Which of the following elements can form diatomic molecules held together by triple covalent bonds?

• A. Fluorine (F)
• B. Nitrogen (N)
• C. Oxygen (O)
• D. Hydrogen (H)

Answer: (B)

Verified step by step guidance

1. Understand that diatomic molecules with triple covalent bonds involve two atoms sharing three pairs of electrons, resulting in a very strong bond.
2. Recall the common diatomic molecules and their bond types: Hydrogen (H\_2) has a single bond, Oxygen (O\_2) has a double bond, Fluorine (F\_2) has a single bond, and Nitrogen (N\_2) has a triple bond.
3. Consider the electronic configuration and valence electrons of each element to determine the possible bond order. Nitrogen has 5 valence electrons, allowing it to share three pairs to complete its octet.
4. Recognize that the nitrogen molecule (N\_2) is unique among these options because it forms a very stable triple bond, which is represented by the Lewis structure with three shared pairs of electrons.
5. Conclude that among the given elements, only nitrogen (N) forms diatomic molecules held together by triple covalent bonds.