Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 13, Problem 7LDRE
Interpretation Introduction
Interpretation:
Whether the Lewis diagram of
Concept introduction:
Lewis diagram is a representation of the chemical formula of substance with valance electrons of atoms. The Lewis structures are also known as electron dot structures. In the Lewis structure, electrons are denoted by dots. Only the valence electrons are presented as dots in the Lewis structure.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
For 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 Cl
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
CO₂
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.
HCN
CH₂CHCl
CH₃CH₃
CO₂
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
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 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. CH₄ O₂ CH₂Cl₂ H₂O CH₃Liarrow_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_forwardCompare the average N–O bond in your Lewis structures of NO2+ and NO2–. Based on the trends you identified above, which average N–O bond do you expect to be stronger? Which do you expect to be shorter? Explain your reasoning. Stronger N–O Bond NO2+ NO2– Shorter N–O Bond NO2+ NO2–arrow_forward
- Draw the Lewis symbols for each of the following elements, both before reaction and after reaction to obtain a complete shell: Before reaction. After reaction. P Br Bearrow_forwardThe Lewis structure of N2H2 shows ________. a nitrogen-nitrogen triple bond a nitrogen-nitrogen single bond each nitrogen has one nonbonding electron pair each nitrogen has two nonbonding electron pairs each hydrogen has one nonbonding electron pairarrow_forwardDecide 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:arrow_forward
- Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D chemical symbol, chemical formula or Lewis structure H-C=C-H H — He Fe -C=N: X boiling point (Choose one) (Choose one) O (Choose one) ŵ (Choose one) Sarrow_forwardanswer these questions for NaOH . Identify the nature of the substance. All types of bonding (primary) present. How the bonding is formed and how this relates to electronegativity values. Explain what the formula represents. State two examples of another substance of the same type with the same bonding. State and explain properties of the substance:o Melting and/or boiling point and state at room temperature o Electrical conductivity in any state o Solubility in water o Shape if molecular or structure if an ionic compound or metallic. An example (application) of what the substance is used for and why.arrow_forward1) Draw the Lewis symbol for each element in the compounds below, then draw a Lewis Structure for the compounds. PH3 SiF4 H2O O2arrow_forward
- Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. chemical symbol, substance chemical formula boiling point or Lewis structure A 0=N - Cl : (Choose one) В CaCl, (Choose one) v : Cl : : Cl: (Choose one) v :Cl : : Cl : Cl, (Choose one) ♥ ?arrow_forwardAnswer the questions in the table below about the shape of the ammonium (NH) cation. (NH+) How many electron groups are around the central nitrogen 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 nitrogen atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) X Śarrow_forwardConsider the molecules of furan and benzene. The dominant Lewis structure of furan and the two resonance structures of benzene are shown below: H K Book H What is the meaning of the double-sided arrow () connecting the two structures of benzene? Furan Benzene H It indicates that electrons in benzene rapidly change their positions corresponding to the two structures. It indicates that there are two independent coexisting forms of benzene. It indicates a chemical equilibrium between the two distinct structures. It indicates that the second structure can be obtained as a mirror image of the first one. It indicates that benzene exists in a single form, which is an average of the two structures.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER