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
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 11, Problem 47IAE
A group of spectroscopists believe that they have detected one of the following species: NeF,
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
According to Huckel theory, what is the difference in total energy between the anion (C6H6) and the dication
(C6H6)2+ of Benzene? In your work, explicitly state which orbitals are occupied in case of the anion and the
dictation and what the total energy of each of the two ions is. The total energy difference is defined as
AE =
Eanion
Ea
dication·
O 2a – 23
O 3a + B
O a + B
O 2a + 28
3a - B
Use the data given below to calculate the bond energies (Do) (in eV) of1H35Cl and 1H81Br molecules. Which bond is stronger?
HCl Ve (cm^-1): 2991, De(cm^-1): 53194
HBr Ve(cm^-1):2649 , De(cm^-1): 34570
If the bond in the AB molecule is considered 100% ionic, the absolute value of the partial charge would be equal to the electron charge (1.602 x 10-19 C). If the distance between A and B atoms is taken as 10-10 m (1Å), the dipole moment between two elementary charges of opposite sign at atomic magnitude (1Å) distance between them is = 1.602x10-19 C x 10-10 m = 1.602 x 10- It is available in 29 Cm (or 4.8 x 10-18 esbcm). Dipole moment is given by debye (D) and 1D = 3.34x10-30 Cm (or 1D = 10-18 esbcm) (esb = electrostatic unit).
1. As can be seen, when the HCl covalent molecule is considered ionic and the bond length is 1.27x10-10 m, calculate the dipole moment. The experimental dipole moment of an HCl polar option is = 1.03 D. Calculate the value character of the H-Cl bond according to the bulletin. How many% covalent is the bond, how many% is ionic? Specify
Chapter 11 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 11 - Prob. 1ECh. 11 - Explain why it is necessary to hybridize atomic...Ch. 11 - Describe the molecular geometry of H2O suggested...Ch. 11 - Describe the molecular geometry of NH2 suggested...Ch. 11 - In which of the following, CO32-,SO2,CCl4,CO,NO3-...Ch. 11 - In the manner of Example 11-1, describe the...Ch. 11 - For each of the following species, identify the...Ch. 11 - Propose a plausible Lewis structure, geometric...Ch. 11 - Describe a hybridization scheme for the central Cl...Ch. 11 - Describe a hybridization scheme for the central S...
Ch. 11 - Match each of the following species with one of...Ch. 11 - Propose a hybridization scheme to account for...Ch. 11 - Indicate which of the following molecules and ions...Ch. 11 - In the manner of Figure 11-18, indicate the...Ch. 11 - Write Lewis structures for the following...Ch. 11 - Represent bonding in the carbon dioxide molecule,...Ch. 11 - Use the method of Figure 11-19 to represent...Ch. 11 - Use the method of Figure 11-19 to represent...Ch. 11 - The molecular model below represents citric acid,...Ch. 11 - Malic is e common organic acid found in unripe...Ch. 11 - Shown below are ball-and-stick models. Describe...Ch. 11 - Shown below are ban-and-stick models. Describe...Ch. 11 - Prob. 23ECh. 11 - The structure of the molecule allene, CH2CCH2 , is...Ch. 11 - Angelic acid, shown below, occurs in symbol root,...Ch. 11 - Dimethylolpropionic acid, shown below, is used in...Ch. 11 - Explain the essential difference in how the...Ch. 11 - Describe the bond order of diatomic carbon, C2 ,...Ch. 11 - Prob. 29ECh. 11 - The paramagnetism of gaseous B2 has been...Ch. 11 - Prob. 31ECh. 11 - Is it correct to say that when a diatomic molecule...Ch. 11 - For the following pairs of molecular orbitals,...Ch. 11 - For each of the species C2+,O2,F2+ , and NO+ ; a....Ch. 11 - Write plausible molecular orbital occupancy...Ch. 11 - We have used the term “isoelectronic” to refer to...Ch. 11 - Consider the molecules NO+ and N2+ and use...Ch. 11 - Consider the molecules CO+ and CN- and use...Ch. 11 - Construct the molecular orbital diagram for CF....Ch. 11 - Construct the molecular orbital diagram for SrCl....Ch. 11 - Explain why the concept of delocalized molecular...Ch. 11 - Explain how it is possible to avoid the concept of...Ch. 11 - In which of the following molecules would you...Ch. 11 - In which of the following ions would you expect to...Ch. 11 - The Lewis structure of N2 indicates that the...Ch. 11 - Show that both the valence bond method and...Ch. 11 - A group of spectroscopists believe that they have...Ch. 11 - Lewis theory is satisfactory to explain bonding in...Ch. 11 - The compound potassium sesquoxide has the...Ch. 11 - Draw a Lewis structure for the urea molecule, CO(...Ch. 11 - Methyl nitrate, CH2NO2 , is used as a rocket...Ch. 11 - Fluorine nitrate, FONO2 , is an oxidizing agent...Ch. 11 - Draw a Lewis structure(s) for the nitrite ion, NO2...Ch. 11 - Think of the reaction shown here as involving the...Ch. 11 - Prob. 55IAECh. 11 - Prob. 56IAECh. 11 - The molecule formamide, HCONH2 , has the...Ch. 11 - Pyridine, C2H2N , is used in the synthesis of...Ch. 11 - Prob. 59IAECh. 11 - The ion F2Cl is linear, but the ion F2Cl+ is bent....Ch. 11 - Prob. 61IAECh. 11 - Prob. 62IAECh. 11 - Prob. 63IAECh. 11 - Prob. 64IAECh. 11 - Histidine, an essential amino acid, serves as a...Ch. 11 - The anion I42 is linear, and the anion I5 is...Ch. 11 - Prob. 67IAECh. 11 - A conjugated hydrocarbon has an alternation of...Ch. 11 - An elusive intermediate of atmospheric reactions...Ch. 11 - Resonance energy is the difference in energy...Ch. 11 - Furan, C4H4O , is a substance derivable from oat...Ch. 11 - As discussed in Are You Wondering 11-1, the sp...Ch. 11 - In Chapter 10, we saw that electronegativity...Ch. 11 - Borazine, B2N2H2 is often referred to as inorganic...Ch. 11 - Which of the following combinations of orbitals...Ch. 11 - Prob. 76FPCh. 11 - Prob. 77SAECh. 11 - Prob. 78SAECh. 11 - Explain the important distinctions between the...Ch. 11 - A molecule in which sp2 hybrid orbitals are used...Ch. 11 - Prob. 81SAECh. 11 - The hybridization scheme for the central atom...Ch. 11 - Of the following, the species with a bond order of...Ch. 11 - The hybridization scheme for Xe in XeF2 is (a) sp;...Ch. 11 - Delocalized molecular orbitals are found in (a)...Ch. 11 - Prob. 86SAECh. 11 - Why does the hybridization sp2d not account for...Ch. 11 - What is the total number of (a) bonds and (b) p...Ch. 11 - Which of the following species are paramagnetic?...Ch. 11 - Use the valence molecular orbital configuration to...Ch. 11 - Use the valence molecular orbital configuration to...Ch. 11 - Which of these diatomic molecules do you think has...Ch. 11 - For each of the following ions or molecules,...Ch. 11 - Draw Lewis structures for the NO2 and NO2+ ions,...Ch. 11 - In which of the following is the central atom sp...Ch. 11 - Prob. 96SAECh. 11 - According to molecular orbital theory, the O22 ion...Ch. 11 - What is the angle between the hybrid orbitals...Ch. 11 - Consider the molecule with the Lewis structure...Ch. 11 - Construct a concept map that embodies the ideas of...Ch. 11 - Prob. 101SAECh. 11 - Construct a concept map that describes the...
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
- Suppose that any given kind of bond, such as 0-H, has a characteristic electric dipole. That is, suppose that elec- tric dipole moments can be assigned to bonds just as bond energies can be. Both are usefully accurate approxi- mations. Consider the water molecule H `H Show that if MOH is the dipole moment of the OH bond, then the dipole moment of water is µ(H2O) = 2µ0H cos (0/2). What is the dipole moment µoH if µ(H,O) is 1.86 D?arrow_forwardThe 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. View Available Hint(s) r = μA Value 6 O Units ? Inits input for part Barrow_forwardCalculate the (molar) energy of electrostatic repulsion between two hydrogen nuclei at the separation in H2 (74.1 pm). The result is the energy that must be overcome by the attraction from the electrons that form the bond. Does the gravitational attraction between the nuclei play any significant role? Hint: The gravitational potential energy of two masses is equal to −Gm1m2/r; the gravitational constant G is listed inside the front cover.arrow_forward
- 9. Resonance and hybridization questions. (a) Write valence bond wavefunction for the resonance hybrid HF + H'F (allow for different contributions for each structure). (b) Write valence bond wavefunction for the resonance hybrid CO + Co* + C*o' (allow for different contributions for each structure).arrow_forwardDescribe the location of the maximum electron density of σ- and π-bonds. How is the difference in the spatial arrangement of the electron density of these bonds reflected on their strength?arrow_forward2. Using the ionization energy of H 1s and CI 3p electrons of 13.6 eV and 13.1 eV, respectively, calculate the (a) energies and (b) compositions of the bonding and antibonding orbitals of HCI. (Use aH = -13.6 eV and acı = -13.1 eV.) Use B=-1.0 eV and S=0.arrow_forward
- The correct Lewis structure of the compound "Phosphoryl nitride" is presented in the following schemes. Assuming that the dipole moment is the same for single, double and triple bonds; what would be the correct analysis of the dipole moments of this compound? ði RESULTANT DIPOLE MOMENT O=P=N: đ+arrow_forwardWrite down the Lewis dot structures of each of the following molecules. Check the formal charge in each case and make use of it to decide on the correct structure where necessary. In cases where delocalised bonding occurs show all the resonance forms. In each case show all steps in arriving at the structure.a) CH2Cl2b) CH3CH2NH3+(here the 3 H atoms are attached to one C atom, and 2 H atoms and a Natom to the other C atom)c) CH3NNN (here 3 H atoms and 1 N are attached to the C atom and the N atoms form a 3atom chain). [Challenging: hint, share leftover electron pairs equally between the two Natoms in the middle after you have completed the octet on the end N]d) NCl3e) ClO3−(chlorate anion = chlorine bonded to 3 oxygen atoms, Hint: Cl does not obey theoctet configuration)arrow_forwardWrite the valence-bond wavefunction for the resonance hybrid N2 ↔ N+N− ↔ N2−N2+ ↔ structures of similar energy.arrow_forward
- Calculate the formal charges of all of the atoms in each of the following molecules. Part A CO Enter the charge in the order in which the atoms are numbered. Seperate each charge with a comma. Make sure to include the appropriate "+" or "-" if the charge is not "O. :C=0: Πν ΑΣφarrow_forwardDetermine the partial negative charge on the chlorine atom in a C- Cl bond. The bond length is 1.77 A and the bond dipole moment is 1.50 D. Express your answer using 3 significant figures. ΑΣφ the partial negative charge on the chlorine atom% =arrow_forwardDraw a Lewis structure for the C3Hg molecule using the connectivity shown in the spacefilling 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. Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = Previous 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 = The total number of unshared pairs = Nextarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_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