Modern Periodic Law and the Present Form of the Periodic Table

Justify the given statement with suitable examples— “The properties of the elements are a periodic function of their atomic numbers”.

An element belongs to $3^{\mathrm{rd}}$ period and group-$13$ of the periodic table. Which of the following properties will be shown by the element?

Comprehension given below is followed by a question. Choose the correct option.
In the modern periodic table, elements are arranged In order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz. $\mathrm{s}, \mathrm{p}, \mathrm{d} \mathrm{and} \text{f}$. The modem periodic table consists of $7$ periods and $18$ groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle, the seven periods $(1 \mathrm{to} 7)$ have $2, 8, 8, 18, 18, 32$ and $32$ elements respectively. To avoid the periodic table being too long, the two series of $\mathrm{f}$-block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.

The elements with atomic numbers $35,53 \mathrm{and} 85$ are all __________.

Comprehension given below is followed by a question. Choose the correct option.
In the modern periodic table, elements are arranged In order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz, $\mathrm{s}, \mathrm{p}, \mathrm{d} \mathrm{and} \mathrm{f}$. The modem periodic table consists of $7$ periods and $18$ groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle, the seven periods $(1 \mathrm{to} 7)$ have $2, 8, 8, 18, 18, 32$ and $32$ elements respectively. To avoid the periodic table being too long, the two series of $\mathrm{f}$-block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.

Which of the elements whose atomic numbers are given below, cannot be accommodated in the present set up of the long form of the periodic table?  

Comprehension given below is followed by a question. Choose the correct option.
In the modern periodic table, elements are arranged In order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz, $\mathrm{s}, \mathrm{p}, \mathrm{d} \mathrm{and} \mathrm{f}$. The modern periodic table consists of $7$ periods and $18$ groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle, the seven periods $(1 \mathrm{to} 7)$ have $2, 8, 8, 18, 18, 32$ and $32$ elements respectively. To avoid the periodic table being too long, the two series of $\mathrm{f}$-block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.

The element with atomic number $57$ belongs to 

Which of the following is not an actinoid?