What is the difference between van der Waals radius and covalent radius?
(N/A) The van der Waals radius is defined as half of the distance between the nuclei of two non-bonded adjacent atoms of the same element in a solid state.
The covalent radius is defined as half of the distance between the nuclei of two atoms bonded by a single covalent bond in a molecule.
Generally,the van der Waals radius is greater than the covalent radius $(r_{vdW} > r_{cov})$.
The covalent radius is defined as half of the distance between the nuclei of two atoms bonded by a single covalent bond in a molecule.
Generally,the van der Waals radius is greater than the covalent radius $(r_{vdW} > r_{cov})$.
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Similar Questions
From the given set of species,point out the species from each set having the least atomic/ionic radius:
$(A)$ $F^{-}, Na^{+}, Mg^{+2}$
$(B)$ $Ni, Cu, Zn$
$(C)$ $N^{-3}, Cs^{+}, H^{-}$
$(D)$ $Li, Li^{+}, Be^{+2}$
$(A)$ $F^{-}, Na^{+}, Mg^{+2}$
$(B)$ $Ni, Cu, Zn$
$(C)$ $N^{-3}, Cs^{+}, H^{-}$
$(D)$ $Li, Li^{+}, Be^{+2}$
Difficult
View SolutionWhich of the following is the correct increasing order of ionic radii for $N^{3-}$,$Na^+$,$F^-$,$O^{2-}$,and $Mg^{2+}$?
Easy
View SolutionThe order of increasing ionic radius of the following is:
Difficult
View SolutionGiven below are two statements:
Statement $I$: The metallic radius of $Na$ is $1.86 \ \mathring{A}$ and the ionic radius of $Na^{+}$ is lesser than $1.86 \ \mathring{A}$.
Statement $II$: Ions are always smaller in size than the corresponding elements.
In the light of the above statements,choose the correct answer from the options given below:
Statement $I$: The metallic radius of $Na$ is $1.86 \ \mathring{A}$ and the ionic radius of $Na^{+}$ is lesser than $1.86 \ \mathring{A}$.
Statement $II$: Ions are always smaller in size than the corresponding elements.
In the light of the above statements,choose the correct answer from the options given below:
How does atomic radius vary in a period and in a group? How do you explain the variation?
Easy
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