Identifying Molecules with a Triple Bond

This question asks us to identify which molecule, from the given options (\(F_2\), \(Cl_2\), \(N_2\), \(O_2\)), contains a triple covalent bond between its atoms. Let's explore the concept of covalent bonds and analyze each molecule.

Understanding Covalent Bonds and the Octet Rule

Atoms form covalent bonds by sharing electrons to achieve a stable electron configuration, often resembling that of a noble gas (like having 8 valence electrons, known as the octet rule).

• Single Bond: Formed when two atoms share one pair of electrons (2 electrons total). Example: \(H-H\).
• Double Bond: Formed when two atoms share two pairs of electrons (4 electrons total). Example: \(O=O\).
• Triple Bond: Formed when two atoms share three pairs of electrons (6 electrons total). Example: \(N \equiv N\).

Step-by-step Analysis of Molecules

We need to determine the number of valence electrons for each atom and how they share electrons to form bonds.

1. Analyzing \(F_2\) (Diatomic Fluorine)

• Fluorine (F) is in Group 17, so each F atom has 7 valence electrons.
• To achieve an octet (8 electrons), each F atom needs 1 more electron.
• Two F atoms can share one pair of electrons, forming a single bond.
• The Lewis structure is \(F-F\), with 6 non-bonding electrons on each F atom. Each F atom effectively has 8 electrons (6 non-bonding + 2 bonding).
• Therefore, \(F_2\) has a single bond.

2. Analyzing \(Cl_2\) (Diatomic Chlorine)

• Chlorine (Cl) is also in Group 17, so each Cl atom has 7 valence electrons.
• Similar to fluorine, each Cl atom needs 1 more electron to complete its octet.
• Two Cl atoms share one pair of electrons, forming a single bond.
• The Lewis structure is \(Cl-Cl\), with 6 non-bonding electrons on each Cl atom. Each Cl atom effectively has 8 electrons.
• Therefore, \(Cl_2\) has a single bond.

3. Analyzing \(N_2\) (Diatomic Nitrogen)

• Nitrogen (N) is in Group 15, so each N atom has 5 valence electrons.
• To achieve an octet, each N atom needs 3 more electrons.
• If two N atoms share electrons, they can share three pairs (6 electrons) to satisfy the octet rule for both atoms.
• The Lewis structure is \(N \equiv N\). Each N atom has 5 valence electrons. They share 3 pairs (6 electrons). Each N atom effectively has 8 electrons (6 bonding + 2 non-bonding lone pair electrons).
• Therefore, \(N_2\) has a triple bond.

4. Analyzing \(O_2\) (Diatomic Oxygen)

• Oxygen (O) is in Group 16, so each O atom has 6 valence electrons.
• To achieve an octet, each O atom needs 2 more electrons.
• Two O atoms share two pairs of electrons (4 electrons), forming a double bond.
• The Lewis structure is \(O=O\), with 4 non-bonding electrons (2 lone pairs) on each O atom. Each O atom effectively has 8 electrons (4 bonding + 4 non-bonding).
• Therefore, \(O_2\) has a double bond.

Conclusion

Based on the analysis:

• \(F_2\) has a single bond.
• \(Cl_2\) has a single bond.
• \(N_2\) has a triple bond.
• \(O_2\) has a double bond.

The molecule that has a triple bond between the two atoms is \(N_2\).