Electrons in Atoms
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Complete list of Terms and Definitions for Electrons in Atoms

Terms Definitions
c= vλ
Photon quanta of light
1 nm (1 nanometer) 10^-9 m
spectrum when the different frequencies separate into a spectrum of colors
Sublevel sublevels of principle energy level, represented by s,p,d, and f.
Electromagnetic Radiation Includes radio waves, microwaves, infrared wave, visible light, ultraviolet waves, x-rays, and gamma rays.
amplitude the height of the wave's crest
electron-dot structure consists of an electrons symbol, representing the atomic nucleus and inner-level electron, that is surrounded by dots representing the atom's valence electrons
ground state lowest energy level for an electron
wavelength The distance between crests of waves, such as those of the electromagnetic spectrum.
Aufbau principle an electron occupies the lowest-energy orbital that can receive it
Quantum The amount of energy required to move an electron from its present energy level to the next higher one
Hund's rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals
Quanta Max Planck discovered in 1900. It is the energy that can only exist in discrete quantities.
electron cloud visual model of the probable locations of electrons in an atom
Electron Configurations The ways in which electrons are arranged in various orbitals around the nuclei of atoms.
energy levels the fixed energies an electron can have.
lowest energy closest to the nucleus, higher the energy further away and each level gets closer
Valence Electron The electrons in an atom's outermost orbitals; determine the chemical properties of an element.
frequency number of waves that pass at a given time
atoms lose energy when electrons go to lower energy levels
pauli exclusion principle an atomic orbital may describe may describe at most two electrons.
Heisenberg Uncertainty Principle it is impossible to know exactly both the velocity and the position of a particle at the same time
Atomic orbital - Often thought as a region of space in which there is a high probability of finding an electron
energy sublevels labeled s, p, d, or f according to the shapes of the atom's orbitals
Democritus proposed the world is made up of empty space and atoms are the smallest particals
sublevels s,p,d,f
Photons Particles of light.
angular momentum quantum shape of orbital
electromagnetic spectrum includes all forms of electromagnetic radiation with the only differences in the types of radiation being their frequencies and wavelengths
gamma rays have the highest frequency and shortest wavelength
Quantum Mechanical The modern description of the behavior of electrons in atoms
electron configuration the arrangement of electrons in an atom, which is prescribed by 3 rules
James Clerk Maxwell 1873, proposed light consists of electromagnetic waves(waves with electric field component & a magnetic field running perpendicularly)
atomic emission spectrum a set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
energy of quanta E(energy of single quanta in whole numbers) = H (planck's constant/ 6.63 x 10^-34) x F (frequency of photon)............................discovered by planck 1900 after observing color changed of solids after heated.
more intense light = more packets of energy or photons. more electrons...velocity never changed. increased frequency is just changed color.
Why don't electrons fall into the nucleus? Bohr proposed a planetary model where electrons orbit the nucleus in an elliptical path much as planets orbit the sun-- earth orbits the sun so fast that it does not crash into the sun. Can only orbit at certain distances.
principle energy level ...
sphere shape of an s orbital
Low Frequency Waves Waves with long wavelengths.
Hertz SI unit of cycles per second
Electromagnetic Radiaton the radiation associated with electric and magnetic field; it caries periodically and travels at the speed if light
c=lambda*nu the speed of light, wavelength times frequency
s orbitals - spherical - the probability of finding an electron at a given distance from the nucleus does not depend on direction
3 The number of valence electrons of B, Al, Ga, In, and Tl.
photoelectric effect high energy light particles shine on piece of metal releases an electron off the metal and completes the circuit
3.00 x 10^8 m/s speed electromagnetic waves travel at in a vacuum
absorbs energy when an electron moves to a higher energy level
quatum amount of energy it takes to move an electron to another energy level
Excited State the state in which an atom had more energy than it does at its ground state
Dual nature of electron why is electron restricted to orbiting nucleus or why energy of hydrogen electron are quantisized (small discrete energy)
Niels Bohr Atomic Model - 1913 - Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus
2nd energy level can hold 8
nucleus positively charged center of an atom contains protons and neutrons
Classical theory molecule/atoms and macroscopic items are NOT governed by the same physical laws. CANNOT explain photoelectric effect. belief that any amount of energy could be released in a radiation process not in small units.
how are the orbitals diff different axes
Niels Bohr proposed that electrons must have enough energy to keep them in constant motion around the nucleus
Rutherford model small dense center, nucleus is positively charged, atom is mostly empty space
Schrodinger's equation determines shape of atomic orbitals. all about the probability of where electron would be.
Excitation When electron absorbs energy, the atom raises from its ground state to an excited state, where n = 2, 3, 4, 5, 6 and so forth - A quantum of energy in the form of light is emitted when the electron drops back to a lower energy level
Noble-Gas Configuration an outer main energy level fully occupied, in most cases, by eight electrons
de Broglie equation predicts that all moving particles have wave characteristics λ=h/mv
principal quantum numbers which the quantum mechanical model assigns to indicate the relative sizes and energies of atomic orbitals
6 The number of valence electrons of O, S, Se, Te, and Po.
energy level the specific energies an electron in an atom or other system can have
loses energy when an electron falls to a lower energy level
J.J. Thomson - 1897 - Discovers the electron - "Plum pudding model" - electrons embedded in a sphere of positive electrical charge
Orbital a region in an atom where there is a high probability of finding electrons
spin quantum number an orbital can hold 2 electrons that spin in opposite directions, electron spins 1/2 or -1/2
Speed of Light - a constant - (c) = (lampda) * (nu)
Albert Einstein - 1905 - Photons Einstein - Light could be described as quanta of energy, that behave as if they were particles Light quanta - Photons