Question

These diagrams show two atoms of fluorine and an atom of magnesium.

Answer 1

The correct steps to the following question will be- A magnesium atom donates two electrons to the fluorine atoms → Each fluorine atom accepts one of the electrons → The magnesium atom becomes a +2 ion → Each fluorine atom becomes a -1 ion.

EXPLANATION:

The electronic configuration of fluorine atom is $1s^22s^22p^5$.

The electronic configuration of magnesium is $1s^22s^22p^63s^2$.

The valence shell of fluorine needs one electron to satisfy inert gas configuration to be stable. On other hand, the magnesium has two electrons in its valence shell. It needs six electrons more to be stable. As it is a electropositive metal, so it will lose two of its electrons to acquire the nearest inert gas configuration i.e neon.

Hence, magnesium will lose two of its valence electrons and becomes a  positively charged cation having +2 charge.

Each of the fluorine atoms will accept one electron from magnesium and becomes negatively charged anion having one unit negative charge.

Now both the cation and anion are attracted by the coulombic force of attraction and forms magnesium chloride.

Answer 2

the answer is D. A magnesium atom donates two electrons to the fluorine atoms → Each fluorine atom accepts one of the electrons → The magnesium atom becomes a +2 ion → Each fluorine atom becomes a -1 ion

because magnesium only has 2 valence electrons, and it would be easier to lose electrons rather gain.

i just took the test, its right.