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There are three types of chemical bonds: ionic, covalent, and metallic. In this blog post, we will discuss the difference between ionic, covalent, and metallic bonds. Ionic bonds are formed when two atoms exchange electrons to create a positive and negative ion. Covalent bonds are formed when atoms share electrons to create a molecule. Metallic bonds are created when metal atoms lose their outermost electron to form positively charged ions. Let’s take a closer look at each type of bond!
What is an Ionic Bond?
Ionic bonds are electrostatic interactions between atoms that are held together by their attraction to each other. In ionic bonds, one atom gives up an electron to another atom, which creates charged ions that are attracted to each other. Ionic bonds are usually between a metal and a nonmetal.
An example of an ionic bond is between sodium (Na) and chlorine (Cl).
What is a Covalent Bond?
A covalent bond is formed when two atoms share electrons. In a covalent bond, the electron pairs are shared evenly between the atoms. Covalent bonds are usually between two nonmetals.
An example of a covalent bond is between hydrogen (H) and oxygen (O).
What is a Metallic Bond?
Metallic bonds are formed when atoms share electrons in a way that creates a “sea” of delocalized electrons. The delocalized electrons allow the atoms to move freely around, which is why metals are usually solid at room temperature (since the atoms can’t move around). Metallic bonds are usually between a metal and another metal.
An example of a metallic bond is between copper (Cu) and zinc (Zn).
Iconic, Covalent and Metallic Bond:Difference
In order to understand the difference between ionic, covalent, and metallic bonds, it is important to first understand on what basis these can be differentiated. Therefore they can be differentiated on the basis of occurrence, conductivity, binding energy, bond, state of presence, melting point, boiling point, ductility, and malleability.
Discuss each of the factors to differentiate iconic, covalent, and metallic bonds.
Occurrence
Ionic bonds occur between a metal and a nonmetal. Covalent bonds occur between two nonmetals. Metallic bonds occur between metals.
Conductivity
Ionic bonds do not conduct electricity in the solid-state but they do in the liquid and molten state. Covalent bonds do not conduct electricity in any state. Metallic bonds are good electrical conductors in all states.
Binding Energy
Ionic bonds have high binding energy. Covalent bonds have low to moderate binding energy. Metallic bonds have low binding energy.
Bond
Covalent bonds are directional whereas covalent and metallic bonds are non-directional.
State of Presence
Ionic bonds are present in the solid, liquid, and gaseous states. Covalent bonds are present in all three states but are strongest in the solid-state. Metallic bonds are present in all three states but are strongest in the solid-state.
Melting Point
Ionic bonds have high melting points. Covalent bonds have low to moderate melting points. Metallic bonds have low melting points.
Boiling Point
Ionic bonds have high boiling points. Covalent bonds have low to moderate boiling points. Metallic bonds have low boiling points.
Ductility
Metallic bonds are ductile. Ionic and covalent bonds are not ductile.
Malleability
Metallic bonds are malleable. Ionic and covalent bonds are not malleable.
From the above discussion, it can be concluded that ionic, covalent, and metallic bonds differ from each other on the basis of occurrence, conductivity, binding energy, bond, state of presence, melting point, boiling point, ductility, and malleability.
There might be more differences between the three types of bonds. However, we have discussed the more major ones in detail in the above sections.
Conclusion
In short, ionic bonds are formed when a metal and a nonmetal come together. Ions are created as the electron from the metal atom transfers to the nonmetal atom. Covalent bonds form when two atoms share electrons in order to fill their outer shells. Metallic bonding is unique in that it occurs when atoms lose their outermost electrons completely. These free-floating electrons then bond with other metal atoms, creating a metallic solid. So what difference does all of this make for students? The key takeaway is that covalent and metallic bonding produce different types of materials with distinct properties. Understanding these differences can help you predict how substances will behave, which can be enormously helpful when trying to solve problems in chemistry or physics labs.
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