Chemistry In Focus
7th Edition
ISBN: 9781337399692
Author: Tro, Nivaldo J.
Publisher: Cengage Learning,
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 5, Problem 4SC
Interpretation Introduction
Interpretation:
The statement, “The Lewis structure of
Concept introduction:
According to VSEPR theory, the geometry of molecules is based on the force of repulsion between the electron pairs in the valence shell. The electron pairs minimize this repulsion by getting as far away from each other as possible.
The number of bonding pairs and lone pairs of electrons determines the shape of the molecule.
The order of force of repulsion between the various electron pairs is as follows:
lone pair-lone pair > lone pair-bond pair > bond pair-bond pair.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Sodium Azide is an ionic compound that is used in automotive air bags. It has the chemical
formula NaN3 (The Azide ion is N , and should not be confused with the Nitride ion,
N°).
a. Give the LEWIS diagram of the Azide ion.
b. What is the geometry of the Azide ion? What is the bond angle of the Azide
ion?
Consider bonding in elemental oxygen and elemental sulfur.
a.Why is O2 more stable as a diatomic molecule than S2?
b.Why does S8 form much more stable ring structure than O8?
6,7,8,9,10 Letters ONLY
Chapter 5 Solutions
Chemistry In Focus
Ch. 5 - Drawing Lewis Structures for Ionic Compounds Draw...Ch. 5 - Using Lewis Structures to Determine the Correct...Ch. 5 - Prob. 5.3YTCh. 5 - Prob. 5.4YTCh. 5 - Drawing Lewis Structures for Covalent Compounds...Ch. 5 - Prob. 5.6YTCh. 5 - Prob. 5.7YTCh. 5 - Prob. 5.8YTCh. 5 - Prob. 5.9YTCh. 5 - Determining if a Molecule Is Polar Is SCl2 a polar...
Ch. 5 - Based on the Lewis structures for hydrogen and...Ch. 5 - Prob. 2SCCh. 5 - Prob. 3SCCh. 5 - Prob. 4SCCh. 5 - Which one of the following bonds is polar? a. a...Ch. 5 - Prob. 6SCCh. 5 - Why is salt, NaCl, relatively harmless even though...Ch. 5 - If sodium is dropped into water, a loud fizzing...Ch. 5 - Explain ionic bonding according to Lewis theory.Ch. 5 - Prob. 4ECh. 5 - Prob. 5ECh. 5 - Prob. 6ECh. 5 - Draw electron dot structures for the following...Ch. 5 - Explain VSEPR theory. According to this theory,...Ch. 5 - Prob. 9ECh. 5 - Prob. 10ECh. 5 - In what ways is water unique? What about the water...Ch. 5 - What is the difference between a polar and a...Ch. 5 - Why do polar molecules have a greater tendency to...Ch. 5 - Prob. 14ECh. 5 - Lewis Structures for Atoms Draw Lewis structures...Ch. 5 - Draw Lewis structures for each of the following...Ch. 5 - Ionic Lewis Structures Draw a Lewis structure for...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Covalent Lewis Structures Draw a Lewis structure...Ch. 5 - Draw a Lewis structure for each molecular...Ch. 5 - General Lewis Structures Determine whether each...Ch. 5 - Determine whether each compound is ionic or...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - Predicting the Shapes of Molecules Use VSEPR...Ch. 5 - Use VSEPR theory to determine the geometry of the...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - CF2Cl2 is a chlorofluorocarbon implicated in ozone...Ch. 5 - Chlorofluorocarbons have been banned because they...Ch. 5 - Determining Molecular Polarity Determine whether...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Explain why water would be a gas at room...Ch. 5 - Prob. 38ECh. 5 - Prob. 39ECh. 5 - One of the observations that led G. N. Lewis to...Ch. 5 - G. N. Lewis developed a model for chemical bonding...Ch. 5 - The opening quote of this chapter states that Man...Ch. 5 - Draw a Lewis structure of the H2 molecule. If you...Ch. 5 - Prob. 44ECh. 5 - The Lewis structures for CH4,N2,andCO2, along with...Ch. 5 - CH3COCH3 (acetone) is a common laboratory solvent...
