(a)
Interpretation:
The electron-pair geometry for 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 predicted by the valence shell electron-pair repulsion theory for the carbon atom in 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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Chapter 13 Solutions
Introductory Chemistry: An Active Learning Approach
- For each of the following ions/molecules, state the number of bond pairs state the number of lone pairs state the bond angle(s) state, or draw, the shapearrow_forwarddiagram of a molecule that shows atoms based on their a periodic table symbols. These symbols are surrounded by pairs of dots to show valence electrons that could be lone pairs or bonding pairs?arrow_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
- Question 10 of 13 > Add formal charges What is the net charge on the species? Select Draw Rings More Erase O +2 O -2 Cl O +1 sä-ö: contact us help terms of use privacy policy 7:22 PM about us careers 10/26/2020 近arrow_forwardAnswer 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)arrow_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_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_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_forwardQUESTION 5 Determine which compound should have a(n) linear molecular geometry. Key Concept: Lewis structures are drawn from a knowledge of the total number of electrons from all the atoms involved in the structure. The element with the lowest electronegativity is the central atom. Fulfill octet of outside atoms first. Molecular shape depends upon the number of atoms and lone pair electrons around the central atom. A H3O+ B ClF2+ C IF2- D AsF5arrow_forward
- Draw the Lewis structure for the IO3- ion before answering the following questions.Answer the following questions for the Lewis structure for the IO3- ion given that Iodine is the central atom and all atoms obey the octet rule. 1. How many bonds does the Iodine atom form? 2. How many electrons surround the Iodine atom? 3. How many lone pairs are around the Iodine atom? 4. How many bonds does each oxygen atom form? 5. How many lone pairs are around each oxygen atom? 6. How many electrons surround each oxygen atom?arrow_forwardIn VSEPR theory, when considering the electron-pair geometry, single bonds, double bonds, and lone pair electrons all count the same when determine the number of electron regions around the central atom. COO O True O Falsearrow_forwardUse Lewis theory to determine the formula for the compound that forms between each of the following pairs of elements. Ca and Te Express your answer as a chemical formula. Mg and Br Express your answer as a chemical formula. Na and S Express your answer as a chemical formula. In and O Express your answer as a chemical formula.arrow_forward
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