CH 101: FINAL EXAM
178 Cards in this Set
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Chemistry
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The study of matter- characteristics, composition and transformation of matter
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energy
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The ability to do work
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matter
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anything that has mass and occupies space
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physical properties of matter
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Properties that can be observed in matter without a change in identity
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chemical properties of matter
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these properties of matter are determined by the way substances react chemically with other substances
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physical change in matter
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this change in matter does not result in a change of identity
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chemical change of matter
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this change in matter results in a change of identity
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4 evidences of chemical change
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1. evolution of a gas (fizzing) 2. color change 3. formation of a precipitate 4. temperature change
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pure substance
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one unique form of matter that cannot be separated by physical means
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element
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a pure substance that cannot be broken down to simpler substances by ordinary chemical means
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compound
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pure substance that can be broken down by ordinary chemical means (formed by the chemical combination of 2 or more elements)
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mixture
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physical combination of two or more materials
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homogeneous mixture
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a mixture that has similar parts throughout
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heterogeneous mixture
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a mixture that has different parts or phases throughout
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atom
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the smallest part of an element with all the properties of that element
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molecule
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the smallest part of matter capable of independent existence
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monatomic molecule
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molecule with only one type of atom
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homoatomic molecule
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molecule with more than one atoms that are the same
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heteroatomic molecule
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molecule with two or more atoms that are not the same (HOH)
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subatomic particles
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protons, neutrons and electrons
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atomic number
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the number of protons in an atom
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mass number
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the sum of the number of protons and neutrons (always a whole number)
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Isotope
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atoms of the same element with the same number of protons and electrons but different numbers of neutrons (same chemical properties but slightly different physical properties)
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nucleus
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small, dense, positively charges center of an atom
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nucleon
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any subatomic particle found in the nucleus of an atom
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atomic mass
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average mass of all the naturally occuring isotopes of an element
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chemical bonds
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attractive forces that hold atoms together in more complex units
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bonds
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these form as a result of electron interaction
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ionic bonds
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these bonds result from the transfer of electrons
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covalent bonds
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these bonds result from the sharing of electrons
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lewis structure
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symbol with one dot to represent each valence electron
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valence electrons
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electrons located in the outer shell only
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octet rule
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this rule states that atoms lose, gain, or share electrons to obtain electron configurations like the noble gas that is nearest to them
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ions
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charged particles
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positive ions
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ions that have lost electrons
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negative ions
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ions that have gained electrons
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isoelectronic species
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chemical units tht have the same electron configuration
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polyatomic ions
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charged groups of atoms
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formula unit
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the smallest whole-number ratio of the components in an ionic compound
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electronegativity
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the relative strength of attraction for bonding electrons
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flourine
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the most electronegative element
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oxygen
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the second-most electronegative element
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nonpolar covalent bond
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this bond has an equal sharing of electrons (same electronegativity)
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polar covalent bond
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this bond has an unequal sharing of electrons (atoms have different electronegativity)
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molecular polarity
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the overall charge distribution on a molecule
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metric system
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the base unit of this system is ten (either divide or multiply by powers of ten to make conversion)
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significant figures
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all non-zero digits, confined zeroes and trailing zeroes with a decimal point are significant when deterimining these
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scientific notation
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the shorthand method for representing either very large or very small numbers
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dimensional analysis
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a problem solving method using units as a guide for setting up a problem (also called unit analysis)
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conversion factors
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ratios that show the mathematical relationships between units
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mole
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6.02 x 10(23 power) parts of anything. aka Avogadro's number
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1.8 x C + 32
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the conversion factor from celcius to farenheit
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F-32/1.8
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the conversion factor from farneheit to celcius
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kelvin temperature scale
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this scale is also known as the absolute temperature scale (the units are the same size as Celcius but the freeszing point is at 0 on celcius and 273 on this)
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heat
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energy; measured in calories
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Hotness or coldness
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measured in degrees
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specific heat
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the amount of heat energy necessary to raise one gram of a substance 1 degree celcius ( cal/g x C)
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q=mc(delta)t
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equation dealing with energy and specific heat
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kinetic energy
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energy of motion ( is a disruptive force)
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potential energy
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energy of position (cohesive forces)
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particle collisions
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the collisions are elastic
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solids
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this state of matteris dominated by cohesive forces
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liquid
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this state of matter is dominated equally by cohesive and disruptive forces
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gas
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this state of matter is dominated by disruptive forces
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Boyle's Law
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this law states that P1V1=P2V2. Has an inverse relationship
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Charle's Law
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this law states that V1/T1=V2/T2. Direct relationship
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combined gas law
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this law states that P1V1/T1=P2V2/T2
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ideal gas law
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this law states that PV=nRT
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Dalton's law of partial pressures
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this law states that Pt= Pa+Pb+Pc...
