3To answer the questions, interpret the following Lewis diagram for CIO₂:O-C-0:[Review Topics][References]Use the References to access important values if needed for t1. For the central chlorine atom:The number of non-bonding electrons 4The number of bonding electronsThe total number of electrons2. The central chlorine atomA. obeys the octet rule.B. has more than an octet.C. has less than an octet.Submit AnswerRetry Entire GroupCengago=82 more group attempts remaining

ClO2- is a yellowish- green gas

To answer the questions, interpret the following Lewis diagram for CIO₂". :Ö-CI-Ö: 1. For the central chlorine atom: 4 The number of non-bonding electrons = The number of bonding electrons The total number of electrons 2. The central chlorine atom A. obeys the octet rule. B. has more than an octet. C. has less than an octet. I 4 = 8

To answer the questions, interpret the following Lewis diagram for CIO₂". :Ö-CI-Ö: 1. For the central chlorine atom: 4 The number of non-bonding electrons = The number of bonding electrons The total number of electrons 2. The central chlorine atom A. obeys the octet rule. B. has more than an octet. C. has less than an octet. I 4 = 8

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 7STP

See similar textbooks

Similar questions

Write Lewis structures and predict whether each of the following is polar or nonpolar. (You can draw the structure and send on Canvas, or attach the file here, or you can also use the draw feature within Inspera in the panel above) a. HOCN (exists as HOOCN) b. COS c. SO2 d. H2CO (C is the central atom)
furicacid, H2SO4 (each H is bonded to an O). (a) WhatLewis structure(s) would you draw to satisfy the octet rule?(b) What Lewis structure(s) would you draw to minimizeformal charge?
Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In each case the first atom listed is the central atom.) a. POCl3, SO42-, XeO4, PO43-, ClO4- b. NF3, SO32-, PO33-.Cl3- c. ClO2-, SCl2, PCl2- d. Considering your answers to part a, b, and c, what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons?
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule.a. BF3b. NH3c. BeCl2d. PCl5*e. OF2f. SF4*g. SF6*h. XeF2*i. SnCl4j. H3O+ Set up your own table to the following formatColumn CharacteristicsA Bonding electronsB Sigma-bondsC Nonbonding electron pairsD Hybrid orbitals havingnonbonding electron pairsE Hybrid orbitals used F 3-D structureG Polar (P) or nonpolar (NP) molecule or ion lewis structure A B C D E F G
Draw the correc (best) Lewis structure (LS) for the ionic compound K2SeO3 (on looose leaf paper--NOT TO BE SUBMITTED) and then answer the following questions.(NOTE: Use the cardinal numbers 0, 1, 2, 3, and so on for any quantity required)a) What charge does the K ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) b) What charge does the SeO3 ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) c) How many lines, if any, attach each K ion to the SeO3 ion? d) How many valence electrons does the SeO3 ion (alone) have? e) How many single bonds does the LS of the SeO3 ion have? f) What is the number of lone electron pairs in the LS of the SeO3 ion?
(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…
In the BEST Lewis structure for the molecule XeF2, how many unshared pairs are there on the central atom? Enter a number.
The formal charge of oxygen in HO− is _____. The number of valence electron of O in HO− is _____. The number of nonbonding electrons of O in HO− is _____. Thenumber of bonding electrons of O in HO− is _____. What are the answers for the Blanks A, B, C, D? Write the answers in a numerical form, not with letters, without any space.
A new compound is made that has a C—C bond length of1.15 Å. Is this bond likely to be a single, double, or tripleC—C bond?
Although I3- is a known ion, F3- is not. (a) Draw the Lewis structure for I3- (it is linear, not a triangle). (b) One of your classmates says that F3 - does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says F3- does not exist because it would violate the octet rule.Is this classmate possibly correct? (d) Yet another classmatesays F3- does not exist because F is too small to make bonds tomore than one atom. Is this classmate possibly correct?
Review the rules for drawing Lewis structures and try to draw the correct Lewis structures for the molecules shown in part A of this exercise.
Part 1) If 3.36 moles of N2 and 3.90 moles of H2 are combined under, which would be considered the limiting reactant? Part 2) How many grams of NH will be formed during the reaction? Part 3) In sufficient detail, describe the most valid Lewis structure of NH3 (types of bonds, presence of unbonded electrons, existence of any formal charges etc.), then specify its molecular geometry. Based on the reaction to form ammonia (NH3