Li is different from its family members due to
Correct answer: D. All of the above
- A. Small size
- B. High charge density
- C. Lower electropositivity
- D. All of the above
Explanation
Lithium's small size, high charge density, and lower electropositivity compared to its heavier alkali metal family members lead to distinct chemical and physical properties. Here's how each factor contributesSmall size: Due to its small size, lithium's nucleus exerts a stronger pull on its single electron, making it harder to remove (higher ionization energy). This results in lower electropositivity compared to larger alkali metals.High charge density: Combining the small size with the single electron leads to a high charge density around the lithium nucleus. This makes it more polarizing, meaning it can distort the electron clouds of neighboring atoms or molecules, influencing its reactivity and bonding behavior.Lower electropositivity: As mentioned, lithium tends to hold onto its electron more tightly, making it less likely to donate it and participate in typical alkali metal reactions like forming ionic bonds with non-metals.These combined factors contribute to several differences between lithium and its family members, such as:Reactivity: Lithium reacts less readily with water than other alkali metals like sodium or potassium.Hydration energy: Lithium ions have lower hydration energy compared to larger alkali metal ions, meaning they attract water molecules less strongly.Bonding: Lithium can form covalent bonds with some elements, whereas other alkali metals typically form purely ionic bonds.Melting and boiling points: Lithium's high charge density leads to stronger interatomic forces, resulting in higher melting and boiling points than some other alkali metals.Therefore, understanding all three factors (small size, high charge density, and lower electropositivity) together provides a comprehensive explanation for why lithium stands out from its alkali metal family
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About s-Block and p-Block Elements
The s and p blocks are studied through their valence-shell configurations, periodic trends and characteristic chemical properties. Work covers the reactions of Group I and Group II elements, the behaviour of Group IV elements, and how atomic size, ionization energy, electronegativity and metallic character change across periods and down groups.
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