chemistry semester 1 finals
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| manipulated variable | variable that changes
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| responding variable | variable that is observed as the result of an experiment
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| scientific method | observe, hypothesize, predict, experiment
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| matter | anything that has mass and takes up space
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| chemical change | creating a new substance by changing the composition, irreversible
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| physical change | properties of materials change but composition does not
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| chemical reaction | reactants yield product
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| compound | 2 or more elements chemically combined in fixed proportions
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| element | purest form of matter, made of 1 substance
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| reactant | substance that undergo a chemical reaction
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| product | result of a chemical reaction
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| heterogeneous | mixture of 2 or more substances that are not uniform
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| homogeneous | 2 or more substances uniformly mixed
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| law of conservation of mass | mass can not be created of destroyed
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| precipitate | solid formed from 2 aqueous reactants in a chemical reaction
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| vapor | gaseous state of substance that is a liquid of solid at room temperature
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| accuracy | how close to the expected value
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| conversion factor | ratio of equivalent measurements
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| dimensional analysis | use of conversion factors to solve problems
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| percent error | % error=|accepted-experimented|/accepted*100
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| precision | how close measurements are to each other
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| scientific notation | a base number times a power of 10
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| significant figures | accurate measurements by the right number of digits
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| atom | smallest part of matter that still holds all properties of an element
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| atomic mass | weighted average of all isotopes of that atom
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| atomic number | number of protons
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| electrons | negatively charges, JJ Thompson
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| proton | positively charged, Goldstein
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| nucleus | protons + neutrons, center of atom
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| group | up and down periodic table
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| period | left and right of periodic table
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| isotope | same number of protons but different number of neutrons
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| mass number | protons + neutrons
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| neutron | no charge, Rutherford
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| atomic orbital | 1s, 3p, 5d, 7f
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| atomic sublevels | s,p,d,f
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| aufbau's principle | electrons enter orbitals in the lowest energy level
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| electron configuration | 1s22s23p6 . . .
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| energy levels | quantum number, n=1, 2, 3, 4 . . .
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| ground state | electron is in the lowest energy level possible
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| hund's rule | electrons enter orbitals with up spin then go back and fill up with down spin
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| pauli exclusion principle | each orbital holds 2 electrons with opposite spins
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| anion | nonmetals, receive electrons, negatively charged ion
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| cation | metals, give away electrons, positively charged ion
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| periodic law | along a period elements have similar properties
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| atomic radius | distance between 2 nuclei of the same element
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| electronegativity (electron affinity) | ability to attract an electron
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| ionization energy | amount of energy it takes to remove an electron
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| metalloids | along the staircase and has both properties of metals and nonmetals
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| metals | left of staircase, good conductor, malleable, strong
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| transition metals | groups 1b to 8b
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| representative elements | groups 1a to 8a, short form
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| nonmetals | right of staircase, not good conductors, mostly gases, brittle
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| chemical formula | use symbols to show element and the number of each in a ionic compound
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| electron dot structure | element symbol surrounded by dots representing valence electrons
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| formula unit | another name for ionic compound
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| ionic bond | transfer of electrons from cation to anion
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| ionic compound | made up of metal cations and nonmetal anions
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| metallic bond | formed by attraction of free flowing valence electrons for positively charged metal ions, "sea of electrons"
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| octet rule | all elements want stable electron configuration like noble gases
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| valance electrons | electrons in the outer most shell
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| covalent bond | bonding of 2 or more nonmetals
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| diatomic molecule | H2, N2. O2, F2, Cl2, Br2, I2, nonmetals that bonds with itself
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| molecule | covalent compound
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| nonpolar | covalent bond where atoms have equal pull (0-.4)
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| polar | covalent bond in which electron are being pulled towards one atom over another (ex. H2O mickey mouse shaped)
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| pi bond | double bond, 2nd bond formed
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| sigma bond | single bond, 1st bond formed
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| polyatomic ion | covalent compound with charge
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| resonance | write 2 or more different lewis structures for the same compound
