Final answer:
The total number of electrons in the s and p orbitals for He, B, N, and Na are 2, 5, 7, and 8, respectively, with He having only s orbital electrons and the others having electrons distributed among s and p orbitals.
Step-by-step explanation:
To determine the total number of electrons in the s and p orbitals for the given elements, we look at their electron configurations:
- Helium (He) has the electron configuration 1s², which means it has 2 electrons in total, all of which are in s orbitals as Helium has no p orbitals filled.
- Boron (B) has the electron configuration 1s² 2s² 2p¹, totaling 5 electrons. It has 2 electrons in s orbitals and 3 electrons in p orbitals.
- Nitrogen (N) has the electron configuration 1s² 2s² 2p³, with a total of 7 electrons. There are 2 electrons in s orbitals and 5 electrons in p orbitals.
- Sodium (Na) has the electron configuration 1s² 2s² 2p¶ 3s¹, with a total of 11 electrons. There are 2 electrons in s orbitals (in the third shell specifically) and 6 electrons in p orbitals (from the second shell).
The correct options for the number of electrons in the s and p orbitals for the elements He, B, N, and Na are 2, 5, 7, and 8, respectively.