To match each element with the correct electron configuration, we need to refer to the periodic table and understand the structure of an atom.
The electron configuration of an atom represents how the electrons are distributed among the energy levels or orbitals.
Let's take a few examples:
1. Hydrogen (H) - Hydrogen is the first element in the periodic table with an atomic number of 1. It consists of a single electron. Therefore, the electron configuration of hydrogen is 1s^1.
2. Oxygen (O) - Oxygen is the eighth element in the periodic table with an atomic number of 8. It has eight electrons. The electron configuration of oxygen can be determined by following the Aufbau principle, which states that electrons fill the lowest energy levels first. Therefore, the electron configuration of oxygen is 1s^2 2s^2 2p^4.
3. Sodium (Na) - Sodium is the eleventh element in the periodic table with an atomic number of 11. It has 11 electrons. Again, using the Aufbau principle, the electron configuration of sodium is 1s^2 2s^2 2p^6 3s^1.
It is important to note that the electron configuration can be determined by filling the orbitals in a specific order based on their energy levels and the number of electrons they can hold.
By using the periodic table and understanding the rules for electron configuration, we can match each element with its correct electron configuration.