Question

question 5 (2 points)
the lewis structure for carbon tetrachloride, ccl4, 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 the number of REDs (Region of Electron Density): In \(CCl_4\), carbon (\(C\)) is the central atom. Carbon has 4 valence electrons and each chlorine (\(Cl\)) atom forms a single bond with carbon. Using the formula for the number of regions of electron density (\(=\text{number of bonding pairs}+\text{number of lone pairs}\)), here, the number of bonding pairs is 4 (since \(C - Cl\) bonds are 4) and the number of lone pairs on \(C\) is 0. So, the number of REDs is 4.
• For the shape: According to VSEPR (Valence - Shell Electron - Pair Repulsion) theory, when the number of regions of electron density around a central atom is 4 and there are no lone pairs on the central atom, the shape is tetrahedral.
• For the bond angles: In a tetrahedral geometry, the bond angles are \(109.5^{\circ}\).

Answer:

1. E. 4
2. O. tetrahedral
3. Q. 109.5