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...
Related questions
Question
This is not a graded question
![**Transcription of Educational Content**
---
**Text:**
Carbon uses [orbitals] hybrid orbitals in the molecule below.
**Diagram:**
The diagram illustrates a Lewis structure of a molecule, specifically Cl-C≡N. Detailed explanation:
- The Chlorine (Cl) atom is depicted with three lone pairs of electrons surrounding it, represented as three pairs of dots.
- The Carbon (C) atom is shown bonded to the Chlorine (Cl) atom via a single bond (−).
- The Carbon (C) atom is also triple-bonded to a Nitrogen (N) atom, depicted with three lines (≡) representing the triple bond.
- The Nitrogen (N) atom is presented with one lone pair of electrons, depicted as a pair of dots beside it.
**Open Space/Box:**
There is an empty rectangular box below the diagram. This might be intended for user input or for providing a response related to the hybrid orbitals used by the Carbon atom in the given molecule.
---
For more detailed understanding:
- **Hybrid Orbitals:** When answering which orbitals carbon uses in this molecule, consider the type of bonds it forms. In this case, carbon forms a triple bond (sp hybridization) and a single bond (sp² hybridization).
For educational purposes, understanding the concept of hybridization can help in predicting the geometry and bond angles within the molecules.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F42517a3c-1f9e-4cb9-8a60-b8d73ceb2073%2F13758efb-92cd-4c34-add4-4ab1d14988d4%2Fjcutgco_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription of Educational Content**
---
**Text:**
Carbon uses [orbitals] hybrid orbitals in the molecule below.
**Diagram:**
The diagram illustrates a Lewis structure of a molecule, specifically Cl-C≡N. Detailed explanation:
- The Chlorine (Cl) atom is depicted with three lone pairs of electrons surrounding it, represented as three pairs of dots.
- The Carbon (C) atom is shown bonded to the Chlorine (Cl) atom via a single bond (−).
- The Carbon (C) atom is also triple-bonded to a Nitrogen (N) atom, depicted with three lines (≡) representing the triple bond.
- The Nitrogen (N) atom is presented with one lone pair of electrons, depicted as a pair of dots beside it.
**Open Space/Box:**
There is an empty rectangular box below the diagram. This might be intended for user input or for providing a response related to the hybrid orbitals used by the Carbon atom in the given molecule.
---
For more detailed understanding:
- **Hybrid Orbitals:** When answering which orbitals carbon uses in this molecule, consider the type of bonds it forms. In this case, carbon forms a triple bond (sp hybridization) and a single bond (sp² hybridization).
For educational purposes, understanding the concept of hybridization can help in predicting the geometry and bond angles within the molecules.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY