Why do noble gases exist as gases at room temperature, while halogens exist as solids, liquids, or gases down the group?
- AOption (a)
Larger atomic size of noble gases
- BOption (b)
Weak intermolecular forces in noble gases
- COption (c)
High reactivity of noble gases
- DOption (d)
Strong chemical bonds in noble gases
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Correct answer
Weak intermolecular forces in noble gases
Why this answer is correct
The correct answer is Weak intermolecular forces in noble gases.
Key Points
- Noble gases, belonging to Group 18 of the periodic table, have a completely filled valence shell electronic configuration (ns2np6), except for Helium (1s2).
- Due to this stable octet, noble gas atoms do not readily share or transfer electrons to form covalent or ionic bonds under standard conditions, causing them to exist as monatomic atoms.
- The only attractive forces existing between these monatomic atoms are extremely weak London Dispersion Forces (a type of Van der Waals force), which arise from temporary dipoles.
- Because these intermolecular forces are so weak, the thermal energy available at room temperature (approximately 298 K) is more than sufficient to overcome the attraction, keeping the atoms in a gaseous state.
- As a result, noble gases have very low melting and boiling points compared to other elements in the same period.
Additional Information
- Halogens (Group 17):
- Unlike noble gases, halogens exist as diatomic molecules (F2, Cl2, Br2, I2).
- Down the group, the atomic size and the number of electrons increase, which enhances the polarizability of the molecule.
- Stronger polarizability leads to stronger London Dispersion Forces. This is why Fluorine and Chlorine are gases, Bromine is a liquid, and Iodine is a solid at room temperature.
- Reactivity and Bonding:
- High reactivity: Noble gases are actually known for their chemical inertness or low reactivity due to high ionization enthalpy and stable configurations.
- Strong chemical bonds: Noble gases do not form strong bonds in their elemental form; strong interatomic forces only appear in compounds like Xenon tetrafluoride (XeF4), which are formed under specific conditions.