In the attached picture, predict the ideal bond angle(s) around each central atom in the molecule.
Hint: Ignore the angles shown in the 2-dimensional Lewis structure and instead, consider what shape the molecule would have in three dimensions. (Ignore any resonance effects.)© BrainMass Inc. brainmass.com December 24, 2021, 10:48 pm ad1c9bdddf
SOLUTION This solution is FREE courtesy of BrainMass!
This is cyanamide:
N?C - NH2
The valence shell of C has 8 electrons, 6 in the triple bond and 2 in the single bond. As it has no lone pairs, the triple and single bonds will be at 180° to one another. The singly bonded N has 8 electrons in its outer shell, 3 single bonds (with 2 electrons each) and a lone pair. These 4 pairs of electrons will take up a tetrahedral arrangement but the repulsion due to the lone pair is slightly greater than that due to the bonding pairs so the bonds will be squeezed slightly closer than the regular tetrahedral angle of 109.5°. Possibly the CNH and HNH angles would be about 107° (as in ammonia).