4.5 Chemical Bonding (BP/MP)

Which of the following best explains why Argon (Ar) has the lowest boiling point in Period 3?

• Argon exists as single atoms with weak Van der Waals forces.

• Argon forms covalent bonds.

• Argon has a giant covalent structure

• Argon has strong metallic bond

What happens to the melting point trend from sodium (Na) to aluminium (Al)?

• It decreases because of stronger Van der Waals forces.

• It increases due to stronger metallic bonds.

• It stays the same due to similar bonding.

• It decreases due to weaker metallic bonds.

Why does the boiling point of chlorine (Cl₂) decrease compared to sulfur (S₈)?

• Cl₂ has fewer valence electrons.

• Cl₂ has weaker Van der Waals forces.

• Cl₂ has a metallic structure.

• Cl₂ exists as a giant covalent structure

What type of forces determine the boiling point of phosphorus (P₄), sulfur (S₈), chlorine (Cl₂), and argon (Ar)?

• Covalent bond

• Metallic bond

• Ionic bond

• Van Der Waal forces

Which of the following elements exists as a giant covalent structure?

• Silicone (Si)

• Sulphur (S)

• Phosphorus (P)

• Magnesium (Mg)

What is the primary reason for the higher boiling point of S₈ compared to P₄?

• Stronger metallic bonds in S₈

• Larger molecular size of S₈

• Stronger ionic bonds in S₈

• Stronger covalent bonds in S₈