Mineral Generalities PDF

Mineral Generalities Date Created @September 20, 2024 3:22 PM Links E_209_02_Minerals_generalities_continued.pdf Minerals and Rocks: Minerals: refers to inorganic and naturally formed solid structures with crystalline structure and a specific chemical composition....

Mineral Generalities Date Created @September 20, 2024 3:22 PM Links E_209_02_Minerals_generalities_continued.pdf Minerals and Rocks: Minerals: refers to inorganic and naturally formed solid structures with crystalline structure and a specific chemical composition. Due to mineral’s solid state structure it makes them impossible to broken down into different mineral structures. Minerals are commonly found with imperfections in colour, form and properties. Mineral Imperfections: Mineralimperfectionsandtheirsignificance Mineralsoftenpresentimperfectionsinform, colorandproperties. Tourmaline:notetheimperfectionsincolor. The image above illustrates the mineral deriving from same species with grey and transparent areas containing pure mineral properties Gallena (check slideshow) Composition process of Minerals: The formation of Minerals can be achieved by a few process, which includes but are not limited to; Molten Matter Crystallization: refers to the process of forming Minerals (solid matter) via the loss of atom mobility and the distinct capacity to form increasingly solid structures. Upon the reach of a certain threshold concentration, the high ion content starts to precipitate new minerals at the Earth’s surface, resulting from a liquid transition to the solid phase. Minerals formation is also possible via some metabolic strategies of certain organisms such as bacteria. The formation of some other mineral is also possible via the rearrangement of both ion and atoms due to significant amount of pressure, extreme temperatures, and chemically active fluid regimes, that allows for preservation of the solid state characteristics. Understanding the Periodic Table of Elements: Periodic Table of Elements: The rows in the periodic table are known as Periods which are ordered by the increasing atomic number of elements The columns in the periodic table are called Groups that are arranged by the similar chemical properties and chemical structures of the elements. Elements situated in Group IA and IIA are capable of losing one or two ions, respectively. Conversely, elements located in Group VIA and VIIA are capable of gaining one or two ions, respectively. The elements between both groups are capable of both losing and gaining or sharing an ion. For instance, Carbon and Silicone demonstrates explicit capability towards electron sharing. In addition, elements located in Group VIIIA are called noble gases and consists of stable electron structures in their outer layer. Therefore, they are not eligible to gain, lose or share electrons to other elements. Atoms, Elements, Isotopes and Ions: According to Democritus’ discovery, atoms are fundamental particles of nature which are indestructible and indivisible. However, in todays context, atoms are not considered as fundamental particles as they are small particles that are precisely arranged and combined. Despite the complex and microscopic dimension of the atoms, it’s distinct parts can still be divided into two, which includes nucleus, and electron;. The nucleus is the core of the atom, comprises of neutrons and protons. In specific, protons are positively charged particles with an electrical charge of +1 and mass of 1, in addition, neutrons are neutrally charged particles with an electrical of charge of 0 and mass of 1. The number of neutrons can be calculated by subtracting the atomic mass from the number of protons. The electron cloud consists of electrons which are negatively charged particles with an electrical charge of -1 and mass of 0. The electron cloud orbits around the nucleus and is believed to be 2000x smaller than protons and neutrons. The atomic number defines the number of protons present in the nucleus. The atomic number may vary from element to element. Moreover, the atomic mass number represents both the number of protons and neutrons in the nucleus and they may vary for other elements. Although, there are some species of the same atoms, that share same number of protons but varies in number of neutrons and are known as Isotopes. For instance, Carbon 12, 13, 14 are derivatives of the same atom but are distinct and unique in their own manner. Types of Bonds in Mineral Structures: Covalent Bonds: It mainly refers to the sharing of electrons between atoms and such phenomenon occurs between non- metals. In specific, the sharing process allows for each atoms to acquire a balanced electron arrangment, which commonly resembles the nearest noble gas. There is no restriction for the number of electrons to be shared, which allows for single, double and triple covalent bonds, in reliance to the number of shared electron pairs. For instance, H₂O demonstrates the sharing of electrons by oxygen with two hydrogen atoms and thus resulting in the formation of Water. Ionic Bonds: Conversely, it mainly refers to the transfer of electrons between atoms and it typically occurs between a non-metal and a metal element. Furthermore, the transferer atom (typically a metal) gains a positvely charged ion (Cations), wheras the receiver (typically a nonmetal) gains a negatively charged ion (Anions). The opposite charges of the ions formulates an electrostatic attraction that holds them together. For instance, NaCl illustrates the tranfer of the Sodium electron to Chlorine atoms, and thus creating Table Salt. Positively Charged Ions are called Cations (+) , whereas Negatively Charged Ions (-) are called Anions (-). Crystalline Network: It refers to the composition and repeating arrangement of ions, atoms, or molecules in a solid matter. In crystal, the particles are arranged in a highly organized and consistent manner which extends the three spatial dimensions. Due to such structural arrangment of the crystals, it provides them distinct geometric shapes and attractive opitcal properties along with strength and conductivity. Unit Cell: it is the smalles repeating unit in the structure, and upon its repitition in three dimensions it formulates the entire Crystalline network. For instance, Quartz and metal such as Iron have all well-defined crystalline networks. Diamond & Graphite: Diamond is the toughest structure in nature, pure due to its atomic properties which includes, atoms of the carbon being situated at the corners of a tetrahedron and each atom being covalently bond by the other four. Diamond are formed under naturally high pressure conditions, and are allocated to the Earth’s surface through high energy volcanic eruptions. Graphite’s structure can be described as rectangular, with parallel layers containing hexagons formed by carbon atoms. The bonds between the carbons atoms in the hexagon corners are covalent; the neighbouring layers are joined by van der Waals forces, which are the weakest bonds in the mineral kingdom Graphite is the byproduct of organic matter decomposition during burial, and is formed after all the other elements- such as oxygen, nitrogen, sulphur, hydrogen, and etc.