Atomic model Flashcards
Dalton
hard ball model
J.J Thomson
Plum pudding model
Rutherford
Empty space model
Bohr
Bohr model
Quantum Mechanical model
Cloud model
Neutron
James Chadwick
Proton
Ernest Rutherford
Electron
Joseph John Thompson
Cathode Ray experiment
J.j Thomson
Gold Foil model
Rutherford
Michael Faraday
certain subs conduct electricity when dissolved in h2o called ions
Svante Arrhenius
discovered that ions are groups of atoms and didn’t need to be dissolved in water to have a charge
Robert Milikan
discovered value for electron charge
also did oil drop experiment
What letters are used to represent orbitals
s, p , d, f
Quantized energy
Electrons have a certain amount of energy at all times
What is an orbital
a subshell within a energy levels
Afbeu principal
electrons build up 1 by 1 into specific orbitals
Isoelectronic
an element has the same electron configuration as a noble gas
Aristotle
Didn’t believe that matter was made up of earth, fire, water, air, ether
Democritus
made the idea that the atom was the basic building block of matter
Empedocles
Made the idea that all matter was made up of four elements
Hunds rule
Electrons are organized in the same energy state
Erwin Schrodinger
Electrons are in orbitals in high-probability areas around the nucleus
Max planck
Came up with the idea of quantized energy
Who borrowed quantized energy and for what reason
Niels Bohr
how electrons jump or drop to different shells
Albert Einstein
light travels in streams of particles called photons
Quantum numbers
4 values are used to help locate electrons around a nucleus
Principal quantum number
describes energy level (n)
Azimuthal quantum number
describes the shape of orbital (l)
Magnetic quantum model
describes the orientation of electrons (ml)
Spin quantum number
spin direction (ms)
Pauli Exclusion principal
no 2 electron can have the same set of 4 quantum numbers
