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 6, Problem 111QRT
(a)
Interpretation Introduction
Interpretation:
The Lewis structure for gamma-aminobutanoic acid has to be written.
Concept Introduction:
Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.
(b)
Interpretation Introduction
Interpretation:
The longest bond in gamma-aminobutanoic acid has to be identified.
(c)
Interpretation Introduction
Interpretation:
The most polar bond in gamma-aminobutanoic acid has to be identified.
(d)
Interpretation Introduction
Interpretation:
The strongest bond in gamma-aminobutanoic acid has to be identified.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?
(a) Complete the Lewis structure for vinyl chloride by
showing all unshared pairs of electrons.
(b) Predict the H-C-H, H-C-C, and Cl-C-H
bond angles in this molecule.
(c) Does vinyl chloride have polar bonds? Is it a
polar molecule? Does it have a dipole?
Consider the following compounds: BeCl 2 , MgBr 2 , and SrBr 2 . Answer the following questions based on expected periodic trends:
(a) Which is expected to have the shortest ionic bonds?
(b) Which is expected to have the highest lattice energy?
(c) Which is expected to have the lowest melting point?
Chapter 6 Solutions
Chemistry: The Molecular Science
Ch. 6.2 - Write Lewis structures for (a) NF3, (b) N2H4, and...Ch. 6.3 - Prob. 6.1ECh. 6.3 - Prob. 6.2PSPCh. 6.4 - Prob. 6.2CECh. 6.4 - Write Lewis structures for (a) nitrosyl ion, NO+;...Ch. 6.5 - Prob. 6.4CECh. 6.5 - Prob. 6.5CECh. 6.5 - Prob. 6.4PSPCh. 6.6 - Prob. 6.5PSPCh. 6.6 - Use Equation 6.1 and values from Table 6.2 to...
Ch. 6.6 - Prob. 6.6CECh. 6.7 - Prob. 6.7PSPCh. 6.7 - Prob. 6.7CECh. 6.8 - Prob. 6.8PSPCh. 6.9 - Prob. 6.9PSPCh. 6.9 - Prob. 6.9CECh. 6.10 - Prob. 6.10PSPCh. 6.11 - Prob. 6.10ECh. 6.11 - Prob. 6.11ECh. 6.11 - Prob. 1CECh. 6.11 - Prob. 2CECh. 6.12 - Repeat Problem-Solving Example 6.11, but use N2...Ch. 6.12 - Use MO theory to predict the bond order and the...Ch. 6 - Prob. 1QRTCh. 6 - Prob. 2QRTCh. 6 - Prob. 3QRTCh. 6 - Prob. 4QRTCh. 6 - Prob. 5QRTCh. 6 - Prob. 6QRTCh. 6 - Which of these molecules have an odd number of...Ch. 6 - Prob. 8QRTCh. 6 - Prob. 9QRTCh. 6 - Prob. 10QRTCh. 6 - Prob. 11QRTCh. 6 - Prob. 12QRTCh. 6 - Explain in your own words why the energy of two H...Ch. 6 - Prob. 14QRTCh. 6 - Prob. 15QRTCh. 6 - Prob. 16QRTCh. 6 - Prob. 17QRTCh. 6 - Prob. 18QRTCh. 6 - Prob. 19QRTCh. 6 -
Write Lewis structures for
tetracyanoethene,...Ch. 6 - Prob. 21QRTCh. 6 - Prob. 22QRTCh. 6 - Prob. 23QRTCh. 6 - Prob. 24QRTCh. 6 - Prob. 25QRTCh. 6 - Prob. 26QRTCh. 6 - Prob. 27QRTCh. 6 - Prob. 28QRTCh. 6 - Prob. 29QRTCh. 6 - For each pair of bonds, predict which is the...Ch. 6 - Prob. 31QRTCh. 6 - Prob. 32QRTCh. 6 - Which bond requires more energy to break: the...Ch. 6 -
Estimate ΔrH° for forming 2 mol ammonia from...Ch. 6 - Prob. 35QRTCh. 6 - Light of appropriate wavelength can break chemical...Ch. 6 - Prob. 37QRTCh. 6 - Prob. 38QRTCh. 6 - Prob. 39QRTCh. 6 - Acrolein is the starting material for certain...Ch. 6 - Prob. 41QRTCh. 6 - Prob. 42QRTCh. 6 - Write the correct Lewis structure and assign a...Ch. 6 - Prob. 44QRTCh. 6 - Prob. 45QRTCh. 6 - Two Lewis structures can be written for nitrosyl...Ch. 6 - Prob. 47QRTCh. 6 - Prob. 48QRTCh. 6 - Prob. 49QRTCh. 6 - Prob. 50QRTCh. 6 - Several Lewis structures can be written for...Ch. 6 - Prob. 52QRTCh. 6 - Prob. 53QRTCh. 6 - Prob. 54QRTCh. 6 - Prob. 55QRTCh. 6 - Draw resonance structures for each of these ions:...Ch. 6 - Three known isomers exist of N2CO, with the atoms...Ch. 6 - Write the Lewis structure for (a) BrF5 (b) IF5 (c)...Ch. 6 - Write the Lewis structure for
BrF3
XeF4
