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Chem 04 Atoms

Terms associated with development of Atomic Theory through Bohr

matter is neither created nor destroyed during (chemical or physical) changes; mass of reactants = mass of products... this is the law of _?_ conservation of mass
elements that chemically combine do so in consistent proportions by mass... this is the law of _?_ definite proportions
gaseous elements that react do so in simple ratios by volume... this is the law of _?_ combining gas volumes
when two elements combine in more than one definite ratio by mass, fixing the mass of the first element reveals the masses of the second element form simple, whole # ratios... this is the law of _?_ multiple proportions
he proposed the first atomic theory (had 5 basic ideas or 'tenets') Dalton
smallest part of element that retains its properties; the building block of matter atom
made of only one kind of atom element
Dalton 1: matter is composed of tiny particles called _?_ atoms
Dalton 2: atoms cannot be _?_, _?_, or _?_ created, destroyed, broken
Dalton 3: atoms of the same element are _?_ identical
Dalton 4: atoms of different elements are _?_, specifically in their _?_ different; weight
Dalton 5: when atoms combine, they do so in simple _?_ whole number ratios
device used by Thomson to discover electrons, the first subatomic particle (plum pudding model) cathode ray tube (CRT)
procedure used by Rutherford to identify and measure characteristics of the atomic nucleus by firing alpha particles at a metal target gold foil experiment
he developed an atomic model placing electrons at specific distances from the nucleus based on specific light frequencies emitted by atoms Bohr
one of the 'fixed' paths followed by electrons as they orbit the nucleus energy level
small, super dense, positive center of atom nucleus
negatively charged region surrounding atom's nucleus electron cloud
positively charged subatomic particle located in nucleus and having a mass of 1 amu proton
1/12th the mass of a C-12 isotope, used for measuring relative mass of atoms amu (u, or dalton)
negatively charged subatomic particle orbiting nucleus, having a mass of nearly 0 amu electron
subatomic particle having no charge (0), a mass of about 1 amu, and located in nucleus neutron
Millikan's procedure for determining the exact mass and charge of an electron oil drop experiment
it tells the number of protons in the nucleus of an atom atomic number
sum of protons + neutrons in atom's nucleus mass number
atoms of same element but with different # of neutrons isotopes
specific isotope used to define the atomic mass unit C-12
way of 'naming' an isotope using super- and subscripts nuclear symbol
name of the H-1 isotope containing 1 e- orbiting 1 p+ protium
name of the H-2 isotope containing 1 e- orbiting 1 p+& 1 n deuterium
name of the rare, radioactive H-3 isotope containing 1 e- orbiting 1 p+ & 2 n's tritium
weighted average of the naturally occurring isotopes of an element atomic mass
quantity found by using the equation "mass # - atomic #" # of neutrons
overall charge of a normal, uncombined atom in which the # of p+ = # e- neutral
maximum capacity of the 1st energy level 2
maximum capacity of the 2nd energy level 8
maximum capacity of the 3rd energy level 18
term used by Democritus to describe indivisible particles he thought matter might be made of (Greek for "uncuttable") atomos
order of discovery of the 3 major subatomic particles electron, proton, neutron
"A.P.E." in A.P.E.M.A.N. means _?_ atomic # = # protons = # electrons
"M.A.N." in A.P.E.M.A.N. means _?_ mass # – atomic # = # neutrons
if an element naturally occurs as nearly or completely one isotope, its atomic mass on the periodic table will be very close to a _?_ whole number
if you know the # of isotopes, their % abundance, and relative mass... you can calculate _?_ average atomic mass
equation for calculating the # of electrons required to fill any energy level "n" 2n^2
the condition of an electron when at its lowest possible energy ground state
describes an electron at a higher than normal energy level excited
a change of energy levels (up or down) of an electron transition
experiment that identifies metal ions by the color of light they make in a fire flame test
light 'fingerprint' emitted by a gaseous element when electrically stimulated emission (bright-line) spectrum
crest to crest distance of a wave wavelength
# of waves that pass a point per second frequency
SI unit of frequency hertz
math relationship between frequency and wavelength for waves in a particular medium inversely proportional
mnemonic for remembering visible light spectrum from longest to shortest wavelength ROY G. BIV
wavelength range of the visible spectrum 400 - 700 nanometers
10^-9 meters nanometer
'speed of light' abbreviation and # c (3.00x10^8 m/s)
variable/letter that stands for wavelength λ
the electron transition from upper level to the 1st produces _?_ light ultraviolet
the electron transition from upper level to the 2nd produces _?_ light visible
the electron transition from upper level to the 3rd produces _?_ light infrared
Created by: goakley



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