### Topic: Bond Angles in the Iodine Tetrachloride Ion \((ICl_4^-)\) #### Question: What is the expected Cl-I-Cl bond angle in the iodine tetrachloride ion \((ICl_4^-)\)? #### Diagram Description: The diagram shows the structural representation of the iodine tetrachloride ion \((ICl_4^-)\). It displays an iodine (I) atom centrally bonded to four chlorine (Cl) atoms. The chlorine atoms are positioned around the iodine atom in a plane, each with three lone pairs of electrons. The iodine atom also has two lone pairs on the perpendicular axis to the square plane of the chlorines, making the structure square planar. The single negative charge is indicated outside the brackets that enclose the entire structure. #### Answer Choices: 1. 90 2. < 109.5 3. 109.5 4. 120 ### Explanation: The iodine tetrachloride ion \((ICl_4^-)\) adopts a square planar geometry due to the presence of two lone pairs of electrons on the central iodine atom. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the lone pairs are positioned opposite each other, reducing the repulsion between them, which arranges the chlorine atoms in a planar configuration around the iodine. Given this geometry: - The expected Cl-I-Cl bond angle in a square planar geometry is \(90^\circ\). **Correct Answer: 90** ### Key Concepts: - **VSEPR Theory**: This theory helps predict the shape of the molecule by minimizing the repulsion between electron pairs around the central atom. - **Square Planar Geometry**: This specific arrangement results in bond angles of \(90^\circ\) between adjacent bonding pairs. Understanding the bond angles in molecular structures such as \((ICl_4^-)\) assists in comprehending the spatial arrangement of atoms, which is crucial for predicting the physical and chemical properties of the molecule.
### Topic: Bond Angles in the Iodine Tetrachloride Ion \((ICl_4^-)\) #### Question: What is the expected Cl-I-Cl bond angle in the iodine tetrachloride ion \((ICl_4^-)\)? #### Diagram Description: The diagram shows the structural representation of the iodine tetrachloride ion \((ICl_4^-)\). It displays an iodine (I) atom centrally bonded to four chlorine (Cl) atoms. The chlorine atoms are positioned around the iodine atom in a plane, each with three lone pairs of electrons. The iodine atom also has two lone pairs on the perpendicular axis to the square plane of the chlorines, making the structure square planar. The single negative charge is indicated outside the brackets that enclose the entire structure. #### Answer Choices: 1. 90 2. < 109.5 3. 109.5 4. 120 ### Explanation: The iodine tetrachloride ion \((ICl_4^-)\) adopts a square planar geometry due to the presence of two lone pairs of electrons on the central iodine atom. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the lone pairs are positioned opposite each other, reducing the repulsion between them, which arranges the chlorine atoms in a planar configuration around the iodine. Given this geometry: - The expected Cl-I-Cl bond angle in a square planar geometry is \(90^\circ\). **Correct Answer: 90** ### Key Concepts: - **VSEPR Theory**: This theory helps predict the shape of the molecule by minimizing the repulsion between electron pairs around the central atom. - **Square Planar Geometry**: This specific arrangement results in bond angles of \(90^\circ\) between adjacent bonding pairs. Understanding the bond angles in molecular structures such as \((ICl_4^-)\) assists in comprehending the spatial arrangement of atoms, which is crucial for predicting the physical and chemical properties of the molecule.
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
Concept explainers
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
Question
Q55
Transcribed Image Text:### Topic: Bond Angles in the Iodine Tetrachloride Ion \((ICl_4^-)\)
#### Question:
What is the expected Cl-I-Cl bond angle in the iodine tetrachloride ion \((ICl_4^-)\)?
#### Diagram Description:
The diagram shows the structural representation of the iodine tetrachloride ion \((ICl_4^-)\). It displays an iodine (I) atom centrally bonded to four chlorine (Cl) atoms. The chlorine atoms are positioned around the iodine atom in a plane, each with three lone pairs of electrons. The iodine atom also has two lone pairs on the perpendicular axis to the square plane of the chlorines, making the structure square planar. The single negative charge is indicated outside the brackets that enclose the entire structure.
#### Answer Choices:
1. 90
2. < 109.5
3. 109.5
4. 120
### Explanation:
The iodine tetrachloride ion \((ICl_4^-)\) adopts a square planar geometry due to the presence of two lone pairs of electrons on the central iodine atom. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the lone pairs are positioned opposite each other, reducing the repulsion between them, which arranges the chlorine atoms in a planar configuration around the iodine.
Given this geometry:
- The expected Cl-I-Cl bond angle in a square planar geometry is \(90^\circ\).
**Correct Answer: 90**
### Key Concepts:
- **VSEPR Theory**: This theory helps predict the shape of the molecule by minimizing the repulsion between electron pairs around the central atom.
- **Square Planar Geometry**: This specific arrangement results in bond angles of \(90^\circ\) between adjacent bonding pairs.
Understanding the bond angles in molecular structures such as \((ICl_4^-)\) assists in comprehending the spatial arrangement of atoms, which is crucial for predicting the physical and chemical properties of the molecule.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
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