Ionic Compounds and Electron Configuration

The video tutorial explains how to write the Lewis structure for barium chloride (BaCl2). It begins by identifying barium as a metal and chlorine as a non-metal, forming an ionic compound. The tutorial details the transfer of valence electrons from barium to chlorine, resulting in stable octets for chlorine and a positive charge for barium. The video concludes with a discussion on the concept of formula units in ionic compounds.

What type of compound is formed when barium and chlorine combine?

• Metallic compound

• Ionic compound

• Molecular compound

• Covalent compound

How many valence electrons does barium have?

• 1

• 2

• 4

• 3

In which group is chlorine found on the periodic table?

• Group 1

• Group 2

• Group 18

• Group 17

What is the role of the periodic table in understanding ionic compounds?

• It helps identify the number of protons.

• It provides the melting point.

• It shows the atomic mass.

• It indicates the number of valence electrons.

What happens to barium's valence electrons in the formation of BaCl2?

• They are transferred to chlorine.

• They are lost to the environment.

• They are shared with chlorine.

• They remain with barium.

What is the stable electron configuration achieved by chlorine after gaining an electron?

• Sextet

• Octet

• Duet

• Quartet

What is the charge on a barium ion after it loses its valence electrons?

• 2-

• 1-

• 2+

• 1+

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

• To highlight their metallic nature.

• To indicate they are part of a covalent bond.

• To show they are shared electrons.

• To denote the transfer of electrons and ionic nature.

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

• It highlights the metallic bond.

• It indicates a covalent bond.

• It shows the smallest ratio of ions.

• It represents a single molecule.

What is the overall charge of the BaCl2 compound?

• Negative

• Variable

• Positive

• Neutral