Identifying the Element with Electron Configuration 1s22s22p63s2: A Comprehensive Guide

The electron configuration 1s22s22p63s2 describes the distribution of electrons in an atom. Understanding this configuration is crucial for identifying the element and its properties. In this comprehensive guide, we will explore the electron configuration, the element, and its properties in the context of the periodic table.

Understanding Electron Configuration

The electron configuration provides valuable information about the atom. Each electron occupies a specific energy level called a shell, and within each shell, electrons are distributed among subshells (s, p, d, f). The configuration 1s22s22p63s2 indicates that:

The first shell (1s) contains 2 electrons. The second shell (2s2, 2p6) contains a total of 8 electrons. The third shell (3s2) contains 2 electrons.

This configuration adds up to a total of 12 electrons, which helps us identify the element by checking the atomic number on the periodic table. This approach works for any neutral atom regardless of whether the electrons are in their ground state or excited state.

The Element: Magnesium

Magnesium (Mg) is the element that fits the electron configuration 1s22s22p63s2. Here are some key details about magnesium:

Atomic and Chemical Information

Symbol: Mg Atomic Number: 12 Atomic Weight: 24.305 Group: 2 (alkaline earth metals) Period: 3

Magnesium is a group 2, or alkaline earth metal, characterized by its relatively high reactivity and ability to form 2 oxidation states. It is a light, soft, and ductile metal with a silvery-white appearance.

Properties of Magnesium

Various physical and chemical properties define magnesium, making it valuable in multiple applications:

Physical Properties

Density: 1.738 g/cm3 Melting Point: 922 K Boiling Point: 1363 K Appearance: Lightweight, malleable, and silvery-white

Chemical Properties

Atomic Radius: 160 pm Atomic Volume: 14.0 cc/mol Covalent Radius: 136 pm Ionic Radius: 66 pm Specific Heat at 20°C: 1.025 J/g·mol Fusion Heat: 9.20 kJ/mol Evaporation Heat: 131.8 kJ/mol Pauling Negativity Number: 1.31 First Ionizing Energy: 737.3 kJ/mol Oxidation States: 2

Electrical Properties

Lattice Structure: Hexagonal

Discovery and Origin

Magnesium was discovered by Sir Humphry Davy in England in 1808. The etymology of the name comes from Magnesia, an ancient city in the district of Thessaly, Greece. Its light weight, malleability, and silvery-white appearance make it a highly valued metal.

Uses and Importance

Magnesium is widely used in various applications due to its unique properties:

Aerospace Industry: Used in the production of light alloys for airplanes, missiles, and other aircraft components. Medicine: Utilized in pharmaceuticals and supplements, particularly for bone health and muscle function. Building Materials: Applied in construction for its lightweight yet strong properties, contributing to sustainable building materials.

Understanding the electron configuration of magnesium not only helps in identifying the element but also in grasping its essential properties and uses.