Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
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Chapter 13, Problem 17E
Interpretation Introduction
Interpretation:
The Lewis diagram for
Concept introduction:
The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also known as Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.
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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:
Many 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
нн
Decide whether these proposed Lewis structures are reasonable.
proposed Lewis structure
Is the proposed Lewis structure reasonable?
Yes.
No, it has the wrong number of valence electrons.
The correct number is:
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are: 0
Yes.
No, it has the wrong number of valence electrons.
a=ö:]
The correct number is:
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are: 0
Yes.
No, it has the wrong number of valence electrons.
:0:
The correct number is: 0
HIC-H
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are:"
* If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many
times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,0".
X 5 ?
: Z:
I
:Z:
Chapter 13 Solutions
Introductory Chemistry: An Active Learning Approach
Ch. 13 - Draw the Lewis diagrams for each of the following...Ch. 13 - Prob. 2ECh. 13 - Prob. 3ECh. 13 - Prob. 4ECh. 13 - Draw the Lewis diagrams for each of the following...Ch. 13 - Prob. 6ECh. 13 - Draw the Lewis diagrams for each of the following...Ch. 13 - Prob. 8ECh. 13 - Prob. 9ECh. 13 - Prob. 10E
Ch. 13 - Prob. 11ECh. 13 - Prob. 12ECh. 13 - Prob. 13ECh. 13 - Prob. 14ECh. 13 - Prob. 15ECh. 13 - Prob. 16ECh. 13 - Prob. 17ECh. 13 - Prob. 18ECh. 13 - Prob. 19ECh. 13 - Prob. 20ECh. 13 - Prob. 21ECh. 13 - Prob. 22ECh. 13 - Prob. 23ECh. 13 - Prob. 24ECh. 13 - Prob. 25ECh. 13 - Prob. 26ECh. 13 - Prob. 27ECh. 13 - Prob. 28ECh. 13 - Prob. 29ECh. 13 - Prob. 30ECh. 13 - Prob. 31ECh. 13 - Prob. 32ECh. 13 - Prob. 33ECh. 13 - Prob. 34ECh. 13 - Prob. 35ECh. 13 - Prob. 36ECh. 13 - Prob. 37ECh. 13 - Prob. 38ECh. 13 - Prob. 39ECh. 13 - Prob. 40ECh. 13 - Prob. 41ECh. 13 - Prob. 42ECh. 13 - Prob. 43ECh. 13 - Prob. 44ECh. 13 - Is the carbon tetrachloride molecule, CCl4, which...Ch. 13 - Prob. 46ECh. 13 - Describe the shapes and compare the polarities of...Ch. 13 - Prob. 48ECh. 13 - Prob. 49ECh. 13 - Prob. 50ECh. 13 - Prob. 51ECh. 13 - Prob. 52ECh. 13 - Prob. 53ECh. 13 - Prob. 54ECh. 13 - Prob. 55ECh. 13 - Prob. 56ECh. 13 - Prob. 57ECh. 13 - Prob. 58ECh. 13 - Prob. 59ECh. 13 - Prob. 60ECh. 13 - Prob. 61ECh. 13 - Prob. 62ECh. 13 - Prob. 63ECh. 13 - Prob. 64ECh. 13 - Prob. 65ECh. 13 - Prob. 66ECh. 13 - Prob. 67ECh. 13 - Classify each of the following statements as true...Ch. 13 - Prob. 69ECh. 13 - Draw Lewis diagrams for these five acids of...Ch. 13 - Prob. 71ECh. 13 - Prob. 72ECh. 13 - Describe the shapes of C2H6 and C2H4. In doing so,...Ch. 13 - Prob. 74ECh. 13 - Prob. 75ECh. 13 - C4H10O is the formula of diethyl ether. The same...Ch. 13 - Prob. 77ECh. 13 - Prob. 78ECh. 13 - Draw Lewis diagrams for water and dihydrogen...Ch. 13 - Prob. 2PECh. 13 - Prob. 3PECh. 13 - Prob. 4PECh. 13 - Prob. 5PECh. 13 - What is the Lewis diagram of butane, C4H10?Ch. 13 - Prob. 7PECh. 13 - Prob. 8PECh. 13 - Prob. 9PECh. 13 - Prob. 10PECh. 13 - In the gas phase, tin (II) chloride is a...Ch. 13 - Prob. 12PECh. 13 - Determine the molecular geometry around each...Ch. 13 - Describe the molecular geometry around each carbon...Ch. 13 - Is the difluoromethane molecule polar or nonpolar?...Ch. 13 - Prob. 1LDRECh. 13 - Prob. 2LDRECh. 13 - Prob. 3LDRECh. 13 - Prob. 4LDRECh. 13 - Prob. 5LDRECh. 13 - Prob. 6LDRECh. 13 - Prob. 7LDRECh. 13 - Prob. 8LDRECh. 13 - Prob. 9LDRECh. 13 - Prob. 10LDRE
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- < 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 3 Draw the Lewis Structure and calculate the formal charge for each atom in all of the following molecules/ions. Show your calculations and label each atom with the formal charge calculated. NH3 NO2 NO3 Attach File Browse My Computer Browse Content Collectionarrow_forwardBased on trends in electronegativity, Rank the following polarity of the bonds. Use numbers 1, 2, 3, 4 to fill in the ranking. 1 represents the MOST polar, 4 represents the LEAST polar! Molecule Н- СІ H - N Н-F Н-С H-CI [ Choose H-N [ Choose ] H-F [ Choose ] Н-С [ Choose ]arrow_forward
- Draw the Lewis Structure for NH2CH2CO2H. Now answer the following questions based on your Lewis structure: (Enter an integer value only.) # single bonds in the entire molecule # double bonds in the entire molecule # lone pairs in the entire moleculearrow_forwardDraw the correct Lewis structure for the following molecules so4-2 OH-arrow_forwardTrue or False.Double and triple bonds are a means by which fewer atoms can satisfy their “octet” rules in a molecule.arrow_forward
- Draw the Lewis structure of these compounds and use the electronegativity values, calculate the polarity of the molecules and write if the compounds will be polar, nonpolar, or ionic. Label the + and -next to the atoms of the molecule if they have charge. Also, write the overall dipole. Cl₂ HCl NH₃ CH₂O CH₄ O₂ CH₂Cl₂ H₂O CH₃Li HCN CH₂CHCl CH₃CH₃ CO₂arrow_forwardWrite a Lewis structure for each of the following molecules. H2CO (carbon is central) Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.arrow_forwardFor the structure CIO3 draw a Lewis structure using Cl as the central atom... For the structure that obeys the octet rule which of the following are correct? There are a total of 26 valence electrons There are a total of 24 valence electrons There are a total of 25 valence electrons OCI has one lone pair of electrons CI makes a double bond to one of the oxygens Each O has a -1 formal charge 20 atoms make a double bond to Cl All 30 atoms make a double bond to Clarrow_forward
- O REPRESENTATIONS OF ORGANIC MOLECULES Converting a skeletal structure to a Lewis structure Convert the structure below to a Lewis structure. NH NH IIarrow_forwardWrite a Lewis structure for each of the following molecules that are exceptions to the octet rule. ClO2 Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and nonbonding electrons. Do not include charges.arrow_forwardUse the References to access important values if needed for this question. 1 What is the total number of valence electrons in the Lewis structure of SF? electrons 2 Draw a Lewis structure for SF₁. • Do not include overall ion charges or formal charges in your drawing. • If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. AFFIL [ ] در ?arrow_forward
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