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55 Cards in this Set
- Front
- Back
Covalent Bond
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shared electrons between two or more atoms
families 13-15 octet rule |
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Ionic Bond
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gain/lose electrons
families 1,2,16,17 weaker than covalent, held by poles |
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Metallic Bond
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electron cloud around multiple atoms
families 3-12 "communism"-pooled and divided resources (electrons) |
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Endothermic
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reaction that absorbs heat
(NH4NO3 {Ammonium Nitrate} + H2O {Water} = cold) |
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Exothermic
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reaction that releases heat
(NaOH {Sodium Hydroxide} + H2O {Water} = hot |
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Exergonic
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lit. (all energy)
reaction that releases energy (heat, sound, light, etc.) |
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Endergonic
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reaction that absorbs energy
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Solution
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a homogenous mixture
can't see difference in substances (air, lemonade, etc.) |
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Solute
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what dissolves
(drink powder) |
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Solvent
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what the solute dissolves into
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Polyatomic Ions
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lit. (multi-atoms ions)
compounds w/ more or less electrons (ionic compounds) |
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Reactant
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substance that reacts with another in a chemical change
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Product
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What is formed or left by a chemical reaction
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Catalyst
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presence of which speeds up a reaction w/out being used up itself
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Ion
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an atom with more or less electrons than it is supposed to have, causing it to be positively or negatively charged (less=+, more=-)
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Isotope
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an atom with more neutrons than usual (increases At mass)
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Alkali Metals
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Family 1A
soft, silvery-white +1 ions react very strongly w/ water, acids, bases (most reactive fam) |
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Alkaline Metals
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Family 2A
+2 ions similar but not as extreme as F1 |
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Transition/Heavy Metals
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typical metals
ductile, malleable, conductive, high melting point |
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Other Metals
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soft, malleable metals
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Non-metals
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not ductile or malleable
bad conductors flaky or crumbly (sulfur) |
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Metalloids
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properties of metals and non, in between
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Halogens
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Family 7A
-1 ions react violently 2nd most reactive |
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Noble Gases
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colorless, odorless
non-reactive almost never form compounds |
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Rare Earth Metals
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Lanthanide/Actinide series
heavy, most radioactive metals |
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Dmitri Mendeleev
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1869- 1st person to make a periodic table of elements (Julias Meyer 2nd)
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Harry D. Hubbard
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1928- standardized the periodic table of elements
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Glen Seaborg
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1944- Lanthanide and Actinide series (two pulled out rows)
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Democritus
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400 BC
"Atomos"- Greek for "atom" first with idea of small, basic building block of matter |
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Robert Boyle
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1691- 1st to question traditional atom model
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John Dalton
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1803-Atoms: in-divisible/ destructable, make up matter; of same element are identical,diff are diff; only combine in small whole # ratios; neither made or destroyed
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J.J. Thompson
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1904- discovered electrons
"Plum Pudding" model |
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Ernest Rutherford
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1911- nucleus hard+atom mostly empty w/ + particles around???????????????
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James Chadwick
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1932- discovered neutrons
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Niels Bohr
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1913- stated that electrons orbit
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Wave Theory
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Modern- electrons bounce randomly and found in energy levels
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Molecular Mass
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# of protons+neutrons in nucleus
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Synthesis
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reactants join together
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Decomposition (Rx Reactions)
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compound splits apart
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Single Replacement
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one reactant replaces part of another
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Double Replacement
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one part of each reactant splits off and swaps with the other
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Combustion
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one reactant undergoes decomposition and the other synthesizes partially with one and partially with the other
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Law of Conservation of Matter
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matter cannot be created or destroyed, but changed from one form to another
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Melt
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S-->L
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Evaporation
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L-->G
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Condensation
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G-->L
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Solidification (freeze)
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L-->S
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Sublimination
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S-->G
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Decomposition (phase changes)
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G-->S
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Mixture
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a mixture of substances that are not chemically bonded
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Pure Substance
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an element or mixture of substances that are chemically bonded
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Heterogeneous Mixture
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you can see the difference in the substances in the mixture
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Homogeneous Mixture
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you can't see the difference between substances in mixture (solution)
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Colloid
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cloudy solution where light illuminates particles but continues through
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Suspension
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large particles or chunks visibly float around in the solution
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