Draw the Lewis structure for the covalent-bonded compound ammonia.

Sure, here are the steps to draw the Lewis structure for the covalent-bonded compound ammonia (NH3):

1. Identify the total number of valence electrons: Nitrogen (N) has 5 valence electrons and Hydrogen (H) has 1 valence electron. Since there are 3 Hydrogen atoms, the total number of valence electrons is 5 (from N) + 3*1 (from 3H) = 8 valence electrons.

2. Draw a skeleton structure of the molecule: Place the least electronegative atom in the center (Nitrogen in this case) and the other atoms (Hydrogen) around it. Draw a single bond (a line) between the central atom and the surrounding atoms. Each line represents 2 electrons.

3. Distribute the remaining electrons as lone pairs: After drawing the single bonds, you have used 2*3 = 6 electrons. You have 2 electrons left (8-6=2). Place these remaining electrons on the central atom (Nitrogen).

4. Check the octet rule: Each atom in the molecule should have an octet (8 electrons) except Hydrogen, which can only have a duet (2 electrons). In this case, each Hydrogen has 2 electrons (from the bond with Nitrogen) and Nitrogen has 8 electrons (3 from the bonds with Hydrogen and 2 lone pair electrons), so the octet rule is satisfied.

So, the Lewis structure for NH3 (ammonia) is N with three H's surrounding it in a 'V' shape, and a lone pair of electrons on the top of the 'V'.