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30 Cards in this Set
- Front
- Back
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unit cell
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The smallest group of particles within a crystal that retains the geometric shape of the crystal
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Gay-Lussac's Law
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The pressure of a gas is directly proportional to the K temp if volume is constant
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Boyle's law
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for a given mass at a constant temp, the volume of gas varies inversly with pressure
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Charles' law
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volume of a fixed amount of gas is directly proporttional to K temp if pressure is kept constant
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diffusion
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the tendency of molecules and ions to move toward areas of lower concentration until the concentration is uniform throughout the system
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effusion
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a process that occurs when a gas escapes through a tiny hole in its container; the diffusion of gases
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electronegativity
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tendency for the atoms of the element to attract electrons when they are chemically combined with atoms of another element
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valence electrons
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electron in the highest occupied energy level of an atom
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surfactant
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wetting agent that stands for the surface active agent and substance whose molecules interface with a hydrogen bonding between water molecules, reducing surface tension
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solvent
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dissolving medium (water)
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solute
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substance being dissolved
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solvation
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process of dissolving an ionic solute; as temp decreases, solubility decreases, same with increasing
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suspension
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mixture from which particles settle out upon standing
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emulsion
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colloidal dispersions of liquids in liquids
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pH
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negative logarithm of hydrogen ion concentration
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indicator
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acid or base that undergoes dissassociation in a known pH range
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titration
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process of adding a known amount of soution of known concentration to determine the concentration of another solution; continued the indicator shows that neutralization has just occurred
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oxidation-reduction reactions
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chemical changes that occur when electrons are transferred between reactants
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oxidation
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complete or partial loss electrons, loss of H, gain of O
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reduction
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complete of partial gain of electrons, gain of H, loss of O
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oxidation-number change method
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balances a redox reaction by comparing the increases and decreases in oxidation numbers
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sublimation
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conversion of a solid to a gas or vapor without passing through the liquid state
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covalent bond
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sharing of electrons to achieve stability
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ionic bond
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forces of attraction that binds oppositely charged ions together
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metallic bond
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attraction of free floating valence electrons for positively charged metal ions
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bond dissassociation energy
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energy required to break a single bond; explains stability of compounds
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unshared pairs of electrons
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valence electrons that are not shared between atoms and dont participate in bonding
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coordinate covalent bond
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covalent bond formed when one atom contributes both bonding electrons
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VSEPR theory
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because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible
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ground state
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lowest energy level of an electron
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