Answer question one please and if you can answer all the other questions if you can Molecular Shape:Questions: (Complete sentences are not necessary)1 Examine the Lewis structure for each of the molecular shapes formedabove. (ignore BrF!) Complete the following table based upon both thenumber of unshared electron pairs around the central atom and also thenumber of band groups that are around the central atom. For example, inthe following Lewis structure of PBr,, phosphorus (the central atom) has onepair of unshared electrons and three bond groups surrounding it.Br:B:(Note: single, double, and triple bonds all count as single bond groups)Number of Unshared ElectronNumber of Bond GroupsAround Central AtomMolecular ShapePairs Around the CentralAtomLinearBentTrigonal PlanarTrigonal PyramidalTetrahedral2. What is the electrostatic charge of all electron groups, either shared (Le. bonds) or unshared?3. Since all electron groups have this same charge, do they attract or repel each other?4. How many unshared electron pairs are present in the carbon atom in Co,?5. Considering your answers to the previous three questions, explain why CO, is not bent?6. Explain why H,O is not linear.

Answered: Image /qna-images/answer/f083147a-d3d4-456b-b007-8e0fcdad44e2.jpg

Answered: Number of Unshared Electron Number of…

Living by Chemistry

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ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

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Sulfur and oxygen form a series of 2 anions including sulfite, SO32, and sulfate, SO42. In addition to these, there are three other more complex anionsdithionite, S2O42, dithionate, S2O62, and tetrathionate, S4O62. Write correct Lewis structures for dithionite, dithionate, and tetrathionate ions.
On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar bond in each of the following pairs. msp;a.OClorOBrc.PSorPOb.NOorNFd.HOorHN
Mixing SbCl3 and GaCl3 in a 1:1 molar ratio (using liquid sulfur dioxide as a solvent) gives a solid ionic compound of empirical formula GaSbCl6 . A controversy arises over whether this compound is (SbCl2+)(GaCl4) or (GaCl2+)(SbCl4) . (a) Predict the molecular structures of the two anions. (b) It is learned that the cation in the compound has a bent structure. Based on this fact, which formulation is more likely to be correct?
On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp;a.HForHClc.HBrorHClb.HClorHId.HIorHBr
How many and bonds are present in the molecule HCN?
Use Lewis symbols and Lewis structures to diagram the formationof PF3 from P and F atoms, showing valence-shellelectrons. (a) How many valence electrons does P have initially?(b) How many valence electrons does each F haveinitially? (c) How many valence electrons surround the P inthe PF3 molecule? (d) How many valence electrons surroundeach F in the PF3 molecule? (e) How many bonding pairs ofelectrons are in the PF3 molecule?
A stable triatomic molecule can be formed that containsone atom each of nitrogen, sulfur, and fluorine. Threebonding structures are possible, depending on which is thecentral atom: NSF, SNF, and SFN.(a) Write a Lewis diagram for each of these molecules,indicating the formal charge on each atom.(b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom?(c) Does consideration of the electronegativities of N, S,and F from Figure 3.18 help rationalize this observedstructure? Explain.
Complete the table by drawing Lewis structures for the following molecules/ions and specifying their shape.
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 classmate of yours is convinced that he knows everythingabout electronegativity. (a) In the case of atoms X and Y havingdifferent electronegativities, he says, the diatomic moleculeX¬Y must be polar. Is your classmate correct? (b) Yourclassmate says that the farther the two atoms are apart in abond, the larger the dipole moment will be. Is your classmatecorrect?
(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?
In Lewis theory, we use electron dot formulas and the VSEPR model to determine electron distributionand geometric structure of covalent particles. Two important basic forms are ??5 and ??6 as outlined here: SEE IMAGE. A ) Iodine (?) often forms compounds with other halogens, such as fluorine (?), chlorine (??) and bromine(??). Compare valid Lewis electron structures and VSEPR geometries of the particles: see image Write down the correct VSEPR classification (?????) for each particle and provide a valid geometry

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