Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Chapter 3, Problem 3.9P
Give Lewis dot structures and sketch the shapes of the following:
a.
b.
c.
d.
e.
f.
g.
h.
i.
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Consider the molecules PF3 and PF5.
A. Draw the Lewis electron-dot structures for PF3 and PF5 and predict the molecular geometry.
B. Is the PF3 polar or non-polar and why?
C. On the basis of bonding principles, predict whether each of the following compounds exists. In each case, explain your prediction.
(i) NF5
(ii) AsF5
Nitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas.
(A) Draw the Lewis structure of NF3 and determine its molecular geometry.
(B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment?
(C) Could BF3 also behave as a greenhouse gas? Explain why or why not.
Which of the following molecules have dipole moments?
(a) CS2
(b) SeS2
(c) CCl2F2
(d) PCl3 (P is the central atom)
(e) ClNO (N is the central atom)
Please show work when calculating answers.
Chapter 3 Solutions
Inorganic Chemistry
Ch. 3.1 - Use electron-dot diagrams and formal charges to...Ch. 3.2 - Predict the structures of the following ions....Ch. 3.2 - Prob. 3.3ECh. 3.2 - Which molecule has the smallest bond angle in each...Ch. 3.2 - Briefly account for the following observations: a....Ch. 3.2 - Does this approach work for different steric...Ch. 3 - The dimethyldithiocarbamate ion, [S2CN( CH 3 )2]-...Ch. 3 - Several resonance structures are possible for each...Ch. 3 - Draw the resonance structures for the...Ch. 3 - Three isomers having the formula N2CO are known:...
Ch. 3 - Show the possible resonance structures for nitrous...Ch. 3 - Nitric acid, which exists as HNO3 molecules in the...Ch. 3 - L. C. Allen has suggested that a more meaningful...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Explain the trends in bond angles and bond lengths...Ch. 3 - Select from each set the molecule or ¡on having...Ch. 3 - a. Compare the structures of the azide ion, N3 ,...Ch. 3 - Consider the series OCl2,O( CH3)2 , and O( SiH3)2...Ch. 3 - Two ions isoelectronic with carbon suboxide, C3O2...Ch. 3 - Explain the following: a. Ethylene, C2H4 , is a...Ch. 3 - Explain the following: a. PCI5 is a stable...Ch. 3 - X-ray crystal structures of ClOF3 and BrOF3 have...Ch. 3 - Make the following comparisons about the molecules...Ch. 3 - Prob. 3.20PCh. 3 - A solution containing the lO2F2 ion reacts slowly...Ch. 3 - The XeOF3 anion has been reported recently (D. S....Ch. 3 - Predict the structure of l(CF3)Cl2 . Do you expect...Ch. 3 - a. Which has the longer axial PF distance, PF2(...Ch. 3 - Prob. 3.25PCh. 3 - SeCl62,TeCl62 , and CIF6 are all octahedral, but...Ch. 3 - Prob. 3.27PCh. 3 - The thiazyldichloride ion, NSCl2- , is...Ch. 3 - Sketch the most likely structure of PCl3Br2 and...Ch. 3 - a. Are the CF3 groups in PCl3( CF3)2 more likely...Ch. 3 - Of the molecules C1SO2CH3,C1SO2CF3 , and ClSO2CCl3...Ch. 3 - Prob. 3.32PCh. 3 - Prob. 3.33PCh. 3 - Prob. 3.34PCh. 3 - Prob. 3.35PCh. 3 - Although the CF distances and the FCF bond angles...Ch. 3 - The Cl...Cl distance in CCl4 is 289 pm, and the...Ch. 3 - The FCF angle in F2CO , shown here, is 109.5°; the...Ch. 3 - Compounds in which hydrogen is the outer atom can...Ch. 3 - For each of the following bonds, indicate which...Ch. 3 - Give Lewis dot structures and shapes for the...Ch. 3 - Give Lewis dot structures and sketch the shapes...Ch. 3 - Which of the molecules in Problem 3.41 are polar?Ch. 3 - Which of the molecules in Problem 3.42 are polar?Ch. 3 - Prob. 3.45PCh. 3 - Prob. 3.46P
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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
- Predict the molecular structure (including bond angles) for each of the following. (See Exercises 25 and 26.) a. ICl5 b. XeC14 c. SeCl6arrow_forwardExplain in terms of bonding theory why all atoms of H2CCCCH2 must lie in the same plane.arrow_forwardA molecular compound is composed of 58.8% Xe, 7.2%. O, and 34.0%. F, by mass. If the molecular weight is 223 amu, what is the molecular formula? What is the Lewis formula? Predict the molecular geometry using the VSEPR model.arrow_forward
- Give two requirements that should be satisfied for a molecule to be polar. Explain why CF4 and XeF4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has a net dipole moment). Is CO2 polar? What about COS? Explain.arrow_forwardWrite Lewis structures and predict the molecular structures of the following. (See Exercises 25 and 26.) a. OCl2, KrF2, BeH2, SO2 b. SO3, NF3, TF3 c. CF4 SeF4, KrF4 d. IF5, AsF5 Which of these compounds are polar?arrow_forwardPredict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts 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? (O3), sulfur dioxide, and sulfur trioxide.arrow_forward
- Predict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. XeCl2 b. ICl3 c. TeF4 d. PCl5arrow_forwardPredict the molecular structure (including bond angles) for each of the following. (See Exercises 25 and 26.) a. XeCl2 b. IC13 c. TeF4 d. PCl5arrow_forwardThere are several molecular structures based on the trigonal bipyramid geometry (see Table 8.9). Three such structures are Which of the compounds in Exercises 91 and 92 have these molecular structures? PF5, SF4, ClF3 and Br3 SF6, ClF5, and XeF4arrow_forward
- The molecule XF3 has a dipole moment. Is X boron or phosphorus?arrow_forwardFrom the electron-pair repulsion model, predict the geometry of the following molecules: a TeF6 b ClF5 c SeF4 d SbF5arrow_forwardConsider the following ion: BrO3−. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. h) What is the molecular formula for Compound C? What is the empirical formula for Compound C? Please andwer f, g and h the image is for g and harrow_forward
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