Introduction

Back to: Rough Diamond Grading and Evaluation

Lesson 1

The Diamond Journey Begins…

In the heart of our planet, deep within the Earth’s mantle, more than 120km below the surface, diamonds are formed.

It begins with the humble carbon atom, which is exposed to immense heat and pressure. The carbon atoms bond together in a cubic or isometric crystal structure, forming a diamond. This type of bonding is called covalent bonding.

Atoms

An atom is the smallest particle of a chemical element that can exist as that element

The Earth and all substances on it, whether gases, liquids, or solids, are made up of atoms. There are many types of atoms, each type is referred to as a chemical element. Most of the atoms on earth are linked: that is, they are bonded together. Each atom is composed of three smaller particles or ‘sub-atomic particles’ called protons, electrons, and neutrons. They are arranged in a specific way so that protons and neutrons are huddled together, in what is known as the ‘nucleus’, and are orbited by electrons in ‘shells’. The number of protons and electrons in an atom is always equal, and the number of neutrons generally follows suit. The number of protons dictates the type of atom, and this is known as an ‘Element’.

Diamond is the only gem formed from a single element – Carbon.

Diamond is typically about 99.95 percent carbon. The other 0.05 percent can include one or more trace elements, which are atoms that aren’t part of the diamond’s essential chemistry. Some trace elements can influence their color or crystal shape.

Crystallography

Earth consists of chemical elements made up of atoms. Most of these atoms are in orderly, solid arrangements. Materials with such orderly atomic arrangements are said to be crystalline and each different atomic arrangement is called a crystal structure. Crystalline materials are made up of different crystalline pieces that have grown together. When a solid crystal structure is formed, the material is said to crystallize. Solid material grows whenever atoms come close enough to share electrons, to form a stable cluster of atoms. The cluster of atoms may continue to build up a rigid structure with further atoms. Diamonds may occur both in single crystals and also in formless (shapeless) crystalline masses. The word ‘crystal’ is often used to describe a single crystal solid with plane crystal faces. It is also used to describe pieces of gem material that consist of a single internal crystal structure, even if the external surfaces are irregular or broken. Crystals are divided into seven main systems of symmetry and diamond forms into the most symmetrical of them, the cubic, also called isometric crystal system.

Crystal Structure

Diamonds form in the isometric (or cubic) crystal system

Diamonds are composed of carbon atoms (like graphite in a lead pencil). A carbon atom has four electrons orbiting in the outer shell. Two carbon atoms can link together by sharing an electron from one, which fills a hole in the shell of the other. As there are 4 electrons and 4 holes to each atom, each atom can link with 4 others; i.e. it has a valency of 4. A carbon atom can share electrons with neighboring carbon atoms to fill its shell to eight. This forms bonds between the atoms. Such bonds are called covalent bonds and can hold atoms together so that they form geometrical structures known as atomic crystals. The lattices are always strong and rigid and the resulting substances are hard solids with high melting-points.

Diamond can be described as a giant saturated molecule of carbon. The 4 bonds to each atom are not, of course, flat, but are always at a 109.5 ° degree angle to each other. This is called the tetrahedral angle.

Each carbon atom is joined to four other carbon atoms by covalent bonds, creating a symmetrical, three-dimensional crystal structure in the form of an imaginary tetrahedron. Every bond is the same, 1.544 ångstrom units long.

Each carbon atom is joined to four other carbon atoms by covalent bonds, creating a symmetrical, three-dimensional crystal structure in the form of an imaginary tetrahedron. Every bond is the same, 1.544 ångstrom units long.

The crystal structure of a diamond is made up of a regularly repeating arrangement of carbon atoms joined to four other carbon atoms via the strongest chemical linkage, covalent bonds. Each carbon atom is in a rigid tetrahedral network where it is equidistant from its neighboring carbon atoms. The structural unit of diamond consists of eight atoms, fundamentally arranged in a cube.

Polymorphism

Carbon is capable of forming many allotropes due to its valency. An allotrope is a single element that can take the form of different crystal structures. This is better known as polymorphism. Carbon is a polymorph. In the case of the element carbon, it can take the form of a diamond as well as graphite. Both diamond and graphite are made almost entirely of the same element – carbon but are completely different in both physical and optical properties due to their atomic crystal structures and covalent bonding.

In graphite, the atoms also form into hexagonal rings, but the rings are flat and in thin plates as shown below. Graphite forms in layers or sheets where the carbon atoms have strong bonds on the same plane or layer, but only weak bonds to the layer above or below. These layers can slide over each other, so graphite is much softer than diamond. The carbon atoms in diamonds, on the other hand, have strong bonds in three dimensions.

The most exceptional atomic crystal structure is that of a diamond. The cubic structure of a diamond, with its strong covalent bonds and rigid and regular repeating arrangement, is what makes it stand out from other substances, and is the key to its unique properties:

• Extreme hardness
• High thermal conductivity
• Resistance to chemicals
• Exceptionally high transparency

The following chart shows how the properties of diamond compare to graphite.

SUBSTANCE	DIAMOND	GRAPHITE
APPEARANCE	TRANSPARENT	BLACK, GREASY
HARDNESS	EXCEPTIONALLY HARD	SOFT, SLIPPERY
DENSITY	HIGH	LOW
ELECTRICAL CONDUCTIVITY	POOR	EXCELLENT

Throughout this course, we will combine theoretical knowledge with practical insights, providing you with a well-rounded perspective on the world of rough diamonds.

In this course, we will explore:

• The Origin and Formation of Diamonds: Discover the incredible natural processes that create diamonds deep within the Earth.
• Mining and Extraction: Explore the techniques and technologies used to extract rough diamonds from their natural environments.
• Identifying Rough Diamonds: Gain the skills to assess the quality and potential of rough diamonds using industry standards.
• Evaluating Rough Diamonds: Learn how to recognize and evaluate the unique characteristics that make each rough diamond one of a kind.
• The Cutting and Polishing Process: Understand how rough diamonds are transformed and follow the intricate process of cutting and polishing diamonds.
• Pricing: Learn how to price individual rough stones and parcels using the Rapaport and Idex Price Lists.
• The Diamond Industry: Understand the dynamics of the global diamond market, from major players and trade practices to market trends and consumer preferences.

By the end of this course, you will have a thorough understanding of the rough diamond journey, from their geological origins to their market value. You will be equipped with the expertise to evaluate rough diamonds and an appreciation for their beauty and significance.

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