Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 8, Problem 154CWP
Predict the molecular structure, bond angles, and polarity (has a net dipole moment or has no net dipole moment) for each of the following compounds.
- a. SeCl4
- b. SO2
- c. KrF4
- d. CBr4
- e. IF3
- f. ClF3
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Which of the following molecular formulas, once the BEST lewis structure has been solved, will always lead to a molecule which is polar because it possesses as bet dipole moment?
a. CH4
b. XeF2
c. NH3
d. PCl5
e. CO2
Which of following molecular formulas, once the BEST Lewis structure has been solved, will always lead to a molecule which is polar because it possesses a net dipole moment?
A.
CH4
B.
CO2
C.
NH3
D.
PCl5
E.
XeF2
Which of following molecular formulas, once the BEST Lewis structure has been solved, will always lead to a molecule which is nonpolar because it possesses NO net dipole moment?
A.
H2S
B.
HCN
C.
CS2
D.
SOCl2
E.
SF4
Chapter 8 Solutions
Chemistry
Ch. 8 - Distinguish between the terms electronegativity...Ch. 8 - When an element forms an anion, what happens to...Ch. 8 - Define the term lattice energy. Why,...Ch. 8 - Explain how bond energies can be used to estimate...Ch. 8 - Prob. 5RQCh. 8 - Explain the terms resonance and delocalized...Ch. 8 - Define formal charge and explain how to calculate...Ch. 8 - Give two requirements that should be satisfied for...Ch. 8 - Consider the following compounds: CO2, SO2, KrF2,...Ch. 8 - Explain the electronegativity trends across a row...
Ch. 8 - The ionic compound AB is formed. The charges on...Ch. 8 - Prob. 3ALQCh. 8 - The bond energy for a CH bond is about 413 kJ/mol...Ch. 8 - Prob. 5ALQCh. 8 - Which has the greater bond lengths: NO2 or NO3?...Ch. 8 - The following ions are best described with...Ch. 8 - The second electron affinity values for both...Ch. 8 - What is meant by a chemical bond? Why do atoms...Ch. 8 - Why are some bonds ionic and some covalent?Ch. 8 - How does a bond between Na and Cl differ from a...Ch. 8 - Arrange the following molecules from most to least...Ch. 8 - Does a Lewis structure tell which electron come...Ch. 8 - True or false? In general, a large atom has a...Ch. 8 - What is the central idea of the VSEPR model?Ch. 8 - In Section 8.13 of the text, the term effective...Ch. 8 - Describe the type of bonding that exists in die...Ch. 8 - Some plant fertilizer compounds are (NH4)2SO4,...Ch. 8 - Some of the important properties of ionic...Ch. 8 - What is the electronegativity trend? 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Show all...Ch. 8 - Prob. 94ECh. 8 - Benzene (C6H6) consists of a six-membered ring of...Ch. 8 - Borazine (B3N3H6) has often been called inorganic...Ch. 8 - An important observation supporting the concept of...Ch. 8 - Consider the following bond lengths: CO143pmC9O123...Ch. 8 - A toxic cloud covered Bhopal, India, in December...Ch. 8 - Prob. 103ECh. 8 - Prob. 104ECh. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures for the species in Exercise...Ch. 8 - Oxidation of the cyanide ion produces the stable...Ch. 8 - When molten sulfur reacts with chlorine gas, a...Ch. 8 - Carbon and sulfur form compounds with each other...Ch. 8 - Prob. 112ECh. 8 - Predict the molecular structure and bond angles...Ch. 8 - Predict die molecular structure and bond angles...Ch. 8 - There are several molecular structures based on...Ch. 8 - Two variations of the octahedral geometry (see...Ch. 8 - Prob. 117ECh. 8 - Consider the molecular structures illustrated in...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Prob. 123ECh. 8 - Which of the molecules in Exercise 120 have net...Ch. 8 - Which of the molecules in Exercise 121 have net...Ch. 8 - Which of the molecules in Exercise 122 have net...Ch. 8 - Write Lewis structures and predict the molecular...Ch. 8 - Write Lewis structures and predict whether each of...