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Use the VSEPR model to predict the structures of (a)
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- If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?arrow_forwardThe Electron pair geometry, molecular geometry and Hybridization for NCl3 is (a) Tetrahedral, Trigonal pyramidal, sp^3 (b) Trigonal planar, Bent, sp^2 (c) Bent, Trigonal planar, sp^2 (d) Nonearrow_forwardDefine the following phenomena with reference to main group compounds: (d) multicenter electron deficient bondingarrow_forward
- Write the ground-state electron configuration for each atomand ion pair-Zr, Zr2+, Co, Co2+, Tc, Tc3+, Os, Os4+?arrow_forwardDescribe the molecular structure around the indicated atom or atoms:(a) the sulfur atom in sulfuric acid, H2SO4 [(HO)2SO2](b) the chlorine atom in chloric acid, HClO3 [HOClO2](c) the oxygen atom in hydrogen peroxide, HOOH(d) the nitrogen atom in nitric acid, HNO3 [HONO2](e) the oxygen atom in the OH group in nitric acid, HNO3 [HONO2](f) the central oxygen atom in the ozone molecule, O3(g) each of the carbon atoms in propyne, CH3CCH(h) the carbon atom in Freon, CCl2F2(i) each of the carbon atoms in allene, H2CCCH2arrow_forwardThe sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.arrow_forward
- Draw the molecular orbital diagrams for Ne(2), N(2) ^2- and Be(2). Are they stable or unstable?arrow_forwardUse the VSEPR model to predict the structure of the cyclicion P₃O₉³⁻arrow_forwardCO, CO₂, CH3OH, and CO32- all contain carbon-oxygen bonds. Draw Lewis structures for these molecules and ions. Given that double bonds are stronger than single bonds and triple bonds are stronger than double bonds, rank the four species in order of increasing CO bond strength. Weakest: Strongest:arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning