Ionic Compounds and Electron Transfer

The video tutorial explains how to write the Lewis structure for magnesium bromide (MgBr2). It begins by identifying Mg as a metal and Br as a non-metal, forming an ionic compound. The tutorial details the transfer of valence electrons from magnesium to bromine, resulting in a stable electron configuration. Magnesium loses two electrons, gaining a 2+ charge, while each bromine atom gains an electron, acquiring a negative charge. The video emphasizes the importance of charge balance and the formation of ionic bonds. It concludes with the complete Lewis structure, highlighting the use of brackets to indicate electron transfer.

What type of compound is formed when magnesium and bromine combine?

• Metallic compound

• Molecular compound

• Ionic compound

• Covalent compound

How many valence electrons does magnesium have?

• 8

• 1

• 2

• 7

In which group is bromine found on the periodic table?

• Group 1

• Group 2

• Group 17

• Group 18

What happens to magnesium's electrons in the formation of MgBr2?

• They are transferred to bromine.

• They are shared with bromine.

• They are lost to the environment.

• They remain with magnesium.

What is the significance of having a full outer shell of electrons?

• It makes the atom stable.

• It makes the atom unstable.

• It makes the atom reactive.

• It makes the atom neutral.

After electron transfer, what charge does magnesium have?

• 2-

• 1-

• 2+

• 1+

What charge do bromine ions have after gaining electrons?

• 1+

• 2+

• 1-

• 2-

What attracts the negative bromide ions to the positive magnesium ions?

• Covalent bonds

• Metallic bonds

• Hydrogen bonds

• Ionic bonds

Why are brackets used around bromide ions in the Lewis structure?

• To denote metallic bonds

• To indicate shared electrons

• To show electron transfer

• To highlight covalent bonds

What is a formula unit in the context of ionic compounds?

• A repeating pattern in a crystal

• A single molecule

• A covalent bond

• An isolated atom