Chapter 5: Electrons in Atoms Flashcards
amplitude
the wave’s height from the origin to a crest, or from the origin to a trough
atomic emission spectrum
the set of frequencies of the electromagnetic waves emitted by atoms of the element. Each element has its own unique spectrum.
(think of neon signs and how they only come in specific colors.)
atomic orbital
a 3-D region around the nucleus. It describes the electron’s probable location.
aufbau principle
a
de Broglie equation
λ=h/mv
m= particle of mass v= velocity
predicts that all moving particles have wave characteristics
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space. According to Einstein in 1905, is both wavelike & particle like
electromagnetic spectrum
aka the EM spectrum. Encompasses all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths.
(short λ bend more than long λ, which results in the Roy. G. Biv sequence)
electron configuration
a
electron-dot structure
a
energy sublevel
labeled s, p, d, f (Smart People Do Fine or Stupid Ppl Do Fail), contained in the principal energy levels. The # of energy sublevels in a principal energy level INCREASES AS n INCREASES.
frequency
(represented by v) the number of waves that pass a given point per second.
ground state
the lowest allowable energy state of an atom.
When atoms gain energy they are said to be in an excited state.
Heisenberg uncertainty principle
states that it is fundamentally impossible to know precisely both the VELOCITY and POSITION of a particle at the same time
Hund’s rule
a
Pauli’s exclusion principle
a
photoelectric effect
electrons (photoelectrons) are emitted from a metal’s surface when light of a certain frequency shines on the surface.
Ex: calculator
photon
a particle of electromagnetic radiation with no mass that carries a quantum of energy
photon’s energy:
E = hv
photon
Planck’s constant
has a value of 6.626x10^-34 J*s
J= joule (SI unit of energy)
For a given v, matter can emit or absorb energy only in whole-# multiples of hv.
principal energy level
n specifies the atom’s major energy levels. (see principal quantum number). An atom’s lowest principal energy level is given a principal quantum # of 1.
principal quantum number
(n) indicates the relative sizes and energies of atomic orbitals. As n increases, the orbital becomes larger, the e- spends more time farther from the nucleus, and the atom’s energy level increases.
quantum
the minimum amount of every that can be gained or lost by an atom
quantum mechanical model of the atom
the atomic model in which electrons are treated as waves (aka the wave mechanical model of the atom) Created by Austrian Erwin Schrodinger, this model makes no attempt to describe the electron’s path around the nucleus.
valence electron
a
wavelength
(represented by λ) the shortest distance between equivalent points on a continuous wave.
Ex: crest-crest or trough-trough
