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Thursday, 9 May 2013

Year 11 Chemistry Chapter 6 Glossary


Year 11 Chemistry Chapter 6 Glossary

Mineral: A naturally occurring compound of a metal. 

Ore: A mineral from which a metal may be economically extracted.

Alloy: A substance with metallic properties, formed when a metal is combined with other elements such as carbon or other metals.

Delocalised electrons: Electrons that are not part confined to a particular location, but are able to move throughout a structure.

Metallic bonding: The electrostatic  attraction between cations and the electrons that move between them.

Grains: the crystals that form the structure of metal.

Work hardened: Repeated hammering or bending of a metal, resulting in a herder, more brittle, metal.

Quenching: Heating a metal then cooling it rapidly, resulting in a stronger, more brittle metal.

Annealing: Heating a metal then cooling it slowly, resulting in a softer, less brittle metal.

Tempering: Heating a quenched metal then cooling it slowly, resulting in a stronger but malleable metal.

Alloying: The process creating an alloy be combining metals with another element such as carbon or another metal.

Substitutionally alloys: An alloy formed when metals with similar sized atom's are mixed.

Interstitial alloys: An alloy formed when the atoms of an alloying element fit (because they are a different size) into the spaces between the cations of the parent metal.

Yr 11 Chemistry Chapter 5 Glossary


Yr 11 Chemistry Chapter 5 Glossary

Chemical bond: forms when outer shell electrons of different atoms come close enough to each other to interact and rearrange themselves into a more stable arrangement.

Valence electrons: Outer shell electrons.

Octet rule: atoms will bond together  in such a way  as to obtain an outer shell containing 8 electrons.

Bond dissociation energy: the amount of energy (per molecule of substance) that must be supplied to separate atoms joined by a chemical bond.

Group: the vertical columns on the periodic table, the group number represents the number of outer shell electrons.

Period: the horizontal rows on the periodic table, the period number represents the number of electron shells.

Electrostatic attraction: the attraction between a negatively charged species and a positively charged species.

Ionic bonding: occurs as a the result of a metal atom donating its outer shell electrons to a non metal atom.

Ion: a charge atom. This means it has an unequal number of protons and electrons.

Cation: a positively charge ion. 

Anion: A negatively charge ion.

Crystalline: Arranged in a regular pattern.

Coordination number: A ratio showing the numbers of oppositely charged ions surrounding each ion in an atomic lattice.

Kinetic theory: A model of molecular motion that is used to explain many of the properties of gases.

Lattice enthalpy: A measure of the energy required to completely separate ions in an ionic lattice.

Electrolyte: A liquid that can conduct an electric current.

Electro valency: The charge on an ion.