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dimeng
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safety
Be familiar with activity before beginning, get approval for student designed procedures, wear appropriate clothing, do not wear contact lenses in the lab, and know the location of all safety equipment
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physical property
a characteristic that can be observed without changing the identity of the substance
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physical change
a change in a substance that does not involve a change in identity
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mixture
a blend of two or more kinds of matter, each of which retains its own identity and properties
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homogeneous
uniform in composition
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heterogeneous
not uniform in composition
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organic chemistry
study of most carbon-containing compounds
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inorganic chemistry
study of non-organic substances, many of which have organic fragments bonded to metals (organometallics)
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physical chemistry
study of the properties and changes of matter and their relation to energy
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analytical chemistry
identification of the components and composition of materials
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biochemistry
study of substances and processes occurring in living things
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theoretical chemistry
the use of mathematics and computers to understand the principles behind observed chemical behavior and to design and predict the properties of new compounds
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chemistry
the study of the composition, structure, and properties of matter, the processes that matter undergoew, and the energy chagnes that accompany these processes
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chemical
any substance that has a definite composition
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basic research
used for only increasing knowledge
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applied research
used to solve a problem
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technological development
involves the production and use of products that improve quality of life
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element
pure substances that cannot be decomposed by chemical changes
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compound
a substance that can be broken down into simple stable substances, elements bonded chemically
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extensive properties
properties that depend on the amount of a substance that is present eg. mass
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intensive properies
do not depend on the amount of a substance that is present eg. melting point
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mass
a measure of the amount of matter
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matter
anything that has mass and takes up space
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volume
the amount of three-dimensional space an object occupies
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chemical change
a change in which one or more substances are converted into different substances
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noble gases
group 18; have complete set of valence electrons (8 except He, which has 2); not reactive
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reactants
substances that react with one another/energy to form product(s)
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products
the results of a chemical change/reaction
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gas
indefinite volume and indefinite shape; particles move very rapidly and are at great distances from one another compared with the particles of liquids and solids, meaning attractive forces have less of an effect
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solids
definite volume and definite shape
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liquids
definite volume and indefinite shape
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conservation of energy
energy is neither destroyed nor created
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heterogeneous examples
salad, clay and water mixture
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homogeneous examples
salt water, sugar water
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metalloids
an element that has some characteristics of metals and some haracteristics of nonmetals
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scientific method
a logical approach to solving problems by observing and collecting data, formulating hypotheses, testing hypotheses, and formulating theories that are supported by data
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the two types of data
qualitative and quantitative
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qualitative
description/qualities
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system
a specific portion of matter in a given region of space that has been selected for study during an experiment or observation
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hypothesis
testable statement
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model
an explanation of how phenomena occur and how data or events are related
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theory
broad generalization that explains a body of facts or phenomena
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quantity
something that has magnitude, size, or amount eg. volume, not teaspoon
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derived units
combinations of SI base units
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density
mass/volume, kg/cubic meter
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difference between weight and mass
weight is effect of gravity; mass is regardless of gravity
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density of pure substances
can be used to identify substances
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calculating density
mass/volume
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converting volume units
cubic meter contains 1million cubic cm
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conversion factor
a ration derived from the equality between two different units that can be used to convert from one unit to the other eg. 4 quarters/1 dollar
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precision
the closeness of a set of measurements of the same quantity made in the same way
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accuracy
the closeness of a measurement to the correct or accepted value of the quantity measured
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percent error
((experimental value - accepted value)/accepted value)*100
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significant figures
all certain digits plus one estimated digit
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significant zeros
