* Understand Electron Configuration: The ground state electron configuration describes how electrons are arranged in an atom's orbitals.

* p-Orbitals: The p-orbitals are found in the second and higher energy levels. Each energy level can have a maximum of 6 p-electrons (two in each of the three p-orbitals).

* Filling Order: Electrons fill orbitals in order of increasing energy. We use the Aufbau principle and Hund's rule to determine the electron configuration.

Let's work through it:

1. Start with the lowest energy level: The first energy level (n=1) only has an s-orbital, which can hold a maximum of 2 electrons.

2. Move to the second energy level: The second energy level (n=2) has both s and p-orbitals. The 2s orbital fills first with 2 electrons.

3. Fill the p-orbitals: The 2p orbitals can hold a maximum of 6 electrons. Since we need 10 p-electrons, we must move to the next energy level.

4. Third energy level: The 3p orbitals can hold 6 electrons. We've already filled 6 in the 2p orbitals, so we need 4 more.

5. Count to find the element: To have a total of 10 p-electrons, the atom must have 10 electrons in total. The element with 10 electrons is Neon (Ne).

Therefore, the element with the lowest atomic number that contains 10 p-electrons in the ground state is Neon (Ne).