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Draw Lewis structures for the following molecules: (a)
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Chemistry
- (a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?arrow_forward3. Use Lewis symbols to diagram the reactions between (a) Ca and Br, (b) Al and O, and (c) K and S.arrow_forward(a) The 03 molecule has a central oxygen atom bonded to two outer oxygen atoms that are another. In the box below, draw the Lewis electron-dot diagram of the 03 molecule. Include all valid resonance structures. 0 - 0 = 0 (b) Based on the diagram you drew in part (a), what is the shape of the ozone molecule? and trigonal Bent Ozone decomposes according to the reaction represented below. 2 03(g) → 3 0₂(8) (c) The bond enthalpy of the oxygen-oxygen bond in O₂ is 498 kJ/mol. Based on the enthalpy of the reaction represented above, what is the average bond enthalpy, in kJ/mol, of an oxygen-oxygen bond in 03 ? Ozone can oxidize HSO3(aq), as represented by the equation below. [0] 1.0 x 10-5. <-> 00: HSO3(aq) + O3(aq) → HSO4 (aq) + O₂(8) A solution is prepared in which the initial concentration of HSO₂ (aq) (6.4 × 10+ M) is much larger than that of O3(aq) (1.0 × 10-5 M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below. 8.0 x…arrow_forward
- Draw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ion s in square brackets with the charge as a superscript outside the right bracket. (a) SO 2 (b) XeO 2 F 2 (Xe is the central atom) (c) ClF 3 (d) ClO 2 F (Cl is the central atom) (e) BrO 4 -arrow_forwardConsider the Lewis Structure for the molecule, [BrCl4]. On your own, make a sketch of the VSEPR shape, and use that to answer the following questions: :Cl: :Cl,Br- -Br÷Cl:arrow_forwardWrite Lewis dot symbols for the following atoms and ions: (a) I, (b) I−, (c) S, (d) S2−, (e) P,(f) P3−, (g) Na, (h) Na+, (i) Mg, (j) Mg2+, (k) Al, (l) Al3+, (m) Pb, (n) Pb2+.arrow_forward
- Na+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardKeeping in mind that some elements violate the octet rule, draw a Lewis structure for each compound: (a) BCl 3; (b) SO 3.arrow_forwardAn ionic compound of formula XY2 (X = cation with two positive charges, Y = anion with one negative charge) has the following mass composition: Mg 10.9%, Cl 31.8%, O57.3%. (a) What is the chemical formula and name of the compound? (b) Give the most probable Lewis structure for the ions contained in the compound.arrow_forward
- (1) What is the total number of valence electrons in the Lewis structure of SF2? electrons (2) Draw a Lewis structure for SF2arrow_forwardConsider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain brieflyarrow_forwardTwo substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.arrow_forward
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