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| unshared pair electrons | lone electrons not active in bond
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| VSEPR theory | repulsion between lone electrons causes shape to bend
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| structural formula | lewis structure with dots and dashes
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| acids | H+ in front
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| bases | OH- at the end
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| binary compound | 2 elements bonded together either ionic or covalent
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| monatomic ion | single element with charge
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| law of definite proportions | chemical compounds have the same composition despite sample size
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| law of multiple proportions | elements combine in whole number rations not decimals
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| avagadro's number | 6.02*10^23
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| empirical formula | smallest ratio of a molecular formula
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| molar mass | mass of 1 mole on an element or compound
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| percent composition | % composition = (mass of element/mass of compound)*100
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| representative particles | atom, molecule, formula unit
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| activity series | ability of an element to replace another in a single replacement
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| balanced equation | has coefficients
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| chemical equations | uses symbols for reactants and products, separated by ---->
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| catalyst | speeds up chemical reaction but not involved
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| synthesis/combination | A+B--->AB
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| combustion | A+O2--->CO2+H20+heat
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| decomposition | AB--->A+B
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| single replacement | A+BC--->B+AC
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| double replacement | AB+CD--->AD+CB
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| skeleton equation | no coefficients
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| spectator ion | not involved in net ionic equations
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| actual yield | what it actually produces
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| excess reagent | left over after chemical reaction
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| limiting reagents | used up in chemical reaction, determines the amount of product produced
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| mole ration | obtained by coefficients in balance equation
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| percent yield | (actual/theoretical)*100
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| stoichiometry | calculating quantities from info provided in balanced equation
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| theoretical yield | what it should produce, have to figure it out using mole island and not given
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| measure the level of lead in the blood | analytical chemistry
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| study non carbon based chemicals in rocks | inorganic chemistry
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| investigate changes that occur as food is digested in the stomach | biochemistry
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| study of carbon based chemicals in coal | organic chemistry
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| explain the energy transfer that occurs when ice melts | physical chemistry
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| what is density of water? | 1 g/mL = 1 g/cm3
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| why is an atom positively charged when it loses an electron? | more protons than electrons
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| why is an atom electrically neutral | same number of protons and electrons
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| name 2 ways that isotopes of the same element differ | number of neutrons and mass
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| how many orbitals are in 2p energy level? | 3
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| how many sublevels are in the n=1 principle energy level? n=4 energy level | 1(s), 4(s, p, d, f)
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| what is the max number of electrons that can go into the 3p sublevel? 4f sublevel? 3d sublevel? | 6,14,10
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| what are 2 ways an ion can form from an atom | gain of lose electrons
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| compare the size of cations to its original element | cations are always smaller than the original element because it lost electrons
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| compare the size of anions to its original element | anions are alway bigger because it gained electons
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| why are ionic compounds chemically neutral? | charges on ions balance out
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| what is the different between ionic bond and covalent bond? | ionic=transfer electrons covalent=share electrons
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| what are the molecular shapes? | linear, bent, trigonal planar, trigonal pyramid, square planar, tetrahedral
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| extensive properties | properties dependent on sample size (ex. mass, volume)
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| intensive properties | properties that are not dependent on sample size but the type of matter (ex. density, color hardness, melting point, malleability)
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| democritus | 1st to suggest idea of atoms, particles that were indestructable and indivisible, no evidence
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| chadwick | neutron
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| who used the gold foil experiment? to find what? | Rutherford used it to find the nucleus
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| what were the curies responsible for | discovery of radioactivity
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| Bohr's model | electrons orbit around nucleus in a fixed path, did not work for any atom than hydrogen
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| electrons behave like _________. | waves of motion
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| quantum | the amount of energy required to move an electron from one energy level to the next
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| what happens when electrons get excited | electron gains energy and move up energy levels, when they return to ground state they emit light as result of electron transition
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| bond dissociation energy | energy needed to break a bond
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| van der waal forces (intermolecular forces) | dipole interactions, dispersion forces
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| dipole | similar properties of an ionic or polar covalent bond but much weaker, 2 polar molecules are attracted to one another
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| dispersion forces | momentary attraction of electrons due to the random motion of electron in an atom
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