Handouts showing the periodic table or a large periodic table wall chartĬlassroom computer projector to show video clips demonstrating chemical reactivity A second set of videos focused on reactivity will encourage students to use their observations to identify trends and predict behavior in reactivity among metals and nonmetals. HOF has been prepared from ice + F 2 but is very reactive, decomposing to HF + O 2.Purpose: After watching a video that introduces them to the periodic table, students will answer questions that prompt them to identify general patterns in the table. In the highest oxidation state (+7) the relative oxidizing ability is: Br> I > Cl and results in the formation of the corresponding +5 oxoanions,ĬlO 4 - + 2e - = ClO 3 - E° = 1.20 V BrO 4 - + 2e - = BrO 3 - E° = 1.85 V IO 4 - + 2e - = IO 3 - E° = 1.63 V The hypohalite ions disproportionate according to the equation:ĢXO - = 2X - + XO 3 - The equilibrium constants are 10 27 for ClO -/Cl - :(the reaction is slow at room temperature), 10 15 for BrO -/Br -, and 10 20for IO -/I. They exhibit an alternation in their oxidizing abilities, and the perbromates are particularly strong oxidizing agents.ġ0. The perhalates, EO 4 -, are only known for Cl, Br, and I. Iodine forms a particularly wide range of oxides.ĩ. Oxygen fluorides are extremely strong and reactive oxidants and have been explored as potential rocket fuels the oxides become less reactive down the column and more numerous. The most extensive series of compounds exists for iodine, e.g., IF 7, IF 5, ICl 4 -, ICl 2 -.Fluorine does not form any interhalogen compounds where it occupies the central position within the molecule.Ĩ. ICl and IBr are widely used in organic synthesis and are commercially available. Neutral, anionic, and cationic interhalogen compounds are known. The halogens form many interhalogen compounds with the less electronegative halogen surrounded by the more electronegative halogens. Only H-F forms strong hydrogen bonds and this is reflected in the boiling and melting points of the hydrogen halides.ħ. The stabilities of the hydrogen halides decrease down the group, but their acid strengths increase.Ħ. The oxidizing ability of the halogens decreases markedly down the group: F 2 > Cl 2 > Br 2 > I 2, and only iodine is oxidized by nitric acid.ĥ. The mean bond enthalpies for E-X bonds are particularly large for fluorine and therefore a wide range of molecular fluorides are known fluorine is particularly effective at bringing out the highest valencies of the non-metals and highest oxidation states of the metals.Ĥ. The atoms also form strong covalent bonds with other non-metals. The cation Br 2 + is known in Br 2 +Sb 3F 16 -, and Br 5 + has been reported.ģ. Iodine has the greatest tendency to form cationic species, e.g., I 2 +, I 5 +, because it has the lowest ionization energy. The ionic compounds MX become progressively less ionic as the relative atomic mass of X increases, because of the decreasing electronegativity of the halogens. They form anionic compounds based on X - (X = halogen), which is associated with a complete octet. The elements are typical non-metals in their physical and chemical properties. All elements are diatomic and molecular and the boiling and melting points increase as a result of the increasing van der Waals interactions between diatomic molecules for the heavier elements.Ģ.
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