Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Chapter 3, Problem 3.37P
The Cl...Cl distance in
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The dipole moment (u) of HBr (a polar covalent molecule) is 0.824D (debye), and its percent ionic character is 12.2 %. Estimate the bond length of the H-Br bond in picometers.
Note that
. 1 D 3.34 x 10-30 Cm and
in a bond with 100% ionic character, Q=1.6 x 10-19 C.
Express your answer to two significant figures and include the appropriate units.
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r =
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Inits input for part B
Draw a Lewis structure for the C4Hg molecule usıng the connectivity shown in the spacefillıng model in the window.
Gray = C; white = H; red = 0; blue = N; dark green = Cl; brown = Br; light green = F; purple = I; yellow = S; orange = P.
%3D
Use your drawing to answer the following questions.
The total number of electrons in C-H bonds =
The number of C-C single bonds =|
The number of C=C double bonds =
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The total number of unshared pairs
%3D
Which 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?
Chapter 3 Solutions
Inorganic Chemistry
Ch. 3.1 - Use electron-dot diagrams and formal charges to...Ch. 3.2 - Predict the structures of the following ions....Ch. 3.2 - Prob. 3.3ECh. 3.2 - Which molecule has the smallest bond angle in each...Ch. 3.2 - Briefly account for the following observations: a....Ch. 3.2 - Does this approach work for different steric...Ch. 3 - The dimethyldithiocarbamate ion, [S2CN( CH 3 )2]-...Ch. 3 - Several resonance structures are possible for each...Ch. 3 - Draw the resonance structures for the...Ch. 3 - Three isomers having the formula N2CO are known:...
Ch. 3 - Show the possible resonance structures for nitrous...Ch. 3 - Nitric acid, which exists as HNO3 molecules in the...Ch. 3 - L. C. Allen has suggested that a more meaningful...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Explain the trends in bond angles and bond lengths...Ch. 3 - Select from each set the molecule or ¡on having...Ch. 3 - a. Compare the structures of the azide ion, N3 ,...Ch. 3 - Consider the series OCl2,O( CH3)2 , and O( SiH3)2...Ch. 3 - Two ions isoelectronic with carbon suboxide, C3O2...Ch. 3 - Explain the following: a. Ethylene, C2H4 , is a...Ch. 3 - Explain the following: a. PCI5 is a stable...Ch. 3 - X-ray crystal structures of ClOF3 and BrOF3 have...Ch. 3 - Make the following comparisons about the molecules...Ch. 3 - Prob. 3.20PCh. 3 - A solution containing the lO2F2 ion reacts slowly...Ch. 3 - The XeOF3 anion has been reported recently (D. S....Ch. 3 - Predict the structure of l(CF3)Cl2 . Do you expect...Ch. 3 - a. Which has the longer axial PF distance, PF2(...Ch. 3 - Prob. 3.25PCh. 3 - SeCl62,TeCl62 , and CIF6 are all octahedral, but...Ch. 3 - Prob. 3.27PCh. 3 - The thiazyldichloride ion, NSCl2- , is...Ch. 3 - Sketch the most likely structure of PCl3Br2 and...Ch. 3 - a. Are the CF3 groups in PCl3( CF3)2 more likely...Ch. 3 - Of the molecules C1SO2CH3,C1SO2CF3 , and ClSO2CCl3...Ch. 3 - Prob. 3.32PCh. 3 - Prob. 3.33PCh. 3 - Prob. 3.34PCh. 3 - Prob. 3.35PCh. 3 - Although the CF distances and the FCF bond angles...Ch. 3 - The Cl...Cl distance in CCl4 is 289 pm, and the...Ch. 3 - The FCF angle in F2CO , shown here, is 109.5°; the...Ch. 3 - Compounds in which hydrogen is the outer atom can...Ch. 3 - For each of the following bonds, indicate which...Ch. 3 - Give Lewis dot structures and shapes for the...Ch. 3 - Give Lewis dot structures and sketch the shapes...Ch. 3 - Which of the molecules in Problem 3.41 are polar?Ch. 3 - Which of the molecules in Problem 3.42 are polar?Ch. 3 - Prob. 3.45PCh. 3 - Prob. 3.46P
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- why the C-O bond distance is nearly identical in CO (113 pm) and CO+ (112 pm)?arrow_forwardWhat is the magnitude of the partial positive and partial negative charges in the HI molecule? (1D = 3.36 x 10¬30 c m; 1e¯ = 1.6022 x 10-19 C; bond length HI = 1.61 angstroms; dipole moment HI = 0.44 D)arrow_forwardThe length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) C≡O(B) C-O ...... (A,B) fill in the blank 1(C) N=N(D) N≡N ...... (C,D) fill in the blank 2arrow_forward
- For each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-Narrow_forwardI have to fill out this graph but I'm not sure how to. The options are for the blanks are: Linear (AX2), Trigonal Planar (AX3), Bent (AX2E), tetrahedral (AX4), Trig pyramidal (AX3E), Trig bipyramidal (AX5), SeeSaw (AX4E), T-shaped (AX3E2), square pyramidal (AX5E), square planar (AX4E2), 180, 120, <120, 109.5, 90 and 120, <90 and <120, <90, 90, <180arrow_forwardThe bond energy of C2 is 599 kJ/mol, the bond distance is 110 pm. Take a rough estimate of the Coulomb repulsion in doubly ionized C2 (i.e., C22+). How far would the C-C bond have to stretch for the Coulomb repulsion to be less than the bond energy in neutral C2? Do you think that the C22+ molecule will still be stable?arrow_forward
- 3. Carbon atoms will bond with each other to form a chain, often with the peripheral atoms being hydrogen. These compounds, hydrocarbons, are organic compounds composed only of carbon and hydrogen. However, when hydrogen atoms are substituted with other elements, such as fluorine, this changes the properties of the molecule. Methylfluoride (CH3F), a substituted hydrocarbon, is used in semiconductor processing. Figure 1 depicts an incorrect Lewis structure for CH3F. (QUestion shown in photo) Which reason best explains why this structure is incorrect? a) Hydrogen lacks an octet. b) Too few electrons are used. c) Carbon cannot exceed an octet. d) Fluorine atom has too many electrons.arrow_forwardDraw the Lewis structure of C2H4CI2 (both Cl atoms on one C atom) and then determine if the molecule is polar or nonpolar.arrow_forwardPredicting deviations from ideal bond angles Consider the nitrogen trifluoride (NF3) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the nitrogen-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-fluorine bonds to be ... 0 口。 (choose one) (choose one) about the same bigger smallerarrow_forward
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