e2pf09key - 1 Rank the following in increasing bond...

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1. Rank the following in increasing bond polarity: CC, BO, NH, LiF a. CC < NH < BO < LiF b. BO < CC < LiF < NH c. NH < BO < LiF < CC d. CC < BO < NH < LiF Homonuclear diatomic molecules are never polar. BO: 3.5 -2 = 1.5 NH: 3 - 2.2 = .8 LiF: 4-1 = 3 2. Which of the following can be polar molecules: I. CO 2 II. Fe(CO) 5 III. O 3 a. I b. I, II, III c. III d. I, II Carbon has double bonds with both oxygens and is therefore linear. The polarity of the bonds in CO 2 cancel out. Fe(CO) 5 has a trigonal bipyramidal geometry. The molecule is symmetric and there is no net dipole. The central oxygen in O 3 will have a positive dipole and the other two oxygens will have negative dipoles. Ozone has a bent molecular geometry and these dipoles do not cancel, making the molecule polar. 3. Which of the following molecules is nonpolar? a. NH3 b. SO4 2- c. SO2 d. BF2Cl SO4 2- has two double bonds to two oxygens and single bonds with the other oxygens. The single oxygens carry the negative charges. Each of these bonds are polar but the molecule has a tetrahedral geometry and the dipoles cancel. 4. Determine the molecular geometry and bond angles of bromine pentafloride (BrF5) a. Octahedral, 90, 120 b. Square Pyramidal, 90 c. Octahedral, 90 d. Square Pyramidal, 90, 120 VSPER says that BrF5 has an octahedral electronic geometry and a square pyramidal molecular geometry since Br has one lone pair. 5. Which hybrid orbitals are present in XeF4? a. dsp3 b. d2sp3 c. d2sp2 d. sp3 Xe has four covalent bonds with F and two lone pairs. There are 6 regions of electrons around Xe so it will hybridize two d atomic orbitals, 1 s orbital, and 3 p orbitals to make 6 hybrid d2sp3 orbitals. 6. Determine the electronic geometry of ICl 2 - . a. Trigonal pyramidal b. Bent c. Tetrahedral
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d. Trigonal Bipyramidal I has 3 lone pairs and two covalent bonds with Cl. 7. Determine the molecular geometry of the oxygen in CH3OH. a. Tetrahedral b. Bent c. Linear d. Seesaw Oxygen has two covalent bonds and two lone pairs. It has a tetrahedral electronic geometry and a bent molecular geometry. 8. How many σ and π bonds are there in C 2 H 2 ? a. 4σ and 1π b. 3σ and 2π c. 2σ and 3π d. 3σ and 1π C 2 H 2 has two single bonds and one triple bond. Every single bond is a sigma bond since the atomic or hybrid orbitals can directly overlap on the internuclear axis. Double bonds and triple bonds always have one sigma bond and one or two pi bonds respectively. The carbons are sp hybridized and these four hybrid orbitals are used in sigma bonding. The remaining four p orbitals are used in triple bonding. 9. What atomic orbitals are used in the bonding of NO?
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This note was uploaded on 03/04/2011 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas.

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e2pf09key - 1 Rank the following in increasing bond...

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