Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 7, Problem 54QRT
Interpretation Introduction
Interpretation:
The Lewis structures to represent the intramolecular and intermolecular hydrogen bonding have to be given. The lone pairs should be given and each hydrogen bonding has to be indicated as a series of three dots.
Concept introduction:
Hydrogen bonding:
The attractive force that holds two polar molecules (containing Hydrogen and highly electronegative atom, such as N, O, or F) is called as hydrogen boding. This is also called as intermolecular hydrogen bonding.
The hydrogen bonding takes place within a molecule is called as intramolecular hydrogen bonding.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Explain the difference between a polar bond and a polar molecule.
Dispersion forces are produced when
an electronegative atom pulls on the electron of a hydrogen atom so much that the proton of the
hydrogen can closely interact with the electronegative atom of another molecule
electronegative atoms pull electrons toward one area of the molecule, creating regions of partial
positive and partial negative charge that are attracted to regions of other molecules with the
opposite charge
electrons are transferred from one atom to another to produce anions and cations that are then
held together in a rigid lattice
electrons in molecular compounds are constantly moving and produce short-term regions of
positive and negative charge that are attracted to regions of other molecules with the opposite
charge
Predict the main type of intermolecular force that would exist between molecules of the following hypothetical compounds, based upon its polarity:
molecules of carbon monosulfide, C―S
molecules of phosphorus monochloride, P―Cl
molecules of hydrogen monophosphide, H―P
Chapter 7 Solutions
Chemistry: The Molecular Science
Ch. 7.2 - Identify the electron-region geometry, the...Ch. 7.2 - Based on the discussion so far, identify a...Ch. 7.2 - Prob. 7.2PSPCh. 7.2 - Determine the electron-region geometry and the...Ch. 7.2 - Prob. 7.2CECh. 7.2 - Prob. 7.3ECh. 7.2 - Prob. 7.4PSPCh. 7.4 - Using hybridization and sigma and pi bonding,...Ch. 7.4 - Prob. 7.4CECh. 7.5 - Decide whether each molecule is polar and, if so,...
Ch. 7.5 - Prob. 7.5ECh. 7.6 - Prob. 7.8PSPCh. 7.6 - Prob. 7.7CECh. 7.6 - Prob. 7.9PSPCh. 7.7 - Prob. 7.8CECh. 7.7 - Prob. 7.9CECh. 7 - Write the Lewis structures and give the...Ch. 7 - The structural formula for the open-chain form of...Ch. 7 - Describe the VSEPR model. How is the model used to...Ch. 7 - What is the difference between the electron-region...Ch. 7 - Prob. 3QRTCh. 7 - Prob. 4QRTCh. 7 - If you have three electron regions around a...Ch. 7 - Prob. 6QRTCh. 7 - Prob. 7QRTCh. 7 - Prob. 8QRTCh. 7 - Prob. 9QRTCh. 7 - Prob. 10QRTCh. 7 - Prob. 11QRTCh. 7 - Prob. 12QRTCh. 7 - Prob. 13QRTCh. 7 - Prob. 14QRTCh. 7 - Prob. 15QRTCh. 7 - Prob. 16QRTCh. 7 - Write Lewis structures for XeOF2 and ClOF3. Use...Ch. 7 - Write Lewis structures for HCP and [IOF4]. Use...Ch. 7 - Prob. 19QRTCh. 7 - Prob. 20QRTCh. 7 - Explain why (I3)+ is bent, but (I3) is linear.Ch. 7 - Prob. 22QRTCh. 7 - Prob. 23QRTCh. 7 - Give approximate values for the indicated bond...Ch. 7 - Give approximate values for the indicated bond...Ch. 7 - Prob. 26QRTCh. 7 - Compare the FClF angles in ClF2+ and ClF2. From...Ch. 7 - Prob. 28QRTCh. 7 - Prob. 29QRTCh. 7 - Prob. 30QRTCh. 7 - Prob. 31QRTCh. 7 - Describe the geometry and hybridization of carbon...Ch. 7 - Describe the geometry and hybridization for each C...Ch. 7 - Describe the hybridization around the central atom...Ch. 7 - The hybridization of the two carbon atoms differs...Ch. 7 - The hybridization of the two nitrogen atoms...Ch. 7 - Identify the type of hybridization, approximate...Ch. 7 - Prob. 38QRTCh. 7 - Prob. 39QRTCh. 7 - Prob. 40QRTCh. 7 - Prob. 41QRTCh. 7 - Methylcyanoacrylate is the active ingredient in...Ch. 7 - Prob. 43QRTCh. 7 - Prob. 44QRTCh. 7 - Prob. 45QRTCh. 7 - Prob. 46QRTCh. 7 - Which of these molecules has a net dipole moment?...Ch. 7 - Prob. 48QRTCh. 7 - Use molecular structures and noncovalent...Ch. 7 - Prob. 50QRTCh. 7 - Explain why water “beads up” on a freshly waxed...Ch. 7 - Explain why water will not remove tar from your...Ch. 7 - Prob. 53QRTCh. 7 - Prob. 54QRTCh. 7 - Prob. 55QRTCh. 7 - Prob. 56QRTCh. 7 - The structural formula for vitamin C is Give a...Ch. 7 - Prob. 58QRTCh. 7 - Prob. 59QRTCh. 7 - Prob. 60QRTCh. 7 - Prob. 61QRTCh. 7 - Prob. 62QRTCh. 7 - Prob. 63QRTCh. 7 - Prob. 64QRTCh. 7 - Prob. 65QRTCh. 7 - Prob. 66QRTCh. 7 - Methylcyanoacrylate is the active ingredient in...Ch. 7 - Prob. 68QRTCh. 7 - Prob. 69QRTCh. 7 - Use Lewis structures and VSEPR theory to predict...Ch. 7 - In addition to CO, CO2, and C3O2, there is another...Ch. 7 - Prob. 72QRTCh. 7 - Prob. 73QRTCh. 7 - Prob. 74QRTCh. 7 - Prob. 75QRTCh. 7 - In the gas phase, positive and negative ions form...Ch. 7 - Prob. 77QRTCh. 7 - Prob. 78QRTCh. 7 - Prob. 79QRTCh. 7 - Prob. 80QRTCh. 7 - Prob. 81QRTCh. 7 - Prob. 82QRTCh. 