The experimental Pb¬Cl bond length in lead(II)chloride, PbCl2, is 244 pm. Based on this value and data in Figure 7.7, predict the atomic radius of Pb.

Verified step by step guidance

1. Identify the given bond length of Pb-Cl in PbCl2, which is 244 pm.
2. Recognize that the bond length is the sum of the atomic radii of Pb and Cl.
3. Look up the atomic radius of Cl from the periodic table, which is 99 pm.
4. Set up the equation: Bond length = Atomic radius of Pb + Atomic radius of Cl.
5. Solve for the atomic radius of Pb by subtracting the atomic radius of Cl from the bond length: Atomic radius of Pb = Bond length - Atomic radius of Cl.

Key Concepts

Bond Length

Bond length is the distance between the nuclei of two bonded atoms. In the case of lead(II) chloride (PbCl2), the experimental bond length of 244 pm indicates the spatial arrangement of lead and chlorine atoms in the compound. This measurement can provide insights into the size of the lead atom, as bond lengths are influenced by the atomic radii of the participating elements.

Atomic Radius

Atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. It varies across the periodic table, generally increasing down a group due to the addition of electron shells and decreasing across a period due to increased nuclear charge. Understanding atomic radius is crucial for predicting chemical behavior and bonding characteristics.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as one moves across or down the periodic table. For instance, atomic radius decreases across a period from left to right and increases down a group. These trends help in estimating the atomic radius of lead based on its position in the periodic table and the bond length provided.