While predicting the shape of a molecule, the least electronegative element is the central atom of the compound. The geometry of a compound can be well explained by the VSEPR Theory which is based on the presumption that a molecule takes a shape in which it is the most stable and has the minimum electron-electron repulsions. Therefore, it becomes necessary to know the VSEPR theory and hybridization concept. It is agreeable that a Lewis structure gives a lot of information about a certain compound, although it is difficult to tell a compound’s geometry and hybridization exactly by this concept. Hence, the formal charge on ICl5is 0, which means that the compound is neutral. Therefore, the formal charge on each chlorine atom will be -1 and not 1.įormal charge on ICl5 = (formal charge of Iodine + formal charges of chlorine atoms) = ( 5 + ( -1 + -1 + -1 + -1 + -1 )) Since chlorine is more electronegative than iodine, it tends to attract the shared electron pair towards itself and therefore, induces a negative charge. Similarly formal charge of Cl (b,c,d,e) = 1 In simple language, it is needed to first calculate the formal charge of each atom individually.įormal charge of Cl (a) = 8 – 2/2 – 6 = 1 The formal charge of a compound is a summation of the formal charge of each bonded atom in the compound. The lewis structure is complete after the formal charge on the compound gets known.įor this, it is required to know the formula to calculate the formal charge. In the Lewis structure (b), it can be clearly seen that ten out of twelve electrons around iodine are involved in bonding (represented by the single bond) and one electron pair acts as the lone pair. In the Lewis structure (a), it can be seen that there are 8 valence electrons around each chlorine atom and a total of 12 valence electrons around the iodine atom (elements belonging to period >= 3 can extend their octet to more than 8 electrons). Step 3: Completing the Lewis structure by fulfilling the octet rule criteria for every atom in the compound. The following image represents the rough lewis diagram of ICl5. Step 2: Sketching out a rough Lewis diagramįor our own feasibility, a skeletal diagram is drawn by just placing the iodine and chlorine atoms in a way where five chlorine atoms surround the iodine atom. It is equal to ((7*1)+ (7*5)) which is equal to a total of 42 valence electrons. of valence electrons in the molecule will be equal to the sum of the valence electrons of iodine and chlorine. group 17, there are seven electrons in the valence shell of chlorine as well. Since chlorine and iodine belong to the same group i.e. Secondly, the electronic configuration of chlorine is 1s22s22p63s23p5. The electronic configuration of iodine is 4d105s25p5.Īs we can see, there are seven electrons in the valence shell of iodine. Step 1: Calculate the total valence electrons in the compound.įor the first step, it is required to know the electronic configuration of iodine and chlorine. The lewis structure of ICl5 can be made by following the following steps: The lewis dot structure gives an idea of the bonding in the ions of a compound based on the octet rule, in terms of shared electron pairs, including bonding as well as the non-bonding ones. To know more about this compound, it is necessary to get acquainted with its bonding characteristics as well as polarity.įor this, it is required to understand Lewis structure, VSEPR theory, and Hybridization concepts. Therefore, ICl5is an example of a polyhalide. Interhalogens in which x = 3,5 & 7 are known as polyhalides. These are of the type ABx where x can take the values: 1,3,5 & 7. In simple language, an interhalogen compound is a type of compound in which two different halogens react with each other. ICl5 falls under the category of interhalogen compounds where iodine is larger in size and more electropositive than chlorine, and also acts as the central atom in this compound. This is why ICl5is freshly prepared in labs whenever it is required to be used in a reaction. This instability occurs mainly due to the larger size of the chlorine atom in comparison to fluorine. Although, unlike IF5, it is not a very popular compound because of its unstable nature. It is a useful compound in scientific laboratories to conduct research work. ICl5is iodine pentachloride, which has a molecular mass of 304.40 g/mol.
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