Given Ammonium, NH4*1. The most electronegative element is b. Draw the skeletal structure, showing one bond between each terminal atom to the center а. but the center element has to be atom. С. The total number of valence electrons for this molecule is d. After subtracting 2 electrons per bond used in part (b) above, the number of electrons left is

Given Ammonium, NH4*1. The most electronegative element is b. Draw the skeletal structure, showing one bond between each terminal atom to the center а. but the center element has to be atom. С. The total number of valence electrons for this molecule is d. After subtracting 2 electrons per bond used in part (b) above, the number of electrons left is

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 6CTQ: It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how...

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It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+
In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
What is the maximum number of atoms to which a central atom in a molecule can bond and still conform to the octet rule? What is the minimum number?
the formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?
Complete the following statements about the molecule COS. Please note that ALL atoms in this molecule obey the octet rule. The molecule COS has total valence electrons. The molecule COS should be drawn with C in the middle, O to the left of the C, and S to the right of the C. After drawing the Lewis structure for COS using the above information, it is evident that the three-dimensional shape (or geometry) of the molecule is , with a bond angle of degrees.
A stable triatomic molecule can be formed that containsone atom each of nitrogen, sulfur, and fluorine. Threebonding structures are possible, depending on which is thecentral atom: NSF, SNF, and SFN.(a) Write a Lewis diagram for each of these molecules,indicating the formal charge on each atom.(b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom?(c) Does consideration of the electronegativities of N, S,and F from Figure 3.18 help rationalize this observedstructure? Explain.
I'm confused as to why the lone pair on nitrogen can't be moved as depicted in the picture. Doesn't nitrogen fulfill the octet rule in both scenarios?
Is an ion considered to be polar, even if it does not contain any polar bonds? think about what the electronegative value applies to? Can electronegativity values be applied to atoms in which electrons have been added or removed from their normal Valencia’s?
I'm having trouble trying to figure out where to move the doule bond, bc wherever I place it seems like it would violate the octet rule. can someone explain simply?
Show how these elements combine into octet-rule ionic compounds, as in the first example. First, draw atomic Lewis structures for the atoms and their O.R. ions. Show their charges, and use them to find the unit formula, and the name. Then draw atomic Lewis structures for all atoms in the formula unit together, show with arrows how all e¯s are transferred to make the ions, and draw the Lewis structure of the ionic compound. Atoms O.R. ions Unit formula Lewis Structure Name Transfer e¯s with arrows Mg + Br Magnesium bromide Li + C Lithium carbide Ge + S