Question

The formula of metal oxide is XO. Then which of the following compounds is not formed by X'is A) X(NO3)2 B) XH2 C) X 2(SO4)3 D) XCI2 ​

Answer 1

Answer:

C) X2 (SO4)3 will not be formed.

Explanation:

Metal oxide of X is of XO type. So X have valency of 2 (balanced with O^-2).

As SO4^-2 have valency of 2; the metal sulfate must have formula of XSO4.

hope this will help you

Answer 2

Answer:

If the formula of metal oxide is XO, then the compound that is not formed by X is option C, $X_2(SO_4)_3$·

Explanation:

It is mentioned that the metal oxide has a formula of XO·

We know that the oxygen belongs to the sixteenth group and have a valency of $2$·

That is,

In order to form a compound, oxygen needs $2$ electrons·

During the formation of a compound, due to its high electronegativity oxygen will get a partial negative charge· So its charge becomes $-2$· To maintain the neutrality of a compound, the charge of X should be $+2$·

So, X is an element with a charge $+2$ in all its compound·

To find out which of the given compounds are not formed by X, we need to check  which of the given compound does not have a charge of $+2$·

$(A)$  $X(NO_3)_2$

The ionic equation follows,

$X(NO_3)_2\ --->\ X^{2+}\ +\ 2\ NO_3^{-}$

So, here the charge of X is $+2$·

$(B)$  $XH_2$

The ionic equation follows,

$XH_2\ --->\ X^{2+} \ +\ 2\ H^-$

So, here the charge of X is $+2$·

$(c)$  $X_2(SO_4)_3$

The ionic equation follows,

$X_2(SO_4)_3\ --->\ 2\ X^{3+}\ +\ 3\ SO_4^{2-}$

So, here the charge of X is $+3$·

$(D)$  $XCl_2$

The ionic equation follows,

$XCI_2\ --->\ X^{2+}\ +\ 2\ Cl^-$

So, here the charge of X is $+2$·

Therefore,

From the above information, the compound $X_2(SO_4)_3$ is not formed by X·