needs to be added. Notice that formal charges are indicated by 1. 2. Ob L C Cb H a ✓b ✓C H a ✓b ✓C H or and that the atoms are NOT labeled in sequence.
needs to be added. Notice that formal charges are indicated by 1. 2. Ob L C Cb H a ✓b ✓C H a ✓b ✓C H or and that the atoms are NOT labeled in sequence.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Concept explainers
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
Question
![### Completing Valence Shells of Labeled Atoms: An Educational Exercise
In this exercise, you are tasked with specifying the number of unshared pairs of electrons needed to complete the valence shell of the labeled atoms, a-c, in the following structures. If no pair of electrons needs to be added, specify "0." Note that formal charges are indicated by \( \oplus \) or \( \ominus \) and that the atoms are NOT labeled in sequence.
#### Structure 1
This structure shows a central carbon atom double-bonded to an oxygen atom labeled "b" and single-bonded to:
- An oxygen atom labeled "a"
- A hydrogen atom labeled "c"
**Graph Explanation:**
O=C (labeled b)
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O (labeled a)
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C-H (labeled c)
**Dropdown Selections for Structure 1:**
- For atom a: [ Dropdown ]
- For atom b: [ Dropdown ]
- For atom c: [ Dropdown ]
#### Structure 2
This structure is similar, showing a carbon atom double-bonded to an oxygen atom labeled "c," and single-bonded to:
- An oxygen atom labeled "a"
- Another carbon atom labeled "b," which is further bonded to three hydrogen atoms
**Graph Explanation:**
O=C (labeled c)
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C (labeled b)
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H H H
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O (labeled a)
**Dropdown Selections for Structure 2:**
- For atom a: [ Dropdown ]
- For atom b: [ Dropdown ]
- For atom c: [ Dropdown ]
#### Instructions:
1. Review each molecular structure carefully.
2. Count the number of electron pairs required to complete the valence shell for each labeled atom.
3. Use the dropdown menu to specify the necessary unshared pairs of electrons for atoms a, b, or c in each structure.
This interactive exercise helps in understanding the concept of valence electrons and formal charges in molecular structures.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd32c0099-d35b-45af-b7af-24c06e9e82b9%2Fea6907c8-3435-4fbe-9a31-51503c4bd489%2F8xtuzl.png&w=3840&q=75)
Transcribed Image Text:### Completing Valence Shells of Labeled Atoms: An Educational Exercise
In this exercise, you are tasked with specifying the number of unshared pairs of electrons needed to complete the valence shell of the labeled atoms, a-c, in the following structures. If no pair of electrons needs to be added, specify "0." Note that formal charges are indicated by \( \oplus \) or \( \ominus \) and that the atoms are NOT labeled in sequence.
#### Structure 1
This structure shows a central carbon atom double-bonded to an oxygen atom labeled "b" and single-bonded to:
- An oxygen atom labeled "a"
- A hydrogen atom labeled "c"
**Graph Explanation:**
O=C (labeled b)
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|
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O (labeled a)
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C-H (labeled c)
**Dropdown Selections for Structure 1:**
- For atom a: [ Dropdown ]
- For atom b: [ Dropdown ]
- For atom c: [ Dropdown ]
#### Structure 2
This structure is similar, showing a carbon atom double-bonded to an oxygen atom labeled "c," and single-bonded to:
- An oxygen atom labeled "a"
- Another carbon atom labeled "b," which is further bonded to three hydrogen atoms
**Graph Explanation:**
O=C (labeled c)
|
|
|
C (labeled b)
|
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H H H
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|
|
O (labeled a)
**Dropdown Selections for Structure 2:**
- For atom a: [ Dropdown ]
- For atom b: [ Dropdown ]
- For atom c: [ Dropdown ]
#### Instructions:
1. Review each molecular structure carefully.
2. Count the number of electron pairs required to complete the valence shell for each labeled atom.
3. Use the dropdown menu to specify the necessary unshared pairs of electrons for atoms a, b, or c in each structure.
This interactive exercise helps in understanding the concept of valence electrons and formal charges in molecular structures.
Transcribed Image Text:### Understanding Polar Covalent Bonds and Electronegativity
When discussing chemical bonding, especially covalent bonds, it is crucial to consider the concept of electronegativity, which measures an atom's tendency to attract electrons in a bond. In this tutorial, we explore how to arrange single covalent bonds in order of increasing polarity.
#### Instructions:
You are given sets of covalent bonds and asked to arrange them based on their polarity. Polarity refers to the distribution of electrical charge over the atoms joined by the bond, with a more polar bond having a greater difference in electronegativity between the bonded atoms.
**Specifics:**
1. Most polar bond is denoted as **b**.
2. Medium polar bond is denoted as **c**.
3. Least polar bond is denoted as **a**.
Using these labels, the expected input format for arranging bonds from least to most polar is **acb**.
*To answer this question, you may consult the table of electronegativity values provided below.*
#### Electronegativity Table:
Here is a periodic table with respective electronegativity values color-coded.
- Colors indicate the range of electronegativity values:
- Green: < 1.0
- Blue: 1.0 - 1.4
- Yellow: 1.5 - 1.9
- Orange: 2.0 - 2.4
- Red: 2.5 - 2.9
- Purple: 3.0 - 4.0
| | 1A | 2A | 3B | 4B | 5B | 6B | 7B | 8B | 1B | 2B | 3A | 4A | 5A | 6A | 7A |
|---|-------|--------|----|----|----|----|----|---------------|------|-----|-------|----|----|----|------|
| H | H 2.1 | | | | | | | | | | | | | | |
| | | Be 1.5 | | | | | | | | | B 2.0 | C
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