When magnesium and fluorine take part in bond formation, they attain
octet configuration by electron transfer. (Atomic number: Mg = 12, F
= 9)
Represent the Electron dot diagram of the above bond formation. And
write the name of bond formed
Answers
Every element has a specific number of electrons present in its atomic orbitals. Out of these electrons, only those participating in bond formation with another atom which is present in the outermost shell of the atom. These electrons which are present in the outermost orbital of an atom are called valence electrons.
Any atom forms a bond with another atom to attain stability by completing its octet. And it is not necessary that each electron present in the valence shell takes part in octet formation. In some cases, it has been observed that one or more pairs of electrons in the valence shell remain unshared during bond formation. Such pairs of electrons in the outermost shell of an atom that remains unshared are known as lone pairs of electrons.
MgF2 is an ionic compound made up of magnesium cation and fluoride anion. To draw the electron dot or Lewis diagram of this compound, we first need to write the electronic configuration of atoms.
Electronic configurations:Mg : 1s22s22p63s23p0F : 1s22s22p5
The magnesium has a total of 2 electrons in its valence shell out of which two electrons will be transferred completely to form an ionic bond with two fluorine atoms having 7 valence electrons each and form a MgF2 molecule. By donating two electrons, magnesium will have a complete octet in its outer shell and since fluorine is just one electron deficient to complete its octet, two fluorine atoms will combine with magnesium to form a stable MgF2 compound.
Answer:
ionic compound
Magnesium and fluorine combine to form an ionic compound. What is the formula for the compound? Mg most commonly forms a 2+ ion. This is because Mg has two valence electrons and it would like to get rid of those two ions to obey the octet rule
Explanation:
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