electrons in atoms
C=
3 × 10^8 m / s
Planck's constant
6.626 x 10^-34
Pauli Exclusion Principle
An atomic orbital may describe at most two electrons, each with opposite spin direction
Aufbau Principle
An electron occupies the lowest-energy orbital that can receive it
Niels Bohr
Danish physicist who studied atomic structure and radiations
D=
Double-dumbell shaped orbitals, contains up to 10
P=
Dumbell-shaped orbitals, contains up to 6
F=
Flower shaped orbitals, contains up to 14
SI unit of cycles
Hertz
How is frequency represented
V (nu) number of wave cycles
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
Bohr Theory
an electron is found only in specific circular paths or orbits around the nucleus
Schrödinger equation
an equation that describes how the quantum state of a physical system changes with time
speed of light
c=λv
The product of the frequency and the wavelength of a wave equals the
constant (c)
Hund's Rule
electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible
radiant energy
energy carried by light speed up to 3 x 10^8 per second
E=hv
energy equation
what is wavelength represented by
lambda (λ) distance between crests
Erwin Schrödinger's Model
model determines how likely it is to find an electron in various locations
Bohr Model
model of the atom in which electrons move rapidly around the nucleus in paths called orbits
S=
spherical orbitals, contains up to 2
electron configuration
the arrangement of electrons in an atom
quantum of energy
the minimum quantity of energy that can be lost or gained by an atom
quantum mechanical model
the modern description, primarily mathematical, of the behavior of electrons in atoms