Understand Difference

Beneath the Earth’s Surface: The Fascinating Properties of Diamonds and Crystals

Introduction to

Diamond and


Diamond and crystal are two fascinating natural substances that have intrigued humans for centuries. The brilliance of diamond and the colors of crystals have been highly valued both for their beauty and practical uses.

In this article, we will explore what diamonds and crystals are, their differences, and the characteristics that make them so unique.


Diamond is one of the most highly prized and sought-after gemstones in the world. It is a mineral made up of highly pressurized carbon that has been formed deep within the Earth’s mantle.

The formation of diamonds requires high pressure and temperature, making it one of the oldest materials in the world, dating back billions of years. Young diamonds are formed deep in the Earth’s mantle through a process that involves carbon and dense minerals.

Once they are formed, they are brought to the Earth’s surface through volcanic activity.

Diamond’s high pressure and temperature during formation are also responsible for its exceptional hardness, making it the hardest steel known to man.

It is interesting to note that not all diamonds are equal.

Diamonds come in different colors, with the most common colors being white and yellow.

However, there are also rare diamonds that come in blue, pink, and red. These diamonds are highly prized and expensive.


The term crystal is a general term that refers to any solid substance with a regular repeating molecular or ionic arrangement.

Crystals can be found in nature or manufactured in laboratories for various uses.

Some common examples include quartz, salt, and sugar. The arrangement of molecules and ions in crystals is highly ordered and uniform, giving them a distinct appearance and properties.

The arrangement of these molecules and ions is called a crystal lattice, and the size and shape of the lattice determine the crystal’s physical properties. Differences between

Diamond and


Despite both being naturally occurring substances, diamonds and crystals differ significantly from one another in several aspects.

Here are some of the key differences between the two:


Diamonds are formed deep in the Earth’s mantle at high pressure and temperature. The carbon atoms are compressed and bonded together in a tetrahedral crystalline fashion, resulting in dense, hard material.

Crystals, on the other hand, can be formed through a variety of different processes, including precipitation, low-pressure environments, and rapid cooling of molten materials.

Hardness and Appearance

Diamonds are the hardest natural substance on earth, ranking ten on the Mohs scale of mineral hardness. They have irregular shapes and often come with inclusions, which are minute flaws or coloring within the diamond.

Their high reflective and conductive properties make them highly valued for use in jewelry and cutting tools. In contrast, crystals are more delicate and cannot match diamonds’ hardness.

They often form regular, smooth, and perfect stones that reflect light in different ways, depending on their composition and structure. Their differences in composition and structure are also responsible for their varied hues and vibrant colors.


Diamonds and crystals are two fascinating natural substances found on the planet.

Diamonds are valued for their exceptional hardness and rarity, while crystals have different hues, shapes, and properties determined by their unique molecular and ionic arrangements.

Understanding the differences between these two materials helps us appreciate the beauty and properties of these fascinating natural substances better.

Bonding and Conductivity

Diamonds are renowned for their exceptional hardness, but they are also unique in their bonding structure. The bonding structure in diamonds is covalent, which means each carbon atom forms four covalent bonds with other carbon atoms surrounding it.

The bonding results from sp3 hybridization, where the carbon atom uses a combination of s and p orbitals to form four hybrid orbitals with equal energy that are then used for bonding. The sp3 hybrid orbitals result in a tetrahedral structure where the carbon atoms are spaced by specific intervals and have a particular directionality.

The unique bonding structure of the diamond results in its extreme hardness. The covalent bonds hold the carbon atoms in place, strongly resisting any force that would cause deformation.

The tetrahedral structure allows for efficient packing of atoms into a limited space. The result is an incredibly dense material with a high degree of symmetry.

Heat Conductivity

Diamonds are also good conductors of heat, losing heat quickly and efficiently. The explanation behind this phenomenon lies in the close-packing of the atoms and the symmetry of the material which allows for efficient transport of kinetic energy.

The high degree of symmetry and directional bonding of the material provides for efficient movement of the heat through the material. The good heat conductivity properties of diamonds make them useful for many industrial applications.

Diamonds are often used in thermal management applications where the material has to transfer heat quickly and safely. This property also makes them ideal for use in electronic devices where the heat dissipation is a critical factor in performance.

Diamonds, however, do not conduct electricity. While diamonds are covalently bonded, the sp3 hybridization leads to stable structures that do not allow for free electrons, hence the lack of electrical conductivity.

Diamond also has a high band-gap energy of 5.45 electron-volt, meaning that it requires a high energy input to liberate electrons and allow them to move freely.

Crystal and Mineral Conductivity

Crystal and mineral substances vary in their conductivity properties, with some being good conductors and others poor conductors. With the close packing of atoms and specific molecular arrangements, some crystals are good conductors of both heat and electricity.

For example, metals such as copper, silver, and gold are good conductors because their atoms have loosely bound valence electrons. In contrast, minerals such as quartz are poor conductors of both heat and electricity.

Organic materials like wood and plastic are also poor conductors of heat and electricity. This is because in crystal and mineral substances, the detailed molecular and ionic arrangements usually result in the unavailability of free electrons or an absence of structured repeating patterns.


Diamond and Carbon

Diamond is a form of carbon that forms deep within the Earth’s crust under high temperature and pressure. The carbon atom forms covalent bonds using sp3 hybridization to create a tetrahedral structure, resulting in a symmetric material with highly directional bonding.

The unique bonding structure results in the extreme hardness of diamond, making it the hardest natural substance on earth. The tetrahedral structure also makes diamond one of the best conductors of heat.


Crystal and Mineral

Crystals and minerals are substances that vary in shape, size, and color. Their conductivity properties vary widely, with some crystals being good conductors of heat and electricity, while others are poor conductors.

The detailed molecular and ionic arrangements are the main factors influencing conductivity properties, as well as other physical and chemical properties of crystals and minerals. In conclusion, the bonding and conductivity properties of diamond and crystal are both fascinating and unique.

Diamond’s exceptional hardness comes from its covalent bonding structure resulting from sp3 hybridization. It is the hardest natural substance on earth, has a high degree of symmetry, and is an efficient conductor of heat.

In contrast, crystal and mineral substances vary in their conductivity properties, and some are good conductors of both heat and electricity, while others are poor conductors. Understanding the detailed molecular and ionic arrangements of these materials helps us appreciate their physical and chemical properties better.

Overall, the study of these natural substances is crucial to developing various industrial, electronic, and thermal management applications.

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