An element A has an atomic number of 17. To w | vedclass

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$(A)$ The atomic number of element $A$ is $17$.The electronic configuration of the element is determined by filling the shells $K, L, M, N$ in order:$

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Group $17$, Period $3$

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$(A)$ The atomic number of element $A$ is $17$.The electronic configuration of the element is determined by filling the shells $K, L, M, N$ in order:$K = 2$$L = 8$$M = 7$$1$. Period: The number of shells occupied by electrons determines the period. Since there are $3$ shells $(K, L, M)$, the element belongs to the $3rd$ period.$2$. Group: For elements with more than $2$ valence electrons, the group number is calculated as $10 + 	ext{valence electrons}$. Here, the valence electrons in the outermost shell $(M)$ are $7$. Therefore, the group number is $10 + 7 = 17$.Thus, element $A$ belongs to Group $17$ and Period $3$.

Group $16$	Group $17$
-	-
-	$A$
-	-
$B$	$C$

An element $A$ has an atomic number of $17$. To which group and period does it belong?

Similar Questions

An element $A$ has an atomic number $16$. To which group and period does it belong?

The position of three elements $A$, $B$, and $C$ in the Periodic Table are shown below:
Group $16$ Group $17$
- -
- $A$
- -
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$(a)$ State whether $A$ is a metal or non-metal.
$(b)$ State whether $C$ is more reactive or less reactive than $A$.

The atomic number of $Na$ and $Mg$ is $11$ and $12$ respectively and they belong to the same period.
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