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77 Cards in this Set
- Front
- Back
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Thomson
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Cathode ray tubes --> electrons are attracted to + pole of plate, deflected by a magnet
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Millikan
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oil drop experiment --> electron has negative charge, mass is 1/2000 mass of H atom
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Rutherford
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alpha particles --> tiny amount of space with dense. + charged matter (Nucleus)
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Chadwick
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discovered neutron
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Bohr
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Bohr model of atom, orbitals, lowest energy states, energy from orbit changes
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Lavoisier
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conservation of matter
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Proust
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Definite mass percentages
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Dalton 1
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all matter is composed of atoms
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Dalton 2
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atoms are indivisible and indestructible
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Dalton 3
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Atom's mass distinguishes one atom from another
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Dalton 4
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Atoms combine in Definite Whole # Ratios when forming compounds
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Law of Conservation of Mass
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mass is neither destroyed nor created during ordinary chemical or physical reactions
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Law of Definite Proportions
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a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size or source of the compound
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Law of Multiple Proportions
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if 2+ diff. compounds are composed of the same 2 elements, then the ratio of the masses of the 2nd element combined with a certain mass of the 1st element is always a ratio of small whole proportions
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Electromagnetic Radiation
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a form of energy that exhibits wave-like behavior as it travels through space
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Types of electromagnetic radiation
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visible light, x-rays, UV light, infrared light, microwaves, radio waves
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Speed of light
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3.0*10^8 m/s
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Wavelength
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distance between crests on adjacent waves (m,cm,nm)
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Frequency
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# of waves that pass a given point in a specific time
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ratio of wavelength to frequency
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Speed of light (c) = wavelength*frequency
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Planck's constant
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6.626810^-34
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Energy of a photon equation
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E-photon = Planck's constant*frequency
(E = hv) |
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Quantum
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the minimum quantity of energy that can be lost or gained by an atom
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H-Atom Line-Emission Spectrum
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a series of specific wavelengths from when the visible portion of the emitted light is passed through a prism
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Equation for the emission of energy
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Ephoton= excited - ground
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photoelectric effect
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the emission of electrons from a metal when light shines on it, a minimum frequency of light required
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UV light
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Lyman series, longer transitions
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Red Light
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Balmer series, medium transitions
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Visible Light
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Paschen series, shorter transitions
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Light behaves as a wave in the
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Photoelectric effect and the line emission spectrum
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Light behaves as a particle when
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Quantum numbers and the Bohr's model of the atom
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Debroglie's equation
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wavelength = planck's constant/(mass*velocity)
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Quantum Mechanics theory was deriven by
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Shrodinger
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Quantum Mechanics theory parts
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Wave Functions
Energy Levels Principal Quantum Numbers |
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Principal Quantum Numbers (n)
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describe main principal energy levels/states
n = 1,2,3... |
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n^2 represents
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# possible orbitals
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2n^2 represents
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maximum # electrons
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Angular Momentum QN (l)
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type of orbital/orbital shape
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Principal QN rule
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n = 1,2,3...
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Angular Momentum QN rule
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l < n-1
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angular momentum value for s orbital
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0
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Magnetic QN meaning
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orientation of an orbital in space
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Magnetic QN rule(ml)
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-L<0<L
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Pauley Exclusion Principle
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no 2 electrons in the same atom can have the same 4 QNs
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Spin QN
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+1/2 or -1/2
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Aufbau Principle
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electrons go into the lowest energy orbitals
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Hund's rule
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electrons occupy equal energy orbitals singly with parallel spin
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Mendeleev organized periodic table according to?
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atomic mass
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Moseley organized the periodic table according to?
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atomic #
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Group 1
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Alkali metals
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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 Gases
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2 columns at bottom of periodic table are called?
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Lactanides and Actinides
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Atomic Radius horizontal pattern?
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decreasing
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Why do the atomic radii __________ horizontally?
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Increasing positive charge of nucleus, pulled closer to more protons
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Atomic Radius vertical pattern?
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increasing
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Why does the atomic radius _________ vertically?
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electrons filling successively higher main energy levels located farther from the nucleus
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Ionization Energy is...
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the energy required to remove one electron from a neutral atom of an element
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Ionization Energy horizontal pattern?
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Increasing
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reason for Ionization energy horizontal energy pattern
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increasing nuclear charge which more strongly attracts electrons in the same energy level, more difficult to remove
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Ionization energy vertical pattern?
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decreases
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Reason for vertical ionization energy pattern
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removed more easily because they are further from the nucleus
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Electron affinity is...?
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the energy change that occurs when an electron is acquired by a neutral atom
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Electron affinity horizontal pattern?
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Increasing (negatively)
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Electron affinity vertical pattern?
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decreases (negatively)
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Cation
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a positive ion
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Cationic radii and ionic radii ___ across a period?
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decrease
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Why do Cationic radii and Anionic ___ across a period?
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because electron cloud shrinks, protons have more affect
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Cationic radii and Anionic ___ down a group?
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increase
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Why do ionic radii ___ down a group?
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because outer electrons are in higher energy levels
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Anion
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a negative ion
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Electronnegativity is...?
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A measure of the ability of an atom in a chemical compound to attract electrons
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The most electronegative element is ?
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Fluorine
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Electronnegativity ____ across a period
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increases
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Why does electronnegativity ___ across a period?
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Closer to noble gas configuration
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Electronegativity ____ down a group
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decreases (in general)
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