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.

The hybridization of carbon is given below

Answered: Carbon uses [orbitals] hybrid orbitals…

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Chemistry

Carbon uses [orbitals] hybrid orbitals in the molecule below. :CI-C=N: 1—C=N:

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 67AE: Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability,...

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