Barium Iodide and Ionic Bonds

The video explains how to draw the Lewis structure for barium iodide (BaI2), an ionic compound. It details the transfer of valence electrons from barium, a metal in group 2 with two valence electrons, to iodine, a non-metal in group 17 with seven valence electrons. The video illustrates why two iodine atoms are needed for each barium atom, resulting in a stable ionic compound with a two-plus charge on barium and a one-minus charge on each iodine. The concept of formula units and the crystal structure of barium iodide are also discussed.

What type of compound is barium iodide?

• Covalent

• Ionic

• Metallic

• Molecular

How many valence electrons does barium have?

• 3

• 4

• 1

• 2

In which group of the periodic table is iodine found?

• Group 1

• Group 2

• Group 17

• Group 18

What happens to the valence electrons of barium in barium iodide?

• They are transferred to iodine.

• They are shared with iodine.

• They remain with barium.

• They are lost to the environment.

What charge does iodine acquire after gaining an electron?

• 1+

• 1-

• 2+

• 2-

Why are brackets used around iodine in the Lewis structure?

• To denote its position in the periodic table.

• To highlight the atom's size.

• To indicate transferred electrons.

• To show shared electrons.

What type of bond is formed between barium and iodine?

• Covalent bond

• Ionic bond

• Metallic bond

• Hydrogen bond

What is a formula unit in the context of barium iodide?

• An isolated atom

• A single molecule

• A repeating pattern in a crystal

• A covalent structure

How does the Lewis structure help in understanding barium iodide?

• It illustrates electron transfer and bonding.

• It describes the physical state.

• It shows the color of the compound.

• It explains the electron sharing.

Why are two iodine atoms needed for every barium atom?

• To balance the charge

• To stabilize the temperature

• To increase the mass

• To enhance the color