Question

24. Two elements X and Y have atomic numbers 12 and 16 respectively. To which period
of the modem periodic table do these two elements belong? What type of bond will be
fomed between themand wily? Also give the chemical fomula of the compound formed.​

Answer 1

Answer:-

Given that,

Two elements X & Y have atomic numbers 12 & 16. That means, the elements are Magnesium (Mg) and Sulphur (S)

So, their electronic configuration is as follows:

• Mg – 1s² 2s² 2p⁶ 3s²

• S – 1s² 2s² 2p⁶ 3s² 3p⁴

We know that,

The shell/orbit where the last electron of an element is filled , it will be the period number.

Here, the last electron is filled in the 3rd shell in both elements.

So , both Mg & S lie in 3rd period.

We know , Mg is a metal and Sulphur is a non metal.

They both form Ionic bond by the transfer of electrons.

Chemical equation:

Mg + S ⟶ MgS

Magnesium Sulphide is formed when 2 electrons of Mg are transferred to S.

Additional Information:-

• Ionic bond - Transfer of electrons from metal to non metal leads to the formation of an Electrovalent or Ionic bond.

For more , Please refer :-

https://brainly.in/question/24189041

https://brainly.in/question/20696767

Answer 2

Answer :-

We have

$\sf Atomic \; Number \begin{cases} \bf X = 16 \\ \bf Y = 12\end{cases}$

So,

They may be broken into Electronic configuration to find the modem

Element X = 2,8,6

Element Y = 2,8,2

Now

We may observe that the both element are divided or have three shells. They belong to third period

                                                                                   

Now

According to the question

The element x will have electropositive ion and  element Y will have the  electronegative ion.

                                                                                   

Chemical equation is

$\sf Mg + S \longrightarrow MgS$