The molecular electronic configuration of `H_(2)^(+)` ion is?

Options

A. `(sigma1s^(2))`
B. `(sigma1s^(2))(sigma^(**)1s^(2))`
C. `(sigma1s^(2))(sigma^(**)1s^(1))`
D. `(sigma1s^(1))`

Answer

To determine the molecular electronic configuration of the `H2^(+)` ion, we can follow these steps:

### Step 1: Determine the number of electrons
- Each hydrogen atom has 1 electron. Therefore, two hydrogen atoms contribute a total of 2 electrons.
- The `H2^(+)` ion has a positive charge, indicating that it has lost one electron.
- Thus, the total number of electrons in `H2^(+)` is:
\[ 2 \text{ (from H atoms)} - 1 \text{ (due to the positive charge)} = 1 \text{ electron} \]

### Step 2: Identify the molecular orbital configuration
- In molecular orbital theory, the electrons are filled into molecular orbitals based on the energy levels.
- For diatomic hydrogen, the molecular orbitals are filled in the following order:
- \(\sigma_{1s}\) (bonding orbital)
- \(\sigma^*_{1s}\) (antibonding orbital)

### Step 3: Fill the molecular orbitals
- Since `H2^(+)` has only 1 electron, it will occupy the lowest energy molecular orbital available, which is \(\sigma_{1s}\).
- Therefore, the configuration for `H2^(+)` is:
\[ \sigma_{1s}^1 \]

### Final Answer
The molecular electronic configuration of the `H2^(+)` ion is:
\[ \sigma_{1s}^1 \]

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