Ionic Compounds and Electron Transfer

The video tutorial explains how to write the Lewis structure for magnesium fluoride (MgF2). It describes MgF2 as an ionic compound where magnesium, a metal, transfers its two valence electrons to two fluorine atoms, non-metals, resulting in a neutral compound. The tutorial highlights the charges on magnesium and fluorine after electron transfer and the use of brackets to denote ionic bonds. The video concludes with a summary of the ionic bonding process in MgF2.

What type of compound is formed when magnesium bonds with fluorine?

• Metallic compound

• Covalent compound

• Polar compound

• Ionic compound

How many valence electrons does magnesium have?

• 1

• 3

• 2

• 4

In which group is fluorine found on the periodic table?

• Group 1

• Group 2

• Group 17

• Group 18

What happens to magnesium's electrons in the formation of MgF2?

• They are shared with fluorine.

• They are lost to the environment.

• They are transferred to fluorine.

• They remain with magnesium.

What charge does magnesium acquire after losing its valence electrons?

• 1+

• 2-

• 1-

• 2+

What is the charge on each fluorine atom after gaining an electron?

• 2+

• 1-

• 2-

• 1+

Why is MgF2 considered a neutral compound?

• Because it is a covalent compound.

• Because it has no net charge.

• Because the total positive and negative charges balance each other.

• Because it has equal numbers of protons and electrons.

What do the brackets around fluorine in the Lewis structure indicate?

• That fluorine is a metal.

• That fluorine is sharing electrons.

• That fluorine has gained electrons.

• That fluorine is losing electrons.

What distinguishes an ionic bond from a covalent bond?

• Ionic bonds are weaker than covalent bonds.

• Ionic bonds involve transfer of electrons.

• Ionic bonds involve sharing of electrons.

• Ionic bonds occur between non-metals only.

What is the role of the positive and negative charges in ionic bond formation?

• They repel each other.

• They attract each other.

• They neutralize each other.

• They have no effect.