The correct answer is Both (ii) and (iii).
Key Points
(i) suggests that elements participate in chemical combinations to gain more electrons. This is incorrect because while non-metals tend to gain electrons, metals typically lose electrons to achieve stability, and some elements share electrons. Therefore, **statement
(i) is incorrect.**
(ii) states that elements aim to achieve inert gas configuration. Atoms are most stable when they have the same electron arrangement as a noble gas (Group 18 elements like Helium, Neon, or Argon), which have completely filled outer shells. **Hence, statement
(ii) is correct.**
(iii) mentions that elements try to complete their octet. The Octet Rule dictates that atoms are most stable when their valence shell contains 8 electrons. Elements react to reach this count through ionic or covalent bonding. **Hence, statement
(iii) is correct.**
(iv) claims elements try to complete their inner shells. In any atom, the inner shells are already filled; chemical combinations primarily involve the valence (outermost) shell. Inner shell electrons do not participate in standard chemical bonding. **Hence, statement
(iv) is incorrect.**
- Therefore, the primary driving force for chemical reactivity is the attainment of a stable, lower-energy state resembling noble gases by completing the valence octet.
Additional Information
- Chemical Bonding: It is the physical process responsible for the attractive interactions between atoms and molecules. Atoms bond to minimize potential energy and maximize stability.
- The Octet Rule: Proposed by G.N. Lewis and Albrecht Kossel in 1916, this rule explains that atoms of elements combine in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas.
- Duet Rule: For elements like Hydrogen, Lithium, and Beryllium, stability is achieved by having 2 electrons in the 1s shell, mimicking the configuration of Helium (He).
- Valence Electrons: These are the electrons present in the outermost shell of an atom. The number of valence electrons determines the valency and the chemical reactivity of the element.
- Noble Gases: Elements like Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn) have a general electronic configuration of ns2np6. Their high ionization enthalpy and stable configuration make them chemically inert under normal conditions.
Important Points
- Methods of Completion: Atoms can complete their octet by transferring electrons (forming Electrovalent or Ionic bonds) or by sharing electrons (forming Covalent bonds).
- Electropositive Elements: Elements (mostly metals in Groups 1 and 2) that lose electrons to achieve a positive charge and a stable configuration.
- Electronegative Elements: Elements (mostly non-metals in Groups 16 and 17) that gain electrons to achieve a negative charge and a stable octet.
- Exceptions to Octet Rule: Some molecules like BF3 (incomplete octet), PCl5 (expanded octet with 10 electrons), and SF6 (expanded octet with 12 electrons) do not strictly follow the rule but remain stable.