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29 Cards in this Set
- Front
- Back
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Datlon's theory |
all matter is composed of tiny indivible particles called atoms atoms cannot becreated nor destroyed atoms of the sameelement are alike in every way atoms of differentelements are different atoms can combinetogether in small numbers to form molecules |
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who discovered electrons |
JJ Thomson using cathode rays (electron megentic nature plum pudding model |
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Who discovered the positiv charged nucleus |
rutherford using the gold foil experiment |
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isotopes |
have the same number of protons and same chemical properties (besides melting and boiling point) but different number of neutrons |
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electromagnetic waves |
travel at the same speed but have different wavelengths, frequencies, and energy |
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equation for speed |
speed= wavelength*frequency speed = speed of light (3*10⁸) |
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continuous spectrum |
mixture of different lights at different wavelengths (colors) like a rainbow when white light is passed through a prism |
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absorption line spectrum |
mostly colors with the corresponding wavelengths missing radiation absorbed when atoms move from lower to higher energy |
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emission line spectrum |
only colors of wavelengths showing radiation emitted when atoms move from higher to lower energy |
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what happens when atoms absorb energy |
electrons are moving in a higher energy level which is more unstable (excited state) |
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what happens when atoms are at its ground state |
electrons are at its lowest level and energy is released in the form of electromagnetic radiation |
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photon |
packet of energy |
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energy= |
placnk's constant (6.63*10⁻³⁴)*frequency |
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Why do atoms emit photons at certain frequencies |
due to the certain orbits they have |
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electrons cannot |
change its energy in a continuous way |
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quantized |
electrons can only change its energy levels in discrete amounts |
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hydrogen spectrum |
produces visible light where electrons fall to the 2nd level, UV ti the 1st, infared to 3rd or higher lines converge at higher energy levels because the energy levels are close together at higher energies refers to the paschen, balmer, and lyman spectrum diagram |
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light behaves as both |
packets of energy and waves diffraction/spreading out of light when it passes through a small slit is explained by wave model scattering of electrons that occur when light is incident on a metal surface is best explained with particle model |
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electrons are often best seen as having what type of properties |
wave-like |
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uncertainty principle |
we cannot know where an electron is at any moment but we can find the probablity of its location |
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when transition metals form ions |
they lose 4s electrons |
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3d sublevels are written with its energy level 3 sub-levels after 4s is filled |
cording and more |
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who sat that electrons had fixed orbitals |
bohr in 1913 electrons share fixed orbitals quantum of energy is needed for an electron to move one energy level to another |
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quantum mechanic model |
about stimated probablity of where electrons are found |
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AZ notation |
top-mass bottom-protons |
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atomic mass |
mass of an atom that refers to what each kid got |
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electromagnetic spectrum |
radio waves microwaves infrared visible ultraviolet x-rays gamma rays |
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properties of electromagnetic spectrum |
large waves, small energy, small frequency high frequency, high energy, small wavelengths |
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stuff to know outside the flashcards |
how to calculate atomic mass, average mass, and determine protons, neutrons, and electrons understand and be able to use diagrams made from the spectrometer (and know the parts of the spectrometer) hydrogen orbitals electron configuration |
