QQuestionChemistry
QuestionChemistry
Please show work.
Lewis Dot Structure:
Electron Pair Geometry
Molecule Shape
Polar/Nonpolar
For H^2Se:
1)
i) What type of intermolecular forces are between molecules of H^2Se? Explain WHY.
ii) Which would have the higher boiling point, H^2Se or H^2O? Explain WHY.
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 step by step, focusing on the Lewis dot structure and intermolecular forces for H^2Se.
Step 2:: Lewis Dot Structure Analysis
- Total valence electrons: $$6 + (2 \times 1) = 8$$ electrons
- Selenium (Se) is in Group 16 (VIA), has 6 valence electrons - Hydrogen (H) has 1 valence electron - Central atom is Se - Structure will be H-Se-H with two lone pairs on Se
Step 3:: Electron Pair Geometry
- $$AX_{2}E_{2}$$ molecular geometry
- Central Se has 4 electron domains (2 bonding, 2 non-bonding) - Electron pair geometry is tetrahedral - Bent molecular shape (due to lone pairs)
Step 4:: Intermolecular Forces in H^2Se
- Primarily weak van der Waals (London dispersion) forces - Reasons:
Step 5:
Molecule is non-polar but has temporary induced dipoles
Step 6:
Larger molecular weight increases dispersion forces
Step 7:
Weak hydrogen bonding possible, but much weaker than H^2O
Step 8:: Boiling Point Comparison
- H^2O has stronger hydrogen bonding - Hydrogen bonds in H^2O are much stronger than London forces in H^2Se - Therefore, H^2O will have a higher boiling point
Final Answer
i) Intermolecular forces: Primarily London dispersion forces ii) H^2O would have the higher boiling point due to strong hydrogen bonding
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