Connect for Chemistry
13th Edition
ISBN: 9781260161854
Author: Raymond Chang, Jason Overby
Publisher: Mcgraw-hill Higher Education (us)
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 9.66QP
In the vapor phase, beryllium chloride consists of discrete BeCl2 molecules. Is the octet rule satisfied for Be in this compound? If not, can you form an octet around Be by drawing another resonance structure? How plausible is this structure?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Some chemists believe that satisfaction of the octet rule should be the top criterion
for choosing the dominant Lewis structure of a molecule or ion. Other chemists
believe that achieving the best formal charges should be the top criterion.
Consider the dihydrogen phosphate ion, HaPO, , in which the H atoms are bonded
to O atoms. (a) What is the predicted dominant Lewis structure if satisfying the
octet rule is the top eriterion? (b) What is the predicted dominant Lewis structure if
achieving the best formal charges is the top criterion?
Complete the following statements about the molecule COS. Please note that ALL atoms in this molecule obey the octet rule.
The molecule COS has total valence electrons.
The molecule COS should be drawn with C in the middle, O to the left of the C, and S to the right of the C.
After drawing the Lewis structure for COS using the above information, it is evident that the three-dimensional shape (or geometry) of the molecule is , with a bond angle of degrees.
3)
The molecule diphosphorus tetraoxide (P,O,) has two central atoms and four different resonance
structures that do not violate the octet rule. Draw two of these resonance structures below.
4)
The compound acetone is a common solvent. It has a chemical formula of CH,COCH, Acetone has
three central atoms.
(a) Draw the Lewis Dot structure for acetone.
(b) Give the Ideal Bond Angle for all three central atoms.
5)
Four covalent molecules are drawn below.
:o:
H.
H-CH
H
H
(1)
(2)
(3)
(4)
a)
Define each of these molecules as polar or non-polar.
(1)
(2)
(3)
b)
Describe the type of intermolecular force that each molecule would use:
(1)
(2)
(3)
(4)
Chapter 9 Solutions
Connect for Chemistry
Ch. 9.1 - Prob. 1RCFCh. 9.1 - Using only the periodic table, determine the Lewis...Ch. 9.1 - To what group on the periodic table does element X...Ch. 9.2 - Use Lewis dot symbols to represent the formation...Ch. 9.2 - Use Lewis dot symbols to represent the formation...Ch. 9.3 - Which of the following compounds has a larger...Ch. 9.3 - Arrange the compounds NaF, MgO, and AIN in order...Ch. 9.4 - Why is it not possible for hydrogen to form double...Ch. 9.4 - Arrange the bonds NN, NN, and NN in order of...Ch. 9.5 - Which of the following bonds is covalent, which is...
Ch. 9.5 - Rank the bonds BH, CCl, and PP in order of...Ch. 9.5 - Classify the following bonds as covalent, polar...Ch. 9.5 - Identify the electrostatic potential maps shown...Ch. 9.6 - Write the Lewis structure for carbon disulfide...Ch. 9.6 - Write the Lewis structure for formic acid (HCOOH).Ch. 9.6 - Write the Lewis structure for the nitrite ion...Ch. 9.6 - Write the Lewis structure for PCl3.Ch. 9.6 - Write the Lewis structure for CN.Ch. 9.6 - The molecular model shown here represents guanine,...Ch. 9.7 - Write formal charges for the nitrite ion (NO2).Ch. 9.7 - Draw the most reasonable Lewis structure of a...Ch. 9.7 - Write the formal charges on H, C, and N,...Ch. 9.7 - Write the formal charges on O and Cl,...Ch. 9.7 - Consider three possible atomic arrangements for...Ch. 9.8 - Draw three resonance structures for the...Ch. 9.8 - Draw three resonance structures for SO2.Ch. 9.8 - The molecular model shown here represents...Ch. 9.9 - Prob. 9PECh. 9.9 - Prob. 10PECh. 9.9 - Prob. 11PECh. 9.9 - Write the Lewis structure of sulfur tetrafluoride...Ch. 9.9 - Both boron and aluminum tend to form compounds in...Ch. 9.9 - Draw a Lewis structure for IF5.Ch. 9.9 - Prob. 3RCFCh. 9.10 - Calculate the enthalpy of the reaction...Ch. 9.10 - For the reaction H2(g)+C2H4(g)C2H6(g) (a) Estimate...Ch. 9.10 - Why does Hrxn calculated using bond enthalpies not...Ch. 9.10 - Using bond enthalpy values, predict the enthalpy...Ch. 9 - What is a Lewis dot symbol? To what elements does...Ch. 9 - Use the second member of each group from Group 1A...Ch. 9 - Prob. 9.3QPCh. 9 - Write Lewis dot symbols for the following ions:...Ch. 9 - Write Lewis dot symbols for the following atoms...Ch. 9 - Explain what an ionic bond is.Ch. 9 - Prob. 9.7QPCh. 9 - Name five metals and five nonmetals that are very...Ch. 9 - Name one ionic compound that contains only...Ch. 9 - Name one ionic compound that contains a polyatomic...Ch. 9 - Prob. 9.11QPCh. 9 - In which of the following states would NaCl be...Ch. 9 - Prob. 9.14QPCh. 