Minerals

Inorganic molecules:

Minerals

Minerals are the constituents of rocks.

The terms mineral, compound, element, atom, and isotope refer to different levels of organization of matter. The next higher level of organization than mineral, from the point of view of Earth Sciences (Geology), is that of rocks.

INDEX:

MINERALS

EXAMPLES

DESCRIPTION 1

ATOM

SCHEME

SCHEME 2

ATOMIC MASS

ATOMIC MASS 2

SCHEME 3

COMPOUNDS

PERIODIC TABLE

TYPE OF ATOMIC

SCHEME 4

CRYST. STRUCTURE

CRYST. SYSTEMS

minerals:

Naturally occurring compound or element:- Inorganic - Solid - With a specific chemical composition - Having an ordered internal structure of atoms ⇒ as a consequence of this internal structure it has a: • crystalline form • physical properties

Examples of what is and what is not mineral:

Diamond vs synthetic diamond Diamond vs carbon Ice vs water

POLYMORPH:

MINERALOID:

Natural solid compound without a specific chemical composition and without a crystalline structure (amorphous). Example: glass, resin, opal

Compound that under different conditions organizes its crystalline structure differentlyExamples:- Calcite vs. Aragonite, different minerals with the same composition: CaCO3- Diamond vs. Graphite, different minerals with the same composition: C (Carbon).- Pyrite vs. Marcasite, different minerals with the same composition: FeS2- Quartz vs Cristobalite vs. Tridymite, different minerals with the same composition: SiO2

ATOM:

The smallest division of matter that retains the chemical characteristics of an element. It is represented as a miniature solar system with a core of protons and neutrons and up to 7 shells of electrons orbiting around the core.a) Protons: Positively charged particles with a mass of 1 AMUb) Neutrons: Electrically neutral particles with a mass of 1 AMU. c) Electrons: Particles of infinitesimal size with a negative electrical charge.Atomic Number = Number of Protons (= # of electrons). This number gives the identity of each Atomic Number 0 to 92 correspond to elements that occur naturally (61 is an exception; 43, 85 and 87 are very unstable, they are only found in the stellar spectrum). From 92 onwards they do NOT occur naturally, when they are produced, they are unstable.

+ inf

atomic mass:

Atomic Mass = ∑ of Protons + Neutrons in the nucleus. The same element can have different atomic masses, since the number of neutrons can vary. Each of these variations is an isotope.

Example: Most H is ma = 1 (1 proton); deuterium is ma = 2 (1 proton, 1 neutron) and tritium is ma = 3 (1 proton, 2 neutrons). The more protons in the nucleus, the more electrons and the more orbital shells there are. In each shell there is up to a certain # of electrons; in the last shell the maximum is 8 inert electrons. Elements with 8 electrons in the last shell are gases and are the most stable. The rest of the elements have < 8 electrons in the last shell, so they are chemically reactive.

Compounds

Atoms of elements react with each other and form compounds. These reactions fill the last layers of the atoms, making them chemically stable. In this process, the atoms:a) gain electrons: Anions.- negatively charged ion (# electrons > # proton) b) lose electrons: Cations.- positively charged ion (# electrons < # protons) Atoms with 1,2 or 3 electrons in the last orbit - tend to lose them. Atoms with 4 or more electrons in the last orbit - tend to gain them. Examples: Na with # atoms = 11 ⇒ with 11 electrons: 2, 8 and 1, is a cation with Na1+ Cl with # atoms = 17 ⇒ with 17 electrons: 2, 8, 7, is an anion with Cl1

TYPE OF ATOMIC BONDS:

The way in which the atoms of compounds are joined together largely determines the ordered internal arrangement of atoms that occurs in minerals. Ionic: An outer electron from one atom is given to another to complete its 8 electrons in the last layer. Example: NaCl, LiF Important characteristic: soluble in water.Covalent. Stronger bond: electrons from both atoms are shared. True covalent bonding only occurs with atoms of the same element. Example: Diamond Characteristic: they are almost NOT soluble. they are almost NOT soluble in water.

The ordered individual atoms of minerals are found together in a network: Crystalline Lattice: In this network each atom or ion is located in the same specific place If they occupy random places → amorphous structure. This internal organization can only occur in a solid. States of Matter. Solid, (low ºT or high ºT and low P) Liquid and Gaseous (high ºT or low ºT and high P)

Crystalline structure of minerals

Crystalline Systems:

There are 6 (7 7) Crystal Systems: Isometric, tetragonal, hexagonal, trigonal, orthorhombic, monoclinic, triclinic. Which are subdivided into 32 classes in total. Crystal Systems: They are characterized by their external shape (angles between faces) but mainly by: their symmetry elements: Symmetry axis: its relative length and angles between these axes. Symmetry planes and Symmetry center.

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