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- 1DaltonBilliard ball
- 2ThompsonPlum pudding
- Cathode ray tube
- Discovered electrons - 3RutherfordGold foil experiment
- Discovered nucleus - 4BohrPlanetary model
- Energy levels - 5PlanckExplained blackbody radiation experiment by Kirchoff by saying that blackbodies, when heated, emitted light in small packages called quanta rather than a continuous stream
- 6HertzPhotoelectric effect
- 7Photoelectric effectLight shone on a metal surface causes the emission of electrons from the surface. Frequency, rather than the intensity of the light, determined the energy of the emitted electrons.
- 8EinsteinExplained photoelectric effect using photons. Proposed electrons were emitted from the surface of a metal due to a collision with a photon. However, it doesn't matter how many photons strike an electron - if it doesn't have the right amount of energy, an electron won't be emitted.
- 9E=hfEnergy of a photon, with h as Planck's constant and f being the frequency in Hz (Hz=s^-1/cycles per second)
- 10c = λfc = speed of light
λ = wavelength
f = frequency - 11Energy of lighthf=KE+IE
IE=hf-KE - 12—Rydberg equation, the possible wavelengths of the photons emitted by a hydrogen atom as its electron makes transitions between different energy levels
- 13Balmer seriesThe Balmer series is the name given to a series of spectral emission lines of the hydrogen atom that result from electron transitions from higher levels down to the energy level with principal quantum number 2
- 143->2Red
- 154->2Teal
- 165->2Blue
- 176->2Purple
- 18d shellsLike to be half filled or fully filled, by taking an electron from the "s" orbital
- 19Number of e- in subshell s2
- 20Number of e- in subshell p6
- 21Number of e- in subshell d10
- 22Number of e- in subshell f14
- 23What does the number of electrons in each subshell correspond with?The number of different shapes (each shape holds two e-)
- 24Four quantum numbersn
l
ml
ms - 25Quantum numbersDescribes the energy level of the orbital and the 3D shape of the region in space occupied by an electron
- 26Principal quantum number, nDescribes the energy level. n ranges from 1 to infinity and is the "shell" around the atom. n=1 is the smallest, closest to the nucleus
- 27Secondary quantum number, l- Defines the 3D shape of the orbital
- Value ranges from 0 to n-1
- Within each shell there are n different shapes for orbitals
- Can be thought of subshells dividing each shell - 28Magnetic quantum number, ml- Defines the spatial orientation of the orbital with respect to a coordinate axes
- Has values between -l to +l, including 0
(e.g. l=1, ml = -1, 0, +1) - 29Zeeman effectIn a magnetic field, original line splits into 3
- 30Spin quantum number, ms- Ferromagnetism and paramagnetism are the result of electron spin
- Spin is described as up or down or as clockwise/counterclockwise
- Given values of -1/2 and +1/2 (never a whole #) - 31Pauli exclusion principlea) Only 2 electrons of opposite spin can occupy an orbital
b) No 2 electrons in an atom can have the same four quantum numbers - 32Aufbau principle- Fill orbitals one at a time in order of increasing energy
- 33Hund's rule- When filling e- at the same sublevel (p-orbitals), each individual orbital gets an e- before any get two e-
- 34Lewis Theory of Bonding- Atoms and ions are stable if they have a stable octet (exception: atoms from H to B after carbon)
- Electrons are most stable when they are paired
- Atoms form chemical bonds to achieve a full octet, either through an ionic or covalent bond - 35—Bonds in a VSEPR shape
- 36VSEPR theoryA method to determine the geometry of a molecule based on the idea that electron pairs are as far apart as possible
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- Fichas sobre Sin título, creado por Nadia Siddique el 28/03/2016.
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- Nadia Siddique
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