H4 H.H:Y:HHThe Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group(red).| bond(s)In this representation, each Y atom needswith atoms of H.|electron(s) to complete its octet, and gains these electrons by formingunshared electron pair(s) and|bonding electron pair(s) in the product molecule.There areThe bonds in the product are|

Lewis Representation - These are the electrons that show the bonds and lone pairs by dots as…

H 4 H. + H:Y:H H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group | (red). In this representation, each Y atom needs with atoms of H. Jelectron(s) to complete its octet, and gains these electrons by forming | |bond(s) There are ]unshared electron pair(s) and | bonding electron pair(s) in the product molecule. The bonds in the product are |

H 4 H. + H:Y:H H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group | (red). In this representation, each Y atom needs with atoms of H. Jelectron(s) to complete its octet, and gains these electrons by forming | |bond(s) There are ]unshared electron pair(s) and | bonding electron pair(s) in the product molecule. The bonds in the product are |

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 33EQ: The Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to...

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Similar questions

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 meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
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 ____.
The Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.
the formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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.
Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp;a.HForHClc.HBrorHClb.HClorHId.HIorHBr
H зн. + H:Y: H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group | (red). In this representation, each Y atom needs bond(s) with atoms of H. ]electron(s) to complete its octet, and gains these electrons by forming There are| Junshared electron pair(s) and | bonding electron pair(s) in the product molecule. The bonds in the product are |