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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
All textbooksBrown 15th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 95a
Chapter 9, Problem 95a

a. Predict the electron-domain geometry around the central Xe atom in XeF2, XeF4, and XeF6.

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1
Step 1: Understand the concept of electron-domain geometry. Electron-domain geometry considers all regions of electron density (bonds and lone pairs) around the central atom.
Step 2: Determine the number of valence electrons for Xenon (Xe) and Fluorine (F). Xenon has 8 valence electrons, and each Fluorine has 7 valence electrons.
Step 3: Calculate the total number of valence electrons for each molecule. For XeF2, XeF4, and XeF6, add the valence electrons of Xe and the appropriate number of F atoms.
Step 4: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the electron-domain geometry. Consider the number of bonding pairs and lone pairs around the central Xe atom.
Step 5: For XeF2, XeF4, and XeF6, identify the electron-domain geometry based on the number of electron domains: linear for 2 domains, square planar for 4 domains, and octahedral for 6 domains.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs surrounding a central atom. According to this theory, electron pairs, whether bonding or non-bonding, will arrange themselves to minimize repulsion, leading to specific molecular shapes.
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Electron-Domain Geometry

Electron-domain geometry refers to the spatial arrangement of all electron domains (bonding and lone pairs) around a central atom. This geometry helps in determining the overall shape of the molecule, which can differ from the molecular geometry if there are lone pairs present that affect the arrangement of bonded atoms.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding pairs of electrons. In the case of xenon compounds like XeF2, XeF4, and XeF6, understanding the hybridization of the central xenon atom is crucial for predicting its electron-domain geometry and the resulting molecular shape.
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Related Practice
Textbook Question

An AB5 molecule adopts the geometry shown here.

c. Suppose the B atoms are halogen atoms. Of which group in the periodic table is atom A a member:

i. group 5A

ii. group 6A

iii. group 7A

iv. group 8A, or

v. is more information needed?

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Textbook Question

The O—H bond lengths in the water molecule (H2O) are 0.96 Å, and the H—O—H angle is 104.5°. The overall dipole moment of the water molecule is 1.85 D. b. Calculate the magnitude of the bond dipole of the O─H bonds. (Note: You will need to use vector addition to do this.)

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Textbook Question

Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (a) Draw the Lewis structure of the azide ion that minimizes formal charge (it does not form a triangle). Is it linear or bent?

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Textbook Question

The lactic acid molecule, CH3CH(OH)COOH, gives sour milk its unpleasant, sour taste. e. What are the approximate bond angles around each carbon atom in the molecule?

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Textbook Question

The molecule C4H5N has the connectivity shown here. a. After the Lewis structure for the molecule is completed, how many 𝜎 and how many 𝜋 bonds are there in this molecule?

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Textbook Question

Which of the following statements about hybrid orbitals is or are true? a. After an atom undergoes sp hybridization, there is one unhybridized p orbital on the atom, b. Under 𝑠𝑝2 hybridization, the large lobes point to the vertices of an equilateral triangle, and c. The angle between the large lobes of 𝑠𝑝3 hybrids is 109.5°.