7 - Prob. 83QRTCh. 7 - Prob. 84QRTCh. 7 - Prob. 85QRTCh. 7 - Prob. 86QRTCh. 7 - Prob. 87QRTCh. 7 - Prob. 88QRTCh. 7 - Prob. 89QRTCh. 7 - Prob. 90QRTCh. 7 - Prob. 91QRTCh. 7 - Prob. 92QRTCh. 7 - Prob. 93QRTCh. 7 - Prob. 94QRTCh. 7 - Which of these are examples of hydrogen bonding?Ch. 7 - Prob. 96QRTCh. 7 - Prob. 97QRTCh. 7 - Prob. 98QRTCh. 7 - Halothane, which had been used as an anesthetic,...Ch. 7 - Ketene, C2H2O, is a reactant for synthesizing...Ch. 7 - Gamma hydroxybutyric acid, GHB, infamous as a date...Ch. 7 - There are two compounds with the molecular formula...Ch. 7 - Piperine, the active ingredient in black pepper,...Ch. 7 - Prob. 105QRTCh. 7 - Two compounds have the molecular formula N3H3. One...Ch. 7 - Prob. 108QRTCh. 7 - Prob. 109QRTCh. 7 - Prob. 110QRTCh. 7 - Prob. 111QRTCh. 7 - Prob. 7.ACPCh. 7 - Prob. 7.BCPCh. 7 - Prob. 7.CCPCh. 7 - Prob. 7.DCP
Knowledge Booster
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
- Which of these are examples of hydrogen bonding?arrow_forwardHalothane, which had been used as an anesthetic, has the molecular formula CHBrClCF3. Write the Lewis structure for halothane. Is halothane a polar molecule? Explain your answer. Can hydrogen bonding occur in halothane? Explain.arrow_forwardFor each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name acetic acid dimethyl ether compound hypobromous acid formula or Lewis structure H :0: H-C-C-O-H H H H-C-0-C H H H T HBrO | H Between molecules of the compound? yes O O no O yes no yes hydrogen-bonding force no Between molecules of the compound and molecules of water? O O yes no yes no yes no Xarrow_forward
- For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name methanol difluoromethane ammonia compound formula or Lewis structure H I H-C-O-H I H CH₂F₂ NH₂ Between molecules of the compound? O yes O no O yes O no hydrogen-bonding force O yes O no Between molecules of the compound and molecules of water? O yes O no O yes O no O yes O no X Sarrow_forwardIn structure (a), four pairs of electrons give ______ electron geometry. The lone pair would cause lone pair-bonded pair repulsions and would have ______molecular geometry. 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_forwardConsider atoms of helium. The average distribution of electrons around each nucleus is spherically symmetrical. The atoms are nonpolar and possess no dipole moment. At a given instant in time, the distribution of electrons around an individual atom, may not be perfectly symmetrical. Both electrons may be on one side of the nucleus. The atoms would have an apparent dipole moment at that instant in time. This will cause the neighboring atoms to be attracted to one another. What type of intermolecular force is this?arrow_forward
- For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name hydrogen lodide methanimine compound dimethyl ether formula or Lewis structure H HIC NIH H HI H H-C-6-C-H HICIH Between molecules of the compound? O yes O no O yes O no hydrogen-bonding force. O yes O no Between molecules of the compound and molecules of water? Oyes O no O yes O no O yes O no ola Earrow_forwardWhat is the difference between polar covalent bonds and hydrogen bonds?arrow_forwardYou are given part of a molecule shown below. Assume that the two atoms are covalently bound to each other and to a larger molecule at the first dash symbol. Can the atom that is underlined (as shown) participate in a hydrogen bond with another atom from a different molecule? −O−H −C−H −N−H −O−H −C−H Can the oxygen of -O-H participate in a hydrogen bond? Can the hydrogen of -C-H participate in a hydrogen bond? Can the nitrogen of -N-H participate in a hydrogen bond? Can the hydrogen of O-H participate in a hydrogen bond? Can the carbon of -C-H participate in a hydrogen bond?arrow_forward
- Please envision this table like it was one long table. (I had to make it two because it hung out of the quiz boundaries and was inaccessible.) It is recommended that you draw the Lewis Structure of the molecules and then complete this table. electronic Molecular Molecule Geometry Geometry CH3F tetrahedral tetrahedral NH3 tetrahedral trigonal pyramidal C2F4 trigonal planar trigonal planar CO2 linear linear main dipole Molecule intermolecular moment force CH3F [ Select ] yes NH3 hydrogen bonding yes C2F4 [ Select ) no CO2 ( Select | no > >arrow_forward3. Identify the strongest intermolecular force in the following compounds (assume you have a bottle full of the molecule listed). You may find it useful to draw Lewis structures to find your answer. a) PF3 b) C₂H6 c) Cl₂ d) CH₂OH e) CH CIarrow_forwardFor each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name methanimine methylamine ammonial compound formula or Lewis structure H H-C=N-H H H 1 C 1 H H T N-H NH₂ Between molecules of the compound? yes O no Oo yes O no yes hydrogen-bonding force O no Between molecules of the compound and molecules of water? O yes O no O yes O no O yes O noarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY