Yes, it's a reasonable structure.No, the total number of valence electrons is wrong.The correct number is:O No, some atoms have the wrong number of electrons around them.The symbols of the problem atoms are:NHỊ [H-N=H]* If two or more atoms have the wrong number of valence electrons around them, just enter the chemicalsymbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number ofelectrons around them, enter the symbol O twice.

H-atom can only form a single bond. H cannot form double or triple bond.

NH₂ H-N=H Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

NH₂ H-N=H Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 107CWP: Complete a Lewis structure for the compound shown below, then answer the following questions. What...

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The valence shell of an atom in a legitimate Lewis structure (see Figure 2.3) has what in commonwith the valence shell of a noble gas? (Noble gases are stable elements found in the last column ofthe periodic table, e.g., He, Ne, Ar, etc.)
The compound whose molecles contain one atom of C and one of O is named carbon monoxide rather than oxygen monocarbide. Why is this the case?
Complete a Lewis structure for the compound shown below, then answer the following questions. What are the predicted bond angles about the carbon and nitrogen atoms? How many lone pairs of electrons are present in the Lewis structure? How many double bonds are present?
Follow the directions of Question 55 for the following polyatomic ions. (a) ClF4- (b) GeCl62- (c) SbCl4-
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
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hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.
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Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure for aspartame is shown below. Aspartame can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure above to give each atom a formal charge of zero when drawing the Lewis structure. Also note that the six-sided ring is shorthand notation for a benzene ring (C6H5). Benzene is discussed in Section 4-7. Complete the Lewis structure for aspartame. How many C and N atoms exhibit sp1 hybridization? How many C and O atoms exhibit sp3 hybridization? How many and bonds are in aspartame?
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H20Sketch the proper Lewis structure for this substance. Be sure to follow octet/duet rules for each atom and use the totalnumber of valence electrons available. Use your drawing to answer the following questions.Count the number of each type of electron domain surrounding the central atom. Do not leave any blank empty. enter O if itis unused.Lone pairs: Single bonds: Double bonds: Triple bonds: Count the total number of electron domains surrounding the central atom. Enter the name corresponding to the electron domain geometry. Options are: linear, trigonal planar, tetrahedral.