9 - An ionic bond is formed between a cation A+ and an...Ch. 9 - Prob. 9.16QPCh. 9 - Use Lewis dot symbols to show the transfer of...Ch. 9 - Prob. 9.18QPCh. 9 - For each of the following pairs of elements, state...Ch. 9 - Prob. 9.20QPCh. 9 - What is lattice energy and what role does it play...Ch. 9 - Explain how the lattice energy of an ionic...Ch. 9 - Specify which compound in the following pairs of...Ch. 9 - Compare the stability (in the solid state) of the...Ch. 9 - Use the Born-Haber cycle outlined in Section 9.3...Ch. 9 - Calculate the lattice energy of calcium chloride...Ch. 9 - What is Lewiss contribution to our understanding...Ch. 9 - Use an example to illustrate each of the following...Ch. 9 - What is the difference between a Lewis dot symbol...Ch. 9 - How many lone pairs are on the underlined atoms in...Ch. 9 - Compare single, double, and triple bonds in a...Ch. 9 - Compare the properties of ionic compounds and...Ch. 9 - Define electronegativity, and explain the...Ch. 9 - List the following bonds in order of increasing...Ch. 9 - Arrange the following bonds in order of increasing...Ch. 9 - Four atoms are arbitrarily labeled D, E, F, and G....Ch. 9 - List the following bonds in order of increasing...Ch. 9 - Classify the following bonds as ionic, polar...Ch. 9 - Classify the following bonds as ionic, polar...Ch. 9 - Summarize the essential features of the Lewis...Ch. 9 - The octet rule applies mainly to the second-period...Ch. 9 - Write Lewis structures for the following molecules...Ch. 9 - Write Lewis structures for the following molecules...Ch. 9 - Write Lewis structures for the following...Ch. 9 - Write Lewis structures for the following...Ch. 9 - The following Lewis structures for (a) HCN, (b)...Ch. 9 - The skeletal structure of acetic acid shown here...Ch. 9 - Prob. 9.49QPCh. 9 - Do formal charges represent actual separation of...Ch. 9 - Write Lewis structures for the following ions: (a)...Ch. 9 - Write Lewis structures for the following ions: (a)...Ch. 9 - Define bond length, resonance, and resonance...Ch. 9 - Is it possible to trap a resonance structure of a...Ch. 9 - Write Lewis structures for the following species,...Ch. 9 - Draw three resonance structures for the chlorate...Ch. 9 - Write three resonance structures for hydrazoic...Ch. 9 - Draw two resonance structures for diazomethane,...Ch. 9 - Draw three resonance structures for the molecule...Ch. 9 - Draw three reasonable resonance structures for the...Ch. 9 - Why does the octet rule not hold for many...Ch. 9 - Give three examples of compounds that do not...Ch. 9 - Because fluorine has seven valence electrons...Ch. 9 - What is a coordinate covalent bond? Is it...Ch. 9 - Prob. 9.65QPCh. 9 - In the vapor phase, beryllium chloride consists of...Ch. 9 - Of the noble gases, only Kr, Xe, and Rn are known...Ch. 9 - Write a Lewis structure for SbCl5. Does this...Ch. 9 - Prob. 9.69QPCh. 9 - Write Lewis structures for the reaction...Ch. 9 - What is bond enthalpy? Bond enthalpies of...Ch. 9 - Explain why the bond enthalpy of a molecule is...Ch. 9 - From the following data, calculate the average...Ch. 9 - For the reaction O(g)+O2(g)O3(g)H=107.2kJ/mol...Ch. 9 - The bond enthalpy of F2(g) is 156.9 kJ/mol....Ch. 9 - For the reaction 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g)...Ch. 9 - Prob. 9.77QPCh. 9 - Which of the following are ionic compounds? Which...Ch. 9 - Prob. 9.79QPCh. 9 - Use ionization energy (see Table 8.2) and electron...Ch. 9 - Prob. 9.82QPCh. 9 - Prob. 9.83QPCh. 9 - Write three reasonable resonance structures for...Ch. 9 - Prob. 9.85QPCh. 9 - Give an example of an ion or molecule containing...Ch. 9 - Draw four reasonable resonance structures for the...Ch. 9 - Prob. 9.88QPCh. 9 - Draw reasonable resonance structures for the...Ch. 9 - Are the following statements true or false? (a)...Ch. 9 - Prob. 9.91QPCh. 9 - Using the following information and the fact that...Ch. 9 - Prob. 9.93QPCh. 9 - Which of the following molecules has the shortest...Ch. 9 - Most organic acids can be represented as RCOOH,...Ch. 9 - Which of the following species are isoelectronic:...Ch. 9 - The following species have been detected in...Ch. 9 - The amide ion, NH2, is a Brnsted base. Represent...Ch. 9 - Draw Lewis structures for the following organic...Ch. 9 - The triiodide ion (I3) in which the I atoms are...Ch. 9 - Compare the bond enthalpy of F2 with the energy...Ch. 9 - Methyl isocyanate (CH3NCO) is used to make certain...Ch. 9 - Prob. 9.103QPCh. 9 - Prob. 9.104QPCh. 9 - Prob. 9.105QPCh. 9 - Draw Lewis structures for the following...Ch. 9 - Prob. 9.107QPCh. 9 - Prob. 9.108QPCh. 9 - Draw Lewis structures for the following organic...Ch. 9 - Write Lewis structures for the following four...Ch. 9 - Prob. 9.111QPCh. 9 - Prob. 9.112QPCh. 9 - Write three resonance structures for (a) the...Ch. 9 - (a) From the following data calculate the bond...Ch. 9 - Prob. 9.115QPCh. 9 - What are the other two reasons for choosing (b) in...Ch. 9 - Prob. 9.117QPCh. 9 - The NO bond distance in nitric oxide is 115 pm,...Ch. 9 - Prob. 9.119QPCh. 9 - Prob. 9.120QPCh. 9 - Prob. 9.121QPCh. 9 - Prob. 9.122QPCh. 9 - Draw a Lewis structure for nitrogen pentoxide...Ch. 9 - In the gas phase, aluminum chloride exists as a...Ch. 9 - The hydroxyl radical (OH) plays an important role...Ch. 9 - Experiments show that it takes 1656 kJ/mol to...Ch. 9 - Calculate Hrxn at 25C of the reaction between...Ch. 9 - Calculate Hrxn at 25C of the reaction between...Ch. 9 - Draw three resonance structures of sulfur dioxide...Ch. 9 - Vinyl chloride (C2H3Cl) differs from ethylene...Ch. 9 - Prob. 9.131QPCh. 9 - The American chemist Robert S. Mulliken suggested...Ch. 9 - Prob. 9.133QPCh. 9 - A student in your class claims that magnesium...Ch. 9 - Shown here is a skeletal structure of borazine...Ch. 9 - Calculate the wavelength of light needed to carry...Ch. 9 - Prob. 9.137QPCh. 9 - From the lattice energy of KCl in Table 9.1 and...Ch. 9 - The species H3+ is the simplest polyatomic ion....Ch. 9 - The bond enthalpy of the CN bond in the amide...Ch. 9 - In 1999 an unusual cation containing only nitrogen...Ch. 9 - Nitroglycerin, one of the most commonly used...Ch. 9 - Give a brief description of the medical uses of...Ch. 9 - Prob. 9.144QPCh. 9 - The isolated O2 ion is unstable so it is not...Ch. 9 - When irradiated with light of wavelength 471.7 nm,...Ch. 9 - Recall from Chapter 8 that the product of the...Ch. 9 - The reaction between fluorine (F2) with ethane...Ch. 9 - A new allotrope of oxygen, O4, has been reported....Ch. 9 - Because bond formation is exothermic, when two...Ch. 9 - Estimate Hf for sodium astatide (NaAt) according...
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
- the formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?arrow_forwardSulfur and oxygen form a series of 2 anions including sulfite, SO32, and sulfate, SO42. In addition to these, there are three other more complex anionsdithionite, S2O42, dithionate, S2O62, and tetrathionate, S4O62. Write correct Lewis structures for dithionite, dithionate, and tetrathionate ions.arrow_forwardMethylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is In this molecule, which is the (a) weakest carbon-containing bond? (b) strongest carbon-containing bond? (c) most polar bond?arrow_forward
- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardDraw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- Two Lewis structures can be written for nitrosyl fluoride, which contains one nitrogen, one oxygen, and one fluorine atom per molecule. Write the two Lewis structures land assign a formal charge to each atom.arrow_forwardChloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.arrow_forwardAlthough I3- is a known ion, F3- is not. (a) Draw the Lewis structure for I3- (it is linear, not a triangle). (b) One of your classmates says that F3 - does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says F3- does not exist because it would violate the octet rule.Is this classmate possibly correct? (d) Yet another classmatesays F3- does not exist because F is too small to make bonds tomore than one atom. Is this classmate possibly correct?arrow_forward
- In nitryl chloride (NO2Cl), the chlorine atom and the twooxygen atoms are bonded to a central nitrogen atom, andall the atoms lie in a plane. Draw the two electron dot resonance forms that satisfy the octet rule and that together areconsistent with the fact that the two nitrogen–oxygenbonds are equivalent.arrow_forwardThe cyanate ion (OCN- ) and the fulminate ion (CNO- ) share the same three atoms but have vastly different properties. The cyanate ion is stable, while the fulminate ion is unstable and forms explosive compounds. The resonance structures of the cyanate ion are explored in Example 9.8. Draw Lewis structures for the fulminate ion—including possible resonance forms— and use formal charge to explain why the fulminate ion is less stable (and therefore more reactive) than the cyanate ion.arrow_forwardIn nitryl chloride (NO2Cl), the chlorine atom and the two oxygen atoms are bonded to a central nitrogen atom, and all the atoms lie in a plane. Draw the two electron dot resonance forms that satisfy the octet rule and that together are consistent with the fact that the two nitrogen–oxygen bonds are equivalent.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher: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
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
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