For the carbon atom highlighted in the given structure, indicate the hybridization, bond angles, and the shape around the atom. H—C?N The hybridization is: sp3 sp sp2 The bond angle is: 109.5° ~120° 180° The shape is: tetrahedral linear trigonal planar
Added by Lourdes S.
Close
Step 1
Hybridization: The carbon atom is bonded to three atoms (one hydrogen and two nitrogen atoms). Therefore, it needs three orbitals to form these bonds. The hybridization that allows for three orbitals is sp2. Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 69 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 hybridization of the nitrogen and the triple-bonded carbon are sp2, giving trigonal planar geometry (C≡N are linear) and a bond angle around the triple-bonded carbon of 180°. The CH3 carbon is sp3 hybridized, tetrahedral geometry, with bond angles about 109°.
Kaden B.
A molecule has sp3d2 hybridization with 1 lone pair. The electron pair geometry of this molecule is: octahedral. The geometry of this molecule is: octahedral. This molecule will have approximate bond angles of (If more than one bond angle is possible, separate each with a space.):
Jennifer H.
Give the hybridization, shape, and bond angle for each carbon in CH3CN. Check all that apply. C — sp3, linear, 109.5° C — sp2, tetrahedral, 109.5° CH3 — sp3, linear, 109.5° CH3 — sp, linear, 180° CH3 — sp2, tetrahedral, 180° C — sp, tetrahedral, 180° C — sp, linear, 180° CH3 — sp3, tetrahedral, 109.5°
Adi S.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD