Answered: There are three possible structures for…

There are three possible structures for PCl2F3 with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 97QRT

See similar textbooks

Related questions

Q: Oxidation of the cyanide ion produces the stable cyanate ion, OCN.The fulminate ion, CNO¯, on the…

Q: Carbon, nitrogen, and oxygen form two different polyatomic ions: cyanate ion (NCO) and fulminate ion…

A: Let's explore the Lewis structures for the cyanate ion (NCO-) and the fulminate ion (CNO-). These…

Q: CTQ 7: Why is it incorrect to describe the process of boiling as 2H,0(1) → 2H,(g) + O,(g)?

A: Boiling is process when any substance gets start boiling.

Q: Draw the Lewis structure of PBr5 and then chose the appropriate number of valence electrons on the…

Q: The electron-pairs geometry around the Si atom in SiCl4 is blank and there are blank lone pairs…

A: In this question, we have to answer the electron-pairs geometry around the Si atom in SiCl4 , lone…

Q: Write an equation for the Lewis acid / Lewis base reaction between boron trifluoride and dimethyl…

Q: Draw the Lewis structure of SOCl₄ (with minimized formal charges) and then determine if the molecule…

A: If all bond dipoles cancel out each other then molecule is called Non-polar otherwise polar.

Q: Consider a hypothetical molecule with the formula X4Y2Z. The atoms X, Y, and Z have…

A: The concept of molecular polarity is crucial in understanding the behavior and properties of…

Q: Draw the best Lewis dot structure for BrO₄⁻, being sure to give the electronic geometry, molecular…

A: Since in Br we have 7 valence electron and in each O we have 6 valence electron And since O is more…

Q: Draw the Lewis structure of SeOF₂ (with minimized formal charges) and then determine the ideal…

A: this is the lewis structure of the SeOF2

Q: 5. (i) Provide possible resonance structure, (ii) evaluate the resonance structures with formal…

A: Resonating structure and formal charge depand structure of molecule

Q: Draw the resonance structures for NO2, SO2, and SO4-2.

Q: Selenium and sulfur are in the same chemical family as oxygen. Hydrogen selenide 1H2Se2 and hydrogen…

A: The Lewis structure of Hydrogen Selenide and Hydrogen Sulfide is given below.

Q: Determine the number of valence electrons in ClF₃ and then draw the corresponding Lewis structure…

A: We need to draw the Lewis structure of ClF3 and calculate its valence electrons. In order to…

Q: Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion…

A: sulphuric acid has a chemical formula H2SO4. in lewis structure, The lines are electron pairs, and a…

Q: Bromomethane, CH;Br, is a very useful fumigant against a wide range of agricultural pests, from…

Q: Although carbon has four bonds in stable molecules, sometimes reactive carbon intermediates that…

A: Draw the Lewis structure of H3C+. Since there are no lone pairs around C, it has sp2 hybridisation…

Q: (a) Determine the formal charge of oxygen in the following structure. If the atom is formally…

A: Formal charge is the net charge on an atom in a molecule or a compound.Formal charge = (no. of…

Q: Draw a lewis structure with the formula C6H12O2. Fill in all lone pairs

A: Lewis’s structure: Lewis’s bonding theory is based on the octet rule. The Lewis structure is a…

Q: Draw the Lewis structure of FeCl3.6H2O and FeCl2.4H2O.

Q: Except for nitrogen, the elements of Group 5A(15) all form pentafluorides and most form…

Q: There are two molecules with the formula C2H6O. Draw electron-dot structures for both. (The…

Q: The molecules CO, CO2, CH3ОH, and CO3? all contain carbon-oxygen bonds. Draw Lewis structures for…

Q: What is the resonance form that describes the distribution of electrons in SeO2 ?

Q: Account for ALL the electron pairs and describe the shape around the central atom in XeF4.

A: Given molecule, Xenon tetrafluoride XeF4

Q: Draw the Lewis structure of SnF₆²⁻ and then determine the ideal bonding angle(s) of the central…

A: The ideal bond angles of SnF62- can be predicted when its Lewis structure is drawn and its molecular…

Q: Draw the Lewis structure of SO42. Calculate the formal charge of central atom.

