Answer all three please ✓ 2 TABLE 13.2 Inorganic Compounds - Be sure to show the proper geometries! Species Lewis Dot Structure and Resonance structures including formal charge VSEPR Theory and Valence Bond Theory Classifications Molecular Geometry HCN Indicate the hybridization of both the C and N Total Valence Electrons SO₂ Show all reso- nance structures and formal charges. Total Valence Electrons AsCl₂ Are the Cl atoms equato- rial, axial, or both? Total Valence Electrons H-C-N bond angle Polarity Hybridization Carbon Nitrogen Orbital Geometry Molecular Geometry Hybridization of central atom Orbital Geometry O-S-O bond angle Polarity Molecular Geometry Hybridization of central atomi Orbital Geometry Cl-As-Cl bond angles and Polarity

Answer all three please ✓ 2 TABLE 13.2 Inorganic Compounds - Be sure to show the proper geometries! Species Lewis Dot Structure and Resonance structures including formal charge VSEPR Theory and Valence Bond Theory Classifications Molecular Geometry HCN Indicate the hybridization of both the C and N Total Valence Electrons SO₂ Show all reso- nance structures and formal charges. Total Valence Electrons AsCl₂ Are the Cl atoms equato- rial, axial, or both? Total Valence Electrons H-C-N bond angle Polarity Hybridization Carbon Nitrogen Orbital Geometry Molecular Geometry Hybridization of central atom Orbital Geometry O-S-O bond angle Polarity Molecular Geometry Hybridization of central atomi Orbital Geometry Cl-As-Cl bond angles and Polarity

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter8: Advanced Theories Of Covalent Bonding

Section: Chapter Questions

Problem 19E: Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the...

See similar textbooks

Similar questions

From models of SF4, BrF3, and XeF4, deduce whether differentatom arrangements, called geometrical isomers, are possible, and,if so, sketch them below.Indicate the preferred geometry foreach case and suggest a reason for your choice.Indicatewhich structures have dipole moments, and show their direction. Molecule Dipole Moment Preferred Geometry SF4 BrF3 XeF4
(a) Using only the valence atomic orbitals of a hydrogenatom and a fluorine atom, and following the model ofFigure 9.46, how many MOs would you expect for the HFmolecule? (b) How many of the MOs from part (a) would beoccupied by electrons? (c) It turns out that the difference inenergies between the valence atomic orbitals of H and F aresufficiently different that we can neglect the interaction ofthe 1s orbital of hydrogen with the 2s orbital of fluorine.The 1s orbital of hydrogen will mix only with one 2p orbitalof fluorine. Draw pictures showing the proper orientationof all three 2p orbitals on F interacting with a 1s orbitalon H. Which of the 2p orbitals can actually make a bondwith a 1s orbital, assuming that the atoms lie on the z-axis?(d) In the most accepted picture of HF, all the other atomicorbitals on fluorine move over at the same energy into themolecular orbital energy-level diagram for HF. These arecalled “nonbonding orbitals.” Sketch the energy-level diagramfor HF using…
Both NH3, NCl3, and NF3 are all polar. Here is a data table with some additional information: Name Melting Point (°C) Boiling Point (°C) Molecular Geometry Nitrogen trihydride (ammonia) -77.7 -33.3 Trigonal Pyramidal Nitrogen trichloride -40.0 71.0 Trigonal Pyramidal Nitrogen trifluoride -207 -129 Trigonal Pyramidal Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? choose one: 1.The molecular geometry makes it the most polar of the compounds 2.The larger mass and larger electron cloud means stronger LDF 3.It can participate in H-bonding 4.Unlike the other substances, it is polar. 5.The small mass means it takes less energy to break the IMF
Is delocalization possible in Hydrogen selenate (HOSeO3- )
There is persuasive evidence for the brief existence of theunstable molecule OPCl.(a) Draw a Lewis diagram for this molecule in which theoctet rule is satisfied on all atoms and the formalcharges on all atoms are zero .(b) The compound OPCl reacts with oxygen to giveO2PCl. Draw a Lewis diagram of O2PCl for which allformal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the real and model modes. Explain the difference observed.
Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KCIO3 contains the ClO3 ion. P4S3 is an unusual molecule with the skeletal structure. (a) Write Lewis structures for P4S3 and the ClO3 ion. (b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species. (c) Assign a hybridization to the P atoms, the S atom, and the Cl atom in these species. (d) Determine the oxidation states and formal charge of the atoms in P4S3 and the ClO3 ion.
Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Draw the shapes of the following molecules and ions in 3-dimension showing clearly the bonds between the atoms and the lone pairs of electrons on the central atom, if any. (a) CH3OH, methanol (b) H2O2, hydrogen peroxide (c) CH3CH=CHCI, 1-chloropropene Provide everything stated in the instructions.
a) What is the difference between a localized π bond and adelocalized one? (b) How can you determine whether a moleculeor ion will exhibit delocalized π bonding? (c) Is the πbond in NO2- localized or delocalized?