For each molecular geometry, list the number of total electron groups, the number of bonding groups, and the number of lone pairs on the central atom. (a) (b) (c)
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- Determine the electron and molecular geometries of each molecule. For molecules with two central atoms, indicate the geometry about each central atom.(a) N2(b) N2H2 (skeletal structure HNNH)(c) N2H4 (skeletal structure H2NNH2)Identify the electron geometry about each charged atom. Where appropriate, indicate the molecular geometry and approximate bond angle as well. (a) (b) (c) (d) CH3 (e) (f) O `NH H3CN-CH3 CH3Draw the shapes of the following molecules and ions in 3-dimension. Show clearly any lone pairs of electrons on the central atom, state the number of bond pairs and lone pairs of electrons on the central atom and name the shape of the molecule or ion. (a) SiCI4, silicon tetrachloride (b) PBr3, phosphorus tribromide (c) CI2O, dichlorine oxide Provide everything stated in the instructions for each compound.
- (b) Determine the molecular geometry for each of the following compound. (i) ASF3 (ii) H2O2For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the direction of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it. (a) TeH2 (c) PCI (b) AsF3 (d) XeFDraw the shapes of the following molecules and ions in 3-dimension. Show clearly any lone pairs of electrons on the central atom, state the number of bond pairs and lone pairs of electrons on the central atom and name the shape of the molecule or ion. (a) AIH4-, aluminium hydride ion (b) CH3-, methyl carbanion (c) POCl3, phosphorus oxychloride Provide everything stated in the instructions for each compound.
- Are these statements true or false? Correct any that are false.(a) Two bonds comprise a double bond.(b) A triple bond consists of one bond π and two bonds σ.(c) Bonds formed from atomic sorbitals are always bonds.(d) A π bond restricts rotation about the σ-bond axis.(e) A π bond consists of two pairs of electrons.(f) End-to-end overlap results in a bond with electron density above and below the bond axis.Please answer all three parts of the question ?Draw a Lewis structure for each of the following molecule: (a) chlorodifluoromethane, CHCIF2 (b) propanoic acid C2H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CN ( the framework is H3C-C-N) (d) allene, H2CCCH2
- Determine the number of electron groups around the central atom for each molecule.(a) CH2Cl2(b) SBr2(c) H2S(d) PCl3The compound SF3N has been synthesized. (a) Draw the Lewis diagram of this molecule, supposing that the three fluoride atoms and the nitrogen atom surround the sulfur atom. Indicate the formal charges. Repeat, but assume that the three fluorine atoms and the sulfur atom surround the nitrogen atom. (b) From the results in part (a), speculate about which arrangement is more likely to correspond to the actual molecular structurThe molecular ion S3N, has the cyclic structure 'N All S-N bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is –0.375 and on each S atom is +0.041. Show that this result is consis- tent with the overall +1 charge on the molecular ion. Z-S