(a)
Interpretation:
The electron-pair geometry for each carbon atom in
Concept introduction:
The electron pairs in Lewis diagrams repel each other in real molecule and thus they distribute themselves in positions around the central atoms which are far away from one another. This arrangement of electron pairs is called electron-pair geometry. The electron pairs may be shared in covalent bond, or they may be lone pairs.
(b)
Interpretation:
The molecular geometry prdicted by the valence shell electron-pair repulsion theory for the molecule
Concept introduction:
Molecular geometry is the precise term that is used to describe the shape of molecules and arrangement of atoms around the central atom. The molecular geometry of a molecule is predicted by valence shell electron-pair repulsion theory or in short VSEPR theory. VSEPR theory applies to substances in which a second period element is bonded to two, three, four, or other atoms.
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Introductory Chemistry: An Active Learning Approach
- 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.arrow_forwardRefer to the structure given below and answer the given questions: CI 18 H 5 13 1 10 15 16 17 19 2 12 14 9 11 20 1 6 ОН О 2 8. 5 Red numbers for Carbon Blue numbers for Nitrogen Green numbers for Oxygen (1) What is the Molecular Formula of the given structure? (2) Which bond is the most polar (specify number if pertaining to C,N, or O) Provide your calculation for the electronegativity difference which was the basis for your answer. (3) What is the total number of lone pairs present in the structure? 6.arrow_forwardAnswer 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 Sarrow_forward
- QUESTION 13 :C=O: Consider the provided Lewis structure for carbon monoxide: CO. Fill in the blanks with the word "true" or "false" following each of the statements below A non-polar molecule has an even, symmetric distribution of electron density Carbon and oxygen have different electronegativity values. An atom with a lower electronegativity exerts more attraction towards electrons in a shared bond The carbon and oxygen atoms in the CO molecule both attract electrons with the same strength. Carbon monoxide is a polar moleculearrow_forwardMany organic compounds belong to a category of molecules called "hydrocarbons", meaning that they only contain hydrogen and carbons. An example of a simple hydrocarbon is shown below. Considering both the VSEPR shape of the molecule and electronegativity values of the elements and state whether you expect this simple hydrocarbon to be polar or nonpolar. Explain your answer. нн H-C-C-H ннarrow_forwardNO3 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.arrow_forward
- Answer the following true or false questions about the molecule acrylaldehyde, its resonance structures, and resonance hybrid. In fairness, many of these statements are false and represent common misconceptions about resonance. If a statement is false as written, change the underlined fragment of the statement to make it true. \ 1) Atoms can be moved around to make a new resonance form 2) The oxygen atom in acrylaldehyde has a full negative charge 3) These three resonance structures exist at different points in timearrow_forwardStep 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 structurearrow_forwardIn which of the following compounds is there only 1 lone pair around the central atom? (Hint--first determine the central atom for each compound. Then draw the dot diagram for that element showing valance electrons. Which would you expect to have only 1 lone pair?) H2O PF3 BF3 HCNarrow_forward
- To answer the questions, interpret the following Lewis diagram for NO,Cl. :0-N=0 1. For the central nitrogen atom: The number of lone pairs The number of single bonds The number of double bonds 2. The central nitrogen atom| :O:arrow_forward< Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and Earrow_forwardPart B: Without building model complete the following table. Total Sketch of Lewis Name of the Molecule is Molecular number of three- polar or nonpolar? electron dot molecular formula valence dimensional structure geometry electrons geometry H2O BF3 NC13 BeH2 PCI3 AICl3 CCI4 C2H6arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning