chem ch 5 & 10 vocab
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- matter is discontinuous
- Democritus Leucippus
- very influential opposed atomic ideas said Democritus & Leucippus were wrong
- Aristotle
- John Dalton
- first atomic theory: all matter composed of atoms (elements), all atoms of same element identical (mass & size), all atoms of different element not alike (mass & size), atoms unite in simple ratios to form compounds, atoms of same element not same (isotopes) law of multiple proportions
- Antoine Lavoisier
- law of conservation of mass oxygen necessary for combustion
- John Proust
- law of definite composition
- William Crookes
- worked with vacuum tubes put gas in tubes and electricity to see what would happen vacuum tubes - crooke's tube - cathode ray tube - tv cathode ray tube
- cathode
- negative terminal
- anode
- positive terminal
- Joseph J. Thomson
- discovered cathode rays were actually electrons made Plum Pudding Model discovered electrons
- GJ Stoney
- named electron
- James Chadwick
- discovered neutron
- Goldstein
- discovered proton
- Robert Milikan
- devised "milikan's oil drop experiment" goal was to find electron mass
- Ernest Rutherford
- used alpha in experiment experiment called "alpha particle gold-foil scattering" shot alpha particles thru gold foil, screen covered with zinc sulfide, thot something of atom was positive charge, dense, massive, empty space- nucleus discovered nucleus proved Thomson's model incorrect Rutherford's model called "nuclear model of atom"
- H. Becquerel
- discovered radioactivity
- Neil Bohr
- created quantum mechanics: where electron is, how they behave (mathematical science, branch of physics), possibility
- E. Schrodinger
- model of atom called "orbital model", "wave mechanical", "quantum mechanical", "charge cloud model"
- electron
- 1/1837 mass of proton
- 1.675x10^-24g
- neutron
- proton
- 1.673x10^-24g
- law of conservation of mass
- # of reacants = # of products
- law of multiple proportions
- atoms of two or more elements may combine in different ratios to produce more than one compound
- law of definite composition
- a compound always contains two or more elements in a definite proportion by mass
- Heisenberg Uncertainty Principle
- impossible to know electron's location and velocity at same time cuz electrons are too small and constantly moving
- Aufbau Principle
- electrons enter orbitals of lowest energy first
- Pauli's exclusion principle
- atomic orbital contain at most two electrons, but have opposite spins
- Hund's Rule
- when electrons occupy orbitals of eqyal energy, one electron enters each orbital until all orbitals contain one electron with parallel spin
- alpha particles
- He+2 (2 protons, 2 neutron)
- beta particles
- high speed electron
- gamma rays
- high speed "light"
- quantum numbers
- n: principle quantum number, indicates energy level of electron. l: sublevel (azimuthal). m: orbital (magnetic). s: spin (clockwise, counterclockwise)
- orbital shapes
- s-type: spherical. p-type: lobed. d-type: multi-lobed. f-type: multi-lobed
- proton(p)
- location: nucleus. charge: +. relative mass: 1 AMU. actual mass: 1.673x10^-24g
- neutron(n)
- location: nucleus. charge: 0. relative mass: 1 AMU. actual mass: 1.675x10^=24g
- electron(e-)
- location: electron cloud. charge: -. relative mass: 1/1837 AMU. actual mass: 9.110x10^-28g
- 1 AMU
- atomic mass unit 1.6606x10^-24g
- wavelength
- lambda distance between consecutive peaks and troughs in a wave
- frequency
- measurement of the number of waves that pass a particular point per second
- speed
- measurement of how fast a wave travels thru space
- photon
- theoretically, tiny packet of energy that streams with others of its kind to produce a beam of light also what electrons give off when jumping or in their excited state
- line spectrum
- colored lines generated when light emitted by a gas is passed thru a spectroscope each element posseses a unique set of line spectra
- quanta
- small discrete increments of energy. from the theory proposed by Max Planck that energy is emitted in energy quanta rather than a continuous stream
- ground state
- lowest available energy level within an atom, electrons are "stable"
- excited state
- no room in energy level, so electrons jump to higher energy levels, "not stable", give off energy by light = "light photons"
- max # of electrons in each group
- 1. 1 2. 3 3. varies 4. varies 5. varies 6. varies 7. varies 8. varies 9. varies 10. varies 11. varies 12. varies 13. 3 14. 4 15. 5 16. 6 17. 7 18. 8