Ikeerences Use the References to access important values if needed for this question. 1 What is the total number of valence electrons in the Lewis structure of PCI, electrons 2 Draw a Lewis structure for PCI,". • Do not include overall ion charges or formal charges in your drawing. If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in ord atom to obey the octet ruke

Ikeerences Use the References to access important values if needed for this question. 1 What is the total number of valence electrons in the Lewis structure of PCI, electrons 2 Draw a Lewis structure for PCI,". • Do not include overall ion charges or formal charges in your drawing. If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in ord atom to obey the octet ruke

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 33E

See similar textbooks

Similar questions

A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central 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 observed structure? Explain.
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
A compound is being tested for use as a rocket propellant. Analysis shows that it contains 18.54% F, 34.61% Cl, and 46.85% O. (a) Determine the empirical formula for this compound. (b) Assuming that the molecular formula is the same as the empirical formula, draw a Lewis diagram for this molecule. Review examples elsewhere in this chapter to decide which atom is most likely to lie at the center. (c) Use the VSEPR theory to predict the structure of the molecule from part (b).
Draw Lewis diagrams for the following compounds. In the formula the symbol of the central atom is given first. (Hint: The valence octet may be expanded for the central atom.) (a) PF5 (b) SF4 (c) XeO2F2
The molecular ion S3N3 has the cyclic structure All SN 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 consistent with the overall +1 charge on the molecular ion.
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?
In the fictitious molecule, highlight the atoms that have nonzero formal charges. Assume all lone pairs are shown.
Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In each case the first atom listed is the central atom.) a. POCl3, SO42-, XeO4, PO43-, ClO4- b. NF3, SO32-, PO33-.Cl3- c. ClO2-, SCl2, PCl2- d. Considering your answers to part a, b, and c, what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons?
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.
Ignoring tables of electronegativity values and guided onlyby the periodic table, arrange these atoms in order ofincreasing electronegativity: S, Cl, Sb, Se, In. Briefly explainyour reasoning.
Give only typing answer with explanation and conclusion draw the lewis structure with charge and the molecular structures for BrF5 (2+) and SeO2 (2-) charges
Can you help me with the explanation of the molecular polarity, partial charge, formal charge and all these terms give me examples too?