among the following series of transition metal ions, the one where all ions have some 3d electronic configuration is

Options

A. `Ti^(2+),Cr^(4+), Mn^(5+),V^(3+) `
B. `Ti^(3+), Ni^(2+), Co^+, Zn^(2+)`
C. `Sc^(2+), Ti^(2+), V^(2+), Cr(2+)`
D. `Mn^(5+), Co^(4+), Ni^(3+),Cu^(2+)`

Answer

To solve the question of which series of transition metal ions has all ions with the same 3d electronic configuration, we will analyze the electronic configurations of the given transition metal ions in each option step by step.

### Step 1: Identify the Electronic Configurations of the Transition Metals
We will first write down the electronic configurations of the transition metals in their neutral states.

1. **Titanium (Ti)** - Atomic number 22:
Configuration: \( \text{Ar} \, 3d^2 \, 4s^2 \)

2. **Chromium (Cr)** - Atomic number 24:
Configuration: \( \text{Ar} \, 3d^5 \, 4s^1 \)

3. **Manganese (Mn)** - Atomic number 25:
Configuration: \( \text{Ar} \, 3d^5 \, 4s^2 \)

4. **Vanadium (V)** - Atomic number 23:
Configuration: \( \text{Ar} \, 3d^3 \, 4s^2 \)

5. **Nickel (Ni)** - Atomic number 28:
Configuration: \( \text{Ar} \, 3d^8 \, 4s^2 \)

6. **Cobalt (Co)** - Atomic number 27:
Configuration: \( \text{Ar} \, 3d^7 \, 4s^2 \)

7. **Zinc (Zn)** - Atomic number 30:
Configuration: \( \text{Ar} \, 3d^{10} \, 4s^2 \)

8. **Scandium (Sc)** - Atomic number 21:
Configuration: \( \text{Ar} \, 3d^1 \, 4s^2 \)

### Step 2: Determine the Electronic Configurations of the Ions
Next, we will determine the electronic configurations of the ions for each option.

#### Option A:
1. **Ti²⁺**: Loses 2 electrons from \( 4s \)
Configuration: \( \text{Ar} \, 3d^2 \)

2. **Cr⁴⁺**: Loses 4 electrons (1 from \( 4s \) and 3 from \( 3d \))
Configuration: \( \text{Ar} \, 3d^2 \)

3. **Mn⁵⁺**: Loses 5 electrons (2 from \( 4s \) and 3 from \( 3d \))
Configuration: \( \text{Ar} \, 3d^2 \)

4. **V³⁺**: Loses 3 electrons (2 from \( 4s \) and 1 from \( 3d \))
Configuration: \( \text{Ar} \, 3d^2 \)

**Conclusion for Option A**: All ions have the same configuration \( 3d^2 \).

#### Option B:
1. **Ti³⁺**: Configuration: \( \text{Ar} \, 3d^1 \)
2. **Ni²⁺**: Configuration: \( \text{Ar} \, 3d^8 \)
3. **Co²⁺**: Configuration: \( \text{Ar} \, 3d^7 \)
4. **Zn²⁺**: Configuration: \( \text{Ar} \, 3d^{10} \)

**Conclusion for Option B**: Different configurations.

#### Option C:
1. **Sc²⁺**: Configuration: \( \text{Ar} \, 3d^1 \)
2. **Ti²⁺**: Configuration: \( \text{Ar} \, 3d^2 \)
3. **V²⁺**: Configuration: \( \text{Ar} \, 3d^3 \)
4. **Cr²⁺**: Configuration: \( \text{Ar} \, 3d^4 \)

**Conclusion for Option C**: Different configurations.

#### Option D:
1. **Mn⁵⁺**: Configuration: \( \text{Ar} \, 3d^2 \)
2. **Co⁴⁺**: Configuration: \( \text{Ar} \, 3d^5 \)
3. **Ni³⁺**: Configuration: \( \text{Ar} \, 3d^7 \)
4. **Cu²⁺**: Configuration: \( \text{Ar} \, 3d^9 \)

**Conclusion for Option D**: Different configurations.

### Final Conclusion
The only correct option where all ions have the same 3d electronic configuration is **Option A**: \( \text{Ti}^{2+}, \text{Cr}^{4+}, \text{Mn}^{5+}, \text{V}^{3+} \) all have the configuration \( 3d^2 \).