A new element, Bw, has been identified to bepart of Period 10 Group VIIA. Draw the properstructure of the polyatomic ion, BwCl2S3 ^ - .According to VSEPR theory, this ion has amolecular shape of [1]. (Type the shape exactlyas written on the table provided to you on theexam data sheet) The formal charge of the Bwatom must be [2]. (Type in the charge including asign and numberi.e. +1, -1, -2, +2, 0, etc.)

Structure of BwCl2^-5 Ion Cl Cl/ \ / \Bw--- Bw---Cl (Bw is the central atom)\ / \ /Cl Cl The…

Answered: A new element, Bw, has been identified…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 86AP

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Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic bond, and pure covalent bond versus polar covalent bond. Characterize the types of bonds in terms of electronegativity difference. Energetically, why do ionic and covalcnt bonds form?
Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates the energy changes involved in the formation of MgO(s) and NaF(s). Why is the lattice energy of MgO(s) so different from that of NaF(s)? The magnesium oxide is composed of Mg2+ and O2 ions. Energetically, why does Mg2+O2 form and not Mg+O? Why doesnt Mg3+O3 form?
The Lewis representation above depicts a reaction between a halogen (blue) and a main-group element from group (7A + (red). In this representation, each Y atom needs 1 electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of X . There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support
One scale for electronegativity is based on the concept thatthe electronegativity of any atom is proportional to theionization energy of the atom minus its electron affinity:electronegativity = k1I - EA2, where k is a proportionalityconstant. (a) How does this definition explain why the electronegativityof F is greater than that of Cl, even though Clhas the greater electron affinity? (b) Why are both ionizationenergy and electron affinity relevant to the notion ofelectronegativity? (c) By using data in Chapter 7, determinethe value of k that would lead to an electronegativity of 4.0for F under this definition. (d) Use your result from part (c)to determine the electronegativities of Cl and O using thisscale. (e) Another scale for electronegativity defines electronegativityas the average of an atom’s first ionization energyand its electron affinity. Using this scale, calculate the electronegativitiesfor the halogens, and scale them so that fluorinehas an electronegativity of 4.0. On this…
(b) 8. Give the formal charges of atoms :0= C= --$- -Br .N. --
Consider the Lewis structure for the polyatomic oxyanionshown here, where X is an element from the third period(Na - Ar). By changing the overall charge, n, from 1- to2- to 3- we get three different polyatomic ions. For each ofthese ions (a) identify the central atom, X; (b) determine theformal charge of the central atom, X; (c) draw a Lewis structurethat makes the formal charge on the central atom equalto zero.
5. What is the electronegativity of C considering SiC is 11% ionic and Xsi = 1.8?
(a) Complete the following table:BESTLewis structureNH4+Draw Lewis structure:VSEPR Formula for central atom: _________________________SOF2Draw Lewis structure:VSEPR formula for central atom: __________________________XeF2Draw Lewis structure:VSEPR formula for central atom: ________________________H2SO3Draw Lewis structure:VSEPR formula for central atom: ________________________3(b) (i) In general, for what two kinds of substances do we draw Lewis structures?____________________________________________________________________________(ii) Complete the following Lewis structure and answer the questions below it.CHNHC OOC C NH HHHWhat is the empirical formula of this compound? __________________________________How many lone pairs of electrons that this compound have? __________________________How many multiple bonds does this compound have? _______________________________How many nonbonding electrons does this compound have? __________________________How many molecules are in 15.0 mg of…
Find the covalent compound among these. O Rb;S O LizS O K2S O H2S
iv. Assign formal charges to the atoms in the following structures and decide which the more important contributor to the resonance hybrid is. (a) (b) H H C=N=N c-N=N H H v. What factor accounts for each of the following differences in bond length? (a) I, has a longer bond than Br,. (b) C-N bonds are shorter than C-C bonds. (c) H-C bonds are shorter than the C-O bond. (d) The C-O bond in formaldehyde, H,C=0, is longer than the bond in carbon monoxide, C=0.
Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.

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