Ch. 6 - Prob. 60QRTCh. 6 - Prob. 61QRTCh. 6 - Prob. 62QRTCh. 6 - All carbon-to-carbon bond lengths are identical in...Ch. 6 - Prob. 64QRTCh. 6 - Prob. 65QRTCh. 6 - Prob. 66QRTCh. 6 - Prob. 67QRTCh. 6 - Prob. 68QRTCh. 6 - Prob. 69QRTCh. 6 - Prob. 70QRTCh. 6 - Using just a periodic table (not a table of...Ch. 6 - The CBr bond length in CBr4 is 191 pm; the BrBr...Ch. 6 - Prob. 73QRTCh. 6 -
Acrylonitrile is the building block of the...Ch. 6 - Prob. 75QRTCh. 6 - Write Lewis structures for (a) SCl2 (b) Cl3+ (c)...Ch. 6 - Prob. 77QRTCh. 6 - Prob. 78QRTCh. 6 - A student drew this incorrect Lewis structure for...Ch. 6 - This Lewis structure for SF5+ is drawn...Ch. 6 - Tribromide, Br3, and triiodide, I3, ions are often...Ch. 6 - Explain why nonmetal atoms in Period 3 and beyond...Ch. 6 - Prob. 83QRTCh. 6 - Prob. 84QRTCh. 6 - Prob. 85QRTCh. 6 - Prob. 86QRTCh. 6 - Which of these molecules is least likely to exist:...Ch. 6 - Write the Lewis structure for nitrosyl fluoride,...Ch. 6 - Prob. 91QRTCh. 6 - Methylcyanoacrylate is the active ingredient in...Ch. 6 - Aspirin is made from salicylic acid, which has...Ch. 6 - Prob. 94QRTCh. 6 - Prob. 95QRTCh. 6 - Prob. 96QRTCh. 6 - Prob. 97QRTCh. 6 - Prob. 98QRTCh. 6 - Nitrosyl azide, N4O, is a pale yellow solid first...Ch. 6 - Write the Lewis structures for (a) (Cl2PN)3 (b)...Ch. 6 - Nitrous oxide, N2O, is a linear molecule that has...Ch. 6 - The azide ion, N3, has three resonance hybrid...Ch. 6 - Hydrazoic acid, HN3, has three resonance hybrid...Ch. 6 - Prob. 104QRTCh. 6 - Experimental evidence indicates the existence of...Ch. 6 - Prob. 106QRTCh. 6 - Prob. 107QRTCh. 6 - Pipeline, the active ingredient in black pepper,...Ch. 6 - Sulfur and oxygen form a series of 2 anions...Ch. 6 - Prob. 110QRTCh. 6 - Prob. 111QRTCh. 6 - Prob. 112QRTCh. 6 - Prob. 113QRTCh. 6 - Prob. 114QRTCh. 6 - Prob. 115QRTCh. 6 - Prob. 116QRTCh. 6 - Prob. 117QRTCh. 6 - Prob. 118QRTCh. 6 - Prob. 6.ACPCh. 6 - Prob. 6.BCPCh. 6 - Prob. 6.CCP
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
- ii. Answer true or false. (a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9. (b) If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will not form a covalent bond. (c) A covalent bond formed by sharing two electrons is called a double bond. (d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of each hydrogen. (e) In the molecule CH4, each hydrogen has an electron configuration like that of helium, and carbon has an electron configuration like that of neon. (f) In a polar covalent bond, the more electronegative atom has a partial negative charge (8-) and the less electronegative atom has a partial positive charge (&+). (g) These bonds are arranged in order of increasing polarity C-Harrow_forwardWrite the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) COarrow_forwardTwo substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.arrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardWhich statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table . (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forwardA resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.arrow_forwardWhich of the following bonds are polar: (a) P—O; (b) S—F; (c) Br—Br; (d) O—Cl? Which is the more electronegative atom in each polar bond?arrow_forwardCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forwardAn elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardConsider the collection of nonmetallic elements O, P, Te,I, and B. (a) Which two would form the most polar singlebond? (b) Which two would form the longest single bond?(c) Which two would be likely to form a compound of formulaXY2? (d) Which combinations of elements would likelyyield a compound of empirical formula X2Y3?arrow_forwardWrite an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ararrow_forwardConsider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain brieflyarrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_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