Periodic Properties Essay Example for Free

Periodic Properties EssayThe halogens F, Cl, Br and I (At has not been included because of its scarcity and nuclear instability) are very reactive non-metals that occur in the penultimate grouping of the periodic table, hence they all require just one electron to empty their valence shell.All of the segments exists as diatomic molecules (F2, Cl2, Br2, I2) in which the atoms are joined by single covalent bonds. handout great deal a group of the periodic table, for successive elements there are more slide fastener levels filled with electrons, so the outer electors are in higher energy levels and farther from the nucleus. Fluorine and centilitre are gases, bromine a liquid and one a hale that forms a purple vaporization on heating. The halogens are all quite electronegative elements. They require just one electron to exhaust their valence shell, hence they readily gain electrons to form the singly charged halide ions (F,Cl,Br,I). The ease with which they gain electrons gained is further from the nucleus and hence less strongly attracted. This means that, in contrast to the alkali metals, the reactivity of the halogens decreases red ink down the group.Method1) Test the solubility of Iodine1. A very small amount of tincture of one was put into body of pee, cyclohexane and KI(aq) respectively2. The colourise swaps of the solutions and the solubility in all(prenominal) solvent were recorded2) Test iodine reacts with starch1. Three drops of I2-KI solution were put into a test tube2. A few drops of starch solution were added after that3. The colouring material of solution was recorded3) Test the acid-base properties1. A few drops of chlorine pissing were put in a test surface, and it was tested with habitual power paper2. This was repeated beginning base apply water and then using iodine solution instead of the chlorine water3. The colorize changes were recorded4) Displacements surrounded by halogen elements1. 2cm reconditeness of each( prenominal) aqueous solution sodium chloride, green bromide and potassium iodide were put into 3 respective test tubes and labeled2. An equal volume of chlorine water was added into each test tube and the results were recorded3. A little hexane was added to form a separate upper degree of a non-polar solvent4. The mixtures were shook and the changes were recorded5. Step 1, 2, 3 and 4 were repeated first using water and then iodine solution instead of chlorine water5) Tests for halide ions Halide ions (Cl-, Br- and I-) with fluid ions1. About 1cm depth of aqueous sodium chloride was put into a test tube2. A little aqueous silver nitrate was added and then the observations were recorded3. The test tube was placed in a sunny place, and left(p) there for about 5 minutes and then it was take ind again4. Step 1, 2 and 3 were repeated using aqueous potassium bromide, then aqueous potassium iodide instead of sodium chloride? info Collection?1) The solubility of iodine in different solv entColorSolubilityWater paleInsolubleCyclohexane purpurateSolubleEthanolYellowSolubleKI(aq)Yellow-brownSoluble2) Test iodine reacts with starchThe color of the solution is black.3) Test the acid-base propertiesCl2Br2I2-KIpH value43124) Displacements between halogen elementsThe color change of the solution after Cl2, Br2, I2 added into NaCl, KBr and KI respectivelyCl2Br2I2NaClNo changeNo changeBrownKBr lookout man colour solutionNo changeBrownKIyellowyellowBrownThe color of the upper beds of the solution after hexane addedCl2Br2I2NaClNo changeNo changePurple redKBrPale purpleNo changePurple redKIpurplePale purplePurple red5) Tests for halide ionsHalide ions (Cl-, Br- and I-) with silver ionsNaClWhite precipitate is producedDarkens after it was placed in cheerKBrCream precipitate is produced.KIYellow precipitate is produced.?Data Analysis?1) The solubility of iodine in different solventsThe solubility is larger in non-polar solvent (water, ethanol) and smaller in polar solvents.(cyl ohexane and KI) The purple color of iodine in cyclohexane is that because in non-polar solvents, iodine froms the violet solution.2) Test iodine reacts with starchAccording to the cosmopolitan knowledge we knew, the phenomenon of this reaction should be blue, but the color observed was black-green. That was because whatever of the starch hydrolysis in water and produced something could make the color darker.3) Test the acid-base properties1. Cl2The color of the universal indicator papers showed that Cl2 is strong acid.2. Br2The color of the universal indicator papers showed that Br2 is a kind of acid, but not very strong.3. I2The color of the universal indicator papers showed that I2 is a strong base. Actually, I2 is acid. The reason is that the original color of I2 is red-brown, that made us cant give ear the phenomenon clearly.4) Displacements between halogen elementsAs what I mentioned above in background, the rule of advisements between halogen elements is that more reactive ones displace less reactive ones.Thats the reason why Br -cant displace Cl -, and I -cant displace Br and Cl-. When there was no reaction between deuce elements, the color we observed was the blend of original colours of the less reactive element and the solution containing the more reactive element. If theres a reaction between two elements, the color we can observe is the color of the displaced element.According to the information we got from Internet, we knew hexane is a kind of oil and is insoluble in water-solvent. That was the reason why we could differentiate the two layers of each solution very clearly.The colors of each solutions infra layer were the original colors of the saline solutions. There were two kinds of instances of the color of upper layer of each solution. For the solutions those do not have I ion, they were colorless. Thats because hexane is colorless and cannot react with Cl or Br -. Another instance is that the solutions include I -, when I meets hexa ne, it lead show the color of itself. That was why we could observe color of purple in this experiment.5) Test for halide ionsWhen halide ions dissolved into silver salts, then the precipitate is appear commonly.The albumin precipitate is AgCl AgNO3+NaClAgCl+NaNO3The off-white precipitate is AgBr AgNO3+KBrAgBr+NaNO3The pale yellow precipitate is AgI AgNO3+NaIAgI+NaNO3After 10 minutes under the sunshine, photodissociation happened on all of them, so the black precipitate on the bottoms of three test tubes are the products of photodissociation.1. Going down the group, the elements of this group have the same effective nuclear charge. Atomic radius of these elements becomes bigger because of the enlarge of the number of energy levels. The attraction between nucleus and valence electrons gets weaker. Less energy is required to prohibit the first electron from one mole of gaseous atoms. The ionization energy exit down the group decreases. The ability to attract electrons becomes wea ker. The electronegativity going down the group decreases.2. Organic solvents always contain the element carbon. Inorganic solvents dont contain the element carbon. The most common solvent, water, is an example of an inorganic solvent. There are umpteen more organic solvents than inorganic solvents. Compare with organic and inorganic solvent, the solubility of iodine is higher in organic solvent.3. The oxidizing power of the halogens decrease going down the group as the size of the atoms increase going down the group as the size of the atoms increases and the attraction between the nucleus and the electrons becomes less. In that case, going down the group, the elements become less powerful oxidising agents. This means that a higher halogen will displace a move halogen from its salts. A lower halogen cannot displace a higher halogen from its salts.4. When starch reacts with iodine, the typical blue black color will appear. Thats a good way for us to identify starch and iodine.5. Af ter photodissociation, the color of some precipitates will change. will become black. Thats the most obvious one. Other precipitates will become darken.1. Because we use solid iodine in the first experiment. If we add the solvent into the test tube first, the test tube will be wet and the solid iodine we put in later will attach on the surface inside instead of fall into the liquid. For this reason we must add solid iodine first in experiment 1.2. According to the first experiment, we found that the solubility of iodine in pure water is very low. But the solubility of iodine in potassium iodide solution is relatively much higher. So we use I2-KI solution to increase the amount of iodine in order to let the phenomenon more obvious. credit1) Chemistry(for use with the International Baccalaureate Diploma Programme)3rd Edition John Green Sadru DamjiFirst published in 2007 by IBID Press, Victoria, Page 77 to 78.2) http//www.epa.gov/ttn/atw/hlthef/hexane.html3) http//baike.baidu.com/view /373611.htm4) http//baike.baidu.com/view/908645.htm