`Ag^(+)` is isoelectronic with

Options

A. `Cu^(2+)`
B. `Zn^(2+)`
C. `Cd^(2+)`
D. `Pd^(2+)`

Explanation

To determine which ion is isoelectronic with Ag^(+), we need to follow these steps:

### Step 1: Understand the concept of isoelectronic species
Isoelectronic species are atoms or ions that have the same number of electrons.

**Hint:** Remember that isoelectronic species can be different elements or ions, but they must have the same total number of electrons.

### Step 2: Determine the number of electrons in Ag^(+)
Silver (Ag) has an atomic number of 47, which means it has 47 electrons in its neutral state. When it loses one electron to form Ag^(+), it has:
\[ 47 - 1 = 46 \text{ electrons} \]

**Hint:** Always subtract the charge from the atomic number to find the number of electrons in an ion.

### Step 3: Identify potential candidates
We need to find an element or ion that also has 46 electrons. We can look at elements and their common oxidation states to find a match.

**Hint:** Consider elements from the periodic table that are close in atomic number to silver.

### Step 4: Check the electron configuration of potential candidates
- **Cadmium (Cd)** has an atomic number of 48. In its neutral state, it has 48 electrons. When it loses two electrons to form Cd^(2+), it has:
\[ 48 - 2 = 46 \text{ electrons} \]
Thus, Cd^(2+) is isoelectronic with Ag^(+).

**Hint:** Look for elements in the same group or period as the element in question, as they often have similar properties.

### Step 5: Conclusion
The ion that is isoelectronic with Ag^(+) is Cd^(2+).

**Final Answer:** Cd^(2+)

### Summary of Steps:
1. Understand isoelectronic species.
2. Calculate the number of electrons in Ag^(+).
3. Identify potential candidates with 46 electrons.
4. Verify the electron count of candidates.
5. Conclude that Cd^(2+) is isoelectronic with Ag^(+).