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37 Cards in this Set

  • Front
  • Back
Dalton
said that an atom was just a dense, positive nucleus, and was wrong because it did not have electrons and said that the nucleus was the smallest particle
Thomson
said that an atom was a dense, positively charged nucleus with electrons scattered through i- did not have orbitals, not in nucleus
Rutherford
didn't know about nuclei
Bohr
said that an atom had electrons traveling in circular motions around a positive nucleus- electrons were actually in orbitals
Electron
a small, discrete unit of energy that CANNOT exist between energy levels
Quantum Energy
the energy it takes to move an electrons from its present energy level to the next higher one
Quantum Mechanical Model
Estimates the probability of finding an electron in a certain position
Different from previous because now has orbitals
principal quantum numbers (n)
major energy levels of electrons
how are px, py, and pz similar and different
have the same number of electrons, but face different ways and have increasing energy
Maximum number of electrons that can occupy a principle energy level
n^2
orbitals
the way in which electrons are arranged around the nuclei of atoms
Aufbau principle
electrons enter orbitals of lowest energy first
works for every element in the periodic table
Pauli exclusion principle
an atomic orbital may describe at most two electrons
Hund's rule
when electrons occupy orbitals of equal energy, one electron enters each orbital unitl all the orbitals contain one electron with parallel spins.
amplitude
the wave's height from the origin to the crest
wavelength
the distance between two crests
frequency
the number of wave cycles to pass a given point per unit of time
electromagnetic spectrum
what is given when passing the light emited by an element through a prism
ground level
the lowest possible energy of an electron
electrons moving from higher to lower levels
lose energy and emit light
Quantum mechanics
the new method of describing the motions of subatomic particles, atoms, and molecules
Principal quantum number
the number of sub levels within that principal energy level
Quantum
the amount of energy required to move an electron from its present energy level to the next higher one
atomic orbitals
the regions around the nucleus within which the electrons have the highest probability of being found
energy level
a region of space around the nucleus of an atom where an electron is likely to be moving
electromagnetic spectrum
the total range of electromagnetic radiation, from the longest radio waves to the shortest gamma waves
orbital
a region of an atom in which there is a high probability of finding one or more electrons
excited state
the condition of an atom in a higher energy state than ground state
line-emission spectrum
distinct lines of colored light that are produced when the light produced by excited atoms of an element is passed through a prism
according to bohr, the further the electron is from the nucleus, the ________ its energy
greater
what happens when an electron moves from a higher (excited) energy state to lower energy level in terms of electromagnetic radiation
releases energy in the form of a wavelength, which corresponds to a certain type of electromagnetic radiation
Periodic law
when the elements are arranged according to their atomic number, theres a periodic repetition of physical and chemical properties
Mendeleev
first chemist to arrange the elements into a periodic table, and arranged them according to weight (atomic mass), which resulted in gaps in the table and various elements being switched out of order
Moseley
used x-ray spectra to prove the existence of the proton, and arranged the periodic table much more effectively according to atomic number, and this is how the modern periodic table is arranged and there are no more gaps
Maximum number any element can have of valence electrons
8
the number of valence electrons dictates the number of ___ an element can form
bonds
the number of bonds an element can form dictates the elements
chemical properties