Question

25. An element with atomic number 12,
burns in presence of oxygen to form basic
oxide.
(i) Identify the element.
(ii) Where it is located in the periodic
table?
(iii) Write a balanced equation when it
burns in the presence of air.
(iv) Draw the electron dot structure
showing formation of its chloride.
Identify the type of bond m
formed in the compound.
BONUS STER​

Answer 1

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(I) The required element is Magnesium. Atomic number of Magnesium is 12 and it is an alkaline earth metal.

(II) It is located in the group of alkaline earth metals that is Group II A. It is below Beryllium. And the period number is 3 in teh periodic table.

(III) Magnesium is a reactive metal and when it reacts with oxygen in the atmosphere, a white dazzling flame can be seen with the formation of grayish-white ash. The reaction that took place can be represented by:

• $\rm{2Mg + O_2 \longrightarrow2MgO}$

Here the magnesium oxide formed is a basic oxide and soluble in water. It is the grayish ash formed after the burning of Magnesium.

(IV) Magnesium forms electropositive ion and Chlorine forms an electronegative one after losing and gaining of electrons respectively. The electron dot structure is in the attachment.

• $\rm{Mg + Cl_2 \longrightarrow MgCl_2}$

And we are done.....

Answer 2

Answer:

magnesium

group 2

2Mg+O2-----2MgO

Explanation: