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# Number of elements present in period $1$ are ______.(A) $2$ (B) $4$ (C) $6$ (D) $8$

Last updated date: 21st Mar 2023
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Hint :Note down the number of subshells present in the atom for principal quantum number $n = 1$ and then to get the total number of elements in the given period, add the number of electrons that can be filled in the subshells.

The modern periodic table arranges the elements in groups and periods and elements are placed according to the increasing value of their atomic number. The modern periodic table consists of $7$ periods and $18$ groups.
For principal quantum number $n = 1$ :
The value of an azimuthal quantum number will be $0$ to $n - 1$ i.e., will have only one value which is equal to zero. This indicates that there is only one subshell present which is $1s$ subshell.
As we know, the total number of electrons that can be filled in the $1s$ subshell is two. Therefore, we can conclude that there are only two elements present in the period $1$ of the modern periodic table.
While writing the number of subshells for principal quantum number $n > 4$ , make sure there are only four subshells available that are s, p, d and f subshells and a total of $120$ electrons can be filled in these subshells.