Questions: There are REDs (Regions of Electron Density) around the central atom a. 0 b. 1 c. 2. d. 3 e. 4 The shape at the central atom is f. diatomic g. linear h. trigonal planar i. bent (120°) j. tetrahedral k. pyramidal l. bent (109.5°) If all of the bonds are polar covalent, is the molecule itself polar? m. yes n. no

There are REDs (Regions of Electron Density) around the central atom a. 0 b. 1 c. 2. d. 3 e. 4 The shape at the central atom is f. diatomic g. linear h. trigonal planar i. bent (120°) j. tetrahedral k. pyramidal l. bent (109.5°) If all of the bonds are polar covalent, is the molecule itself polar? m. yes n. no
Transcript text: There are $\square$ REDs (Regions of Electron Density) around the central atom a. 0 b. 1 c. 2. d. 3 e. 4 The shape at the central atom is $\square$ f. diatomic g. linear h. trigonal planar i. bent $\left(120^{\circ}\right)$ j. tetrahedral k. pyramidal l. bent $\left(109.5^{\circ}\right)$ If all of the bonds are polar covalent, is the molecule itself polar? $\square$ m. yes n. no
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Solution

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Solution Steps

Step 1: Determine the Number of Regions of Electron Density (REDs)

To determine the number of regions of electron density (REDs) around the central atom, we need to consider both bonding pairs and lone pairs of electrons. The number of REDs can be found by examining the Lewis structure of the molecule.

Step 2: Identify the Shape at the Central Atom

The shape at the central atom is determined by the number of REDs and the arrangement of these regions around the central atom. This can be predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory.

Step 3: Determine the Polarity of the Molecule

If all the bonds are polar covalent, the overall polarity of the molecule depends on the symmetry of the molecule. If the molecule is symmetrical, the dipoles may cancel out, resulting in a nonpolar molecule. If the molecule is asymmetrical, the dipoles do not cancel out, resulting in a polar molecule.

Final Answer

  1. The number of REDs around the central atom is \(\boxed{4}\).
  2. The shape at the central atom is \(\boxed{\text{tetrahedral}}\).
  3. If all of the bonds are polar covalent, the molecule itself is \(\boxed{\text{yes}}\).
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