Fluorine differs from other halogens in some of its properties. This is due to
Fluorine differs from other halogens in some of its properties. This is due to
Its smaller size and high electronegativity
Lack of d-orbitals
Low bond dissociation energy
All of the these
The Correct Option is D
Solution and Explanation
Fluorine differs from other halogens due to several unique characteristics:
- Smaller Size and High Electronegativity: Fluorine is the smallest halogen, leading to a high electron density around its nucleus. This contributes to its extremely high electronegativity, making it the most electronegative element in the periodic table.
- Lack of d-Orbitals: Fluorine does not have d-orbitals in its valence shell, which limits its ability to expand its octet and participate in certain chemical reactions compared to heavier halogens that can use d-orbitals.
- Low Bond Dissociation Energy: The bond dissociation energy of the F-F bond is low due to the small size of the fluorine atom causing repulsion between non-bonded electrons of the two fluorine atoms when bonded, making the bond weaker.
Thus, these properties: smaller size, high electronegativity, lack of d-orbitals, and low bond dissociation energy, together, differentiate fluorine from other halogens.
Therefore, the correct answer is: All of the these.
Top Questions on p -Block Elements
Given below are two statements.
In the light of the above statements, choose the correct answer from the options given below:- JEE Main - 2025
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Given below are the pairs of group 13 elements showing their relation in terms of atomic radius. $(\mathrm{B}<\mathrm{Al}),(\mathrm{Al}<\mathrm{Ga}),(\mathrm{Ga}<\mathrm{In})$ and $(\mathrm{In}<\mathrm{Tl})$ Identify the elements present in the incorrect pair and in that pair find out the element (X) that has higher ionic radius $\left(\mathrm{M}^{3+}\right)$ than the other one. The atomic number of the element (X) is
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Statement II: Nitrogen does not form halides with +5 oxidation state due to the absence of d-orbital in it.
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II. 'O' is a dibasic acid
III. 'O' is a monobasic acid
IV. 'C' on reaction with acetic acid gives 'O'- TS EAMCET - 2025
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Assertion (A): phosphorus can form both phosphorus (III) and phosphorus (V) chlorides but nitrogen cannot form nitrogen(V) chloride.
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Concepts Used:
P-Block Elements
- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
- P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
P block elements consist of:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family