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EXPERIMENT B2: Molecular Geometry and Chemical Bonding (Home based) Study Chapter 8 and 9 in Chemistry: 7th edition by Brady, Jespersen & Hyslop. Aims of this experiment 1. To write the Lewis formula for a molecule or a polyatomic ion. 2. To determine and build the geometry of a compound or polyatomic ion. 3. To determine if a compound is polar or non-polar from the Lewis structure and geometry of the molecule or polyatomic ion. Introduction The key to understanding molecular geometry comes from visualizing their shapes and being able to write down that shape using certain chemical tools. Below are a set of specific instructions which will serve as tools for predicting molecular shape, geometry and subsequently the bonding of a particular molecule or polyatomic ion. This experiment uses the concepts of valence electrons, Valence Shell Electron Pair Repulsion Theory (VSEPR), electronegativity, hybridization, polar bonds, formal charges and polar molecules. Tool 1 - Steps to writing the Lewis Formula of a molecule or ion: 1. Select a suitable (symmetrical) skeleton for the molecule or ion. The least electronegative element is usually the central atom; however, hydrogen is never the central atom. The central atom is also usually the one needing the most electrons to fill its octet. Oxygen atoms do not bond to other oxygen atoms except in O3, O2, and peroxides such as H2O2. The skeleton is also preferred to as the spider. 2. Count the valence electrons present. 3. Try to fill in the valence electrons in such a way that only single bonds and non- bonding valence electrons are present. 4. Check the compliance with the "octet rule". If some atoms have less than the octet of electrons, consider the possibility of multiple bonds. Remember that most elements do not form multiple bonds. If there are more electrons than needed for single bonds and non- bonding electrons to satisfy the octet rule, consider expanding the octet on the central atom. 5. Adjust the drawing to account for bonding knowledge, resonance, etc. Tool 2 - Steps to determine the geometry of the compound or ion: 1. Follow the steps contained in Tool 1 above. 2. Count the regions of high electron density "on" the central atom. 3. Determine the electronic or base geometry by giving each region of high electron density its maximum space. 4. Determine the molecular (or actual) geometry by describing the shape created within the electronic geometry by only bonded atoms. 5. Adjust the molecular geometry to account for difference space needs for different sized electronic groups. 81
Tool 3 - Steps to determine if a compound is polar or non-polar. 1. Follow the steps contained in Tool 1 and 2 above. 2. Ask the following three questions. a) Is the compound an ion? b) Are there polar bonds that are arranged so that they do not cancel? c) Are there lone pairs on the central atom that are arranged so that they do not cancel? 3. If the answer to any of the questions is yes, the compound is polar.
Activities 1) Complete the following pre-experiment questions. You can either do it directly on this document or copied on a separate piece of paper, which you then take a picture of. Upload your work on Blackboard under the "online practical” section. Initials and Surname Student number Date Demonstrator 1. Distinguish between ionic, covalent, and metallic bonding. 2. Which of the following molecules possess polar covalent bonds: Br2; O2; HI; SO2 and NH3? 3. How many equivalent orbitals are involved in each of the following sets of hybrid orbitals: sp: sp: sp'; sp'd and sp’d? 4. Define the term formal charge.
2) Examine the table provided. Entries 1 to 5 should be completed in full as well as two entries you have selected from 6 to 16. To assist you, entry 1 has been completed as an example. Total valence electrons Lewis Electron structure domain geometry Molecular Ideal Deviation Bond Polar/ / geometry bond from ideal polarity non-polar angles bond molecule angles 1 NH: 8 H-N H Tetrahedral Trigonal pyramidal H Polar 109.59 <109.5° (H-N-H) >109.5° 1 H H (lone pair- N-H) 2 PCI 에 3 NO, 4 SF. 에 5 PCI 6 IF; 7 XeFs 이 8 SO, 9 CH,Br 10 ICI 84
11 NO, 12 BF 13 HOOH 14 SbCI, 15 BrF 16 ICI 3) Construct a model of the two additional samples you have chosen from entries 6 to 16. You can use anything, for example matchsticks and some glue. See the example of NH3 below where ice-cream sticks and Prestik were used (delete this picture and replace with your own) Include your details and that of the molecule in the picture. Upload your work to Blackboard under the practical section, either as Word/PDF file, or separate as text pages and model pictures.