Question

The atomic radius of silver (Ag) is closest to which of the following values?

• A. \( 144 \, \mathrm{pm} \)
• B. \( 172 \, \mathrm{pm} \)
• C. \( 160 \, \mathrm{pm} \)
• D. \( 128 \, \mathrm{pm} \)

Hint:

The atomic radius generally decreases across a period from left to right and increases as you move down a group in the periodic table. Transition metals like silver (Ag) have slightly smaller radii than expected due to the increasing nuclear charge and the shielding effect of the d-orbitals.

Answer 1

The Correct Option is A

The atomic radius of an element is defined as the distance from the nucleus to the outermost shell of electrons. This size is influenced by several factors, including the nuclear charge, the number of electron shells, and the shielding effect from inner electrons. It is typically measured in picometers (pm) or angstroms (Å).
Step 1: Define the Atomic Radius of Silver. Silver (Ag) is a transition metal with an atomic number of 47. The electron configuration of silver is \( [\text{Kr}] \, 4d^{10} \, 5s^1 \), meaning that silver has a filled \( 4d \)-subshell and a single electron in its outermost \( 5s \)-orbital. The atomic radius is influenced by: Metallic bonding: The metallic bonding in silver results in a relatively large atomic radius, as the electrons are delocalized. Shielding effect: The inner electrons in the \( [\text{Kr}] \) core shield the outer electron from the full nuclear charge, allowing for a larger radius.
Step 2: Reference Values for Atomic Radius. According to experimental data and periodic trends, the **atomic radius** of silver is: \[ \text{Atomic radius of Ag} = 144 \, \mathrm{pm}. \]
Step 3: Comparison with Options. When we compare this value to the given options: - Option (1) \( 144 \, \mathrm{pm} \) matches the known value for the atomic radius of silver.
Conclusion: Thus, the atomic radius of silver (Ag) is \( \mathbf{144 \, \mathrm{pm}} \), which corresponds to option \( (1) \).