General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
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Textbook Question
Chapter 10, Problem 52E
Draw Lewis structures for the following species, indicating formal charges and resonance where applicable:
a.
b.
c.
d.
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Students have asked these similar questions
1. SiHA
2. CHO;
3. NO+
4. S2,2-
5. NOCI
Draw the following:
1. Lewis structure
2. Assign formal charges (for elements with non-zero formal charges only).
3. Draw resonance forms (if applicable), pick the most plausible structure (if possible) on the basis of formal charge and electronegativity.
We can draw three inequivalent Lewis structures for the tellurite ion, TeO3²- . The concepts of formal
charge and electronegativity can help us choose the structure that is the best representation.
1. Assign formal charges to the elements in each of the structures below.
Note: Count oxygen atoms starting from the left for each structure.
Formal Charge
Te
01
02
03
Te
Te
Te
:0:
B
C
2. The best Lewis structure for TeO3²¯ is |
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For CIO,OH, write a resonance structure with the octet rule satisfied for the central atom and a second resonance structure that
minimizes formal charges. In the one that satisfies the octet rule, which atoms have a formal charge of zero?
Select one or more:
Da. H
a b. CI
C. The 3 equilvalent O.
d. The O bonded to the H.
x x >
Chapter 10 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 10 - Write Lewis symbols for the following atoms. (a)...Ch. 10 - Write Lewis symbols for the following ions. (a)...Ch. 10 - Write plausible Lewis structures for the following...Ch. 10 - Each of the following molecules contains at least...Ch. 10 - By means of Lewis structures, represent bonding...Ch. 10 - Which of the following have Lewis structures that...Ch. 10 - Prob. 7ECh. 10 - Suggest reasons why the following do not exist as...Ch. 10 - Describe what is wrong with each of the following...Ch. 10 - Describe what is wrong with each of the following...
Ch. 10 - Prob. 11ECh. 10 - Indicate what is wrong with each of the following...Ch. 10 - Write Lewis structures for the following ionic...Ch. 10 - Under appropriate conditions, both hydrogen and...Ch. 10 - Derive the correct formulas for the following...Ch. 10 - Each of the following ionic compounds consists of...Ch. 10 - Assign formal charges to each of the atoms in the...Ch. 10 - Assign formal charges to each of the atoms in the...Ch. 10 - Both oxidation state and formal charge involve...Ch. 10 - Prob. 20ECh. 10 - Prob. 21ECh. 10 - Assign formal charges to the atoms in the...Ch. 10 - Prob. 23ECh. 10 - Show that the idea of minimizing the formal...Ch. 10 - Write acceptable Lewis structures for the...Ch. 10 - Two molecules that have the same formulas but...Ch. 10 - The following polyatomic anions involve covalent...Ch. 10 - Represent the following ionic compounds by Lewis...Ch. 10 - Write a plausible Lewis structure for...Ch. 10 - Prob. 30ECh. 10 - Write Lewis structures for the molecules...Ch. 10 - Write Lewis structures for the molecules...Ch. 10 - Write Lewis structures for the molecules...Ch. 10 - Write Lewis structures for the molecules...Ch. 10 - Identify the main group that the element X belongs...Ch. 10 - Prob. 36ECh. 10 - Use your knowledge of electronegativities, but do...Ch. 10 - Which of the blowing molecules would you expect to...Ch. 10 - What is the percent ionic character of each of the...Ch. 10 - Prob. 40ECh. 10 - Prob. 41ECh. 10 - Use a cross-base arrow () to represent the...Ch. 10 - Which electrostatic potential map corresponds to...Ch. 10 - Prob. 44ECh. 10 - Two electrostatic potential maps are shown, one...Ch. 10 - Prob. 46ECh. 10 - Prob. 47ECh. 10 - Which of the following