Beryllium Dichloride (BeCl₂)

Beryllium chloride is formed by carbothermal reduction of beryllium oxide. Hybridization is the process of creating a new hybrid structure combining an element’s atomic orbital; the formed hybrid will have a different shape and energy. Bond angle is the angle between any two bonds which is common to a single atom. It is usually measured in degrees. The molecular geometry and bond angle of a compound largely depends on the hybridization of its atomic orbital.

Beryllium dichloride

• A colourless inorganic compound. 
• It is used as a raw material in beryllium electrolysis 
• Catalyst in the friedel-crafts reaction. 
• Beryllium oxide is carbon thermally reduced to form beryllium chloride.

Hybridization

Hybridization is the process of creating a new hybrid structure combining an element’s atomic orbital. Compounds with the same molecular formula might have different structures due to the difference in atomic orbital they filled. It is established that the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a set of orbitals with the same energy. Hybridization can explain a molecular shape. Based on the types of orbital, the hybridization can be sp3, sp2, sp, sp3d, sp3d2, sp3d3.

Sp hybridization

It is a hybridization in which 50 % of ‘s’ and 50% of ‘p’ characters are shown. It is the mixing of one s and one p orbital of equal energy. It is also called diagonal hybridization. Examples include BeCl₂, BeF₂, BeH₂ and all carbon compounds having a triple bond.

Sp3 hybridization

‘s’ and ‘p’ orbitals of the second shell are mixed and form a four hybridised sp3 orbital. Since each orbital has a space, four bonds are possible (one unpaired electron in every orbital). Sp3 hybridised orbitals are ‘not so perfect’ dumbbell-shaped orbitals – one lobe is bigger than the other. In such hybridization, hybrid orbitals are a tetrahedral structure with a bond angle of 109 degrees 28′, that is, 109.5 degrees.

Beryllium dichloride (BeCl₂) Molecular geometry and bond angle

Beryllium chloride has two hybridizations in different states. It is sp hybridised in gaseous state and sp3 hybridised in solid state. Bond angle is the angle between any two bonds which is common to a single atom. It is usually measured in degrees.

BeCl₂ in gaseous state

Becl2 is sp hybridised in its gaseous state. Beryllium has two valence electrons and its electron configuration is (1s2 2s2).  One of its 2s electrons is promoted to an empty 2p orbital. Thus in the excited state, the electronic configuration of ‘Be’ is 1s2 2s1 2p1.  Beryllium must be angular if it is formed with its pure orbital. But In the excited state, the beryllium atom undergoes ‘sp’ hybridization by mixing 2s and one 2p orbital. These two half-filled orbitals form two σ bonds with chlorine. Therefore BeCl2 is necessarily linear since two sp hybridised orbital forms have a bond angle of 180°.

BeCl₂ in solid state

But in the solid-state, beryllium dichloride exists as a polymer. Therefore one beryllium forms a covalent bond with two chlorine and coordinates bonds with two chlorine. It exhibits sp3 hybridization and is a polymeric chain in structure. Bond angles are 92 degrees and 82 degrees.

Conclusion

 In the excited state, the electronic configuration of Beryllium is 1s2 2s1 2p1, since one of its 2s electrons is promoted to an empty 2p orbital. In the solid-state, beryllium dichloride exists as a polymer. It exhibits sp3 hybridization and is a polymeric chain in structure. The bond angle of Beryllium Dichloride is 180 degrees.

In its free state, the metal does not exist as a single atom as it either forms metallic bonds or ionic bonds with similar atoms. Not every metal leads to the formation of metallic bonds when they exist in the free state. For example, mercury forms the metal-metal covalent bond when it exists in the free state. Today, we are going to discuss the concept of metallic bonding importance in detail. So, without any further delay, let’s get started! 

What is Metallic Bonding? 

The metallic bond is a chemistry term used for describing the overall sharing of the sea of the Valance electrons between multiple positively charged ions of metal. Metallic bonding can be defined as a common type of chemical bonding which is responsible for several metal properties, including their malleability, their conductivities for electricity and heat, and their shiny lustre. 

Example – Metallic bonding in the sodium 

The sodium’s electron configuration is 1s22s22p63s1. It mainly has a single electron in its valence shell. Metallic sodium features several Na+ ions in the solid-state, which are surrounded by the sea of 3s electrons. 

Here is an illustration showing the metallic bonding importance in the sodium – 

What are Metals? 

Metals can be defined as substances or minerals formed naturally on the earth’s surface. Mostly, metals are shiny and lustrous; however, they are made of components that were never alive on the earth; therefore, metals are inorganic. Generally, metals are found in rocks washes by groundwater, surface water, or atmospheric dust. 

Metals are extremely durable and strong; as a result, it is nearly impossible to change their shapes using hands. Several things are made up of metals. These include cooking utensils, satellites, automobiles, etc. Certain metals such as sodium and potassium are not as hard as other metals; as a result, they can be cut using a knife. In the world of metals, mercury is an exception as it is in the liquid state at room temperature. 

The extraction and isolation of metals take place over several major steps. These include –

• Ore concentration 
• Metal isolation from concentrated ore
• Metal purification 

Here are the steps involved in the metal extraction from ores-  

• Crushing and Grinding 

Metals are generally found in big chunks inside the earth’s crust. In the first metal extraction step, the ores are crushed and grounded in crushers and ball mills. It increases the chunk’s surface area, which results in better chemical action. This method is known as pulverisation. 

• Concentrating Ore

The second step involves concentrating the ore, which is related to the removal of impurities. This process is known as ore dressing that involves several methods such as Hydrolytic Method, Magnetic Separation, Froth Floatation, and lastly, Chemical Separation. 

• Roasting and Calcination 

Once the ore is finely concentrated, it is then heated in the absence or the presence of the air, depending on the chemical properties of the extracted metals. For example, sulphide ores are mostly heated in the presence of oxygen, whereas carbonated metal ores are heated in the presence of a vacuum. 

Properties Attributed by Metallic Bonding

Metallic bonding features an array of properties that makes them desirable. Here are some of the properties attributed to metallic bonding – 

• Electrical Conductivity

Electricity conductivity can be described as the substance’s ability to move charge through it. Since the electron movement is not restricted, the current can easily pass through the metal. As the potential difference gets introduced to metals, delocalised electrons move towards positive charges, which is why metals are great conductors of electric current. 

• Thermal Conductivity

The material’s thermal conductivity can be described as its ability to transfer or conduct heat. Every time an end of the metallic substance is heated, it leads to a rise in the electron’s kinetic energy, which later gets transferred to other electrons through collisions. 

• Malleability and Ductility

When the ionic crystal including sodium chloride crystal gets beaten through the hammer, it breaks down into smaller pieces. The force-induced through the hammer leads to fracture of the crystal structure leading to shattering of the crystal.

• High Melting and Boiling Points

Metals generally have high melting and boiling points as attractive force laying between the metal atoms is pretty strong. To overcome this force, a great amount of energy is needed as a result, metals possess high boiling and melting points. The exceptions are cadmium, zinc, and mercury. 

Conclusion 

With this, we come to an end of the topic What is Metallic Bonding. Metals as substances or minerals are formed naturally on the earth’s surface. Mostly, metals are shiny and lustrous; however, they are made of components that were never alive on the earth; therefore, metals are inorganic. They are found in rocks washes by groundwater, surface water, or atmospheric dust. Metallic bonding is a common type of the chemical bonding which is responsible for several metal properties including their malleability, their conductivities for electricity and heat, and their shiny lustre. We ended the topic with four major properties of metallic bonding and metallic bonding importance.