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 3.38P
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8) Which molecules or molecule from the list below is or are polar?
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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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- The ions ClF2 and ClF2+ have both been observed. Use the VSEPR model to predict the FClF bond angle in each.arrow_forwardWhich of the following statements is(are) true? Correct the false statements. a.The molecules SeS3, SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle, which is approximately 120. b.The bond angle in SO2 should be similar to the bond angle in CS2 or SCl2. c.Of the compounds CF4, KrF4, and SeF4, only SeF4 exhibits an overall dipole moment (is polar). d.Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.arrow_forwardA friend tells you that the 2s orbital for fluorine starts off at a much lower energy than the 2s orbital for lithium, so the resulting 2s molecular orbital in F2 is more stable than in Li2. Do you agree?arrow_forward
- Explain in terms of bonding theory why all four hydrogen atoms of allene, H2CCCH2, cannot lie in the same plane.arrow_forwardBecause the structure of a tetrahedrom molecule uses 3 dimensions, a tetrahedron has a bond angle of 109.5 instead of the expected 90 degrees. True or False?arrow_forwardThe gaseous potassium chloride molecule has a measured dipole moment of 10.3 D, which indicates that it is a very polar molecule. The separation between the nuclei in this molecule is 2.67 Å. What would the dipole moment of a KCl molecule be if there were opposite charges of one fundamental unit (1.60 × 10-19 C) at the nuclei?arrow_forward
- The F−As−F bond angle in the AsF3 molecule is slightly less than __________. Group of answer choices 109.5° 90° 60° 120° 180°arrow_forwardFor the following molecules: A. XeO2F2 (neutron diffraction experiment by Peterson, Willett and Huston.[1] showed that F-Xe-F bond angle is 180o) B. ClF3 (1) Draw the valid Lewis structure, identify the (2) molecular group geometry, (3) electron group geometry, (4) polarity of the bonds, (5) over-all polarity, (6) number of lone pairs, and (7) number of bonding pairs.arrow_forwardBased on the relative likelihood of these possibilities and any other potential structures that YOU can draw, determine the bond order for the first N—N bond. If your answer is a fraction, use that fraction as the decimal equivalent (i.e. 1 1/4 = 1.25, etc.)arrow_forward
- The kinetic energy of an electron ejected from the σ*2s molecular orbital of N2 using58.4 nm radiation is 4.23 x 10-19 J. What is the ionization energy, in both kJ/mol and eV,of an electron from this orbital?arrow_forwardEstimate the dipole moment of an HCl molecule from theelectronegativities of the elements and express the answer in debyeand coulomb meters (C m).arrow_forwardPhenylalanine is one of the natural amino acids and is a “breakdown” product of theartificial sweetener aspartame. Estimate the values of the indicated angles in theamino acid. Explain why the —CH2—CH(NH2)—CO2H chain is not lineararrow_forward
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