Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. :F: .. O No, the total number of valence electrons is wrong. BF, The correct number is: .. F-B-F: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: L O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. 0=0=0 The correct number is: U O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. :F: CIF3 The correct number is:I .. :F - CI –F: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: L * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. :F: .. O No, the total number of valence electrons is wrong. BF, The correct number is: .. F-B-F: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: L O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. 0=0=0 The correct number is: U O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. :F: CIF3 The correct number is:I .. :F - CI –F: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: L * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

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

7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
In each of the following diatomic molecules. which end of the molecule is positive relative to the other end? msp;a.hydrogenfluoride,HFb.chlorinemonofluorideClFc.iodinemonofluorideICl
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+
For each of the following numbers of electrons, give the formula of a positive ion that would have that number of electros, and write the complete electros configuration for each ion. msp;a.10electronsc.18electronsb.2electronsd.36electrons
In each of the following diatomic molecules, which end of the molecule is negative relative to the other end? msp;a.hydrogenchloride,HClb.carbonmonoxide,COc.brominemonofluoride.BrF
Acetic acid is the active ingredient of vinegar. Its chemical formula is CH3COOH , and the second carbon atom is bonded to the first carbon atom and to both oxygen atoms. Draw a Lewis diagram for acetic acid and use Table 3.6 to estimate its bond lengths.
Acrylonitrile is the building block of the synthetic fiber Orlon. Acrylonitrile Which carbon-carbon bond is shorter? Which carbon-carbon bond is stronger? Which bond is the most polar? What is the partial negative end of that bond?
The Lewis structures for CH4,N2,andCO2, along with the corresponding space-filling molecular images, are shown here: Use Lewis theory and VSEPR theory to draw similar space-filling molecular images of a.COb.NH3c.H2Sd.SiH4
Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.
A compound is being tested for use as a rocket propellant. Analysis shows that it contains 18.54% F, 34.61% Cl, and 46.85% O. (a) Determine the empirical formula for this compound. (b) Assuming that the molecular formula is the same as the empirical formula, draw a Lewis diagram for this molecule. Review examples elsewhere in this chapter to decide which atom is most likely to lie at the center. (c) Use the VSEPR theory to predict the structure of the molecule from part (b).