zeros at the end and to the right of a decimal point are significant;9.000
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adding or subtracting with significant figures
highest place value significant figure in least specific number in problem is highest place value significant figure in answer
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multiplying or dividing with significant figures
number of figures in number with less significant figures in problem is number of significant figures in answer
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inversely proportional
one value increases as another decreases; negative slope of line if graphed
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Dalton's atomic theory
matter is composed of atoms, atoms of one element are identical in size, mass, and other properties; of different elements are different, atoms cannot be divided, created, or destroyed, atoms combine to form chemical compounds, and in chemical reactions, atoms are combined, separated, or rearranged
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law of definite propportions
a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size or source of the sample
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law of conservation of mass
mass is neither created nor destroyed during ordinary chemical reactions or physical changes
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law of multiple proportions
if two or more different compounds are composed of the same two elemetns, then the ration of the masses of the second element combined with a certain mass of the first element is always a ration of small whole numbers
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modern atomic theory
atoms can be further divided and atoms of the same element can have different masses, but atoms of the same element do share properties, and all matter is composed of atoms
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thomson's cathode ray tube experiment
discovery of electrons led to by passage of electric current through a cathode which showed existance of negatively charged particles
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rutherford's gold foil experiment
ernest rutherfort shot positively charged particles at extremely thin gold foil, and some were reflected, showing a positive particle in the atom
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rutherford's discovery of the nucleus
rutherford reasoned based on his gold foil that the region of positive charge must have very low volume and high density because it only reflected about 1/8000 strongly
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nuclear forces
forces of attraction between protons and neutrons
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isotopes
atoms of same elements with different atomic mass
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atomic mass
number of protons in an atom
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average atomic mass
the weighted average of the atomic masses of the naturally occurring isotopes of an element
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atomic mass unit
1/12 the mass of a carbon-12 atom
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mole
amount of a substance that contains as many particles as there are atoms in exactly 12 grams of carbon-12
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avogadro's number
the number of particles in exactly one mole of a pure substance, 6.022*10 to the 23rd
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relative mass
mass of atoms is measured relatively to carbon-12
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converting moles to atoms
given/Avogadro's number
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converting moles to grams
given*molar mass of element
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converting atoms to grams
given/Avogadro's number*molar mass
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wave behavior of electromagnetic radiation
speed of 3*10 to the 8th, frequency varies inversely proportionally to wavelength
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photon
particle of electromagnetic radiation having zero mass and carrying a quantum of energy
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line emission spectrum
a set of specific frequencies of electromagnetic radiation emitted as a result of excitement of an atom's electrons
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Bohr's model of the atom
electrons exist at specic energy levels, and can lose only specific amounts of energy
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ground state
all electrons in the atom are at their lowest possible energy levels
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excited state
electrons in the atom are at higher energy levels than their minimum energy levels
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Bohr's atomic theory
when an electron absorbs energy, it moves up a level(s). when it loses energy, it moves down energy levels
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4 quantum numbers
principal, angular momentum, magnetic, and spin
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principal quantum number
symbolized by n, indicates main energy level, positive integer
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angular momentum quantum number
symbolized by l, indicates shape of orbital, positive integers less than n
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magnetic quantum number
symbolized by m, indicates orientation of an orbital around the nucleus, values are integers from -l to +l
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spin quantum number
indicates spin direction, either + or - 1/2
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Aufbau principle
an electron occupies the lowest-energy level that can receive it
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Pauli exclusion principle
no two electrons in the same atom can have the same set of 4 quantum numbers
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Hund's rule
no orbital can hold a second electron until all other orbitals of the same amount of energy have at least 1 electron
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DeBroglie
proposed that electrons may behave as waves
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wave behavior of electrons
electron waves can exist only at certain frequencies, electrons can be diffracted and interfere
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Heisenberg Uncertainty Principle
it is impossible to determine simultaneously the position and velocity of an electron or any other particle
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s orbital
spherical, one per energy level
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p orbital
dumbell-shaped w/ small hole, three per energy level
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d orbital
5 per energy level
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f orbital
7 per energy level
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electron configuration of ground state selenium
1s2;2s2;2p6;3s2;3p6;3d10;4s2;4p4
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mendeleev's contribution to the periodic table
designed first periodic table in order of increasing atomic mass
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