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
- only 12 and 13arrow_forwardThe formula for nitryl chloride is CINO2 (in which N is the central atom). a.Draw the Lewis structure for the molecule, including all resonance structures. b.What is the N-O bond order? c.Describe the electron-pair and molecular geometries and give values for all bond angles. d.What is the most polar bond in the molecule? Is the molecule polar? e.The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A =-0.03, B = -0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?arrow_forward5. If there are four (4) electron pairs around the central atom of a molecule, these electron pairs are in a arrangement. A. linear B. trigonal planar C. tetrahedral D. octahedral 6. A list of non-metale giver bele K 1Whieharrow_forward
- 2. Identify the true statement. a. Polar covalent compounds result from a complete transfer of at least one electron. b. Sodium is unlikely to form a bond with lithium. c. Covalent compounds exist in large lattices. d. The smallest unit of an ionic compound is a molecule. 3. A piece of zinc metal is placed in an aqueous solution of magnesium sulfate. The products of this reaction are a. ZnMg(s) + SO4(aq) b. Mg(s) + ZnSO4(aq) c. MgS(s) + ZnO4(aq) d. ZnO(s) + MgSO4(aq) e. There will be no reaction. 4. The shape of the NC13 molecule is a. linear b. trigonal planar c. tetrahedral d. trigonal pyramidal e. V-shaped Imi 5. Which of the following would have the highest boiling point? a. NH3 b. PH3 c. AsH3 d. They would all have approximately the same boiling point. 20 6. Aqueous solutions of silver nitrate and sodium sulfate are mixed. The products of the reaction are a. Ag2SO4(aq) + 2 NaNO3(aq) b. AgSO4(s) + Na2(NO3)2(aq) c. Ag2SO4(s) + 2 NaNO3(aq) d. AgSO4(aq) + Na2(NO3 e. There will be no…arrow_forwardConsider the compound xenon dichloride, XeCl2 a.What is the polarity of the molecule? b. What type of bond is the Xe-Cl bond? c. How many bonding pairs of electrons are there?arrow_forwardExplain formation of covalent bonds in the following chemical compounds (using three theories). SO? · HF CC4. C:BrzH2 . H2 CO3.arrow_forward
- o=c=0 ö-s=ö 10. Lewis electron dot diagrams for CO2 and SO2 are given above. Which of the following is true regarding the molecular geometry and the polarity for both substances? A. they are both linear because they only have two non-central atoms B. they are both polar molecules due to the polar bonds between the central atom and oxygen C. the lone pair of electrons on the S atom in SO, make it a polar bent molecule D. they are both nonpolar because the formal charge on each atom is zero 150 to 140 130arrow_forwardThe molecular structure of NCI 3 is A. pyramidal O B. bent C. none of these O D. octahedral O E. trigonal planararrow_forwardThe common name of Si I 4 is tetraiodosilane. What isits molecular compound name?A. silane tetraiodideB. silane tetraiodineC. silicon iodideD. silicon tetraiodidearrow_forward
- Galium (Ga) is an element in group III with atomic number 31. By referring to the Periodic Table, answer the following questions. i. Explain how the atomic radius of gallium differs from aluminum. ii. Explain how the electronegativity of gallium differs from aluminum. iii. Explain how the electronegativity of gallium differs from germanium. iv. Explain how the ionization energy of gallium differs from germanium. v. Explain how the ionization energy of gallium differs from indium.arrow_forwardWhat is the electron- pair geometry of the central oxygen atom of O-Zone (O3) ? Abu U A. Linear B. Trigonal planner C. Tetrahedral D. Trigonal bipyramidal Land okarity isarrow_forward5. In CIF3, the electron pairs are arranged about the chlorine atom in a. a square plane. b. a tetrahedron. c. an octahedron. d. a trigonal pyramid. e. a trigonal bipyramid.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
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
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