Question

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):

• In VSEPR theory, for a molecule with 3 bonding pairs and 1 non - bonding pair (total 4 REDs).

1. Bonding and Non - bonding:

• From the structure (3 green atoms bonded to the central red atom), there are 3 bonding REDs.
• Using the formula \(n=\text{bonding pairs}+\text{non - bonding pairs}\), if \(n = 4\) and bonding pairs \(= 3\), then non - bonding pairs \(=1\).

1. Molecular Shape:

• A molecule with 3 bonding pairs and 1 non - bonding pair of electrons around the central atom has a pyramidal shape.

1. Bond Angles:

• For a pyramidal shape (derived from a tetrahedral electron - pair geometry, where the ideal tetrahedral angle is \(109.5^{\circ}\), but the presence of a lone pair slightly compresses the bond angles, and the approximate bond angle is \(109.5^{\circ}\)).

Answer:

1. E. 4
2. D. 3
3. B. 1
4. M. pyramidal
5. U. \(109.5^{\circ}\)