Chapter 7 - Ionic Compounds & Metals
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Created by:
qtpiexoxo23 on June 18, 2011
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chemistry preparation
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39 terms
Terms | Definitions |
|---|---|
 octet rule | atoms tend to gain, lose, or share electrons in order to acquire eight valence electrons |
| cation | positively charged ion |
| anion | negatively charged ion |
| chemical bond | the force that holds two atoms together |
| compound | a chemical combination of two or more different elements |
| ionic bond | the electrostatic force that holds oppositely charged particles together in an ionic compound |
| ionic compound | compounds that contain ionic bonds |
| crystal lattice | a three-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and vice-versa |
| electrolyte | an ionic compound whose aqueous solution conducts electric current |
| lattice energy | the energy required to separate 1 mol of the ions of an ionic compound |
| nonmetal | an element that is generally a gas or a dull, brittle solid and is a poor conductor of heat and electricity |
| formula unit | represents the simplest ratio of the ions invovled in an ionic compound |
| monatomic ion | a one-atom ion |
| oxidation number (oxidation state) | the charge of a monatomic ion |
| polyatomic ion | made up of more than one atom |
| oxyanion | a polyatomic ion composed of an element, usually a nonmetal, nonded to one or more oxygen atoms |
| physical property | a characteristic of matter that can be observed or measured without altering the sample's composition |
| electron sea model | proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons, which surrounds the metal cations in the lattice |
| delocalized electron | electrons that are free to move |
| metallic bond | the attraction of a metallic cation for delocalized electrons |
| alloy | a mixture of elements that has metallic properties |
| chemical bond | the force that holds two atoms together |
| covalent bond | the chemical bond that results from sharing valence electrons |
| molecule | formed when two or more atoms bond covalently |
| Lewis structure | electron-dot diagrams that used to represent the arrangement of electrons in a molecule |
| sigma bond | single covalent bonds represented by the symbol σ |
| pi bond | forms when parallel orbitals overlap and share electrons, represented by the symbol π |
| endothermic reaction | occurs when energy to break existing bonds in the reactants is greater than the amount of energy released when new bonds are formed in the products |
| exothermic reaction | occurs when a greater amount of energy is released during product bond formation than during the breaking of bonds in the reactants |
| multiple covalent bond | a bond that consists of one sigma bond and at least one pi bond |
| oxyacid | an acid that contains both a hydrogen and an oxyanion |
| structural formula | a molecular model that uses letter symbols and bonds to show relative positions of atoms |
| resonance | a condition that occurs when more than one valid Lewis structure can be written for a molecule or ion |
| coordinate covalent bond | forms when one atom donates both of the electrons to be shared with an atom or ion that needs two electrons to form a stable arrangement with lower potential energy |
| VSEPR model | Valence Shell Electron Pair Repulsion model, based on an arrangement that minimizes the repulsion of shared an unshared electron pairs around the central atom |
| hybridization | a process in which atomic orbitals mix and form new identical hybrid orbitals... yea fix this.. |
| atomic orbital | the region around an atom's nucleus that defines an electron's probable location |
| electronegativity | the relativeability of an atom to attract electrons in a chemical bond |
| polar covalent bond | unequal sharing of electrons between elements of different electronegativities |
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