species requires a...Ch. 10 - Dinitrogen oxide (nitrous oxide, or "laughing...Ch. 10 - The Lewis structure of nitric acid, HONO2, is a...Ch. 10 - Draw Lewis structures for the following species,...Ch. 10 - Draw Lewis structures for the following species,...Ch. 10 - Write plausible Lewis structures for the following...Ch. 10 - Write plausible Lewis structures for the following...Ch. 10 - Which of the following species would you expect to...Ch. 10 - Write a plausible Lewis structure for NO2 , and...Ch. 10 - In which of the following species is it necessary...Ch. 10 - Prob. 58ECh. 10 - Use VSEPR theory to predict the geometric shapes...Ch. 10 - Use VSEPR theory to predict the geometric shapes...Ch. 10 - Each of the following is either linear, angular...Ch. 10 - Predict the geometric shapes of (a) CO ; (b)...Ch. 10 - One of the following ions has a trigonal-planer...Ch. 10 - Two of the following have the same shape. Which...Ch. 10 - Prob. 65ECh. 10 - Sketch the probable geometric shape of molecule of...Ch. 10 - Use the VSEPR theory to predict the shapes of the...Ch. 10 - Use the VSEPR theory to predict the shape of (a)...Ch. 10 - The molecular shape of BF2 is planar (see Table...Ch. 10 - Explain why it is not necessary to find the Lewis...Ch. 10 - Comment on the similarities and differences in the...Ch. 10 - Comment on the similarities and differences in the...Ch. 10 - Draw a plausible Lewis structure for the following...Ch. 10 - Draw a plausible Lewis structure for the following...Ch. 10 - Sketch the propyne molecule, CH2CCH. Indicate the...Ch. 10 - Sketch the propene molecule, CH2CHCH2. Indicate...Ch. 10 - Lactic acid has the formula CH2CH(OH)COOH. Sketch...Ch. 10 - Levulinic acid has the formula CH2(CO)CH2CH2COOH....Ch. 10 - Prob. 79ECh. 10 - Prob. 80ECh. 10 - Predict the shapes of the following molecules, and...Ch. 10 - Which of the blowing molecules would you expect to...Ch. 10 - The molecule H2O2 has a resultant dipole moment of...Ch. 10 - Prob. 84ECh. 10 - Without referring to tables in the text, indicate...Ch. 10 - Estimate the lengths of the blowing bonds and...Ch. 10 - A relationship between bond lengths and...Ch. 10 - In which of the following molecules would you...Ch. 10 - Prob. 89ECh. 10 - Prob. 90ECh. 10 - A reaction involved in the formation of ozone the...Ch. 10 - Use data from Table 10.3, but without performing...Ch. 10 - Use data from Table 10.3 to estimate the enthalpy...Ch. 10 - One of the chemical reactions that occurs in the...Ch. 10 - Estimate the standard enthalpies of formation at...Ch. 10 - Prob. 96ECh. 10 - Use bond energies from Table 10.3 to estimate rH...Ch. 10 - Equations (1) end (2) can be combined to yield the...Ch. 10 - One reaction involved in the sequence of reactions...Ch. 10 - Prob. 100ECh. 10 - Given the bond-dissociation energies:...Ch. 10 - Prob. 102IAECh. 10 - Prob. 103IAECh. 10 - Prob. 104IAECh. 10 - Prob. 105IAECh. 10 - Draw Lewis structures for two different molecules...Ch. 10 - Sodium azide, NaN2 is the nitrogen gas-forming...Ch. 10 - Prob. 108IAECh. 10 - Prob. 109IAECh. 10 - A few years ago the synthesis of a salt containing...Ch. 10 - Prob. 111IAECh. 10 - In certain polar solvents, PCI, undergoes an...Ch. 10 - Prob. 113IAECh. 10 - Prob. 114IAECh. 10 - Use the VSEPR theory to predict a probable shape...Ch. 10 - The standard enthalpy of formation of...Ch. 10 - Prob. 117IAECh. 10 - Prob. 118IAECh. 10 - Prob. 119IAECh. 10 - R. S. Mulliken proposed that the electronegativity...Ch. 10 - When molten sulfur reacts with chlorine gas, a...Ch. 10 - Hydrogen azide, HN2 , can exist in two forms. One...Ch. 10 - Prob. 123IAECh. 10 - Prob. 124IAECh. 10 - Prob. 125IAECh. 10 - One of the allotropes of sulfur is a ring of eight...Ch. 10 - One of the allotropes of phosphorus consists of...Ch. 10 - In this problem, we examine the basis of three...Ch. 10 - Prob. 129FPCh. 10 - Prob. 130FPCh. 10 - Prob. 131SAECh. 