Difficult
The ions $O^{2-}, F^{-}, Na^{+}, Mg^{2+}$ and $Al^{3+}$ are isoelectronic. Their ionic radii show
- Aan increase from $O^{2-}$ to $F^{-}$ and then decrease from $Na^{+}$ to $Al^{3+}$
- Ba decrease from $O^{2-}$ to $F^{-}$ and then increase from $Na^{+}$ to $Al^{3+}$
- Ca significant increase from $O^{2-}$ to $Al^{3+}$
- Da significant decrease from $O^{2-}$ to $Al^{3+}$
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Which of the following has the largest ionic radius?
Easy
View SolutionIdentify the correct order in which the covalent radius of the following elements increases: $(I) \ Ti, (II) \ Ca, (III) \ Sc$.
The statement$(s)$ that are correct about the species $O^{2-}$,$F^{-}$,$Na^{+}$,and $Mg^{2+}$.
$(A)$ All are isoelectronic
$(B)$ All have the same nuclear charge
$(C)$ $O^{2-}$ has the largest ionic radii
$(D)$ $Mg^{2+}$ has the smallest ionic radii
Choose the most appropriate answer from the options given below :
$(A)$ All are isoelectronic
$(B)$ All have the same nuclear charge
$(C)$ $O^{2-}$ has the largest ionic radii
$(D)$ $Mg^{2+}$ has the smallest ionic radii
Choose the most appropriate answer from the options given below :
Which group elements have the smallest atomic radii in their respective periods?
Which of the following represents the correct order of atomic radii?
Difficult
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