Properties and Behavior of Compounds

The video explains the nature of compounds, focusing on ionic, covalent, and metallic bonds. Ionic bonds involve electrostatic attraction between ions, forming a crystal lattice with high melting points and solubility in water. Covalent bonds involve electron sharing, with low melting points and poor solubility. Metallic bonds feature a lattice of cations and delocalized electrons, leading to high conductivity and melting points.

What is the primary reason ionic compounds have high melting points?

• They are soluble in water.

• They are composed of large molecules.

• They have strong ionic bonds that require a lot of energy to break.

• They are made of metals.

Why do ionic compounds conduct electricity when dissolved in water?

• The ions are free to move and carry charge.

• The water molecules are charged.

• The ions are neutralized.

• The water increases the temperature.

What distinguishes a dative covalent bond from a regular covalent bond?

• It involves the sharing of electrons between two atoms.

• Both electrons in the bond come from the same atom.

• It is stronger than a regular covalent bond.

• It is weaker than a regular covalent bond.

Why are covalent compounds generally not soluble in water?

• They are neutral and do not interact with water molecules.

• They are too dense.

• They are too large to dissolve.

• They form strong bonds with water.

What is the main reason metals have high melting points?

• They have strong electrostatic attractions between cations and electrons.

• They are composed of large atoms.

• They are soluble in water.

• They are made of ionic compounds.

How do metals conduct electricity?

• By forming covalent bonds.

• Through the movement of ions.

• Through the movement of delocalized electrons.

• By dissolving in water.