How many electrons does an atom of each of the following elements need to lose to achieve a noble gas configuration? By losing that many electrons, which noble gas configuration is achieved?


(c) Magnesium

Verified step by step guidance

1. Identify the atomic number of magnesium, which is 12, indicating it has 12 electrons in its neutral state.
2. Determine the electron configuration of magnesium: 1s^2 2s^2 2p^6 3s^2.
3. Recognize that magnesium is in Group 2 of the periodic table, meaning it has 2 valence electrons in the 3s orbital.
4. To achieve a noble gas configuration, magnesium needs to lose its 2 valence electrons, resulting in the electron configuration of neon, which is 1s^2 2s^2 2p^6.
5. Conclude that by losing 2 electrons, magnesium achieves the noble gas configuration of neon.

Key Concepts

Noble Gas Configuration

Noble gas configuration refers to the electron arrangement of noble gases, which have full outer electron shells, making them stable and unreactive. Atoms tend to lose, gain, or share electrons to achieve this stable configuration, typically resembling the nearest noble gas in the periodic table.

Electron Loss in Metals

Metals, such as magnesium, tend to lose electrons to achieve a stable electron configuration. The number of electrons lost corresponds to the number of valence electrons in the outer shell. For magnesium, which has two valence electrons, losing these electrons allows it to attain a noble gas configuration.

Periodic Table and Group Trends

The periodic table organizes elements by their atomic number and electron configuration. Elements in the same group exhibit similar chemical properties, including the number of valence electrons. Magnesium is in Group 2, indicating it typically loses two electrons to achieve the stable electron configuration of neon, the nearest noble gas.