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(C) Valence electrons: Each group is characterized by its valence electrons,i.e.,the number of electrons in the outermost shell of the elements are th

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Valence electrons

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(C) Valence electrons: Each group is characterized by its valence electrons,i.e.,the number of electrons in the outermost shell of the elements are the same within a group. Thus,the common oxidation states for the elements of the same group are fixed.Due to the same number of valence electrons,elements of the same group show similar chemical properties.Atomic size: Moving down the group,a new shell is added with each period.The electron in the new shell also increases shielding. Therefore,the $Z_{eff}$ decreases along with which the attractive force of the nucleus decreases,and thus the size increases.Density: Density $= \frac{	ext{Mass}}{	ext{Volume}}$. Moving down the group,mass as well as volume increases. Therefore,density depends on the dominating factor. Usually,down the group,density increases,i.e.,the effect of mass dominates.Metallic character: Moving down the group,the nuclear attractive force on outer electrons decreases due to a decrease in $Z_{eff}$ which is due to an increase in shielding by inner shells. As a result,the ionization energy decreases down the group,and therefore,metallic character increases.Hence,the correct answer is valence electrons.

Element	Period and Group
$Q$	Period $2$,Group $15$
$P$	Period $3$,Group $2$

Which of the properties remains unchanged on descending a group in the periodic table?

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What would be the formula of the compound formed between the following elements?
$(i)$ Aluminium and Bromine
$(ii)$ Sodium and Oxygen
$(iii)$ Silicon and Oxygen
$(iv)$ Phosphorus and Chlorine

Consider the following information about elements $P$ and $Q$:

Element Period and Group

$Q$ Period $2$,Group $15$

$P$ Period $3$,Group $2$

Then the formula of the compound formed by $P$ and $Q$ elements is:

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