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- provide the following information including the lewis structucre and 3D sketch for SeO3^2- and HNO3a) Using Valence Bond Theory,NOT VSEPR, thoroughly show how silicon is able to form four identical atomic orbitals available for bonding in the compound SiF4. Be sure todiscuss bond angles/shape. b) Draw and name the correct orbitals involved when a Si atom and four F atoms come together to form SiF4. Your drawing should clearly show “before” and “after” forming the bonds. Draw the orbitals as clearly as you can, but you only have to show the orbitals for ONE of the Si—F bonds being formed -- don’t draw all four.+ 7. The shape of CH3 is
- Draw the Lewis dot structure for acetic acid (HC2H3O2, CH3COOH). Determine the optimum formal charge structure. Determine the VSEPR domain and molecular geometries for the central carbon atoms. Determine the hybridization of the carbons and oxygens. Determine the polarity of the molecule; show the polarity arrows and partial charges for the molecule. (Electronegativities: H 2.1,C 2.5, O 3.5)1)Using molecular orbital theory, determine the electronic structure of the first excited electronic state of N2. What differences are expected in the properties of the excited state of N2 compared with the same properties of the ground state? 2)Describe the bonding (including σ and п bonds) on an N atom in dinitrogen difluoride, N2F2, using valence bond theory. 3)Magic numbers are associated with protons and neutrons in a nucleus. State the magic numbers for protons and neutrons, and give two evidences to support the existence of these magic numbersWrite the best Lewis dot structure for POCl₃, be sure to give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the central element.
- CTQ 7: Why is it incorrect to describe the process of boiling as 2H,0(1) → 2H,(g) + 0,(g)?1. lewis structure of Cesium 2-hydroxyacetate, HOCH2CO2Cs 2. assign the VSEPR model of the central atom3. Value of the corresponding theoretical angle4. classify 3 of the different bonds around the central atom as ionic or covalent5. draw the complete 3-D structure with respect to the central atom (s)6. draw the lewis structure for another mnolecule or species with a different atomic arrangementDetermine the Lewis structure of CF3PCF2. Determine the hybridization of the P atom and the approximate angles between P-C bonds.
- Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-.Determine which of the following statements are true and which are false. True or false? : Bond length increases with increasing bond order while bond energy decreases.The number of unpaired electrons in O2- and O2 is, respectively, 1 and 2. The electron configuration of O2 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)1. The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)3. The bond order in O2- and O22- is, respectively, 2.5 and 1. The bond lengths increase in the order: O22- < O2- < O2 < O2+.For 3d structure and state geometry. Draw the Lewis structure for L2O3. Assume that all the valence electrons from L are required.What are the angles a and b in the actual molecule of which this is a Lewis structure? H- H a-0° b = 1⁰ C H a b H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X S
