OTHERS

Question 1

Ability to be stretched into thin wires (e.g., copper, gold).

Answer 1

Ductility

Question 2

Similar to ductility but refers to the ability to be flattened into sheets (e.g., aluminum foil).

Answer 2

Malleability

Question 3

Resistance to bending or deformation (e.g., steel beams in construction).

Answer 3

Rigidity

Question 4

Materials that break easily under stress rather than deforming (e.g., glass, ceramics).

Answer 4

Brittleness

Question 5

Resistance to scratching or denting (e.g., diamonds are extremely hard).

Answer 5

Hardness

Question 6

Ability to return to its original shape after being stretched or compressed (e.g., rubber bands).

Answer 6

Elasticity

Question 7

The ability of a substance to allow electricity or heat to pass through it (e.g., metals are good conductors, while rubber is an insulator).

Answer 7

Conductivity

Question 8

The attraction between different substances (e.g., water sticking to glass).

Answer 8

Adhesion

Question 9

The attraction between molecules of the same substance (e.g., water droplets forming beads).

Answer 9

Cohesion

Question 10

The movement of a liquid through narrow spaces due to adhesive and cohesive forces (e.g., water moving up a plant’s stem).

Answer 10

Capillary Action

Question 11

Higher temperatures usually increase the solubility of solids in liquids but decrease the solubility of gases.

• Example (Solids in Liquids): Sugar dissolves faster in hot coffee than in iced coffee because higher temperatures increase molecular movement.
• Example (Gases in Liquids): Cold soda holds more carbonation (CO₂) than warm soda because gases dissolve better at lower temperatures.

Answer 11

Temperature

Question 12

Affects the solubility of gases in liquids but has little effect on solids or liquids dissolving.

• Example: Carbonated drinks stay fizzy under high pressure. When you open a soda bottle, the pressure drops, and gas escapes as bubbles.

Answer 12

Pressure

Question 13

Determines how well substances dissolve based on polarity and intermolecular forces.

• Example: Salt (ionic) dissolves in water (polar) but not in oil (nonpolar) because “like dissolves like.”
• Example: Oil does not mix with water because oil is nonpolar, while water is polar, so their molecules do not interact well.

Answer 13

Nature of the Solute and Solvent

Question 14

Increases contact between solute and solvent, helping the solute dissolve faster.

Answer 14

Agitation (Stirring)

Question 15

Breaking solute into smaller pieces increases surface area, speeding up dissolution.

Answer 15

Powdering (Particle Size Reduction)