Question

An element has atomic number 10. What would be its period and group in the periodic table?

Answer 1

2nd period as it has 2 shells and 18 group as it is a noble gas (neon)

Answer 2

$\bold{MODERN \: PERIODIC \: TABLE}$

In modern periodic table the elements are arranged in horizontal groups and vertical periods according to their increasing order of their atomic number.

$\bold{GIVEN}$

Atomic number of an element is 10

So, its electron configuration will be,

= (2,8)

We can observe that , the outermost shell is filled with 8 electrons and is stable by octate rule so it will neither lose or will gain electron and hence its valence is 0.

✳The elements of group 18 contains zero valency and are completely stable so the Given compound belongs to$\bold{Group \: 18}$

✳Since the number of shells decide the number of period it belongs to so the given element have 2 shells so it belongs to $\bold{Period \: 2}$.

We can convey that the given element is the noble gas $\bold{neon}$.