If molecule `X_(2)` has a triple bond, then X will have the electronic configuratin.

Options

A. `1s ^(2)2s ^(2) 2p^(5)`
B. `1s^(2) 2s^(2)2p^(3)`
C. `1s^(2) 2s ^(1)`
D. `1s^(2)2s^(2)2p^(1)`

Answer

To determine the electronic configuration of the element \( X \) in the molecule \( X_2 \) that has a triple bond, we can follow these steps:

### Step 1: Understand the nature of a triple bond
A triple bond consists of three shared pairs of electrons between two atoms. This means that each atom contributes three electrons to the bond, resulting in a total of six shared electrons.

### Step 2: Determine the valency of element \( X \)
Since \( X_2 \) has a triple bond, it indicates that each \( X \) atom must have a valency of 3. This means that each atom needs to share three electrons to achieve a stable electronic configuration.

### Step 3: Analyze the electronic configuration
To find the electronic configuration of \( X \), we need to identify an element that can form three bonds. The most common elements that can achieve this are those in Group 15 of the periodic table, such as nitrogen, which has the electronic configuration of \( 1s^2 2s^2 2p^3 \).

### Step 4: Confirm the octet rule
For \( X \) to form a triple bond, it must have 5 valence electrons (2 from the \( s \) orbital and 3 from the \( p \) orbital). By sharing three electrons with another \( X \) atom, it will complete its octet, achieving a stable electronic configuration of \( 2s^2 2p^6 \).

### Step 5: Conclusion
Thus, the electronic configuration of \( X \) that allows it to form a triple bond in \( X_2 \) is \( 1s^2 2s^2 2p^3 \).

### Final Answer
The electronic configuration of element \( X \) is \( 1s^2 2s^2 2p^3 \).

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