Topic - Chemistry: Chemical Bonding and Molecular Structure
Step 1: Understanding the Question:
We need to identify the molecule where the vector sum of all individual bond dipole moments is zero.
Step 2: Key Formula or Approach:
A molecule has a zero dipole moment (\(\mu = 0\)) if it is perfectly symmetrical and the bond dipoles cancel each other out.
Step 3: Detailed Explanation:
1. \(NH_3\): It has a pyramidal shape with a lone pair. The bond dipoles and lone pair moment add up, so \(\mu \neq 0\).
2. \(H_2O\): It has a bent (V-shape) structure with two lone pairs. The dipoles do not cancel, so \(\mu \neq 0\).
3. \(NF_3\): Similar to \(NH_3\), it has a pyramidal shape. Although \(N-F\) dipoles oppose the lone pair, they don't cancel perfectly, so \(\mu \neq 0\).
4. \(CCl_4\): It has a perfect tetrahedral geometry. All four \(C-Cl\) bonds are identical and directed towards the corners of a tetrahedron. The vector sum of these four dipoles is exactly zero.
Step 4: Final Answer:
\(CCl_4\) has a net dipole moment of zero.