10 - Briefly describe each of the following ideas: (a)...Ch. 10 - Explain the important distinctions between (a)...Ch. 10 - Prob. 134SAECh. 10 - The formal charges on the O atoms in the ion...Ch. 10 - Which molecule is nonlinear?...Ch. 10 - Which molecule is nonpolar?...Ch. 10 - The highest bond-dissociation energy is found in...Ch. 10 - The greatest bond length is found in...Ch. 10 - Draw plausible Lewis structures for the blowing...Ch. 10 - Predict the shapes of the following...Ch. 10 - Which of the following ionic compounds is composed...Ch. 10 - Which of the following molecules does not obey the...Ch. 10 - Which of the following molecules has no polar...Ch. 10 - The electron-group geometry of H2O is (a)...Ch. 10 - For each of the following compounds, give the...Ch. 10 - Use bond enthalpies from Table 10.3 to determine...Ch. 10 - Prob. 148SAECh. 10 - Prob. 149SAECh. 10 - What is the VSEPR theory? On what physical basis...Ch. 10 - Prob. 151SAECh. 10 - Prob. 152SAECh. 10 - Prob. 153SAECh. 10 - Prob. 154SAE
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- Write Lewis structures for the following: (a) H2 (b) HBr (c) PCl3 (d) SF2 (e) H2CCH2 (f) HNNH (g) H2CNH (h) NO (i) N2 (j) CO (k) CNarrow_forwardDraw the structure of hydroxylamine, H3NO, and assign formal charges; look up the structure. Is the actual structure consistent with the formal charges?arrow_forwardConsider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forward
- Bond 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_forwardA common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.arrow_forwardWrite Lewis formulas for the BF molecule (two with a single BF bond, two with a double BF bond, and one with a triple BF bond) in which the octet rule is satisfied for at least one of the atoms. Obtain the formal charges of the atoms. Based on the information you have, is there one formula that you think best describes the molecule? Explain. For this best Lewis formula, give the valence bond description of the bonding.arrow_forward
- Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule: (a) IF (b) IF3 (c) IF5 (d) IF7arrow_forwardWe can draw three inequivalent Lewis structures for the arsenite ion , AsO3. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. 3- As O: :0: :0: :O: B Formal Charge As 01 02 03 2. The best Lewis structure for AsO, is Submit Answer Try Another Version 2 item attempts remaining Previous Next Email InstruCarrow_forwardDraw the Lewis structure (with formal charges) of the chemical species: 1. CINO2 (N is the central atom) 2. CO3^2- 3. NO2- 4. SO3 5. BrNO2 (N is the central atom) 6. HCO3- (H is bonded to one of the O's) 7. SeO2 8. HC2O4- (each C has two O atoms and H is on one of the O's) 9. HNO3 (H is bonded to one of the O's) 10. CH3NO2 11. HCO2- (H and both O's are bonded to C)arrow_forward
- References] Consider the following reaction: H. H. CI CI CC (9) + CLg) H-C-C-H( AH-172 kJ H. H H Estimate the carbon-chlorine bond energy given that the C-0 bond energy is 347 /mol, the 0-C bond energy is 614 kJmol, and the Cl-O1 bond energy is 239 KJmol. Doa Umolarrow_forwardWe can draw three inequivalent Lewis structures for the arsenite ion, AsO3¹. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge As 01 -0₂ 03 FO: As. -Ö: A :0³ 2. The best Lewis structure for AsOy is FO: As. :0: B 0. As. :0: с 10: Nextarrow_forwardH 2 H. + ::H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group в (red). In this representation, each Y atom needs bond(s) with atoms of H. electron(s) to complete its octet, and gains these electrons by forming There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are Submit Answer Retry Entire Grouparrow_forward
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