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Change of state
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the process in which a substance is transformed from one physical state to another
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endothermic
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this change of state requires energy (ex. melting, evaporation, sublimation. Goes from a solid into a gas)
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exothermic
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this change releases energy (ex. freezing, condensation, deposition. Goes froma gas into a solid)
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vapor
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gaseous form of a substance that is a solid or liquid at room temperature (usually a liquid)
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vapor pressure
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pressure exerted by vapor above a liquid at equilibrium. Can also be described as the "escaping tendency" of a liquid.
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volatile substance
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a substance which readily evaporates at room temperature- has high vapor pressures
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boiling
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conversion from liquid to vapor within the body of the liquid
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boiling point
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the temperature at which the vapor pressure equals the atmospheric(surrounding) pressure
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dipole-dipole
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the type of attraction when the the negative end of one molecule is attracted to the positive end of another molecule
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hydrogen bonds
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these bonds are not true chemical bonds. They occur when H is attracted to O, F, or N of another molecule
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london forces
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weak, temporary forces of attraction. result from temporary, uneven distribution of charge
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solute
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part that is dissolved
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solvent
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solvent part in which the solute is dissolved
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solubility
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maximum amountof solute that will dissolve in a given amount of solute at a given temperature
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unsaturated
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this type of solvent can dissolve more solute under the conditions given
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saturated
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the type of solvent has dissolved the maximum amount of solute it normally can under the conditions given
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supersaturated
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this type of solvent is temporarily holding more solute than it normally can unfer the conditions given
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aqeous solution
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water is the solvent in this type of solution
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molarity
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the formula for this is M= moles solute/L solution
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dilution
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the formula for determining this is CsVs=CdVd (C= concentration, s= stock, d= diluted)
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tyndall effect
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the scattering of light by colloidal particles
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colligitave properties
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the physical properties of a solution based on the number of particles present
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osmosis
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the passage of solvent molecules across a semipermeable membrane
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hypotonic
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water is more concentrated outside the cell in this type of solution (results in hemolysis)
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hypertonic
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water is more concentrated inside the cell in this type of solution (results in crenation)
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dialysis
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passage of solvent molecules, ions, and small molecules across a semipermeable membrane
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chemical reaction
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process in which at least one new substance is formed as a result of chemical change
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products
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reactants yield these
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redox reaction
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this type of reaction occurrs from the transfer of electrons from one reactant to another reactant
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non-redox
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this type of reaction occurs when there is no transfer
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oxidation number
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the apparent charge of an atom in a bond
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oxidation
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this term is used for the loss of electrons (increase in oxidation number)
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reduction
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this term is used for the gain of electrons (reduction in oxidation number)
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OIL RIG
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the acronym for remembering how oxidation works (oxidation is gain... reduction is loss)
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oxidizing agent
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part that causes oxidation, therefore it is the part that gains electrons and is itself reduced
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reducing agent
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part that causes reduction to occur, therefore is the part that loses electrons and is therefore the reducing agent
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collision theory
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this theory states the conditions that must be met for a chemical reaction to take place
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catalyst
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the presence of these in a chemical reaction only reduces the required activation energy, it does not change the position of equilibrium
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chemical equilibrium
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this happens when opposing reactions occur at the same rate
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equilibrium constants
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definite values that show a relationship between the concentrations of products and reactants in a system at equilibrium
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keq
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equilibrium expression
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gases
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only dissolved substances such as aq and ________ show up in keq
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more
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a keq of 10(to the 3rd power) or greater yields ________ products
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more
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a keq of 10(-3rd power) or less yields ______ reactant
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significant
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a keq of 10(3rd power) - 10(-3rd power) yields a ___________ amount of both products and reactants
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Le Chatelier's Principle
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this principle states that "when stress is applied to a system at equilibrium, the equilibrium will shift to reduce the stress"
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arrhenius acid
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H contianing compound that produces H+ ions in water
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arrhenius base
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OH containing compound that produces OH- ions in water
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ionization
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formation of positive and negative ions from a covalent compound (when placed in water)
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dissociation
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separation of ions from an ionic compound (when placed in water)
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bronsted-lowry acid
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this is defined as a proton donor
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bronsted-lowry base
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this is defined as a proton acceptor
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conjugate acid
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this is formed from a base + H+
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conjugate base
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this is formed from an acid- H+
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amphiprotic
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these types of compounds can either donate or accept a proton
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monoprotic
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this type of acid donates one H+
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polyprotic
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this type of acid donates two or more H+
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strengths
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the _________ of acids or bases are determined by the extent to which they donate or accept protons
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strong
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________ acids transfer 100% of their ionizable protons to water
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weak
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_______ acids transfer less than 5% of ionizable protons to water
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neutralization
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what kind of reaction between an acid and a base results in the formation of a salt and a water?