A: Lewis’s structure: The Lewis structure is a simplified representation of the valance shell electrons…

Q: Write the Lewis structure for SO3 where the central sulfur atom obeys the octet rule. Do not include…

A: Lewis Structure is defined as a very simplified representation which shows the total number of…

Q: If a C-O bond length is 1.66 pm and a C=O bond length is 1.52 pm, how long would the carbon oxygen…

A: Given that, the C-O bond length is 1.66 pm. And, the C=O bond length is 1.52 pm. We have to…

Concept explainers

Quantum Mechanical Treatment of the Valence Bond Theory

Quantum mechanical treatment of valence bond theory refers to the relationship established between the quantum mechanical theory and the valence bond theory to describe the chemical bonding in a particular molecule.

Question

There are three possible structures for PCl₂F₃ with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Quantum Mechanical Treatment of Valence Bond Theory

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The hydrocarbon cyclobutane, C4H8, is represented above. At high temperatures, cyclobutane quickly decomposes into ethene, C2H4. (see attached image) (a) Draw a Lewis electron-dot diagram of the ethene molecule in the following box, and estimate the value of the H−C−H bond angle in ethene.
Although carbon has four bonds in stable molecules, sometimes reactive carbon intermediates that contain carbon atoms without four bonds are formed for very short time periods. Examples of these unstable intermediates include the methyl carbocation (CH 3) + and the methyl carbanion (CH 3) −. Draw Lewis structures for both unstable ions and predict the shape around carbon.
Write a Lewis structure for the amide ion, NH2─, and assign formal charges to each atom.
Chloral, Cl3C—CH=O, reacts with water to form the sedative and hypnotic agent chloral hydrate, Cl3C—CH(OH)2. Draw Lewis structures for these substances, and describe the change in molecular shape, if any, that occurs around each of the carbon atoms during the reaction.
Carbon, nitrogen, and oxygen form two different polyatomic ions: cyanate ion (NCO) and fulminate ion (CNO). Write Lewis structures for each anion, including near-equivalent resonance structures (do not add any arrows between structures) and indicating formal charges. The isocyanate ion also has two near-equivalent structures, but the formal charge on the nitrogen attom cannot be reduced to zero: Cyanate ion (NCO)
Hydrogen cyanide can be catalytically reduced with hydrogen to form methylamine. Use Lewis structures and bond energies to determine ΔH°rxn for HCN(g) + 2 H2(g) ⟶ CH3NH2(g)
Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with formal charges) can be written for formamide. Write both resonance structures, and predict the bond angles about the carbon and nitrogen atoms for each resonance form. Are they the same? Describe how the experimental determination of the HNH bond angle could be used to indicate which resonance form is more important.
It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?
Consider the pyrosulfate ion, S2O72-. It has no sulfurâ€“sulfur nor oxygenâ€“oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two Oâ€”S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?
Phosphorus forms a number of oxohalides, X3PO, in which X may be a F, Cl, or Br atom. The most common of these, phosphoryl chloride, is obtained through the reaction 2 PC1₂(g) + O₂(g) → 2 Cl₂PO(g) Draw the Lewis structure for phosphoryl chloride (Cl3PO). Optimize formal charges. Select / |||||| Draw P Cl O Templates More Erase
Determine the number of valence electrons in sulfuric acid (H₂SO₄) and then draw the corresponding Lewis structure (with minimized formal charges).
Except for nitrogen, the elements of Group 5A(15) all form pentafluorides and most form pentachlorides. The chlorine atoms of PCI5 can be replaced with fluorine atoms one at a time to give, successively, PCI4F, PCI3F2, ..., PF5. (a) Given the relative sizes of F and Cl, would you expect the first two F substitutions to be at axial or equatorial positions? О axial O equatorial This answer has not been graded yet. (b) Which of the five fluorine-containing molecules have no dipole moment? (Select all that apply.) O PCI3F2 O PCI2F3 O PCIF4 O PF5 O PCI4F