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- vo/index.html?deploymentld%35575082893 288909969212&elSBN=9781305657571&snapshotld%3D2199898&id%3D1... NDTAP Q Search this cour Use the References to access important values if needed for this question. Draw (on paper) a Lewis structure for SF2 and answer the following questions based on your drawing. Do not draw double bonds unless they are needed for the central atom to obey the octet rule. 1. For the central sulfur atom: the number of lone pairs the number of single bonds the number of double bonds = Numeric input field 2. The central sulfur atom A. obeys the octet rule. B. has an incomplete octet. C. has an expanded octet. Submit Answer 5 question attempts remainingUse 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.1. Which of the following Lewis Structures are correct? Select all that apply. 2. Which of these compounds are polar molecules? Select all that apply.
- Could someone help me?? The answer to this question must look similar to the example attached. Back ground info: Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…b Draw Lewis structure(s) for the acetaldehyde molecule (CH,CHO). If there are equivalent resonance structures, draw all of them. symbol. • Draw one structure per sketcher box, and separate added sketcher boxes with the • Do not include overall ion charges or formal charges in your drawing. • Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. CH3CHO:Answer the questions in the table below about the shape of the phosgene (COCI,) 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)
- 3a.Draw the best Lewis structure for the HClO3 acid molecule. (Hint: the acidic H is bonded to O in an oxy-acid molecule).Evaluate each atom using formal charge to prove you have the best structure. Show your math work as well as your formal charge answers. 3b. Draw all the resonance structures for the ClO3– polyatomic anion. (Hint: make sure you have the best initial structure first!)VISUALIZATION Drawing Lewis StructuresI Clear F Available Electrons: 32 F C F F Create the Lewis structure of CF4. NOTE: do only the step asked for in each part and then click Check-don't work ahead to solve the final structure. Step 1. Count valence electrons in the molecule or ion. Do this by adding the periodic group numbers for each atom in the structure and adjusting for charge. Enter and Check. Step 2. Connect each pair of bonded atoms with a single bond by dragging bonds onto the molecule. Each bond decreases the number of available electrons by 2. Check.Draw the Lewis structures of the following molecules with less than an octet. Write your answer on your answer sheet.
- 1. Consider the structure shown below and then answer the following questions. a. Complete the structure by adding the missing formal charges. All atoms and lone pairs are explicitly shown. (Hint: Consider the number of bonds neutral atoms have.) :Ö: H ‚H H H b. Draw two more resonance structures of the molecule from part a by adding the missing î bonds, lone pairs, and formal charges. All atoms in both structures should possess an octet. (All atoms and o bonds are drawn for you; remember, only lone pairs and bonds move in resonance structures.) Additional guidelines are given for each structure. All atoms in this structure will be neutral (no formal charges). One oxygen atom has a +1 formal charge and one oxygen atom has a -1 formal charge. H H H H H H H H HDraw the Lewis structure for H2S Before answering the following questions (You do NOT submit a picture just answer the questions. Given that sulfur obeys the octet rule WARNING: Do NOT USE the internet or other sources to find the structures. Use ONLY the rules taught in class. Answer the following questions for the Lewis structure for H2S given that sulfur obeys the octet rule. Give answers as numbers (1,2,3 ...etc.) not words (one, two three etc.) How many double bonds exist in this structure How many single bonds exist in this structure How many bonds does the sulfur atom form How many electrons surround the sulfur atom How many lone pairs are around the sulfur atom How many bonds does each hydrogen atom form How many lone pairs are around each hydrogen atom How many electrons surround each hydrogen atomAttempts ****** 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.