Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Concept explainers

Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds b…
Polarizability In Organic Chemistry
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Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate…
Question

review the section on Bond Polarity and Partial Ionic Character and the figure that has ionic character on the Y axis and delta EN on the X axis (this is figure 9.24 on page 393 of the 8th edition).

Review the graph and Critique the following statement: HF is a covalent molecule and LiI is an ionic compound. Provide as much detail and explanation as possible in 100 word or less. As stated previously, equations, formulas etc. may be substituted for words.

**Figure 9.24** - ΔEN Ranges for Classifying the Partial Ionic Character of Bonds This figure illustrates how the difference in electronegativity (ΔEN) between two bonded atoms can be used to classify the type of bond based on its ionic character. The vertical gradient bar is labeled with different ΔEN values and associated bond types: - ΔEN from 0.0 to 0.4: **Nonpolar covalent** bonds - ΔEN from 0.4 to 1.7: **Mostly covalent** bonds - ΔEN from 1.7 to 3.3: **Polar covalent** bonds - ΔEN above 3.3: **Mostly ionic** bonds On the right side of the gradient bar, there are illustrations showing the distribution of electron density in these types of bonds: 1. **Nonpolar covalent**: Shown with two identical atoms sharing electrons equally. The electron cloud is symmetrically distributed. 2. **Polar covalent**: Depicted with one atom partially positive (δ+) and the other partially negative (δ-), indicating uneven electron distribution. 3. **Mostly ionic**: The electron cloud is shown significantly shifted toward the atom with higher electronegativity, forming a clear positive and negative side. This diagram helps in understanding how electronegativity differences affect bond character, ranging from equal sharing (nonpolar covalent) to complete transfer of electrons (mostly ionic).
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Transcribed Image Text:**Figure 9.24** - ΔEN Ranges for Classifying the Partial Ionic Character of Bonds This figure illustrates how the difference in electronegativity (ΔEN) between two bonded atoms can be used to classify the type of bond based on its ionic character. The vertical gradient bar is labeled with different ΔEN values and associated bond types: - ΔEN from 0.0 to 0.4: **Nonpolar covalent** bonds - ΔEN from 0.4 to 1.7: **Mostly covalent** bonds - ΔEN from 1.7 to 3.3: **Polar covalent** bonds - ΔEN above 3.3: **Mostly ionic** bonds On the right side of the gradient bar, there are illustrations showing the distribution of electron density in these types of bonds: 1. **Nonpolar covalent**: Shown with two identical atoms sharing electrons equally. The electron cloud is symmetrically distributed. 2. **Polar covalent**: Depicted with one atom partially positive (δ+) and the other partially negative (δ-), indicating uneven electron distribution. 3. **Mostly ionic**: The electron cloud is shown significantly shifted toward the atom with higher electronegativity, forming a clear positive and negative side. This diagram helps in understanding how electronegativity differences affect bond character, ranging from equal sharing (nonpolar covalent) to complete transfer of electrons (mostly ionic).
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