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 3.14P
Consider the series
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For the following descriptions of molecules, draw the Lewis structure (showing all
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An organic compound with the molecular formula H3CNO2. C is sp2
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An organic compound with the molecular formula H2CNO*. Both C
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Write the ground-state electron configuration of O2 and calculate the bond order.
Write the best Lewis dot structure for NH₄⁺, being sure to give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the central element.
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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- Draw the Lewis structures and predict the hybridization (sp, sp2, sp3), geometry (linear, trigonal, tetrahedral), and bond angles (180°, 120°, 109.5°) for the central atoms in the following compounds. C and N in C CH3CNarrow_forward2. In measurements of the structure of molecules, some interesting trends are observed. The bond angle (H-C-H) in CH4 is 109°, as we would expect for a molecule in the tetrahedral VSEPR class. However, other molecules in the same VSEPR class, such as ammonia (NH3, H-N-H= 107°) and water (H2O, H-O-H = 105°), have smaller bond angles than expected. Explain the basis for the bond angle trend: CH4 > NH3 > H2O. %3Darrow_forwardDescribe the hybrid orbitals used by the carbon atom inN=C-Cl. Predict the geometry of the molecule.arrow_forward
- suppose you forget to take into account the presence of unshared pair of electrons on nitrogen in the molecule nh3. what would you then predict for the h-n-h bond angles and geometry of ammonia?arrow_forwardHow would you describe the molecular geometry of C2H2F2, and what are its bond angles?arrow_forwardDraw a line-bond structure for propene, CH3CH=CH2. Indicate the hybridization of the orbitals on each carbon, and predict the value of each bond angle.arrow_forward
- 2a) The molecule ethene (or ethylene), which has the molecular formula C₂H4, contains two carbon atoms with planar geometry. Construct a model of ethene by first connecting two black balls with two springs. Use four short sticks and four yellow balls to complete the structure. Sketch a perspective representation (a three dimensional drawing) of the structure. 2b) What is the C=C-H bond angle in ethene?arrow_forwardPredict the hybridization, geometry, and bond angles for the carbon atoms in acetylene, C2H2.arrow_forwardA student investigates the physical and chemical properties of various carbon-containing compounds. The complete Lewis electron-dot diagrams and boiling points for two compounds, Q and X are shown in the following table. Identify the hybridization of the valence orbitals of the carbon atom in compound X that is indicated by the arrow in the diagram. The C-H bonds in compound Q are shorter than the C-C bonds in compound X. Explain the reason for this difference using principles of atomic structure. For each compound, list all intermolecular forces present. Q = X =arrow_forward
- Write the best Lewis dot structure for N₃⁻, give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the central element.arrow_forwardDraw the best Lewis dot structure for BrO₄⁻, being sure to give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the central element.arrow_forwardA particular allotrope of nitrogen, N4, was first detected in 2002. (Allotrope just means a chemical form in which an element can exist. Oxygen, for example, has two allotropes on earth: O2 and O3.) The all-nitrogen compound only lasts a short while before breaking down to N2. The compound cannot be isolated, so its structure is not yet confirmed experimentally; we can only hypothesize what its bonding and shape are. This allotrope is generally believed to be either a single ring of four nitrogens or a single chain of four nitrogens. 1. Draw the Lewis structure for both the linear form and the single ring form.arrow_forward
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