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- The cations O2+ and N2+ are formed when molecules of O2 and N2 are subjected to intense, high-energy solar radiation in Earths upper atmosphere. Write the electron configuration for O2+. Predict its bond order and magnetic behavior.arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardSolid sulfur normally consists of crystals of S8 molecules, but when heated strongly, the solid vaporizes to give S2 molecules (among other molecular species). Describe the bonding in S2 in molecular orbital terms, assuming the orbitals are analogous to those of the preceding period. What would you expect to happen to the sulfur sulfur bond length if two electrons were added to give the S22 ion? What would you expect to happen to the bond length if, instead, two electrons were taken away to give S22+?arrow_forward
- Calculate the bond order of the dioxygen molecule and those of the molecular ions O2-,O22- and O2+? Rank these molecules and ions by order of increasing bond length. Explain your answer. aarrow_forwardAcetylene (C2H2) has a tendency to lose two protons (H+) and form the carbide ion (C22−), which is present in a number of ionic compounds, such as CaC2 and MgC2. (a) What is the bond order of the carbide dianion C22−? (b) For comparison, what is the bond order of C2?arrow_forwardThe existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground-state electron configurations. Is XeF likely to have a shorter or longer bond than XeF+?arrow_forward
- Molecules can be polar because of the unsymmetrical distribution of electrons. The dipole moment, μ Q r μ=Q×r The SI unit of dipole moment is the coulomb-meter (C⋅m), but another common unit is the debye (D). The two are related as 3.336×10^−30 C⋅m=1 D The percent ionic character is a comparison of the measured dipole moment of the bond to the expected dipole moment if electrons are instead transferred: %ionic character=measured dipole/if electrons transferred×100% The dipole moment if electrons are completely transferred is one for which a full unit of charge (1.60×10^−19 C) exists on each end of the bond. The dipole measured for HI is 0.380 D. The bond distance is 161 pm. What is the percent ionic character of the HI bond? Express your answer as a percent to three significant figures. Describe the molecular dipole of OCl2.arrow_forwardAmmonia (NH,) and silane (SiH,) are small molecules, each of which has four electron pairs in the valence shell of the central atom. Account for the difference in bond angle between the two molecules, 107.3° in ammonia and 109.5° in silane.arrow_forwardIn an experimental study of the SO2 molecule, it has been obtained that the angle OSO is equal to 119° and the bond distance S=O is equal to 1.45 Å. Calculate the dipole moment of the bond S=0 and the corresponding percentage of ionic bond. Discuss the results obtained. Data: SO2 dipole moment = 1.65 D; elemental electric charge = 1.602x1019 C; 1 D = 3.336x1030 C m.arrow_forward
- Using hybridization, predict how the bond length of the C − C σ bond in HC ≡ C − C ≡ CH should compare with the C − C σ bonds in CH3CH3 and CH2 = CH − CH = CH2.arrow_forwardDraw the Lewis structure for chloroform, CHCl3. What are its electron-pair and molecular geometries? What orbitals on C, H, and Cl overlap to form bonds involving these elements?arrow_forward9 Beryllium chloride (BeC12) is less soluble in water compared to calcium chloride (CaC12). Justify your answer. Apply valence bond theory to write a hybridization and bonding scheme for ethane, H,C=CH2. Label all bonds using the o and/or a notation followed by the type of overlapping orbitals. Arrange the following sets of bonds in order of increasing bond enthalpy. () Н-Н, Н- С, Н-Narrow_forward
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