Test 2 Flashcards
Discovered the atomos
- solid, homogenous, indivisible, indestructible
- properties of matter are due to shape and movement of atoms
- atomos cannot change
Democritus
Original founder no one believed
4 elements
Earth fire water air
Aristotle
Confirmed the existence of atoms and that they are indestructible cannot be divided created or destroyed
Dalton
Used cathode rays to discover electrons and then created the Plum Pudding Model
(Electrons floating around in positively charged matter)
Thomson
Oil drop experiment
Determined exact charge of electron: 1.6 * 10 ^-19 coulombs
Millikan
Gold Foil Experiment proved plum pudding wrong by discovering the nucleus “alpha particles”
Electrons orbit around nucleus
Rutherford
Found the proton
Goldstein
Found the neutrons
Chadwich
Model of the atom newer version of Rutherford using quantum mechanics with a positively charged nucleus orbited by negatively charged electrons
Bohr
a kind of radiation including visible light, radio waves, gamma rays, and X-rays, in which electric and magnetic fields vary simultaneously.
Electromagnetic radiation
two electrons occupying the same orbital in an atom or molecule.
Electron pair
the lowest energy state of an atom or other particle.
Ground state
The exhibition of both wavelike and particlelike properties by a single entity, as of both diffraction and linear propagation by light.
Wave-particle nature
a particle representing a quantum of light or other electromagnetic radiation. THIS carries energy proportional to the radiation frequency but has zero rest mass.
Photon
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom’s nucleus.
Electron cloud
the rate at which a vibration occurs that constitutes a wave, either in a material (as in sound waves), or in an electromagnetic field (as in radio waves and light), usually measured per second.
Frequency
cursive l - measure of orbital angular momentum, shape of the orbital
Orbital quantum number (sub shell)
n - describes the energy level
ℓ - describes the subshell
mℓ - describes the orbital of the subshell
ms - describes the spin
quantum numbers
n- distance of the electron from the nucleus as “n” increases the radius increases
Principle quantum number = shell = energy level
M- orbital around the 3 axes in space (orientation in space)
Magnetic quantum number
the number of protons in the nucleus of an atom determines the chemical properties of an element and its place in the periodic table.
Atomic number
the total number of protons and neutrons in a nucleus.
Mass number
unit of mass used to express atomic and molecular weights, equal to one-twelfth of the mass of an atom of carbon-12. It is equal to approximately 1.66 x 10-27 kg.
Amu = atomic mass unit
mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes.
Atomic mass
Neutrons
No charge
Located in nucleus
Discovered by Chadwick
This + protons = mass number
Protons
Discovered by Goldstein Positive charge In nucleus This = atomic # This + neutrons = mass #
Electrons
Negative charge
Same as protons when there Is no charge
orbit the nucleus
Discovered by Thomson
An atom or group of bonded atoms that have a positive or negative charge
Ion
Atoms of the same element that have different masses
Isotope
An electron configuration notation in which only the valence electrons of an atom of a particular element are shown
Electron dot structure
Particle that makes up protons and neutrons
Quark
The emission of electrons from a metal when light shines on the metal
Photoelectric effect
M(little)s tells the electrons spin on it’s axis
Spin quantum number
a band of colors, as seen in a rainbow, produced by separation of the components of light by their different degrees of refraction according to wavelength
Spectrum
The distance between corresponding points on adjacent waves
Wavelength
the speed at which light travels in a vacuum; the constancy and universality of the speed of light is recognized by defining it to be exactly 299,792,458 meters per second
Speed of light
Orbital
Region within an energy level where there is a probability of finding an electron
A state in which an atom has a higher potential energy than it has in it’s ground state
Excited state
waves that travel through a secondary object. Water is an example
Wave mechanical model
Hunds rule
Within a sublevel place 1 e per orbital before pairing them
Pauli exclusion principle
2 electrons in same orbital must have opposite spins
Afbau principle
Electrons fill the lowest energy orbitals 1st
It is impossible to determine simultaneously both the position and velocity of an electron or any other particle
Heisenberg uncertainty principle