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salts
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ionic compounds with metals or NH4+ as the positive ion and any negative ion except OH-
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acidic
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when the [H3O+] is greater than [OH], the solution is said to be _______
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basic
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when the [OH-] is greater than [H3O+] the solution is said to be _________
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neutral
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when the [H3O+] equals [OH-] the solution is said to be ______
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pH
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-log[H3O+]
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antilog(-pH)
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how do you find the [H3O+] using only the pH?
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pH+pOH=14
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the equation relating pH and pOH
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inverse
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pH and [H3O+] have a/an _________ relationship
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neutral
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strong acid + strong base = _________ salt and water
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acidic
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strong acid + weak base = _______ salt and water
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basic
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weak acid + strong base = ______ salt + water
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hydrolysis
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reaction of substance with water to produce hydronium or hydroxide ions (or both)
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buffers
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aqueous solutions with substances that resist a change in solution pH when limited amounts of acids or bases are added
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buffering systems
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a weak acid and a salt of its anion(conj. base) and a weak base and a salt of its cation(conj. acid) are both examples of ________ ________
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acidosis
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a blood pH of 7.1 to 7.2 results in ________
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alkalosis
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a blood pH of 7.5 results in __________
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electrolyte
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a substance that conducts electricity when dissolved in water
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non-electrolyte
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substance that does not conduct electricity when dissolved in water
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weak
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a ________ electrolyte is a weak conductor of electricity, only partially ionize
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strong electrolytes
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good conductors of electricity, 100% ionization (strong acids and bases that are very soluble)
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titration
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process in which a solution of known concentration is used to determine the concentration of another solution
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nuclides
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atoms with specific numbers of neutrons and protons (can aka isotopes)
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unstable
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a/an ________ nuclide can easily undergo change
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stable
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a/an ________ nuclide does not easily undergo change
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radioactivity
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radiation emitted from the nucleus of an unstable nuclide
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radioactive nuclide
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this nuclide spontaneously emits radiation
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Bequerel
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this man discovered radioactivity
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Marie Curie
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this woman gave the name radioactivity. She also died as a result of her exposure to radiation
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Rutherford
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man who discovered the nature of emissions (radiation)
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Alpha particle
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positive particle with two protons and two neutrons, +2 charge, mass of 4 amu
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beta particle
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negative particle, charge and mass of electron (0 amu)
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gamma rays
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rays that are not particles in nature: energy
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radioactive decay
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the giving off of nuclear particles causing a change from the nuclide of one element into a nuclide of a different element
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parent
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original nuclide
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daughter
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new nuclide
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alpha decay
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loss of four particles (2n,2p) . Atomic number of daughter is two less than the parent, mass number is four less
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beta decay
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change of a neutron to a beta particle + a proton. Atomic number of daughter is greater than that of the parent, mass number is the same
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half life
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time for 1/2 of a given quantity of the nuclide to decay
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bombardment
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a ________ reaction is when high speed small particles collide with an element and cause a nuclear reaction
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radioactive decay series
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sequence of nuclear reactions from a large unstable nuclide to a smaller stable nuclide
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alpha
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______ particles are 1/10 the speed of light, do not penetrate the skin and are stopped by a sheet of paper
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beta
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_____ particles are 9/10 the speed of light, penetrates skin, causes burns, stopped by a 1 cm thick sheet of Al
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gamma
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____ rays are the speed of light, have the greatest penetrating power (organs, bones and other tissues), not totally stopped by lead and concrete
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ion pairs
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these are formed when radiation strikes an atom
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free radicals
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highly reactive uncharged fragments of a molecule with unpaired electrons
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cancer
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this is one example of the therapeautic use of nuclear medicine
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fission
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splitting of an atom with the release of high amounts of energy
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fusion
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small nuclei are put together with the release of a great amount of energy
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CH 101: EXAM 3