QQuestionChemistry
QuestionChemistry
Write the following for KrF₄:
Lewis structure
Molecular geometry
Hybridization
Bond angle(s)
Polarity
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this problem step by step for KrF₄, carefully following the LaTeX formatting guidelines:
Step 2:: Determine the Central Atom and Valence Electrons
- Total valence electrons: $$8 + (4 \times 7) = 36$$ electrons
- Central atom is Kr (Krypton) - Kr is in Group 18 with 8 valence electrons - Each F atom contributes 7 valence electrons
Step 3:: Lewis Structure
\begin{array}{c}
- Arrange F atoms symmetrically around Kr - Place single bonds between Kr and each F atom - Distribute remaining electrons as lone pairs - Lewis structure shows: F \ | \ Kr \ | \ F \end{array} - Four single Kr-F bonds - Multiple lone pairs on Kr and F atoms
Step 4:: Molecular Geometry
- Central atom Kr has 4 bonds and 0 lone pairs - Molecular geometry is square planar - Follows AX₄ molecular geometry type
Step 5:: Hybridization
- Kr uses $$d^{2}sp^{2}$$ hybridization
- Combines 2 d-orbitals and 2 p-orbitals - Creates four equivalent hybrid orbitals in square planar arrangement
Step 6:: Bond Angles
- Bond angles are $$90°$$ between adjacent F atoms
- Square planar geometry - Symmetric arrangement around Kr
Step 7:: Polarity
- Despite symmetric geometry - Kr-F bonds are polar due to electronegativity difference - Net molecular polarity is zero due to symmetrical arrangement
Final Answer
- Lewis Structure: Square planar KrF₄ with single Kr-F bonds - Molecular Geometry: Square planar - Hybridization: d^{2}sp^{2} - Bond Angles: 90° - Polarity: Non-polar molecule
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students