Choose the statement that best describes the PbCl4 molecule in the gas phase.

A. The molecule has a dipole moment.

B. The bond angles are all about 109.

C. The molecule is polar.

D. The bonds are non-polar.

E. More than one of these choices are correct.

The correct answer is B. The bond angles are all about 109.

Explanation:

In bibliography or in the periodic table you can see that lead Pb has an electronic configuration of:

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p²

Valencia electrons are the electrons found in the last electronic layer (called valence orbitals). These electrons are what determine the ability of the atom to form bonds. When an element joins another, it does so through its valence electrons.

In this case at the last level, level 6, there are 4 electrons, which are the valence electrons that will react with Cl. Since the compound PbCl₄ has 1 Pb and 4 Cl, this indicates that the 4 valence electrons of the lead Pb will react with each of the chlorine Cl. In this way they comply with the octet rule, which is the tendency of atoms to complete its energy level with eight electrons to achieve stability.

Then, around the central atom, Pb, there are 4 pairs of electrons (4 valence electrons of lead and 4 that are compatible with chlorine). Of these electron pairs, all are bonded. So the geometry is tetrahedral, with a link angle of 109.5 °.

Then, the correct answer is B. The bond angles are all about 109.