🤓 Based on our data, we think this question is relevant for Professor Halihan's class at OKSTATE.
Electron Regions Electronic Geometry Bond Angles
2 linear 180˚
3 trigonal planar 120˚
4 tetrahedral 109.5˚
5 trigonal bipyramidal 90˚, 120˚, and 180˚
6 octahedral 90˚ and 180˚
For NH3: N is the central atom.
Total valence electrons:
Group Valence Electrons
N 5A 1 × 5 e– = 5 e–
H 1A 3 × 1 e– = 3 e–
Total: 8 valence e–
Why is the H–N–H angle in NH3 smaller than the H–C–H bond angle in CH4? Why is the H–N–H angle in NH4+ identical to the H–C–H bond angle in CH4?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Bond Angles concept. You can view video lessons to learn Bond Angles. Or if you need more Bond Angles practice, you can also practice Bond Angles practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Halihan's class at OKSTATE.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.