POST-LAB QUESTIONS1. Should all of the angles in methane (CH4) be equal? Why or why not?2. In terms of molecular structure, what additional information does the VSEPR theory giveyou beyond electron dot structures?3. Sketch the molecular shape of the following compounds. Be sure to label the bondangles.Hint: Look up the bond angles in a textbook or on the internet.CompoundH2Cl2SO2NH3MoF6Sketch of Molecular Shape

Step 1:- Q 1. Should all of the angles in methane (CH₄) be equal? Yes, all the angles in methane…

Answered: POST-LAB QUESTIONS 1. Should all of the…

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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Question 105 of 170 Retry Draw the Lewis structure of water (H2O) and then determine its electron domain and molecular geometries. Incorrect, 2 attempts remaining Your submission: Feedback: You have submitted an incorrect skeletal structure. Not all of the elements in the given molecular formula are included in your structure. `H C) tetrahedral / bent (109.5º)| Correct geometry or geometries Activate Windows
Molecular Formula SO₂ SiCl4 Total # of valence electrons CH₂Cl₂ Lewis Structure # of Electron Groups Bond Electron Geometry Angle Molecular Geometry QUESTION 1. Using the molecular model kit, make and compare the molecular models for CO₂, H₂O, and SO₂. Even though each molecule has 3 atoms, the molecular geometries (shapes) are very different. Explain why the shapes are different. on. -C Polar or Nonpolar Attractive Force O <
Determine if the structural formula below are acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. CH3 CH;-N-CH-CH3 ČH3 A. This structure is correct because the valance of Nitrogen is complete. B. This is not a correct Lewis structure because Nitrogen can accommodate more atoms. C. This is not a correct Lewis structure because Nitrogen has a charge if it does not have three bonds. D. This is a correct Lewis structure.
Attempts ****** n Force Once started, this test must be completed in one sitting. Do not leave the test before clicking Save and Submit. Completion Your answers are saved automatically. Remaining Time: 1 hour, 57 minutes, 27 seconds. * Question Completion Status: Moving to another question will save this response. Question 12 For the molecule: NO3 What is the geometry of the molecule? Are resonance forms possible? What is the hybridization of the central atom? Is the molecule polar? A Moving to another question will save this response.
3. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. CH3CH₂OH b. CHCl, Br C. CH3NH₂ d. CHỊCH,CH,CH,CH3 e. CH3SCH 3 4. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. HCN b. CH3COOH c. H₂CCONHCH3 d. HCCH e. C6H12
|| Predicting deviations from ideal bond angles Consider the carbonyl fluoride (CF₂O) 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 carbon-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the carbon-fluorine bonds to be ... 口。 (choose one) (choose one) about the same bigger smaller
11 Name: Maddie Klink Instructor: Lab Day: Models of Organic Molecules Please bring your molecular model kits to lab for the completion of these exercises. Molecular Modeling: This lab is designed to help you become comfortable using model kits to visualize molecular structures in three dimensions. Part I: Answer these questions before doing any work with your model kit 1. How many bonds must each of the following atoms have in order to have no formal charge? 4 valence 1450na a. Carbon b. Hydrogen bond c. Oxygen d. Chlorine 7 valence e. Nitrogen 5 valence Octet H- H Complete octet = 8-4 H 8-S = 3 3bonds 2. Using the information from question #1, determine whether each of the following structures is possible or impossible? (Note that if no formal charges are shown, this implies that all formal charges are zero.) 6 valence Octet = 8.6 H H с-н H 01C C -K = 2 bonas 8-1-1 bond H H H-C Lab Time: H -C-H H H H-C-CI- C-H ++ H H -H HIC C-H H VEUR 1
How does adding an atom affect the position and angles of existing atoms or lone pairs? How does adding a lone pair affect the position and angles of existing atoms and lone pairs? Is the effect of adding bonded atoms and lone pairs to the central similar? Explain your answer. Describe what is meant by the "Steric #". Explain the difference between the terms "Electron Geometry" and "Molecule Geometry". How does changing a bond to a double or triple bond affect the shape of the molecules? List the molecules in Part III where the real bond angles differ from the theoretical model values. Why do you think the values differ?
ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the chlorite (C102) a anion. 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 chlorine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the chlorine-oxygen bonds to be... 0 0 (choose one) X 3 1/5
THIS is the equation N2H4 + O2 → N2 + H2O PLEASE HELP AND LOOK AT THE PICTURE FOR DATA PLEASE HELP! I REALLY NEED HELP BECAUSE MY TEACHER HASENT TAUGHT ME HOW TO DO THIS PLEASE HELP!!!!! Balance the equation (if not already balanced) Draw the models of the molecules in the equation, using Lewis structures, ball and stick models or something else that represents each of the atoms and how they are connected. Identify bonds being formed or broken. Use bond energy values from below to Calculate the overall energy of the reaction. Determine if the reaction is exothermic or endothermic. Draw a potential energy diagram showing the ∆H, reactants and products. Create one example of mass (g) to mass (g) stoichiometry problem.
Answer the questions in the table below about the shape of the methanone (H₂CO) molecule. How many electron groups are around the central carbon 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 carbon atom? (You may need to use the scrollbar to see all the choices.) (choose one) X S
Topic: Di: Quiz 3: C Thought Lab 2 - P CHEM& O CHEM 7courses/2126119/quizzes/6159306/take Question 6 0. On a separate sheet of paper, complete the following task. Scan or take a photo of y work and upload it here to receive credit. Your work must be .pdf file type. Label the polar bonds in each molecule and then decide if the molecule is polar or nonpolar. NOTE: there are no capital i's in this example a. HCI b. C2H, c. CH2F2 d. CCI4 Upload Choose a File Quiz saved at 9:26pm

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