Final answer:
The NH₂-CH=O structure features a nitrogen with a tetrahedral electron-pair geometry and a trigonal pyramidal shape, the first carbon (C1) with a tetrahedral geometry, and the second carbon (C2) with a linear geometry and 180° bond angles.
Step-by-step explanation:
When examining the NH₂-CH=O structure, we can apply the VSEPR theory to determine the geometries and bond angles. The nitrogen (N) atom has three hydrogen (H) atoms and one lone pair of electrons, resulting in a tetrahedral electron-pair geometry, but a trigonal pyramidal local structure due to the lone pair taking up more space. The central carbon atom (C1) in the NH₂ group is single-bonded to four other atoms (N and three Hs), which also results in a tetrahedral electron-pair geometry, as well as a tetrahedral local structure with H-C-H bond angles of approximately 109.5°.
For the carbon atom (C2) in the -CH=O fragment, it is doubly bonded to oxygen (O) and nitrogen (N), forming a linear geometry as there are only two regions of electron density surrounding the carbon. This gives C2 bond angles of approximately 180° around the carbon. Therefore, the statements that C2 will have linear geometry and the bond angles around C2 are approximately equal to 180° are correct, while the statement that C1 will have a tetrahedral geometry is also correct.