Question

question 14 (0.5 points)
the following shape has 1 reds, 2 are bonding and 3 are nonbonding. the shape is called 4 and the bond angles are 5.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 5 g. 6 h. diatomic
i. linear j. planar trigonal k. bent l. tetrahedral m. pyramidal
n. hexahedral o. seesaw p. t - shape q. octahedral r. square pyramidal
s. square planar t. 90° u. 109.5° v. 120° w. 180° x. 90°, 120°, and 180° y. 90° and 180°

Explanation:

• 1. REDs (Regions of Electron Density): Count the total number of electron - density regions (bonding and non - bonding). In this octahedral - like structure (central atom with 6 electron - density regions), there are 6 REDs.
• 2. Bonding REDs: Count the number of atoms bonded to the central atom. There are 4 atoms bonded (green spheres), so 4 bonding REDs.
• 3. Non - bonding REDs: Subtract the number of bonding REDs from the total REDs. \(6 - 4=2\) non - bonding REDs.
• 4. Shape: With 4 bonding and 2 non - bonding electron - density regions, the molecular shape is square planar.
• 5. Bond angles: In a square planar geometry, the bond angles are \(90^{\circ}\) (between adjacent atoms) and \(180^{\circ}\) (for atoms opposite each other).

Answer:

1. G. 6
2. E. 4
3. C. 2
4. S. square planar
5. Y. \(90^{\circ}\) and \(180^{\circ}\)