Question

question 12 (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 (Region of Electron Density):

• In the given molecular - like structure (assuming it's a common electron - pair geometry), if we count the positions around the central atom (red sphere) where electrons are located (either in bonding or non - bonding pairs). For an octahedral - like electron - pair geometry (since there are 6 positions around the central atom), the number of REDs is 6.

1. Bonding REDs:

• Looking at the green spheres (which represent atoms bonded to the central atom), there are 6 bonding regions.

1. Non - bonding REDs:

• Since all the electron - density regions are involved in bonding (no lone pairs indicated by the structure), the number of non - bonding REDs is 0.

1. Shape Name:

• When there are 6 bonding pairs and 0 non - bonding pairs, the molecular shape is octahedral.

1. Bond Angles:

• In an octahedral geometry, the bond angles are \(90^{\circ}\) and \(180^{\circ}\). For example, the bonds along the axes (e.g., \(x\), \(y\), \(z\)) have \(90^{\circ}\) angles between adjacent bonds in the plane perpendicular to an axis and \(180^{\circ}\) for bonds along a straight line (e.g., along the \(x\) - axis).

Answer:

1. G. 6
2. G. 6
3. A. 0
4. Q. octahedral
5. Y. \(90^{\circ}\) and \(180^{\circ}\)