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Two different compounds exist having the formula...Ch. 8 - Two different compounds have the formula XeF2Cl2....Ch. 8 - Arrange the following in order of increasing...Ch. 8 - For each of the following, write an equation that...Ch. 8 - Use bond energies (table 3-3), values of electron...Ch. 8 - Write Lewis structures for CO32, HCO3, and H2CO3....Ch. 8 - Which member of the following pairs would you...Ch. 8 - What do each of the following sets of...Ch. 8 - Prob. 139AECh. 8 - Although both Br3 and I3 ions are known, the F3...Ch. 8 - Prob. 142AECh. 8 - Which of the following molecules have not dipole...Ch. 8 - Prob. 145AECh. 8 - Look up the energies for the bonds in CO and N2....Ch. 8 - Classify the bonding in each of the following...Ch. 8 - List the bonds PCl, PF, OF, and SiF from least...Ch. 8 - Arrange the atoms and/or ions in the following...Ch. 8 - Use the following data to estimate E for the...Ch. 8 - Use bond energy values to estimate E for the...Ch. 8 - Which of the following compounds or ions exhibit...Ch. 8 - The formulas of several chemical substances are...Ch. 8 - Predict the molecular structure, bond angles, and...Ch. 8 - Use Coulombs Jaw, V=Q1Q240r=2.311019Jnm(Q1Q2r) to...Ch. 8 - Prob. 156CPCh. 8 - Calculate the standard heat of formation of the...Ch. 8 - Given the following information: Energy of...Ch. 8 - Prob. 159CPCh. 8 - Think of forming an ionic compound as three steps...Ch. 8 - The compound NF3 is quite stable, but NCl3, is...Ch. 8 - Three processes that have been used for the...Ch. 8 - The compound hexaazaisowurtzitane is one of the...Ch. 8 - Many times extra stability is characteristic of a...Ch. 8 - The study of carbon-containing compounds and their...Ch. 8 - Draw a Lewis structure for the N,...Ch. 8 - Prob. 167CPCh. 8 - Consider the following computer-generated model of...Ch. 8 - Cholesterol (C27H46O) has the following structure:...Ch. 8 - A compound, XF5, is 42.81% fluorine by mass....Ch. 8 - Identify the following elements based on their...
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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 molecule XF3 has a dipole moment. Is X boron or phosphorus?arrow_forwardHow many central atoms does the molecule H2NCH3 have, and what is the shape about each?arrow_forwardA molecular compound is composed of 58.8% Xe, 7.2%. O, and 34.0%. F, by mass. If the molecular weight is 223 amu, what is the molecular formula? What is the Lewis formula? Predict the molecular geometry using the VSEPR model.arrow_forward
- Why is the geometric structure of a molecule important, especially for biological molecules?arrow_forwardWhich of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments? (a) CIF5 (b) CIO2 (c) TeCI42 (d) PCl3 (e) SeF4 (f) PH2 (g) XeF2arrow_forwardG. N. Lewis developed a model for chemical bonding that you have learned in this chapter. His theory was extremely successful and is used today at all levels of chemistry, from the introductory class to the research laboratory. Why was Lewis theory so successful?arrow_forward
- Write a Lewis structure for each of the following simple molecules. Show all bonding valenceelectron pairs as lines and all nonbonding valence electron pairs as dots.a. H2S b. SiF4 c. C2H4 d. C3H8arrow_forwardWhich of the following molecular formulas, once the BEST lewis structure has been solved, will always lead to a molecule which is no polar because it possesses NO net dipole moment? a. HCN b. SF4 c. CS2 d. H2S e. SOCl2arrow_forwardDetermine the electron geometry, molecular geometry, and ide- alized bond angles for each molecule. In which cases do you ex- pect deviations from the idealized bond angle? a. PF3 b. SB12 c. CHCI3 d. CS2arrow_forward
- 6. Which bond is likely to be polar? A. F2 B. HF C. I2 D. H2arrow_forwardWrite a Lewis structure for each of the following simple molecules. Show all bonding valenceelectron pairs as lines and all nonbonding valence electron pairs as dots.a. H2 b. HCl c. CF4 d. O2arrow_forwardDetermine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. PF3 b. SBr2 c. CHCl3 d. CS2arrow_forward
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