Molecular Shape:trigonal planarQuestions: (Complete setences are not necessary)1 Examine the Lewis structure for each of the molecular shapes formedabove. (ignore BrF!) Complete the following table based upon both thenumber of unshared electron pairs around e central atom and also thenumber of bond groups that are around thelcentral atom. For example, inthe following Lewis structure of PBr,, phosphorus (the central atom) has onepair of unshared electrons and three bond groups surrounding itEr::Br -P:(Note: single, double, and triple bonds all count as single bond groups)Molecular ShapeNumber of Unshared ElectronPairs Around the CentralNumber of Bond GroupsAround Central AtomAtomLinearBentTrigonal PlanarTrigonal PyramidalTetrahedral2. What is the electrostatic charge of all electron groups, either shared (Le. bonds) orr unshared?

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Answered: Molecular Shape Number of Unshared…

Living by Chemistry

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ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 7STP

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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
Sulfur and oxygen form a series of 2 anions including sulfite, SO32, and sulfate, SO42. In addition to these, there are three other more complex anionsdithionite, S2O42, dithionate, S2O62, and tetrathionate, S4O62. Write correct Lewis structures for dithionite, dithionate, and tetrathionate ions.
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.
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.
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.OClorOBrc.PSorPOb.NOorNFd.HOorHN
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 structure of pyridine is When a proton becomes bonded to the nitrogen atom by way of its unshared electron pair, the result is _____________________________
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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?
The molecules BH3 and SF6 and the ion SO42 exist and are stable. Draw a Lewis structure of each,and comment on whether they are exceptions to Lewis’ octet rule.
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+
the formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?

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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