point, boiling point, and other physical properties are shown in the following table: increase night guard in melting point and boiling point from top to bottom in the periodic table due to London forces between halogen molecules progressively increased with increasing bond length. Style is directly proportional to the distance or bond length. Halogen reactivity can be learned from their atomic radii. From top to bottom, atomic night guard radius increases so the attractive force of the nucleus admission (affinity) electron weaker. As a result, night guard the reactivity of the halogen elements decreases from top to bottom. Halogen reactivity can also be learned from the electron affinity. The greater electron affinity, the more reactive elements. From top to bottom in the periodic table, the electron affinity of halogen elements become smaller so that its reactivity: F Cl Br I. Therefore the halogens readily accept electrons then all the halogens are strong oxidizing agents. Oxidizing strength night guard of the halogen decreases from top to bottom in the periodic table. night guard It can be seen from the standard reduction potential: According to the standard reduction potential can be concluded that F 2 is the most powerful oxidizer. Therefore, the halogens can oxidize other halogens that lies beneath the periodic table, but the return of reaction does not occur. Oxidizing strength F 2, Cl 2, Br 2, and I 2 can be seen from the reaction antarhalogen. Fluorine night guard gas can oxidize halogen elements that are underneath: F 2 (g) + 2Cl - (aq) 2F - (aq) + Cl 2 (g) F 2 (g) + 2Br - (aq) 2F - (aq) + Br 2 (g) F 2 (g) + 2l - (aq) 2F - (aq) + I 2 (s) Similarly if chlorine gas is added to a solution containing Br - ion or ions I - , will form bromine and iodine. Cl 2 (aq) + 2Br - (aq) 2 Cl - (aq) + Br 2 (aq) Cl 2 (aq) + 2I - (aq) 2 Cl - (aq) + I 2 (aq) The reaction of Cl 2 with Br - or I - can be used for identification of bromine and chlorine in an ion. Halogen can react with almost all the elements, both metallic and non-metallic elements. Similarly with other halogen compounds can form antarhalogen, such as ClF, BrF, IBr, ClF 3, ClF 5, and IF 7. In antarhalogen compound, a positive night guard oxidation state is owned by the halogen electronegativity smaller. For example, the molecule ClF 3, Cl = +3 oxidation state and oxidation state of F = -1. Halogens react with metals to form ionic compounds. night guard With non-metal elements, halogens form covalent compounds. Both ionic and covalent compounds, halogen generally have oxidation number 1. All elements can form halogen oxo acids, except fluorine. Ranging oxidation number of +1, +3, +5, and +7. Examples can be seen in the following table.
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