For the second period elements the correct increasing

Q1:

Which of the following orders of ionic radii is correctly represented?

(A)

\(\large H^{-}> H^{+}> H\)

(B)

\(\large Na^{+}> F^{-}> O^{2-}\)

(C)

\(\large F^{-}> O^{2-}> Na^{+}\)

(D)

\(\large Al^{3+}> Mg^{2+}> N^{3-}\)

(E)

Non of the above

NEET - Medical UG-2014 Medium

Q2:

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

(A)

\(\large Ca^{2+}< Ar< K^{+}\)

(B)

\(\large Ca^{2+}< K^{+}< Ar\)

(C)

\(\large K^{+}< Ar< Ca^{2+}\)

(D)

\(\large Ar< K^{+}< Ca^{2+}\)

NEET - Medical UG-2015 Medium

Q3:

The formation of the oxide ion, O\(\large ^{2-}\) (g), from oxygen atom requires first an exothermic and then an endothermic step as shown below

\(\large O(g)+e^{-}\rightarrow O_{(g)}^{-}\: ;\: \Delta _{f}H^{\Theta }\: =\: -141\: \: kJ\: \: mol^{-1}\)

\(\large O^{-}(g)+e^{-}\rightarrow O_{(g)}^{2-}\: ;\: \Delta _{f}H^{\Theta }\: =\: +780\: \: kJ\: \: mol^{-1} \)

Thus process of formation of O\(\large ^{2-}\) in gas phase is unfavourable even thought O\(\large ^{2-}\) is isoelectronic with neon. It is due to the fact that,

(A)

Oxygen is more electronegative

(B)

Addition of electron in oxygen results in larger size of the ion

(C)

Electron repulsion outweighs the stability gained by achieving noble gas configuration

(D)

O\(\large ^{-}\) ion has comparatively smaller size than oxygen atom

NEET - Medical UG-2015 Hard

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For the second period elements the correct increasing order of first ionisation enthalpy is:

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