General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Cengage Learning
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Textbook Question
Chapter 10, Problem 10.5QP
Explain why nitrogen trifluoride has a small dipole moment even though it has polar bonds in a trigonal pyramidal arrangement.
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Chapter 10 Solutions
General Chemistry - Standalone book (MindTap Course List)
Ch. 10.1 - An atom in a molecule is surrounded by four pairs...Ch. 10.1 - Use the VSEPR method to predict the geometry of...Ch. 10.1 - Prob. 10.2ECh. 10.2 - Bromine trifluoride, BrF3, has a nonzero dipole...Ch. 10.2 - Which of the following would be expected to have a...Ch. 10.2 - Two molecules, each with the general formula AX3,...Ch. 10.3 - Using hybrid orbitals, describe the bonding in NH3...Ch. 10.4 - Describe the bonding on the carbon atom in carbon...Ch. 10.4 - Dinitrogen difluoride (see Example 10.5) exists as...Ch. 10.4 - Prob. 10.3CC
Ch. 10.6 - The C2 molecule exists in the vapor phase over...Ch. 10.6 - Give the orbital diagram and electron...Ch. 10 - Describe the main features of the VSEPR model.Ch. 10 - According to the VSEPR model, what are the...Ch. 10 - Why is a lone pair expected to occupy an...Ch. 10 - Prob. 10.4QPCh. 10 - Explain why nitrogen trifluoride has a small...Ch. 10 - Prob. 10.6QPCh. 10 - What is the angle between two sp3 hybrid orbitals?Ch. 10 - Prob. 10.8QPCh. 10 - Prob. 10.9QPCh. 10 - How does the valence bond description of a...Ch. 10 - Prob. 10.11QPCh. 10 - What factors determine the strength of interaction...Ch. 10 - Prob. 10.13QPCh. 10 - Prob. 10.14QPCh. 10 - Prob. 10.15QPCh. 10 - Describe the bonding in O3, using molecular...Ch. 10 - Prob. 10.17QPCh. 10 - Which of the following molecular geometries does...Ch. 10 - Which of the following would be a polar molecule?...Ch. 10 - Prob. 10.20QPCh. 10 - Best Lewis Formula and Molecular Geometry A...Ch. 10 - Prob. 10.22QPCh. 10 - Prob. 10.23QPCh. 10 - Which of the following molecular models correctly...Ch. 10 - Prob. 10.25QPCh. 10 - Prob. 10.26QPCh. 10 - Indicate what hybrid orbital depicted below is...Ch. 10 - An atom in a molecule has two bonds to other atoms...Ch. 10 - Two compounds have the same molecular formula,...Ch. 10 - A neutral molecule is identified as a...Ch. 10 - Acetic acid, the sour constituent of vinegar, has...Ch. 10 - What are the bond angles predicted by the VSEPR...Ch. 10 - Predict the shape or geometry of the following...Ch. 10 - Use the electron-pair repulsion model to predict...Ch. 10 - Predict the geometry of the following ions, using...Ch. 10 - Use the VSEPR model to predict the geometry of the...Ch. 10 - For each of the following molecules, state the...Ch. 10 - For each of the following molecules, state the...Ch. 10 - Prob. 10.39QPCh. 10 - From the electron-pair repulsion model, predict...Ch. 10 - Predict the geometries of the following ions,...Ch. 10 - Name the geometries expected for the following...Ch. 10 - a The molecule AsF3 has a dipole moment of 2.59 D....Ch. 10 - a The molecule BrF3 has a dipole moment of 1.19 D....Ch. 10 - Which of the following molecules would be expected...Ch. 10 - Which of the following molecules would be expected...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - a Mercury(II) chloride dissolves in water to give...Ch. 10 - a Nitrogen trifluoride, NF3, is a relatively...Ch. 10 - a Carbonyl fluoride, COF2, is an extremely...Ch. 10 - a The molecule HNNH exists as a transient species...Ch. 10 - The hyponitrite ion, ONNO, exists in solid...Ch. 10 - Fumaric acid, C4H4O4, occurs in the metabolism of...Ch. 10 - Describe the electronic structure of each of the...Ch. 10 - Use molecular orbital theory to describe the...Ch. 10 - Prob. 10.59QPCh. 10 - Write the molecular orbital configuration of the...Ch. 10 - Predict the molecular geometry of the following: a...Ch. 10 - Prob. 10.62QPCh. 10 - Which of the following molecules or ions are...Ch. 10 - Which of the following molecules or ions are...Ch. 10 - Describe the hybrid orbitals used by each carbon...Ch. 10 - Prob. 10.66QPCh. 10 - Explain how the dipole moment could be used to...Ch. 10 - Two compounds have the formula Pt(NH3)2Cl2....Ch. 10 - Explain in terms of bonding theory why all four...Ch. 10 - Explain in terms of bonding theory why all atoms...Ch. 10 - What is the molecular orbital configuration of...Ch. 10 - Prob. 10.72QPCh. 10 - Calcium carbide, CaC2, consists of Ca2+ and C22...Ch. 10 - Sodium peroxide, Na2O2, consists of Na+ and O22...Ch. 10 - The oxygen oxygen bond in O2 is 112 pm and in O2...Ch. 10 - The nitrogennitrogen bond distance in N2 is 109...Ch. 10 - Using molecular orbital theory, determine the...Ch. 10 - The ionization energy of O2 is smaller than the...Ch. 10 - Prob. 10.79QPCh. 10 - Prob. 10.80QPCh. 10 - Prob. 10.81QPCh. 10 - Prob. 10.82QPCh. 10 - What is the biological importance of stratospheric...Ch. 10 - Prob. 10.84QPCh. 10 - Prob. 10.85QPCh. 10 - The bond length in C2 is 131 pm. Compare this with...Ch. 10 - Calcium carbide, CaC2, has an ionic structure with...Ch. 10 - Write Lewis formulas for the BF molecule (two with...Ch. 10 - Boron trifluoride, BF3, reacts with ammonia, NH3,...Ch. 10 - Prob. 10.90QPCh. 10 - Allene (1,2-propadicne), a gas, has the following...Ch. 10 - Prob. 10.92QPCh. 10 - The triiodide ion, I3, and the azide ion, N3, have...Ch. 10 - Hydrogen azide (also known as hydrazoic acid),...Ch. 10 - Prob. 10.95QPCh. 10 - A molecule XF6 (having no lone pairs) has a dipole...Ch. 10 - Describe the molecular orbital configurations of...Ch. 10 - Prob. 10.98QPCh. 10 - Three different compounds have the same molecular...Ch. 10 - Prob. 10.100QPCh. 10 - Prob. 10.101QPCh. 10 - Solid sulfur normally consists of crystals of S8...Ch. 10 - Prob. 10.103QPCh. 10 - Consider the bonding in nitrate ion, NO3. First...Ch. 10 - A molecular compound is composed of 52.5% Xe,...Ch. 10 - A molecular compound is composed of 58.8% Xe,...Ch. 10 - A compound of chlorine and fluorine. ClFn, reacts...Ch. 10 - Excess fluorine, F2(g), reacts at 150C with...Ch. 10 - Prob. 10.109QPCh. 10 - One resonance formula of benzene, C6H6, is What is...
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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
- How many central atoms does the molecule H2NCH3 have, and what is the shape about each?arrow_forwardWhat is the possible identity of X for a molecule XCl3- with a molecular geometry of trigonal pyramidal?arrow_forwardPlace the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H2O H3O+arrow_forward
- Explain what is wrong with each molecular geometry and provide the correct molecular geometry, given the numbers of lone pairs and bonding groups on the central atom. Match the words in the left column to the appropriate blanks in the sentences on the right. a bent a trigonal bipyramidal an octahedral a trigonal planar a square planar a trigonal pyramidal a tetrahedral a seesaw a linear In structure (a), four pairs of electrons give cause lone pair-bonded pair repulsions and would have Reset electron geometry. The lone pair would molecular geometry. Help In structure (b), five pairs of electrons give electron geometry. The lone pair occupies an equatorial position to minimize lone pair-bonded pair repulsions, and the molecule would have molecular geometry. In structure (c), six pairs of electrons give electron geometry. The two lone pairs would occupy opposite positions to minimize lone pair-lone pair repulsions, and the molecule would have molecular geometry.arrow_forwardPredict the geometry and bond angles around atom A for molecules with the general formulas AB3 and AB2E, where B represents another atom and E represents an electron pair.arrow_forwardCH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules. Explain.arrow_forward
- Answer the questions in the table below about the shape of the xenon tetrafluoride (XeF4) molecule. How many electron groups are around the central xenon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central xenon atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedralarrow_forwardwhich of the following statement is not true? 1)Nitrogen s relative inertness is due to formation of strong and stable bond between 2 nitrogens atom. 2)the bond energy of N2 is relatively higher that makes it relatively inert. 3)the bond energy of an O-H bond is always the same in all compounds that contain an O-H bond 4)carbon-carbon single bond is the longest among all sorts of carbon-carbon bonds 5)a shorter bond in general ,is a stronger bond than a longer bondarrow_forwardFind the electron and molecular geometries around the central atom. Is the Electron Geometry: bent, trigonal pyramidal, tetrahedral, linear, or trigonal planar? Molecular Geometry: bent, trigonal pyramidal, tetrahedral, linear, or trigonal planar?arrow_forward
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