Question : Is the specie paramagnetic ?
STATE-1 : The atomic number of speicie is `29`.
STATE-2 : The charge on the specie is `+1`.

Options

A. Statements `(1)` alone is sufficient but statement `(2)` is not sufficient
B. Statement `(2)` alone is sufficient but statement `(1)` is not sufficient
C. Both statement together are sufficient but neither statement alone is sufficient
D. Statement `(1) % (2)` together are not sufficient

Explanation

To determine if the species with atomic number 29 and a charge of +1 is paramagnetic, we need to analyze the electronic configuration of the species.

### Step 1: Identify the Element
The atomic number 29 corresponds to the element Copper (Cu).

### Step 2: Determine the Electronic Configuration
The electronic configuration of a neutral copper atom (Cu) is:
- \( \text{Cu: } [\text{Ar}] 3d^{10} 4s^1 \)

### Step 3: Analyze Unpaired Electrons in Neutral Copper
In the neutral state, copper has:
- 10 electrons in the 3d subshell (which are all paired)
- 1 electron in the 4s subshell (which is unpaired)

Since there is 1 unpaired electron in the 4s subshell, a neutral copper atom is **paramagnetic**.

### Step 4: Consider the Charge on the Species
The species has a charge of +1, which means it has lost one electron. When copper loses one electron to become \( \text{Cu}^+ \):
- The electron is removed from the 4s subshell.

Thus, the electronic configuration of \( \text{Cu}^+ \) becomes:
- \( \text{Cu}^+: [\text{Ar}] 3d^{10} \)

### Step 5: Analyze Unpaired Electrons in \( \text{Cu}^+ \)
In the \( \text{Cu}^+ \) state:
- The 3d subshell has 10 electrons (all paired)
- The 4s subshell has 0 electrons (since it lost its single unpaired electron)

Since there are no unpaired electrons in \( \text{Cu}^+ \), it is **diamagnetic**.

### Conclusion
The species with atomic number 29 and a +1 charge is **not paramagnetic**; it is **diamagnetic**.

### Final Answer
- The species is **not paramagnetic**.

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