Final answer:
To complete the Lewis dot structure for NH₂Cl, one must arrange N as the central atom, calculate the total valence electrons, create single bonds with H and Cl, add lone pairs to fulfill the octet rule, and use a double bond if necessary to complete the octets.
Step-by-step explanation:
To complete the Lewis dot structure of NH₂Cl, we must follow a series of steps, which involve arranging atoms, determining valence electrons, and forming bonds while taking into account lone pairs and octets:
Arrange the atoms with nitrogen (N) as the central atom, hydrogen (H) and chlorine (Cl) atoms as terminals.
Determine the total number of valence electrons. Nitrogen has 5, each hydrogen has 1 (for a total of 2 from hydrogen), and chlorine has 7, adding up to 14 valence electrons in total.
Place a single bond between nitrogen and each hydrogen, and between nitrogen and chlorine, using up 6 electrons.
Add three lone pairs to chlorine to give it an octet, using another 6 electrons.
This leaves 2 electrons, which are placed as a lone pair on nitrogen.
Now nitrogen has only 6 electrons around it; to complete its octet, we form a double bond by using a lone pair from either oxygen or chlorine. Since oxygen is not present in this compound, we ignore this option. Nitrogen cannot form a double bond with chlorine, so the central nitrogen atom simply keeps the lone pair and the structure is complete with single bonds only.
Place the final lone pair on the nitrogen to give it a stable electron configuration.
The final Lewis structure of NH₂Cl will have a pair of electrons on nitrogen, single bonds connecting nitrogen to each hydrogen and to chlorine, and chlorine with three lone pairs.