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CHE 101: Final Exam
molarity
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moles/L
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molality
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moles/kg
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less than
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The vapor pressure of a solution is _______ that of the pure solvent.
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less than
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The freezing point of a solution is _______ that of the pure solvent.
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greater than
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The boiling point of a solution is ______ that of the pure solvent.
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1st law of thermodynamics
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Energy cannot be created or destroyed. It can be changed from one form to another.
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2nd law of thermodynamics
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The universe spontaneously tends toward more disorder or randomness.
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increase concentration, and add catalyst
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What speeds up a reaction?
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energy
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Is the ability to do work.
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hydrogen
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Acid dissociates to form _______ in water
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hydroxide
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Base dissociates to form _______ in water
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proton donor
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Acids are ______ _______
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proton acceptors
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Bases are _______ ________
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Acid
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taste sour, conducts electricity, and turns litmus paper red.
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Base
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taste bitter, conducts electricity, and turns litmus paper blue.
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oxidation
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Is the loss of electrons. Oxidation number increases.
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reduction
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is the gain of electrons. Oxidation number decreases.
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voltaic
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the type of electrical cell that produces energy
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electrolytic
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the type of electrical cell that uses energy to bring about a chemical reaction
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Polyprotic
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more than one H
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potential
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related to the motion of an object or its position relative to gravity, stored energy
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kinetic
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related to flow of electrons, moving energy
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exothermic reaction
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gives off heat
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endothermic reaction
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takes in heat
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mechanical
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related to the motion of an object or its position relative to gravity
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electrical
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related to the flow of electrons
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chemical
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related to the energy stored in the bonds of a molecule.
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enthalpy
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term chemists use for energy changes in reactions. Heat
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entropy
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term that refers to the disorder in a system. Disorder or randomness
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activation energy
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the energy needed to get a reaction started
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electromagnetic radiation
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type of energy that consists of electrical and magnetic waves
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heat
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the transfer of thermal energy between two bodies at different temperatures
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sound
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type of energy transmitted by the compression and expansion of molecules
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specific heat
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the amount of heat needed to raise the temperature of one grams of a substance by one degree Celsius
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joule
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unit uses to measure energy
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catalysts
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is a substance that speeds up a chemical reaction but can be recovered unchanged at the end of the reaction
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equilibrium
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a chemical reaction that can run to make both products and reactants
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forward
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reaction that runs from left to right
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reverse
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reaction that runs from right to left
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neutralization
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reaction between an acid and a base, products are salt and water.
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buffer
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resist changes in pH
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osmosis
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the movement of a solvent from a dilute solution to a more concentrated solution through a semipermeable membrane.
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system
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the process we are studying
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surroundings
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everything else in the universe
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spontaneous
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exothermic reactions are _______
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not spontaneous
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endothermic reactions are _________
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completely
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a strong acid or base dissociates __________ in water
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partially
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a weak acid or base dissociates _________ in water
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Boyle's Law
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A principle that describes the relationship between the pressure and volume of a gas at constant temperature
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Charle's Law
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the law relating volume and temperature
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Ideal Gas Law formula
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PV = nRT
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Kelvin =
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C+ 273
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Crystalline
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having a regular, repeating structure
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Amorphous
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having no organized structure
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22.4 L
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the volume of 1 Mole of gas at STP is
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Solution
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a homogeneous mixture of two or more substances (after water and kool-aid have mixed)
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solute
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what is being dissolved (kook-aid)
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solvent
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what does the dissolving (the water)
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two measurements of pressure
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atm and mm Hg
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what is the size of a solution particle
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small
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what is the size of a colloid particle
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medium
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what is the size of a suspension particle
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large
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Ionic Bonds
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Electrons are transferred from one atom to another
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Covalent bond
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A chemical bond that involves sharing a pair of electrons between atoms in a molecule
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metals
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form cations
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nonmetals
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have high ionization energies
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metals
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have low electron affinities
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intramolecular forces
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are attractive molecules within an atom and determine shape and polarity of molecules.
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intermolecular forces
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Forces between atoms or molecules in a substance that determine the phase of matter.
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dipole
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A molecule that has two poles
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trigonal planer
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F-B-F
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120
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bond angle for a trigonal planer
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electronegativity
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Atom's ability to attract and hold electrons.
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polyatomic ions
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composed of 2 or more atoms bonded together
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metalloids and nonmetals
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generally only form covalent bonds
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crystalline solid
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A solid that is made up of crystals in which particles are arranged in a regular, repeating pattern
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amorphous solid
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A solid made up of particles that are not arranged in a regular pattern
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resonance
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a condition that occurs when more than one valid Lewis structure can be written for a particular molecule
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molecules
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Chemical substances made of two or more atoms that are bonded together by covalent bonds. H20, O2, CO2, H2, N2, etc, are naturally occurring examples. Compare with ions, which are NOT held together by covalent bonds.
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formula unit
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is the smallest collection of atoms or ions
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the identity of the atom and
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what info does a formula unit give
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formula mass
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the sum of the atomic masses of all the elements in a formula unit of the compound
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Ionic bond
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More than 2.0 electronegativity
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0.5 - 1.9 electronegativity
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Polar covalent
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Non polar bond
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Less than .5
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energy
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the ability to do work
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calorie or joule
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how energy is measured
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4.184 joules
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1 calorie =
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density
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mass of a given volume of a material
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D=(m/v)
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Density =
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M=D*V
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Mass =
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atom
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smallest unit of an element that has the properties of that element
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proton, neutron, electron
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atoms are themselves composed of 3 subatomic particles know as:
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-1
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what charge does an electron have
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0
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what charge does a neutron have
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1
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what charge does a proton have
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electron
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e-
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proton
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p+
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neutron
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n
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Dalton 1808
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first proposed atomic theory in early 1800's
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TRUE
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T/F Most of Daltons original theory is correct
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Rutherford 1903
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who came up with the first idea that atoms have a nucleus and they nuclei are "massive"
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Bohr
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who cam up with electrons can only occupy fixed energy levels around the nucleus
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chemistry
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the study of matter and the changes that matter undergoes
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matter
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anything that has mass and occupies space
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hypothesis
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an attempt to explain observation in a commonsense way
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theory
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a hypothesis supported by extensive testing that explains and predicts facts
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physical property
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can be observed or measured without changing the composition or identity of a substance
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physical change
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produces a recognizable difference in the appearance of a substance without causing any change in its composition or identity
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chemical properties
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results in a change in composition and an be observed by only through chemical reactions
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chemical reaction
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a chemical substance is converted to one or more different substances by rearranging, removing, replacing, or adding atoms
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element
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is a pure substance that cannot be changed into a simpler form of matter by any chemical reaction
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compound
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a substance resulting from the combination of two or more elements in a definite, reproducible way
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Biochemistry
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the study of life at the molecular level
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Organic chemistry
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the study of matter containing cordon and hydrogen
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Inorganic chemistry
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the study of matter containing other elements not organic
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analytical chemistry
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analyze matter to determine identity and composition
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physical chemistry
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study of matter using physics concepts and mathematics
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w`456\
n 4 op\][poiuytrewquclear chemistry
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study of the structure and properties of the nucleus
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Observation, formulation of a question, pattern recognition, developing theories, experimentation, summarizing information
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list the scientific method
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state and composition
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two ways to categorize matter
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gas
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no fixed shape, no fixed volume
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liquid
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no fixed shape, fixed volume
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solid
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fixed shape, fixed volume
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solid, liquid, gas
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what are the 3 states of matter
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mixture
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combination of two or more pure substances in which each substance retains its own identity
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intensive property
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a property of matter that is independent of the quantity of the substance. (color, melting)
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extensive property
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a property of a substance that depends on the quantity of the substance. (mass, volume)
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homogeneous mixture
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has a uniform composition. ex. alcohol
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heterogeneous mixture
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has a nonuniform composition. ex. concrete
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C
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P/C a freshly cut apple turns brown
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P
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P/C when cooled to 0*C liquid water turns to ice
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C
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P/C fermentation of sugar to alcohol
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C
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P/C frying an egg
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chemical properties
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results in a change in composition and can be observed only through chemical reactions
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P
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P/C detecting the odor cyanide during anautopsy
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P
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P/C property, Color
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C
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P/C property, flammability
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P
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P/C property, hardness
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P
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P/C property, odor
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C
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P/C property, Taste
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Intensive property
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I/E property, color
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Intensive property
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I/E property, melting point
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Extensiv property
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I/E property, mass
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mass, volume, length, and time
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name the main units used in chemistry
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grams
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name the main unit used in chemistry to measure mass
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liter
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name the main unit used in chemistry to measure volume
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meter
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name the main unit in chemistry to measure length
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seconds
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name the main unit in chemistry to measure time
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celsius
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name the main unit in chemistry to measure temperature
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significant figures
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all digits in a number representing data or results that are know with certainty plus one uncertain digit
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scientific notation
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the representation of a number as a power of ten
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error
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the difference between the true value and our estimation, or measurement, of the value
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accuracy
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the degree of agreement between the true value and the measured value
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uncertainty
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the degree of doubt in a single measurement
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precision
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a measure of the agreement of replicate measurements
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k 1000
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Kilo
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c 0.01
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Centi
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m 0.001
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Milli
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5
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how many sig figs in 60.052
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4
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how many sig figs in 45.42
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3
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how many sig figs in 100
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2
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how many sig figs in 0.000023
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kinetic and potential energy
|
Two classifications of energy
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kinetic
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the energy of motion
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potential energy (stored energy
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the energy of position
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calorie or joule
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two units of energy
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4.184 joules
|
1 calorie=
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nucleus
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a small, dense, positively charged region on the center of the atom
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proton, neutron, electron
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what are the 3 main subatomic particles of an atom
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atomic number
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AKA equal to the number of protons in the atom
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mass number
|
AKA equal to the sum of the number of protons and neutrons
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A-mass number
X-element symbol
Z-atomic number
|
describe the element represented
A
...X
Z
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atomic number
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the weighted average of the masses of each isotope that makes up the element
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Horizontal rows
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periods
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vertical columns
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groups or families
|
group 1
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Alkali Metal
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group 2
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Alkaline Earth Metals
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Group 17
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halogens
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Group 18
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Noble or inert gas
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Isotopes
|
are different forms of the same element
|
ions
|
electrically charged particles that result from a gain of one or more electrons by the parent atom
|
anions
|
negative ions
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cations
|
positive ions
|
ionization energy
|
the energy required to remove an electron from an isolated atom
|
the periodic law
|
the physical and chemical properties of the elements recur in a systematic and predictable way when the elements are arranged in order of increasing atomic number.
|