Question

question 4 (2 points)
the lewis structure for nitrogen trichloride, ncl3, has 1 reds, the shape is 2, and the bond angles are 3°.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 5 g. 6 h. 7 i. 8
j. no shape, atoms or ions k. diatomic l. linear m. trigonal planar
n. bent o. tetrahedral p. pyramidal q. 109.5 r. 120 s. 180
t. no bond angles, no central atom

Explanation:

• For REDs (Region of Electron Density): Nitrogen has 5 valence electrons. In \(NCl_3\), it forms 3 single bonds with Cl atoms (using 3 electrons) and has 1 lone pair (2 electrons). So, the total number of REDs is \(3 + 1=4\) (single bonds + lone pairs).
• For shape: Using VSEPR (Valence - Shell Electron - Pair Repulsion) theory, with 4 REDs (3 bonding pairs and 1 lone pair), the molecular shape is pyramidal.
• For bond angles: For a molecule with 4 REDs (in a tetrahedral electron - pair geometry) and 1 lone pair, the bond angles are approximately \(109.5^{\circ}\) (close to the tetrahedral bond angle of \(109.5^{\circ}\) but slightly less due to lone - pair repulsion).

Answer:

1. E. 4
2. P. pyramidal
3. Q. 109.5