To evaluate the statements about the relative potential energy of electrons, we need to consider both the principal quantum number (n) and the shape of the orbitals.
Statement A: An electron in the 2p orbital of the second electron shell has more potential energy than an electron in the 3p orbital of the third electron shell.
- This statement is incorrect. As the principal quantum number (n) increases, the potential energy of an electron generally increases. The 3p orbital is in a higher energy level (n=3) compared to the 2p orbital (n=2), so the electron in the 3p orbital has more potential energy.
Statement B: An electron in the 2p orbital of the second electron shell has more potential energy than an electron in the 2s orbital of the second electron shell.
- This statement is also incorrect. Within the same shell (n=2), the general trend is that s orbitals (2s) have lower potential energy than p orbitals (2p). Therefore, the electron in the 2s orbital has lower potential energy than the electron in the 2p orbital.
Statement C: An electron in the 3p orbital of the third electron shell has more potential energy than an electron in the 2p orbital of the second electron shell.
- This statement is correct. The 3p orbital (n=3) is higher in energy than the 2p orbital (n=2), so the electron in the 3p orbital has more potential energy.
In summary, the correct statement about the relative potential energy of electrons is:
C. An electron in the 3 p orbital of the third electron shell has more potential energy than an electron in the 2 p orbital of the second electron shell.
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