Question

White phosphorus matches ignite very easily, but red phosphorus matches need friction. Which statements correctly explain these differences in activation energy?

(Select the three correct answers.)

(3 points)
Responses

The bonds in white phosphorus are easier to break.
The bonds in white phosphorus are easier to break.

Red phosphorus requires less energy to ignite.
Red phosphorus requires less energy to ignite.

White phosphorus has a lower activation energy.
White phosphorus has a lower activation energy.

The bonds in red phosphorus are easier to break.
The bonds in red phosphorus are easier to break.

White phosphorus has a higher activation energy.
White phosphorus has a higher activation energy.

Red phosphorus requires more energy to ignite.

Answer 1

Correct choices:
- The bonds in white phosphorus are easier to break.
- White phosphorus has a lower activation energy.
- Red phosphorus requires more energy to ignite.

Brief explanation: White phosphorus exists as strained P4 tetrahedra with weaker P–P bonds and so reacts (oxidizes) with a lower activation energy, while red phosphorus has a more stable polymeric structure and therefore needs more input (friction/heat) to ignite.