Which of the following pairs represents an iso-electronic species?
- A$F^{-}, O^{2-}$
- B$F^{-}, O$
- C$F^{-}, O^{+}$
- D$F^{-}, O^{2+}$
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Similar Questions
Find the number of neutrons,electrons,and protons in the following species:
$(i)$ $_{15}^{31}P$
$(ii)$ $_{11}^{23}Na^{+}$
$(iii)$ $_{16}^{32}S^{2-}$
$(iv)$ $_{101}^{235}X$
$(v)$ $_{20}^{40}Ca^{2+}$
$(vi)$ $_9^{19}F^{-}$
$(i)$ $_{15}^{31}P$
$(ii)$ $_{11}^{23}Na^{+}$
$(iii)$ $_{16}^{32}S^{2-}$
$(iv)$ $_{101}^{235}X$
$(v)$ $_{20}^{40}Ca^{2+}$
$(vi)$ $_9^{19}F^{-}$
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View SolutionIdentify the isoelectronic pair from the following.
An isotope of oxygen has a mass number of $18$. Other isotopes of oxygen will have the same:
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View SolutionAn atom which has lost one electron would be
Easy
View SolutionTo determine the masses of the isotopes of an element,which of the following techniques is useful?
Medium
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