On the basis of molecular orbital theory predict which of the following is paramagnetic.
` He_2 and He_(2)^(+)`

Explanation

To determine which of the given species, \( \text{He}_2 \) or \( \text{He}_2^+ \), is paramagnetic based on molecular orbital theory (MOT), we can follow these steps:

### Step 1: Determine the number of electrons in each species
- **For \( \text{He}_2 \)**: Each helium atom has 2 electrons. Therefore, \( \text{He}_2 \) has a total of \( 2 + 2 = 4 \) electrons.
- **For \( \text{He}_2^+ \)**: This species has one less electron than \( \text{He}_2 \). Thus, \( \text{He}_2^+ \) has \( 4 - 1 = 3 \) electrons.

### Step 2: Write the molecular orbital configuration for each species
- **For \( \text{He}_2 \)**:
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