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(A) The acidic strength of oxides increases as the non-metallic character increases across a period or as the oxidation state of the central atom incr

Vedclass · Accepted Answer

$Cl_2O_7 > SO_2 > P_4O_{10}$

Vedclass · Answer

(A) The acidic strength of oxides increases as the non-metallic character increases across a period or as the oxidation state of the central atom increases. For option $A$: $Cl_2O_7$ ($Cl$ is $+7$),$SO_2$ ($S$ is $+4$),$P_4O_{10}$ ($P$ is $+5$). The order of electronegativity and oxidation state supports $Cl_2O_7 > SO_2 > P_4O_{10}$. In general,non-metallic oxides are acidic,and their acidity increases with the oxidation state of the central atom. $Cl_2O_7$ is a strong acidic oxide,while $P_4O_{10}$ is less acidic than $SO_2$ due to the lower oxidation state and lower electronegativity of $P$ compared to $S$ and $Cl$.

Oxide	Nature
$a$. $CO$	$i$. Basic
$b$. $BaO$	$ii$. Neutral
$c$. $Al_2O_3$	$iii$. Acidic
$d$. $Cl_2O_7$	$iv$. Amphoteric

Which of the following represents the correct order of acidic strength?

Similar Questions

Match the following:

Oxide Nature

$a$. $CO$ $i$. Basic

$b$. $BaO$ $ii$. Neutral

$c$. $Al_2O_3$ $iii$. Acidic

$d$. $Cl_2O_7$ $iv$. Amphoteric

Which of the following is the correct option?

Among the following,the least and most metallic elements will be respectively:
$(I) [He] 2s^1$
$(II) [Kr] 5s^2 4d^{10} 5p^5$
$(III) [Xe] 6s^1$
$(IV) [He] 2s^2 2p^5$

Show by a chemical reaction with water that $Na_{2}O$ is a basic oxide and $Cl_{2}O_{7}$ is an acidic oxide.

In the periodic table,with an increase in atomic number,how does the metallic character of an element change?

$Mg$ and $Li$ are similar in their properties due to

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