Use the following information to determine the Lewis structure, find the electron and moleculargeometry of the molecule, determine the angle of the molecule, and determine the polarity. If theatoms are not the same, you may assume that the difference in their electronegativities are between0.4 and 2.0.Atom information:A: 6 valence electrons, CANNOT exceed the octet. Further from fluorine on the periodictable than X.X: 5 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic tablethan A.Molecule: AX2Electron Geometry: Select ]Molecular Geometry: I Select]Bond Angle: [ Select ]Polarity: [ Select]

Answered: Image /qna-images/answer/44da5e7a-ad5b-4fe6-a73f-7b8523720c6f.jpg

Answered: Use the following information to…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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F3 # 3 E X |H|V R E You will use the known periodic trends to compare properties for elements indicated with letters in this periodic table. Consider their relative positions for these questions. Your answers will be letters as indicated above, not the actual element symbol they would coordinate to. (Do not use a real periodic to answer this question.) Type the letter of the element that is a halogen in the 2nd period A/ B DELL F8 N O Ei F4 144 $ 4 R F5 D11 % 5 F6 T A 6 F7 Y & 7 F9 * 00 8 P F10 ( 9 T F11 O * ) O D L/Q PO A F12 P S PrtScr Activate Go to Setti 83°F Sunny Insert
Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar
Step 1 – Write the Lewis structure from the molecular formula.Step 2 – Assign an electron-group arrangement by counting all electron groups (bonding plus nonbonding) around the central atom (or around each centralatom, if more than one central atom in structure).Step 3 – Predict the ideal bond angle from the electron-group arrangement and the effect of any deviation caused by lone pairs or double bonds.Step 4 – Name the molecular shape by counting bonding groups and nonbonding groups separately.Step 5 – Predict whether the molecule is polar or nonpolarStep 6 – Describe the hybridization around the central atom and identify the total number of σ and π bonds in the structure
To draw a Lewis Structure, start with the atomic symbol in the middle, then put dots around the symbol until all of the valence electrons are represented. Try to envision a box around the atom symbol, and the electrons on each side of the box. The valence electrons should be drawn around the element symbol one on each side before pairing the electrons up. The maximum number of electrons that could be on one side of a Lewis Structure is two, and the maximum number of electrons around an element symbol is eight. To figure out how many valence electrons each element has, use the Periodic Table. Remember, the number of valance electrons for Group A elements is equal to the Group A number the element is in on the Periodic Table. Use the data you collected in Table 1 to a draw Lewis structure model to show the formation of any one of the compounds you assembled, then explain the model you drew. Remember, you should be explaining and supporting your answers by referencing and citing the…
Can you help me with the OF2 step-by-step for number (Step 6)? I need help with the central atom surrounded by an identical electron group. I need help with the molecule polar.
Draw a Lewis structure for the molecular formula: NOCl This molecule only contains nitrogen, oxygen, and chlorine atoms. All atoms in this molecule should have formal charges of zero. What is the geometry of the electron groups around oxygen?
Please find the question in the attachment.
Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to build amolecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
Show how these pairs of elements combine into octet-rule molecular compounds, as in the first example. First, draw their atomic Lewis structures, then use any number of these atoms to build an O.R. molecule, with multiple bonds if needed (you may not add a charge to make it O.R. as an ion!). Draw the O.R. Lewis structure, write its formula and chemical name. Atoms O.R. molecule Formula Name Carbon dioxide •¢. and ö. ö=c=ö CO2 H + Se I + S
Write a Lewis structure for each of the following molecules that are exceptions to the octet rule. ClO2 Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and nonbonding electrons. Do not include charges.
NO3 Sketch the proper Lewis structure for this substance. Be sure to follow octet/duet rules for each atom and use the total number of valence electrons available. Use your drawing to answer the following questions. Count the total number of electron domains surrounding the central atom. Enter the value only. Enter the name corresponding to the electron domain geometry. Choices are: linear, trigonal planar, or tetrahedral. Enter the name corresponding to the molecular geometry. Choices are: linear, trigonal planar, tetrahedral, bent, or trigonal pyramidal. Predict the bond angle. Enter the value without units. Use a "<" if needed.
For Nitrogen atom answer the following questions: 1) How many protons does it have? 7 protons 2) How many electrons does it have? 7 electrons 3) How many valence electrons does it have? 5 valence electrons 4) Show full electron configuration (use format similar to this example: 1s2 2s2 2p6 3s2) 1s2 25 2 2p 3 5) The number of dots on the Lewis structure 5 6) How many electrons does it need to lose or gain to achieve the stable octet? (lose/gain) electrons 7) What is the net charge after losing/gaining some electrons? 2 8) Did it become a cation or an anion? neither 9) Show electron configuration after transformation to cation or anion? (use format similar to this example: 1s2 2s2 2p6 3s2) 10) Now which noble gas has an electron configuration identical to electron configuration this ion? Helium

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