Subjective Type

Arrange the following in increasing order of the property indicated: $$ Mg^{2+}, O^{2-}, Na^+ , F^-$$ and $$N^{3-}$$ (ionic size)

Solution

Cations has less radius than the neutral atom because the electrons are expelled from the neutral atom to form cation whereas the no. of proton is same in both neutral and cation. Therefore the outermost electron are pulled towards nucleus more in the cation which led to reduce the radius. However the anions has higher radius than neutral atom due to $$e^--e^-$$ repulsion in the outermost shell.

The order is:

$$ Mg^{2+} < Na^+ < F^- < O^{2-} < N^{3 -} $$

SIMILAR QUESTIONS

Chemical Bonding

Which of the following arrangements represents the increasing order (smallest to largest) of ionic radii of the given species $$O^{2-}, S^{2-}, N^{3-}, P^{3-}$$?

Chemical Bonding

The ionic radii (in $$\mathring{A}$$) of $$N^{3-}$$, $$O^{2-}$$ and $$F^{-}$$ are respectively :

Chemical Bonding

The increasing order of the ionic radii of the given isoelectronic species is:

Chemical Bonding

The correct order of decreasing ionic radius among the following anions would be:

Chemical Bonding

Which of the following have the largest ionic size?

Chemical Bonding

The species $$Ar, K^+$$ and $$Ca^{2+}$$ contain the same number of electrons. In which order do their radii increase?

Chemical Bonding

What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions. (i) F$$\displaystyle ^{-}$$ (ii) Ar (iii) Mg$$\displaystyle ^{2+}$$ (iii) Rb$$\displaystyle ^{+}$$

Chemical Bonding

The size of isoelectronic species $$F\displaystyle ^{-}$$, $$Ne$$ and $$Na\displaystyle ^{+}$$ is affected by :

Chemical Bonding

$$K^{+}$$ and $$Cl^{-}$$ ions are isoelectronic. Which of the following statements is not correct?

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