(D) The ionization energy values are $IE_1 = 100 \ kJ/mol$,$IE_2 = 250 \ kJ/mol$,and $IE_3 = 1500 \ kJ/mol$. There is a large jump between $IE_2$ and

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(D) The ionization energy values are $IE_1 = 100 \ kJ/mol$,$IE_2 = 250 \ kJ/mol$,and $IE_3 = 1500 \ kJ/mol$. There is a large jump between $IE_2$ and $IE_3$,which indicates that the element $M$ has $2$ valence electrons. Since the element has $2$ valence electrons,its valency is $2$. Therefore,the formula of its oxide is $MO$.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Valency and oxidation state

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The formula of the oxide of an element $M$ having $IE_1 = 100 \ kJ/mol$,$IE_2 = 250 \ kJ/mol$ and $IE_3 = 1500 \ kJ/mol$ should be:

A
$M_2O$
B
$MO_2$
C
$M_2O_3$
D
$MO$

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Class 11

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Classification of Elements and Periodicity in Properties

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Valency and oxidation state

The most common oxidation state of an element is $-2$. The number of electrons present in its outermost shell is

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The number of elements among $O, Cl, F, N, P, Sn, Ti, K, Sc$ which show more than one non-zero oxidation state is:

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The maximum valency of an element with atomic number $7$ is

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Which of the following elements has a valency of zero?

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Arrange the acids $(I)$ $H_2SO_3$,$(II)$ $H_3PO_3$,and $(III)$ $HClO_3$ in the decreasing order of acidity.

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The formula of the oxide of an element $M$ having $IE_1 = 100 \ kJ/mol$,$IE_2 = 250 \ kJ/mol$ and $IE_3 = 1500 \ kJ/mol$ should be:

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