The bond angles (predicted based on shape) marked a, b, and c in the molecule below are about , respectively: and H H FII Show work in detailed
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![The bond angles (predicted based on shape) marked a, b, and c in the molecule below are about
, respectively:
and
H
H
FII
Show work in
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- 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.Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
- Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the direction of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it. (a) TeH2 (b) AsF3 (c) PCl4+ (d) XeF5+A paper published in the research Journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important green-house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulfur and a major precursor of hygroscopic (i.e., cloud-forming) particles in clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean. (a) Sketch the Lewis structure of dimethylsulfide, CH3SCH3, and list the bond angles in the molecule. (b) Use electronegativities to decide where the positive and negative charges lie in the molecule. Is the molecule polar? (c) The mean seawater concentration of DMS in the ocean in the region between 15 north latitude and 15 south latitude is 2.7 nM (nanomolar). How many molecules of DMS are present in 1.0 m3 of seawater?
- ences to STU JO papaaU II :X:Y: The Lewis representation above depicts a reaction between a halogen (blue) and a main-group element from group |(red). In this representation, each Y atom needs | with atoms of X. electron(s) to complete its octet, and gains these electrons by forming bond(s) There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product areOzone (O3) has a nonzero dipole moment. In the moleculeof O3, one of the oxygen atoms is directly bonded to theother two, which are not bonded to each other.(a) Based on this information, state which of the following structures are possible for the ozone molecule:symmetric linear, nonsymmetric linear (for example,different OUO bond lengths), and bent. (Note: Evenan OUO bond can have a bond dipole if the twooxygen atoms are bonded to different atoms or if onlyone of the oxygen atoms is bonded to a third atom.)(b) Use the VSEPR theory to predict which of the structures of part (a) is observed.Use the information on the fictious nonmetal elements. to answer the following Element Colomn EN ff 1.9 14 17 3.1 2.3 3.6 15 Nn 16 Shoos one of the followng mokcular compounds and completc the queSTIons: Nn Oyzlshape is benti V) ODraw a leuis Structure Shoudng all lalonce electrons. ) Calculate the electrongativity the bond. State what a paar covalert band, notate the partial difference for Gf bond will form If it is charges d) Detamine if the molecule is polar or polar. non-
- and uith notatich. 5.Assuming that C and N have similar electronégativities raw te mdeular orbital diagram valence orbitals Include onty tle s for (N and CN Include onty the and label all tb atonic pund Pub Standakd hotatich. Also, label the moecular orebitals that are HOMO and LUMO, D.o these mclecults stable state Cexplain 1\Jour wn S 910 101 o the し||| = 43°F Clear O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting the arrangement of electron groups around the centr... Answer the questions in the table below about the shape of the chlorine pentafluoride (CIF) molecule. How many electron groups are around the central chlorine atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central chlorine atom? (You may need to use the scrollbar to see all the choices.) Explanation Check 10 (choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral Q Search 0/3 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center www.OTAPETY AccessibiIn the actual molecule of which this is a Lewis structure, which of the labeled distances can change? marked unmarked H. You can click the unmarked tab to see the molecule without any of the distances marked List all the distances that can change. For example, suppose all the distances were meesured at a certain time, and again 0.Is later. If distance A might be 501 bigger or smaller the second time, but all the other distances are certain to be the same, you should write "A. IA and B might be different the second time, but no other distances, you would write "A, B. And so on Note for advanced students: you can assume the molecuie is dissolved in an appropriate solvent at room temperature.
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