Hydrogen cyanide, HCN, is a highly poisonous compound that vaporizesslightly above room temperature.a) How many valence electrons does C have?b) How many valence electrons does H have?c) How many valence electrons does N have?d) How many total valence electrons does the HCN molecule have?e) Draw the Lewis structure for HCN that minimizes the formal charges on allatoms.f) How many electron domains are on the central atom?g) What is the molecular geometry of HCN?h) Is the molecule polar?

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Answered: Hydrogen cyanide, HCN, is a highly…

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 35EQ: In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and...

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Similar questions

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 ____.
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 ?
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.
Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
lodine trichloride, ICI3, is a bright yellow solid and an oxidizing agent. a) How many valence electrons does the I have? b) How many valence electrons does CI have? c) How many total valence electrons does the ICI3 molecule have? d) Draw the Lewis structure for ICI3 that minimizes the formal charges on all atoms. e) How many electron domains are on the central atom? f) What is the electron domain geometry of ICI3? g) What is the molecular geometry of ICI3? h) Is the molecule polar?
Molecular Shape.trigonal planar Questions: (Complete sentences are not necessary) 1. Examine the Lewis structure for each of the molecular shapes formed above. (ignore BrF!) Complete the following table based upon both the number of unshared electron pairs around the central atom and also the number of bond groups that are around the central atom. For example, in the following Lewis structure of PBr,, phosphorus (the central atom) has one pair of unshared electrons and three bond groups surrounding it Br P: (Note: single, double, and trıple bonds all count as single bond groups) Number of Unshared Electron Pairs Around the Central Number of Bond Groups Around Central Atom Molecular Shape Atom Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral 2. What is the electrostatic charge of all electron groups, either shared (Le. bonds) or unshared?
Molecular Shape:trigonal planar Questions: (Complete sentences are not necessary) 1. Examine the Lewis structure for each of the molecular shapes formed above. (ignore BrF!) Complete the following table based upon both the number of unshared electron pairs around the central atom and also the number of bond groups that are around the central atom. For example, in the following Lewis structure of PBr,, phosphorus (the central atom) has one pair of unshared electrons and three bond poups surrounding it. Br: Br P: : Br: (Note: single, double, and triple bonds all count as single bond groups) Molecular Shape Number of Unshared Electron Pairs Around the Central Number of Bond Groups Around Central Atom Atom Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral 2. What is the electrostatic charge of all electron groups. either shared (Le. bonds) or unshared? mnel cach other?
A newly discovered element Bm has 7 valence electrons. It is found to form the following molecular ion. :C: Bm-Cl: (click here e if you cannot see the image) The formal charge on the central Bm atom is [ Select ] Based on the Lewis structure for BmCl* given above, the VSEPR predicted molecular geometry (i.e., molecular shape) is [Select] Based on the Lewis structure for BmCl,* given above, there are [Select] pi bonds in this molecule. The hybrization of the central Bm atom is predicted to be ISelect) v. (Because of a formatting issue, the numbers could not be superscripted) The bond angles between CI atoms surrounding the central Bm atom is predicted to be [ Select ) degrees.
Molecular Shape:trigonal planar Questions: (Complete sentences are not necessary) 1 Examine the Lewis structure for each of the molecular shapes formed above. (ignore BrF!) Complete the following table based upon both the number of unshared electron pairs around the central atom and also the number of bond groups that are around the central atom. For example. in the following Lewis structure of PBr,, phosphonus (the central atom) has one pair of unshared electrons and three bond ypoups surrounding it. :Br: Br (Note: single, double, and triple bonds all count as single bond groups) Number of Bond Groups Number of Unshared Electron Pairs Around the Central Atom Molecular Shape Around Central Atom Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral 2. What is the electrostatic charge of all electron groups. either shared (Le. bonds) or unshared? Since all electron groups have this same charge. do they attract or repel each other?
Draw three resonance structures for CS,. This species has its three atoms bonded sequentially in the following fashion: S-C-S. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Select the choices from below which make the statements true about this (most important) resonance structure. (a) The leftmost bond (between S and C) is a single v bond. (b) The rightmost bond (between C and S) is a single v bond. (c) The formal charge on the leftmost (S) atom is -Select-v (d) The formal charge on the central (C) atom is -Select---v (e) The formal charge on the rightmost (S) atom is Select-v (f) The number of nonbonding pairs (lone pairs) of electrons in the leftmost (S) atom is Select-v pairs. (g) The number of nonbonding (lone) pairs of electrons in the rightmost (S) atom is -Select-- v pairs.
Molecular Shape:trigonal planar Questions: (Complete setences are not necessary) 1 Examine the Lewis structure for each of the molecular shapes formed above. (ignore BrF!) Complete the following table based upon both the number of unshared electron pairs around e central atom and also the number of bond groups that are around thelcentral atom. For example, in the following Lewis structure of PBr,, phosphorus (the central atom) has one pair of unshared electrons and three bond groups surrounding it Er: :Br -P: (Note: single, double, and triple bonds all count as single bond groups) Molecular Shape Number of Unshared Electron Pairs Around the Central Number of Bond Groups Around Central Atom Atom Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral 2. What is the electrostatic charge of all electron groups, either shared (Le. bonds) orr unshared?

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