Chapter 11 Flashcards
Length of a wave (measured in nm); the distance between peaks
Wavelength (T)
Energy transmitted from one place to another by light in the form of waves
Electromagnetic radiation
The vertical distance from the middle of the wave to the crest/trough
Amplitude
The top of a wave
Peak/crest
The number of waves that pass through a specific point in a given amount of time (measured in waves/sec or hertz (Hz)
Frequency (V)
Waves of electromagnetic radiation from short to long
Gamma rays, x-rays, ultraviolet, visible light, infrared, microwaves, radio waves
Light shining on a metal emits electrons
Photoelectric effect
Packets of light (quantum); particles of electromagnetic radiation (have no mass)
Photons
Planck’s equation
E=h•V
H= 6.626•10^-34
Speed of light equation
C=T•V
C=3.0•10^8
Rainbow colors within a given range
Continuous spectrum (visible spectrum)
Consists of several distinct lines of color each with its own frequency; each element has one
Bright line spectrum (line emission spectrum)
Finite quantity of energy that can be gained or lost by an atom
Quantum
Lowest energy state
Ground state
Atom has higher potential energy than at ground state
Excited state
Describes mathematically the wave properties of electrons and other very small particles
Quantum Theory
Properties of orbitals and electrons in the orbitals
Quantum numbers
3-D place around the nucleus that indicates the probable location of an electron
Orbital
Main energy level occupied by an electron; as it increases so does electrons energy and distance (1-7)
Principle quantum number (n)
Sublevels (l) indicate the shape of the orbital (s,p,d,f)
Angular momentum quantum number
Orientation of an orbital around a nucleus
Magnetic quantum number
Two values (Clockwise or counterclockwise)
Spin quantum number
Arrangement of electrons in an atom
Electron configuration
It is impossible to determine simultaneously both the position and velocity of an electron or other particles
Heisenberg principle