Section 1
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Cards (65)
Section 1
(50 cards)
Node
A point with no energy
Speed of Light
3.00 x 10^8
Quantum Theory
Energy moves in levels and is not continuous
D-Subshell
5 Orbitals and can hold up to 10 electrons
Formula used to find λ or Frequency
C=λf. λ has to be in meters
Orange
λ= 650 nm
Indigo
λ= 450 nm
Classical Theory
Energy moves continuously upwards on a ramp
Quantization
The concept that energy can occur only in discrete units called quanta
Properties of Electrons
A free electron with velocity has a wavelength.
Violet
λ= 400 nm
Quantum Number
A set of numbers used to identify the election's position in the atom.
Amplitude
The vertical distance from the midline of a wave to the crest or trough and is related to the wave intensity. The higher it is the brighter it is.
Atomic Spectra
The component wavelengths of the light given off from a glowing gas
Relationship between λ and frequency
Inversely proportional
Standing Wave
A pattern of vibration that simulates a wave that is standing still
Electromagnetic Spectrum
All of the frequencies or wavelengths of electromagnetic radiation
Photon
A particle of electromagnetic radiation with no mass that carries a quantum of energy. If it has enough energy the electron will be ejected
X-ray
after ultraviolet; come from stars and Sun
Blue
λ= 500 nm
Plank's Theory
Vibrating atoms in a heated object give rise to the certain EM Radiation
Yellow
λ= 600 nm
Electron Configuration
The arrangement of electrons in the orbitals of an atom
P-Subshell
Dumbbell shaped and can hold up to 6 electrons
Coulomb's Law
The relationship among electrical force, charges, and distance
Hydrogen's Atomic Spectra
Violet, Blue-Violet, Green, Red
Uncertainty Principle
It is impossible to know an electron's position in the atom.
Photoelectric Effect
The emission of electrons from a metal surface induced by light.
Bohr Model
model of the atom in which electrons move rapidly around the nucleus in paths called orbits
Black Bodies
An object that absorbs all radiation falling on it, at all wavelengths
The Nature of Light
Light behaves as a particle and a wave
Quantum Behavior
What behavior do electrons exhibit?
Beer's Law
Explains the relationship between absorbance, at a given wavelength and concentration, A = εbc
Wave Mechanical Model
Modern model of the atom, atoms have electrons in "orbitals" that are like clouds around the nucleus
Green
λ= 550 nm
Electromagnetic Waves
A form of a standing wave that is produced by the vibrational motion of electrically charged particles.
Ultraviolet
Electromagnetic waves of frequencies higher than those of violet light.
Spectrophotometry
Measurement of quantity of matter in solution by passing light through spectrum
Antinode
A point of maximum amplitude on a standing wave
Electron Density
The relative probability of finding an electron in a certain region of space.
Aufbau Principle
An electron occupies the lowest-energy orbital that can receive it
Frequency (v.)
The number of waves (cycles) per second that pass a given point in space.
Valence Electron
Electrons found in the outermost electron shell
S-Orbitals
Spherical & contain a max of 2 electrons
Ground State
Lowest energy level an electron can be. Some electrons can be at a higher level if the lowest level is full.
Schrodinger's Cat
A metaphor used to explain quantum mechanics
Red
λ= 700 nm
Wavelength (λ)
The distance between two consecutive peaks or troughs in a standing wave.
Gamma
Electromagnetic waves with the shortest wavelengths and highest frequencies
Quantum
A packet of energy that emits light
Section 2
(15 cards)