Question

question 4 (2 points)
consider carbon tetrachloride, ccl₄. the lewis structure has 4 single bonds and no double bonds.
the number of reds is 1.
the bond angles are 2° and the shape is 3.
ccl₄ is a 4 symmetrical/asymmetrical molecule.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 180 g. 90 h. 120
i. 109.5 j. diatomic k. linear k. planar trigonal m. bent
n. pyramidal o. tetrahedral p. symmetrical q. asymmetrical

Explanation:

• Number of REDs (Region of Electron Density): In \(CCl_4\), carbon forms 4 single bonds (no lone pairs). So, the number of REDs is equal to the number of bonding pairs.
• Bond Angles: For a molecule with 4 REDs (tetrahedral electron - pair geometry), the bond angles are \(109.5^{\circ}\).
• Shape: Since there are 4 bonding pairs and no lone pairs, the molecular shape (based on VSEPR theory) is tetrahedral.
• Symmetry: \(CCl_4\) has a symmetrical tetrahedral shape. All the \(C - Cl\) bonds are identical and the dipoles (if any, but \(C\) and \(Cl\) have a small electronegativity difference and the symmetry cancels out any net dipole) are symmetrically arranged. So, it is a symmetrical molecule.

Answer:

1. E. 4
2. I. 109.5
3. O. tetrahedral
4. P. symmetrical