Which statement correctly explains a difference between white and red phosphorus? (1 point)
Responses
White phosphorus has less chemical potential energy than red phosphorus.
White phosphorus has less chemical potential energy than red phosphorus.
White phosphorus has a higher activation energy than red phosphorus.
White phosphorus has a higher activation energy than red phosphorus.
White phosphorus has more chemical potential energy than red phosphorus.
White phosphorus has more chemical potential energy than red phosphorus.
White phosphorus has a lower activation energy than red phosphorus.
Correct Answer: White phosphorus has a lower activation energy than red phosphorus.
The correct statement is:
White phosphorus has a lower activation energy than red phosphorus.
The correct statement that explains a difference between white and red phosphorus is:
White phosphorus has a lower activation energy than red phosphorus.
To understand why this statement is correct, we need to have a basic understanding of activation energy. Activation energy is the threshold energy that needs to be surpassed for a chemical reaction to occur. It is the energy required to break the existing bonds in the reactants before new bonds can be formed in the products.
In the case of white and red phosphorus, they are both allotropes of phosphorus, which means they have the same chemical formula (P4) but different structures and physical properties.
White phosphorus exists as tetrahedral P4 molecules, where each phosphorus atom is bonded to three other phosphorus atoms. These molecules are highly reactive due to the weak bonds between the atoms. Because of this, white phosphorus has a lower activation energy, meaning it requires less energy to initiate a chemical reaction compared to red phosphorus.
On the other hand, red phosphorus forms a network structure in which each phosphorus atom is bonded to three other phosphorus atoms through stronger covalent bonds. This results in a more stable and less reactive form of phosphorus. Therefore, red phosphorus has a higher activation energy, meaning it requires more energy to initiate a chemical reaction compared to white phosphorus.
In summary, white phosphorus has a lower activation energy than red phosphorus because of its highly reactive structure, which consists of tetrahedral P4 molecules with weaker bonds.