Answer: The complete ground state electron configuration for the carbon atom is 1s2 2s2 2px1 2py1.
Explanation: The ground state electron configuration represents the arrangement of all electrons in an atom’s energy levels (shells) and subshells when the atom is in its lowest energy state.
Carbon, with an atomic number of 6, has six electrons. According to the Aufbau principle, electrons fill the lowest energy levels first.
The ground state electron configuration of carbon is 1s2 2s2 2p2. The p-subshell has three orbitals. The orbitals are px, py, and pz and each orbital can have a maximum of two electrons.
In the carbon ground-state electron configuration, the two electrons of the 2p orbital are located in the px, py orbitals and the spin of the two electrons is the same.
Then the correct electron configuration of carbon in the ground state will be 1s2 2s2 2px1 2py1.
Significance: Understanding the complete ground state electron configuration of carbon provides insights into its chemical behavior and its properties as an element.
The arrangement of electrons in different subshells contributes to its position in the periodic table and its reactivity.