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- The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.Draw the Lewis structures for each of the following moleculesor ions. Identify instances where the octet rule is notobeyed; state which atom in each compound does not followthe octet rule; and state how many electrons surround theseatoms: (a) NO, (b) BF3, (c) ICl2-, (d) OPBr3 (the P is the centralatom), (e) XeF4.8:38 OT A moodle.nct.edu.om Not yet answered Marked out of 4.00 P Flag question Explain the chemical bonding between Magnesium and Fluorine using Lewis electron dot structure. Answer the following for the structure given below. CI b(i) no of bond pair electrons b(ii) no of lone pair electrons b(i) no of single bond b(iv) no of double bond A- B I of -> 11 •.. :: +
- 10. The following Lewis structures for (a) HCN, (b) C3H;, (c) SnOz, (d) BF3, (e)HOF are incorrect. Explain what is wrong with each one and give a correct structure for the molecule. (Relative positions of atoms are shown correctly.) (a) H-ëN (b) HCC-H (c) 0-Sn-0 (d) :F B :F: (e) H-O-F:The SF5- ion is formed when SF4(g) reacts with fluoridesalts containing large cations, such as CsF(s). Draw theLewis structures for SF4 and SF5- , and predict the molecularstructure of each.Which of the following bonds are polar? Which is the more electronegative atom in cach polar bond? (a) B-F (b) Cl-CI (c) Se-O (d) H–I Arrange the bonds in cach of the following sets in order of inereasing polarity: (a) C-F, O–F, Be-F; (b) 0-CI, S-Br, C-P; (c) C-S, B–F, N-0.
- 9. The following figure shows the potential energy as a function of the distance between two hydrogen atoms. (a) Label the axes (include reasonable units!) and indicate the equilibrium bond distance. (b) What is the energy when the atoms are infinitely far apart? (c) On the same plot, sketch what you think the potential energy of the anion H; might look like. Consider where you would put the equilibrium bond distance and how deep the potential energy dips down.(a) State whether or not the bonding in each substance islikely to be covalent: (i) iron, (ii) sodium chloride, (iii) water,(iv) oxygen, (v) argon. (b) A substance XY, formed from twodifferent elements, boils at -33 °C. Is XY likely to be a covalentor an ionic substance?Which of the following bonds are polar? C-O, Cl-Cl, O=O, N-H, C-H.(Electronegativites: C = 2.5, H = 2.1, Cl = 3.0, O = 3.5, N = 3.0). In the selected bonds indicatewhich direction the electron density is greatest.
- Carbon monoxide, CO, is isoelectronic to N2. (a) Draw aLewis structure for CO that satisfies the octet rule. (b) Assumethat the diagram in Figure 9.46 can be used to describethe MOs of CO. What is the predicted bond order forCO? Is this answer in accord with the Lewis structure youdrew in part (a)? (c) Experimentally, it is found that thehighest energy electrons in CO reside in a σ-type MO. Isthat observation consistent with Figure 9.46? If not, whatmodification needs to be made to the diagram? How doesthis modification relate to Figure 9.43? (d) Would you expectthe π2p MOs of CO to have equal atomic orbital contributionsfrom the C and O atoms? If not, which atom wouldhave the greater contribution?Draw the Lewis structures for each of the following ionsor molecules. Identify those in which the octet rule is notobeyed; state which atom in each compound does not followthe octet rule; and state, for those atoms, how manyelectrons surround these atoms: (a) PH3, (b) AlH3, (c) N3-,(d) CH2Cl2, (e) SnF62-.(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?