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22 Cards in this Set
- Front
- Back
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Mineraology
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Study of minerals
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Rock
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Aggregate of minerals. In a rock, minerals occur as a mixtures, so each mineral retains distinctive properties.
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Singular Rock Aggregate Composition
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Some are comosed of entirely one Mineral: Limestone, Quartz
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Multiple Rock Aggregate Composition
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Most rocks are this way. Granite, Gneiss
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Non mineral Rocks
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Coal, very few are this way
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Atom
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The smallest part of matter that still retains the characteristics of an element.
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Nucleus
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Central region of atom that contains protons and neutrons. This number determines the the atomic number
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Mineral
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A mineral is a naturally occurring inorganic solid that posses a definite chemical structure, giving it a unique set of physical properties
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Mineral Neccessities
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1. Most occur naturally
2. Most be inorganic 3. Must be solid 4. Must posses and orderly internal structure (atoms must be arranged in an definite pattern) 5. Must have definite chemical composition that may vary within specified limts 6. Made up of H20 and SiO2 |
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Proton
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Positive charge, inside nucleus
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Neutron
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Neutral charge, inside nucleus
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Atomic Number
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Determined by the number of proton's in an atom's nucleus
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Valence Electrons
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The electrons involved in the bonding process, the electrons occupying the highest principle energy level of an atom.
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Valence
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The outermost shell of an atom
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Electrons
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Negative charge, orbit tht nucleus
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Compound
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When two or more elements chemically bond in definite proportions
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Ionic Bond
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One of more valence electrons are transferred from one atom to another. One atom loses and electron while the other atom gains it. When electron transfer takes place, atoms are no longer neutral.
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Ion
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Atoms with an electrical charge, or uneven amount of protons and electrons.
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Covalent Bonds
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Occur when atoms share electrons. By sharing, each atom will have 8 electrons on its outer shell. Example: Cl2. Silicon readily forms a covalent bond with oxygen...this bond occurs in the most abundant mineral group- the silicates. Stronger than Ionic Bonds
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Mass Number
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The mass number of an atom is simply te totla of its neutrons and protons in the nucleus. Atoms of the same elements always have the same number of protons but hte number of neutrons may vary.
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Isotopes
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Variants of the number of protons and neutrons in a nucleaus of the same element. Example: Carbon has three well known isotopes (Carbon-12,13, &14). Although most atoms have a stable nucleus, some elements have isotopes in which the nucleus is unstable- these unstable isotopes (carbon-14) disintegrate through a process known as radioactive decay
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Silicon-Oxygen Tretahedron
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The fundamental building block for all atoms. Not a compound, rather it is an ion with a charge of -4.
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