21. This is the Lewis structure for acetic acid. The bond angles are not drawn to scale. Predict the H—C—H bond angle, in degrees A. 90° B. 109.5° C. 120° D. 180°
Added by Luc-A T.
Close
Step 1
This is because oxygen has two lone pairs of electrons and two bonded pairs of electrons. The bond angle in this type of molecular geometry is typically 109.5 degrees. Show more…
Show all steps
Your feedback will help us improve your experience
Jennifer Hudspeth and 95 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The C-C=O bond angle in acetic acid, shown below, is closest to 180°. 90°. 109.5°. 120°.
Jennifer H.
Sri K.
The bond angles in $\mathrm{H}_{3} \mathrm{O}^{+}$ are less than _______ and greater than _______. SOLUTION The carbon atom in $\mathrm{CH}_{4}$ has no lone pairs; its bond angles are $109.5^{\circ} .$ The oxygen atom in $\mathrm{H}_{3} \mathrm{O}^{+}$ has one lone pair. A lone pair is more diffuse than a bonding pair, so the $\mathrm{O}-\mathrm{H}$ bonds squeeze together to minimize electron repulsion. However, they do not squeeze as closely together as they do in water $\left(104.5^{\circ}\right),$ where oxygen has two lone pairs. Therefore, the bond angles in $\mathrm{H}_{3} \mathrm{O}^{+}$ are less than $109.5^{\circ}$ and greater than $104.5^{\circ} .$
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD