Electron Location and Charge of Molecules Essay

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Valence Shell Electron Pair Repulsion and Molecular Polarity Simulation ActivitiesInstructions: Perform the two simulations below and answer all questions. You can either type in your answers in the provided spaces or handwrite your answers and then scan the file to submit in assignments1.Phet Molecular Shapes VSEPR Simulation ActivityIntroductionAtoms bond to satisfy their need for more electrons. Most atoms will share electrons to satisfy the Octet Rule – every atom wants 8 electrons to fill the s and p orbitals in the outer energy level. But, as you will see, sometimes atoms can deviate from and not follow the Octet Rule.Because electrons have a negative charge and atoms occupy space, bonds and electrons will spread out as much as possible. Since we write in a two-dimensional plane on paper, it is difficult to visualize the true geometry of these molecules. This activity and the program you are about to use allows us to visualize on a more 3-dimensional scale.ProcedureLog on to https://phet.colorado.edu/en/simulation/molecule-shapes either by Googling “phet simulations molecule shape.” Click on .Part 1 – Model Generic MoleculesClick on .Fill in the chart below by creating the generic molecules below. On your screen in the right side click on “remove all” to be left with just the purple central atom. On your screen in the lower left corner, click on “molecule geometry”, and on “electron geometry”. Add atoms and electron pairs as needed to produce the generic formula. Once the molecule is assembled, click and drag the screen to spin the atom around. Click on the “Show bond angles.” Use the following key:·· A – central purple atom – cannot be removed· B – single bonded white atom· C – double bonded white atom· D – triple bonded white atom· E – Electron pairs not bondedIn each box below:1. Draw the molecule you create to the best of your ability2. Write the Electron Geometry (EG) and the Molecule Geometry (MG) name in the box3. Label the bond angle4. Look at the central atom, is its octet satisfied?Before moving on to the next molecule for each of the molecules you create: with your mouse left click/hold and move your mouse around to move the molecule and get the feel for the 3D shape.MoleculeMoleculeACEG ___Linear__________________________MG _____Linear___________Bond angle: 180 degrees_____________Octet? ___Yes, for the central atom A, if it is a typical element that follows the octet rule, the triple bond provides it with six electrons, and it\'s presumed that the central atom also has another bond (possibly a hidden lone pair or implied second atom not mentioned in AC) to satisfy its octet.__ABE3EG ________Tetrahedral_____________________MG ________Trigonal Pyramidal Bond Angle: Approximately 107 degrees_____________________ Octet? ____Yes, the central atom\'s octet is satisfied with one bond to atom B and three lone pairs._AB3EEG _______tetrahedral ____bond angle: 107______MG _____trigonal pyramidal________________ Octet? ____Yes_ABEG ___________linear__bond angle: 180___________MG _______linear_____________ Octet? __Yes___ACE2EG ______trigonal planar______bond angle: 104.5_MG _______________bent______________ Octet? _____yesAB2E2EG ______ Tetrahedral_____bond angle: 104.5_______MG _______bent______________________ Octet? _____yesAB2CEG __________tetrahedral, bond angle: 109.5___________________MG ________trigonal planar_____________________ Octet? __yes___AB3EG _____Trigonal Planar________bond angle 120________________MG ____Trigonal Planar_________________________ Octet? _____yesAB4EG ___ Tetrahedral____bond angle: 109.5___________MG _____ Tetrahedral________________________ Octet? _____yesADEEG ______linear, bond angle 180__________MG ___linear__________________________ Octet? _____dependsPart 2 – Real MoleculesClick on the “Real Molecules” tab at the bottom of the page. Using the pull down menu, select the molecules below and fill in the chart. Match the molecule to the generic structure above in terms of Electron Geometry EG and Molecular Geometry MG. Fill in the generic bond angles as expected according to the generic model shapes from Part 1. Fill in the True bond angles as given by the simulation.MoleculeGeneric StructureGeneric (expected) bond angles (from Part 1)True Bond AnglesH2OEG____Tetrahedral___________MG_________Bent_____104.5104.5CO2EG____Linear___________MG______Linear________180180CH4EG_____Tetrahedral__________MG________ Tetrahedral ___104.

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…Atom B. What happened to the bond dipole and the partial charges? It flipped.5. Change the electronegativity of Atom B so that it is all the way to the left under “less.” Keep the slider for Atom A all the way under “more.” What happened to the bond dipole and the partial charges? It lengthened.6. Change the electronegativities of Atom A and Atom B so that they are the same. What happens to the bond dipole and the partial charges? They disappeared.Part 27. At the bottom of the screen, choose Three Atoms.8. Under View, click the boxes so that Bond Dipoles, Molecular Dipole, and Partial Charges are all showing.9. Without changing anything else, answer the following questions:a. What is the molecular shape of the molecule shown? Trigonal planarb. Which atom(s) is more electronegative? Bc. Which atom(s) has the partial negative charge(s)? Bd. Which atom(s) has the partial positive charge(s)? A, Ce. In the space below, sketch the diagram that’s on the screen, including the bond dipoles, molecular dipole, and partial charges.f. How is the molecular dipole related to the bond dipoles? It points away from them10. Change the electronegativities of Atom A and Atom C all so that they are both all the way to the right under “more.” What happened to the bond dipoles, molecular dipole, and partial charges? They all reversed.11. Click on Atom C and drag it until you make a linear molecule. What happens to the bond dipoles, molecular dipole, and partial charges? Molecular dipole disappears, bond dipoles stay the same, charges stay the same.12. Change the electronegativity of Atom C all so that it is all the way to the left under “less.” What happened to the bond dipoles, molecular dipole, and partial charges? Bond dipole between B and C reverses, the molecular dipole appears from….....

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