1. Atomic Number and Electron Configuration:
* Sodium (Na) has an atomic number of 11, meaning it has 11 protons and 11 electrons. Its electron configuration is 2, 8, 1.
* Magnesium (Mg) has an atomic number of 12, meaning it has 12 protons and 12 electrons. Its electron configuration is 2, 8, 2.
2. Number of Valence Electrons:
* Sodium has one valence electron in its outermost shell.
* Magnesium has two valence electrons in its outermost shell.
3. Reactivity:
* Sodium is highly reactive due to its single valence electron, which it readily loses to form a +1 ion. It reacts vigorously with water and air.
* Magnesium is less reactive than sodium because it needs to lose two valence electrons to achieve stability. It is also less reactive than sodium with water and air.
4. Physical Properties:
* Sodium is a soft, silvery-white metal.
* Magnesium is a silvery-white, strong, and lightweight metal.
5. Chemical Properties:
* Sodium forms ionic compounds with non-metals, readily losing its valence electron to achieve a stable octet.
* Magnesium also forms ionic compounds, but it requires more energy to lose its two valence electrons.
6. Uses:
* Sodium is used in various applications, including the production of sodium hydroxide (NaOH), sodium chloride (NaCl), and sodium carbonate (Na2CO3).
* Magnesium is used in alloys, fireworks, and as a reducing agent in chemical reactions.
In summary: Sodium and magnesium differ in their atomic structure, reactivity, physical properties, chemical properties, and uses. These differences arise from the varying number of valence electrons and their associated electron configurations.
