Explain about Group $17$ elements.

The outermost subshell electronic configuration of an element is $3{\mathrm{d}}^5 4{\mathrm{s}}^2$.

This element shows a variable oxidation state why?

The last subshell of an element is 3p and there are 3 electrons in it. 

Write the complete electronic configuration of the element.

The outermost subshell electronic configuration of an element is ${\mathrm{d}}^5 4{\mathrm{s}}^2$.

Identify its block and period.

The outermost shell electronic configuration of an element 'A' (symbol given is not real) is $3{\mathrm{s}}^{2}3{\mathrm{p}}^4$. 

Find the group number of the element.

Match List - I with List - II

Choose the correct answer from the options given below:

The last subshell of an element is 3p and there are 3 electrons in it. 

Identify its period and group. 

The outermost shell electronic configuration of an element 'A' (symbol given is not real) is $3{\mathrm{s}}^{2}3{\mathrm{p}}^4$. 

To which period of the periodic table does this element belong to?

The outermost shell electronic configuration of an element 'A' (symbol given is not real) is $3{\mathrm{s}}^{2}3{\mathrm{p}}^4$. 

Which is the block to which the element belongs?

The outermost subshell electronic configuration of an element is $3{\mathrm{d}}^5 4{\mathrm{s}}^2$.

Write the complete subshell electronic configuration of this element

The correct match among the following is

(a) Lithium, Sodium, Potassium            (i) Alkaline earth metals
(b) Beryllium, Magnesium, Calcium      (ii) Semi-metals
(c) Oxygen, Sulphur, Selenium             (iii) Alkali metaIs
(d) Silicon, Germanium, Arsenic           (iv) Chalcogens