Class 11ChemistryClassification of Elements and Periodicity in PropertiesExtended or long form of periodic table
EasyHow would you justify the presence of $18$ elements in the $5^{\text{th}}$ period of the Periodic Table?
(N/A) For the $5^{\text{th}}$ period,the principal quantum number is $n=5$.
The orbitals available for filling are $5s$,$4d$,and $5p$.
The number of orbitals in each subshell are: $5s$ ($1$ orbital),$4d$ ($5$ orbitals),and $5p$ ($3$ orbitals).
The total number of orbitals is $1 + 5 + 3 = 9$.
According to the Pauli Exclusion Principle,each orbital can hold a maximum of $2$ electrons.
Therefore,the total number of electrons that can be accommodated is $9 \times 2 = 18$.
Since each element corresponds to the addition of one electron,there are $18$ elements in the $5^{\text{th}}$ period.
The orbitals available for filling are $5s$,$4d$,and $5p$.
The number of orbitals in each subshell are: $5s$ ($1$ orbital),$4d$ ($5$ orbitals),and $5p$ ($3$ orbitals).
The total number of orbitals is $1 + 5 + 3 = 9$.
According to the Pauli Exclusion Principle,each orbital can hold a maximum of $2$ electrons.
Therefore,the total number of electrons that can be accommodated is $9 \times 2 = 18$.
Since each element corresponds to the addition of one electron,there are $18$ elements in the $5^{\text{th}}$ period.
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Which of the following statements related to the modern periodic table is incorrect?
$(a)$ The $p$-block has $6$ columns,because a maximum of $6$ electrons can occupy all the orbitals in a $p$-shell.
$(b)$ The $d$-block has $8$ columns,because a maximum of $8$ electrons can occupy all the orbitals in a $d$-subshell.
$(c)$ Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
$(d)$ The block indicates value of azimuthal quantum number $(l)$ for the last subshell that received electrons in building up the electronic configuration.
$(a)$ The $p$-block has $6$ columns,because a maximum of $6$ electrons can occupy all the orbitals in a $p$-shell.
$(b)$ The $d$-block has $8$ columns,because a maximum of $8$ electrons can occupy all the orbitals in a $d$-subshell.
$(c)$ Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
$(d)$ The block indicates value of azimuthal quantum number $(l)$ for the last subshell that received electrons in building up the electronic configuration.
Match the following:
List-$I$ (Atomic number)
List-$II$ (Group number and Period number)
$A$. $56$
$I$. $9, 4$
$B$. $50$
$II$. $3, 6$
$C$. $27$
$III$. $14, 5$
$D$. $58$
$IV$. $2, 6$
| List-$I$ (Atomic number) | List-$II$ (Group number and Period number) |
|---|---|
| $A$. $56$ | $I$. $9, 4$ |
| $B$. $50$ | $II$. $3, 6$ |
| $C$. $27$ | $III$. $14, 5$ |
| $D$. $58$ | $IV$. $2, 6$ |
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