**Drawing the Lewis Structure for Xenon Tetrafluoride (XeF₄)**Welcome to our interactive learning session on the Lewis structures of molecules! Today, we will focus on drawing the Lewis structure for xenon tetrafluoride (XeF₄).### Step-by-Step Guide1. **Identify the Total Number of Valence Electrons:** - Xenon (Xe) has 8 valence electrons. - Each fluorine (F) atom has 7 valence electrons. - Total number of valence electrons in XeF₄: \( 1 \, \text{Xe} \times 8 \, \text{electrons} + 4 \, \text{F} \times 7 \, \text{electrons} = 8 + 28 = 36 \, \text{electrons} \).2. **Draw the Skeleton Structure:** - Place the least electronegative atom (Xe) in the center. - Attach the four fluorine atoms to the xenon atom using single bonds.3. **Distribute the Remaining Electrons:** - Each single bond (X-F) requires 2 electrons, thus, 4 bonds use \( 4 \times 2 = 8 \) electrons. - Subtract the bonded electrons from the total valence electrons: \( 36 - 8 = 28 \) electrons remaining. - Distribute these remaining 28 electrons around the fluorine atoms, ensuring each fluorine receives 8 electrons to complete its octet (bonding pair + lone pairs).4. **Distribute Lone Pairs to Central Atom:** - After satisfying the octets of the fluorine atoms, any remaining electrons are placed on the central xenon atom. - Xenon can accommodate more than 8 electrons (expanded octet) because it is in Period 5 of the periodic table.### Diagram Tools- There is an interactive canvas on the right with tools for drawing: - **Bond Tool (single bond):** Used to draw bonds between atoms. - **Lone Pair Electron Tool:** Used for adding lone pairs to atoms. - **Erase Tool:** For correcting mistakes. - **Undo Button:** To revert the last action. - **Help Button (? symbol):** Access help documentation.These tools will aid in accurately representing the Lewis structure of XeF

Answered: Image /qna-images/answer/5358cae4-ca45-4973-9601-1f3c5d987b64.jpg

Answered: Draw the Lewis structure for the xenon…

Draw the Lewis structure for the xenon tetrafluoride (XeF4) molecule.

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...

Similar questions

Draw Lewis structures for CCl 4 and C 2Cl 4. Give the molecular shape around each carbon atom. Explain why the carbon atoms in the two molecules have different shapes.
Write the Lewis structure for carbonate ion.
The physical and chemical properties of a molecule depend on its structure. Here are two ball-and-stick models for two compounds that have the same molecular formula but different structures and different chemical properties. Ethanol Dimethyl ether
Draw the Lewis structure of FeCl3.6H2O and FeCl2.4H2O.
Why SiH4 has lowest freezing point than CH4?
Draw the lewis structure of the neutralatom and the ion of nitrogen
What is the molecular geometry of ClF4+? Be detailed (Lewis structure, electron arrangement, and molecular geometry). Draw its structure
What Lewis structure describes BF3?
What is the Lewis structure of C61H67N9O17S4.
Illustrate the Lewis structure for C2Cl4. Determine the polarity of the compound.
What is the greenhouse effect? How does the excess CO2 gas in the atmosphere cause the greenhouse effect?
Write the Lewis structure for XeF4.