Consider the phosphorus trifluoride (PF,) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the phosphorus- fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the phosphorus-fluorine bonds to be ... (choose one)

Consider the phosphorus trifluoride (PF,) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the phosphorus- fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the phosphorus-fluorine bonds to be ... (choose one)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.123QE

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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?
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.
How many LONE pairs of electron does ONE water molecule have? a. two b. three c. one d. none I need explanation in a research way. Please don't base the answer to any articles that can be seen in google instead base it with a research paper or any studies with authors. Book-supported is also okay.
what are the issues that are the evident of the failure of the plum pudding model of atoms? why the mvr= nh/2π formula does not work properly with this model? state the logical arguements in bullet points.
Part A) Consider the structural changes that occur in the following molecules. Begin by drawing the best Lewis Structure for each of the following molecules. BH3 CH4 NH3 H2O HF Part B)What are the ideal bond angles for each structure, and which are expected to be distorted? For the ones that are distorted look up on the internet and record their experimental values here: Part C)According to Lewis and VSEPR theory, why do these changes occur?
Using Lewis symbols and Lewis structures, diagram the formationof SiCl4 from Si and Cl atoms, showing valence-shellelectrons. (a) How many valence electrons does Si have initially?(b) How many valence electrons does each Cl haveinitially? (c) How many valence electrons surround the Siin the SiCl4 molecule? (d) How many valence electrons surroundeach Cl in the SiCl4 molecule? (e) How many bondingpairs of electrons are in the SiCl4 molecule?
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. PCl5* OF2 SF4* A=Bonding electronsB= Sigma-bondsC =Nonbonding electron pairsD= Hybrid orbitals havingnonbonding electron pairsE =Hybrid orbitals usedF= 3-D structure (NAME)G =Polar (P) or nonpolar (NP) MOLECULE OR ION LEWIS STRUCTURE A B C D E F G
Which of the following molecule is an example of C infinity V? HCN, CCl4, NH3, BCl3
Consider the molecule PF4Cl. (a) Draw a Lewis structure forthe molecule, and predict its electron-domain geometry.(b) Which would you expect to take up more space, a P¬Fbond or a P¬Cl bond? Explain. (c) Predict the molecular geometryof PF4Cl. How did your answer for part (b) influenceyour answer here in part (c)? (d) Would you expect the moleculeto distort from its ideal electron-domain geometry? Ifso, how would it distort?
Draw the lewis structure of SO2 ( best resonance) and 2nd best resonance showing the shape and bond angles of each one, the 3D structure with polar bonds or bonds dipole of each one and the molecular polarity. Here is an example of what I want the answer to be like:
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3 Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
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?