15 ! describe the characteristics of a molecule of ammonia (nh3). the lewis structure and table of electronegative are given. the bond polarities are blank, the molecular shape is blank 2, and the molecule is blank 3. blank 1 options: nonpolar, polar blank 2 options: bent, linear, tetrahedral, trigonometry planar, trigonal pyramidal. blank 3 options: nonpolar, polar each blank has one option.

Blank 1: polar
The difference in electronegativity between N and H causes electrons to preferentially orbit N, making the bond polar.

Blank 2: trigonal pyramidal
There are four “things” attached to N - 3 H’s and 1 lone pair of electrons. The four things together are arranged into a tetrahedral formation. However, the lone pairs don’t actually contribute to the shape of the molecule per se; it’s only the actual atoms that do. The lone pair creates a bit of repulsion that pushes the 3 H’s down, creating a trigonal pyramidal shape (as opposed to a trigonal planar one).

Blank 3: polar
The molecule as a whole is also polar because the “things” around it, though arranged in a tetrahedral pattern, are not all the same. The side of the molecule with the lone pair is slightly negative, while the side with the 3 H’s is slightly positive due to the differences in electronegativity described above.

Ireally don’t know this

The closer the atoms are to becoming ionic the more highly dense the negatively charged side gets.