Molecular Shape of CS2 (1) Carbon (2) sulfur (3) Sulfur 4₁ B2₂ E2 = AB₂E2 Step 1: Find the Central Atom Central atom is: с Look your line bond structure on page 1. S=C=S Step 3: Choose the ABE classification Circle the correct AB, E, notation. Recall, we use (A) to represent the central atom, (B) to represent the number of atoms bonded to the central atom, and (E) to represent the number of lone pairs AB₁E; AB₁E2 AB₁E AB₂E AB₂E₂ AB₂ AB E AB3 AB4 Step 5: Use the Molecular Shape table from your notes to draw the ball and stick representation Central atom A Batom surrounding central atom) lone pair Elone pair central atom/ Step 2: Count number of atoms bonded to the central atom (B) # of atoms bonded to central atom = B = Count number of lone pairs on the central atom (E) # of lone pairs on central atom = E=Q Step 4: Use the Molecular Shape Table from your notes to select the molecular shape and bond angles. Molecular Shape- Bent Bond angles = ~110° Step 6: Determine Polarity Is the central atom surrounded by identical electron groups? Circle one: yes If the answer was yes, then the molecule is nonpolar. If the answer is no, then the molecule is polar. Is the molecule polar? no Circle one: yes no 22

Molecular Shape of CS2 (1) Carbon (2) sulfur (3) Sulfur 4₁ B2₂ E2 = AB₂E2 Step 1: Find the Central Atom Central atom is: с Look your line bond structure on page 1. S=C=S Step 3: Choose the ABE classification Circle the correct AB, E, notation. Recall, we use (A) to represent the central atom, (B) to represent the number of atoms bonded to the central atom, and (E) to represent the number of lone pairs AB₁E; AB₁E2 AB₁E AB₂E AB₂E₂ AB₂ AB E AB3 AB4 Step 5: Use the Molecular Shape table from your notes to draw the ball and stick representation Central atom A Batom surrounding central atom) lone pair Elone pair central atom/ Step 2: Count number of atoms bonded to the central atom (B) # of atoms bonded to central atom = B = Count number of lone pairs on the central atom (E) # of lone pairs on central atom = E=Q Step 4: Use the Molecular Shape Table from your notes to select the molecular shape and bond angles. Molecular Shape- Bent Bond angles = ~110° Step 6: Determine Polarity Is the central atom surrounded by identical electron groups? Circle one: yes If the answer was yes, then the molecule is nonpolar. If the answer is no, then the molecule is polar. Is the molecule polar? no Circle one: yes no 22

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.30PAE: 7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For...

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?
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?
= 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 phosphorus trifluoride (PF3) How many electron groups are around the central phosphorus 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 phosphorus atom? (You may need to use the scrollbar to see all the choices.) (choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral molecule.
Determine the approximate bond angles in the following ions and molecules approx. 180 аpprox. 120 No Answers Chosen No Answers Chosen approx. 109.5 аpprax, 90 No Answers Chosen No Answers Chosen mix of 120 and 9o No Answers Chosen Possible answers | (SCNJ- (C: central atom) I (NO3)- (N: central atom) I (PO3]3- (P: central atom) I SF4 (S: central atom)
Based on the figure below . Match each of the following with its correct answer : : : : :O: (A) (В) The formal charges on the sulfur atom for structure (B) is Choose... v Choose... zero The bond 2 is ( shorter, longer) than the bond 1 . . stronger +2 weaker shorter The less important structure to the over all properties of the molecule is longer Choose... The bond 1 is .. .(stronger, weaker ) than the bond 2 Choose... v The formal charges on the sulfur atom for structure (A) is Choose...
Formula HCN SBr₂ NSF (N is central) SO3 Total valence e- (show calc) COBR2 (C is ventrall 1+4+5=10 e- Structure H—C=N: Total electron groups 2 Geometry (Shape) linear Angle 180° Polar? Y/ N if yes state why outer atoms different
(a) Construct a Lewis structure for hydrogen peroxide, H2O2,in which each atom achieves an octet of electrons. (b) Howmany bonding electrons are between the two oxygen atoms?(c) Do you expect the O¬O bond in H2O2 to be longer orshorter than the O¬O bond in O2? Explain.
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?
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.
Which of the following bonds are polar? Which is the more electronegative atom in cach polar bond? (a) B-F (b) Cl-CI (c) Se-O (d) H–I Arrange the bonds in cach of the following sets in order of inereasing polarity: (a) C-F, O–F, Be-F; (b) 0-CI, S-Br, C-P; (c) C-S, B–F, N-0.
N MyLab and Mastering Course Home b Search results for "Which of the At Electronegativity Table of the Ele x + A openvellum.ecollege.com/course.html?courseld=16418591&OpenVellumHMAC=fd2ce09746a2194453c324a109d1a8ec#10001 Scores Part A Pearson eText Part B Study Area Indicate the more electronegative atom in each pair. Match the atoms in the left column to the appropriate blanks in the sentences on the right. Document Sharing User Settings Reset Help Course Tools > B Given the bond P-N, the more electronegative atom in the bond is Given the bond B-F, the more electronegative atom in the bond is Br Given the bond H-Br, the more electronegative atom in the bond is H P N Submit Request Answer P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy. | Permissions | Contact Us | 2:55 AM P Type here to search 4/14/2021
Draw a Lewis structure for the C3Hg molecule using the connectivity shown in the spacefilling model in the window. • Gray C; white = H; red = 0; blue = N; dark green= Cl; brown = Br; light green = F; purple I; yellow = S; orange = P. Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = Previous Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds = The number of C=C double bonds = The total number of unshared pairs = Next