Electronegativity and Ionic Compounds

The video explores whether cesium chloride (CsCl) is an ionic or covalent compound. It begins by identifying cesium as a metal and chlorine as a non-metal, suggesting an ionic nature. The video then examines the electronegativity difference between cesium (0.79) and chlorine (3.16), which is 2.37, indicating a significant ionic character. Despite a slight covalent character, CsCl is classified as an ionic compound.

What type of elements are involved in cesium chloride that initially suggests its ionic nature?

• Two non-metals

• A metalloid and a non-metal

• Two metals

• A metal and a non-metal

Why is the presence of a metal and a non-metal in CsCl important?

• It changes the color of CsCl

• It affects the solubility of CsCl

• It suggests an ionic bond

• It alters the density of CsCl

What is the significance of the electronegativity difference between cesium and chlorine?

• It shows the melting point of CsCl

• It determines the boiling point of CsCl

• It helps classify CsCl as ionic or covalent

• It indicates the color of CsCl

What is the calculated electronegativity difference between cesium and chlorine?

• 1.37

• 2.37

• 4.37

• 3.37

Based on the video, how would you classify cesium chloride?

• Amphoteric compound

• Covalent compound

• Metallic compound

• Ionic compound

What minor characteristic does cesium chloride have despite being classified as ionic?

• Metallic character

• Non-metallic character

• Covalent character

• Amphoteric character