Which of these atoms can form molecules with five or six...

Which of these atoms can form molecules with five or six pairs of valence electrons surrounding the atom?
(a) $\mathrm{C}$
(b) $\mathrm{P}$
(c) 0
(d) $\mathrm{F}$
(e) Cl
(f) $\underline{B}$
(g) Se
(h) $\underline{\mathrm{Sn}}$

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Key Concepts

Periodic Trends and Orbital Availability

The ability of an atom to expand its octet and form hypervalent compounds is dependent on its position in the periodic table. Atoms from the third period onward have access to d-orbitals that are absent in second period elements, making them capable of accommodating extra electron pairs.

Hypervalency

Hypervalency refers to the phenomenon where an atom in a molecule has more than eight electrons in its valence shell, exceeding the traditional octet rule. This typically occurs for larger atoms with available d-orbitals, enabling them to form stable compounds with additional bonded electron pairs.

Expanded Octet

The expanded octet concept applies to atoms in the third period and beyond, which have accessible d-orbitals in their valence shells. These additional orbitals allow such atoms to accommodate more than eight electrons, so they can form molecules where the central atom is surrounded by five or six electron pairs.

Octet Rule

The octet rule is a basic chemical principle stating that atoms tend to combine in such a way that they each have eight electrons in their valence shell, providing a noble gas configuration and increased stability. This rule commonly explains bonding patterns for many elements, particularly those in the second period.

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