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(D) Acidic strength of oxides increases with non-metallic character: $Na_2O$ (basic) $< MgO$ (basic) $< CO_2$ (acidic) $< SO_3$ (acidic). Thi

Vedclass · Accepted Answer

Decreasing order of boiling points: $He > Ne > Ar > Xe$

Vedclass · Answer

(D) Acidic strength of oxides increases with non-metallic character: $Na_2O$ (basic) $< MgO$ (basic) $< CO_2$ (acidic) $< SO_3$ (acidic). This order is correct. $(B)$ Ionic radius decreases as the number of shells decreases or charge increases for isoelectronic species. The correct order is $K^+ (1.38 \ \mathring{A}) > Na^+ (1.02 \ \mathring{A}) > Mg^{2+} (0.72 \ \mathring{A}) > Li^+ (0.59 \ \mathring{A})$. This order is correct. $(C)$ Boiling point depends on the extent of hydrogen bonding. $H_2O$ has two $H$-bonds per molecule,$HF$ has one,and $NH_3$ has one (but weaker). The order $H_2O > HF > NH_3$ is correct. $(D)$ For noble gases,boiling point increases down the group due to increasing van der Waals forces with increasing molecular mass. The correct order is $Xe > Ar > Ne > He$. The given order $He > Ne > Ar > Xe$ is incorrect.

Select the option containing the incorrect order of the parameters given.

Similar Questions

Which of the following orders is incorrect?

The cause of the diagonal relationship is:

Which has maximum $EA$,$EN$ and $IP$ respectively $:-$
$A = 1s^2 \ 2s^2 \ 2p^6$
$B = 1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^5$
$C = 1s^2 \ 2s^2 \ 2p^5$
$D = 1s^2 \ 2s^2 \ 2p^6 \ 3s^1$

Outermost electronic configuration of a group $13$ element,$E$,is $4s^2 4p^1$. The electronic configuration of an element of $p$-block,period $5$,placed diagonally to element $E$ is:

Which of the following does not depend on stable electronic configuration?

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