The number of unpaired electrons present in a magnesium atom is
The Correct Answer and Explanation is:
The correct answer is 0.
Explanation:
Magnesium (Mg) is an element in the second period and is located in Group 2 of the periodic table. It has an atomic number of 12, meaning it has 12 electrons in total in its neutral state.
To determine the number of unpaired electrons, we need to write the electron configuration of magnesium:
Electron Configuration:
1s² 2s² 2p⁶ 3s²
- 1s²: The first energy level contains 2 electrons in the s-orbital (fully paired).
- 2s²: The second energy level contains 2 electrons in the s-orbital (fully paired).
- 2p⁶: The second energy level also contains 6 electrons in the p-orbital (fully paired).
- 3s²: The third energy level contains 2 electrons in the s-orbital (fully paired).
In this configuration, all of the electrons are paired, meaning there are no unpaired electrons in a neutral magnesium atom. The 12 electrons are arranged in pairs within their respective orbitals.
Summary:
Magnesium, with its electron configuration of 1s² 2s² 2p⁶ 3s², has 0 unpaired electrons. The electrons fill the available orbitals in a way that ensures they are paired, and no single electron is left unpaired in the outermost shell or any other shells.
